DEPARTMENT OF CHEMISTRY

BSc. (Hons.) Chemistry

Category-I
DISCIPLINE SPECIFIC CORE COURSE -1 (DSC-1):
Atomic Structure & Chemical Bonding

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE

COURSE

Course t itle & Credits Credit distribution of the course Eligibility Pre-
Code Lecture Tutorial Practical/ criteria requisite o f
Practice the course
(if any)
Atomic Structure 04 03 __ 01 Physics, --
& Chemical Chemistry,
Bonding (DSC- Mathematics
1: Inorganic
Chemistry -I)

Learning Objectives

The course reviews the structure of the atom, which is a necessary pre-requisite in
understanding the nature of chemical bonding in compounds. It provides basic knowledge
about ionic and covalent bonding, and explains that chemical bonding is best regarded as a
continuum between the two cases. It discusses the periodicity in properties with reference to
the s and p block, which is necessary in understanding their group chemistry. The student will
also learn about the fundamentals of acid-base and redox titrimetric analysis.

Learning outcomes
By the end of the course, the students will be able to:

● Solve the conceptual questions using the knowledge gained by studying the quantum
mechanical model of the atom, quantum numbers, electronic configuration, radial and
angular distribution curves, shapes of s, p, and d orbitals, and periodicity in atomic radii,
ionic radii, ionization enthalpy and electron affinity of elements.
● Draw the plausible structures and geometries of molecules using radius ratio rules,
VSEPR theory and MO diagrams (homo- & hetero-nuclear diatomic molecules).
● Understand the concept of lattice energy using Born-Landé and Kapustinskii equation.
● Calibrate the apparatus used in titrimetric analysis and prepare standard solutions for
titration
● Understand the theory and application of various acid-base and redox titrations.
● Comprehend the theory of acid-base indicators

96
SYLLABUS OF DSC-1

UNIT – I (15 Hours)

Unit 1: Atomic Structure
Recapitulation of concept of atom in ancient India, Bohr’s theory & its limitations, atomic
spectrum of hydrogen atom.
de Broglie equation, Heisenberg’s Uncertainty Principle and its significance. Postulates of
wave mechanics, Time independent Schrödinger’s wave equation, well behaved wave
function, significance of ψ and ψ2. Quantum mechanical treatment of H- atom, Quantum
numbers and their significance. Normalized and orthogonal wave functions. Sign of wave
functions. Radial and angular wave functions for hydrogen atom. Radial function plots,
radial probability distribution plots, angular distribution curves. Shapes of s, p, and d orbitals,
Relative energies of orbitals.

Pauli’s Exclusion Principle, Hund’s rule of maximum spin multiplicity, Aufbau principle
and its limitations.

UNIT – II (6 Hours)
Unit 2: Periodic properties of Elements & Periodic Trends
Brief discussion of the following properties of the elements, with reference to s- & p-
block andtheir trends:
(a) Effective nuclear charge, shielding or screening effect and Slater’s rules
(b) Atomic and ionic radii
(c) Ionization enthalpy (Successive ionization enthalpies)
(d) Electron gain enthalpy
(e) Electronegativity, Pauling’s scale of electronegativity. Variation of electronegativity
with bond order and hybridization.

UNIT – III (12 Hours)

Unit 3: Ionic bond
General characteristics, types of ions, size effects, radius ratio rule and its limitations.
Packing of ions in crystals. Lattice energy, Born-Landé equation with derivation, Madelung
constant, importance of Kapustinskii equation for lattice energy. Born-Haber cycle and its
applications.
Covalent character in ionic compounds, polarizing power and polarizability. Fajan’s rules
and consequences of polarization.

UNIT – IV (12 Hours)

Unit 4: Covalent bond
Valence shell electron pair repulsion (VSEPR) theory, shapes of the following simple
molecules and ions containing lone pairs and bond pairs of electrons: H2O, NH3, PCl3, PCl5,

97
SF6, ClF3, I3, BrF2+, PCl6-, ICl2- ICl4-, and SO42-. Application of VSEPR theory in
predicting trends in bond lengths and bond angles.
Valence Bond theory (Heitler-London approach). Hybridization, equivalent and non-
equivalent hybrid orbitals, Bent’s rule.
Ionic character in covalent compounds: Bond moment and dipole moment. Percentage ionic
character from dipole moment and electronegativity difference.
Molecular orbital diagrams of homo & hetero diatomic molecules [N2, O2, C2, B2, F2, CO,
NO] and their ions; HCl (idea of s-p mixing and orbital interaction to be given).

Practical component
Practicals: Inorganic Chemistry-I (30 Hours)
(Laboratory periods: 15 classes of 2 hours each)
1. Titrimetric Analysis:
(i) Calibration and use of apparatus
(ii) Preparation of solutions ofdifferent Molarity/Normality.

2. Acid-Base Titrations: Principles of acid-base titrations to be discussed.

(i) Estimation of oxalic acid using standardized NaOH solution
(ii) Estimation of sodium carbonate using standardized HCl.
(iii) Estimation of carbonate and hydroxide present together in a mixture.
(iv) Estimation of carbonate and bicarbonate present together in a mixture.

3. Redox Titration: Principles of oxidation-reduction titrations to be discussed.

(i) Estimation of oxalic acid using standardized KMnO4 solution
(ii) Estimation of water of crystallization in Mohr’s salt by titrating with KMnO4.
(iii) Estimation of oxalic acid and sodium oxalate in a given mixture.

Essential/recommended readings
References:
Theory :

1. Lee, J.D. (2010), Concise Inorganic Chemistry, Wiley India.

2. Huheey, J.E.; Keiter, E.A.; Keiter; R. L.; Medhi, O.K. (2009), Inorganic
Chemistry-Principles of Structure and Reactivity, Pearson Education.
3. Douglas, B.E.; McDaniel, D.H.; Alexander, J.J. (1994), Concepts and Models of
Inorganic Chemistry, John Wiley & Sons.
4. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010),
Shriver and Atkins Inorganic Chemistry, 5th Edition, Oxford University Press.
5. Pfennig, B. W. (2015), Principles of Inorganic Chemistry. John Wiley & Sons.
6. Housecraft, C. E.; Sharpe, A. G., (2018), Inorganic Chemistry, 5th Edition, Pearson.
7. Wulfsberg, G (2002), Inorganic Chemistry, Viva Books Private Limited.
8. Miessler, G.L.; Fischer P.J.; Tarr, D. A. (2014), Inorganic Chemistry, 5th Edition,
Pearson.

98
9. Shiver, D.; Weller, M.; Overton, T.; Rourke, J.; Armstrong, F. (2014), Inorganic
Chemistry, 6th Edition, Freeman & Company
10. Das, A. K.; Das, M. (2014), Fundamental Concepts of Inorganic Chemistry, 1st
Edition, Volume CBS Publishers & Distributors Pvt. Ltd.

Practicals:
1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook
of Quantitative Chemical Analysis, John Wiley and Sons.
2. Harris, D. C.; Lucy,C. A.(2016), Quantitative Chemical Analysis, 9th Edition, Freeman
andCompany

Note: E xamination s cheme a nd m ode s hall be a s pr escribed by t he E xamination

Branch, University of Delhi, from time to time.

DISCIPLINE SPECIFIC CORE COURSE – 2 (DSC-2): Basic Concepts and

Aliphatic Hydrocarbons

Credit distribution, Eligibility and Prerequisites of the Course

Course t itle & Credits Credit distribution of the course Eligibility Pre-requisite
Code Lecture Tutorial Practical/ criteria of the course
Practice (if any)
Basic Concepts 04 03 -- 01 Physics, --
and Aliphatic Chemistry,
Hydrocarbons Mathematics
(DSC-2: Organic
Chemistry-I)

Learning Objectives

The core course Organic Chemistry I is designed in a manner that it forms a cardinal part of
the learning of organic chemistry for the subsequent semesters. The course is infused with the
recapitulation of fundamental concepts of organic chemistry and the introduction of the
concept of visualizing the organic molecules in a three-dimensional space. To establish the
applications of these concepts, the functional groups-alkanes, alkenes, alkynes are
introduced. The constitution of the course strongly aids in the paramount learning of the
concepts and their applications.

Learning outcomes

On completion of the course, the student will be able to:

• Understand and explain the electronic displacements and reactive intermediates and
their applications in basic concepts.
• Formulate the mechanistic route of organic reactions by recalling and correlating the
fundamental concepts.

99
 • Identify and comprehend mechanism for free radical substitution, electrophilic
addition, nucleophilic substitution and elimination reactions.
• Understand the fundamental concepts of stereochemistry.
• Understand and suitably use the chemistry of hydrocarbons

SYLLABUS OF DSC- 2

UNIT – I ( 9 Hours)
Unit I: Basic Concepts of Organic Chemistry

Electronic displacements and their applications: inductive, electromeric, resonance and

mesomeric effects and hyperconjugation. Dipole moment, acidity and basicity.

Homolytic and heterolytic fissions with suitable examples. Types, shape and relative stability
of carbocations, carbanions, carbenes and free radicals.

Electrophiles & nucleophiles, and introduction to types of organic reactions: addition,

elimination and substitution reactions.

UNIT – II (18 Hours)

Unit II : Stereochemistry

Stereoisomerism: Optical activity and optical isomerism, asymmetry, chirality, enantiomers,

diastereomers. specific rotation; Configuration and projection formulae: Newman, Sawhorse,
Fischer and their interconversion. Chirality in molecules with one and two stereocentres;
meso configuration.

Racemic mixture and their resolution. Relative and absolute configuration: D/L and R/S
designations (CIP rules).

Geometrical isomerism: cis-trans, syn-anti and E/Z notations.

Conformational Isomerism: Alkanes (Conformations, relative stability and energy diagrams

of Ethane, Propane and butane). Relative stability of cycloalkanes (Baeyer strain theory),
Cyclohexane conformations with energy diagram. Conformations of monosubstituted
cyclohexanes.

UNIT – III (18)

Unit III: Aliphatic Hydrocarbons
Alkanes: Preparation, Halogenation of alkanes, Concept of relative reactivity v/s selectivity.
Alkenes and Alkynes: Methods of preparation of alkenes using Mechanisms of E1, E2, E1cb
reactions, Saytzeff and Hoffmann eliminations. Electrophilic additions, mechanism with
suitable examples, (Markownikoff/Anti-markownikoff addition), syn and anti-addition;
addition of H2, X2, oxymercuration-demercuration, hydroboration-oxidation, ozonolysis,
hydroxylation, reaction with NBS, Reactions of alkynes; acidity, Alkylation of terminal
alkynes, electrophilic addition: hydration to form carbonyl compounds, Relative reactivity of
alkenes and alkynes, 1,2-and 1,4-addition reactions in conjugated dienes, Diels Alder reaction
(excluding stereochemistry)

Practical component

100
Practical (30 Hours)
Credits: 01
(Laboratory periods: 15 classes of 2 hour each)
Note: Students should be provided with handouts prior to the practical class

1. Calibration of a thermometer and determination of the melting points of the organic

compounds using any one of the following methods-Kjeldahl method, electrically heated
melting point apparatus and BODMEL).

2. Concept of melting point and mixed melting point.

3. Concept of recrystallisation using alcohol/water/alcohol-water systems (Any two).

4. Determination of boiling point of liquid compounds (boiling point lower than and more
than 100 °C by distillation, capillary method and BODMEL method)

5. Separation of a mixture of two amino acids/sugars by radial/ascending paper

chromatography.

6. Separation of a mixture of o-and p-nitrophenol or o-and p-aminophenol by thin layer

chromatography (TLC).

7. Detection of extra elements

Essential/recommended readings

References:
Theory
1. Morrison, R.N., Boyd, R.N., Bhattacharjee, S.K. (2010), Organic Chemistry,
7th Edition, Dorling Kindersley (India) Pvt. Ltd., Pearson Education.
2. Finar, I.L. (2002), Organic C hemistry, Volume 1, 6th Edition, Dorling Kindersley
(India) Pvt. Ltd., Pearson Education.
3. Eliel, E.L., Wilen, S.H. (1994), Stereochemistry o f O rganic C ompounds; Wiley:
London.

Practicals

1. Mann, F.G., Saunders, B.C. (2009), Practical O rganic C hemistry, 4th Edition,
Pearson Education.
2. Ahluwalia, V.K., Dhingra, S. (2004), Comprehensive Practical O rganic
Chemistry: Qualitative Analysis, University Press.
3. Furniss, B.S., Hannaford, A.J., Smith, P.W.G.; Tatchell, A.R (2004), Vogel's
Textbook of Practical Organic Chemistry, Pearson.
4. Leonard, J., Lygo, B., Procter, G. (2013) Advanced Practical O rganic C hemistry,
3rd Edition, CRC Press.
5. Pasricha, S., Chaudhary, A. (2021), Practical O rganic C hemistry: V olume–I, I K
International Publishing house Pvt. Ltd, New Delhi

101
Suggestive readings

Additional Resources:

1. Solomons, T.W.G., Fryhle, C.B., Snyder, S.A. (2017), Organic C hemistry, 12th
Edition, Wiley.
2. Bruice, P.Y. (2020), Organic Chemistry, 8th Edition, Pearson.
3. Clayden, J., Greeves, N., Warren, S. (2014), Organic Chemistry, Oxford.
4. Nasipuri, D. (2018), Stereochemistry o f O rganic C ompounds: P rinciples a nd
Applications, 4th Edition, New Age International.
5. Gunstone, F.D. (1975), Guidebook to Stereochemistry, Prentice Hall Press.
6. Gupta, S.S. (2018), Basic S tereochemistry o f O rganic Mo lecules, 2nd Edition,
Oxford University Press.

DISCIPLINE SPECIFIC CORE COURSE– 3 (DSC-3): Gaseous and Liquid

Credit distribution, Eligibility and Pre-requisites of the Course

Course t itle & Credits Credit distribution of the course Eligibility Pre-requisite
Code Lecture Tutorial Practical/ criteria of t he co urse
Practice (if any)
Gaseous and 04 02 -- 02 Physics, --
Liquid State Chemistry,
(DSC-3: Mathematics
Physical
Chemistry-I)

Learning Objectives

The objective of this course is to develop basic and advance concepts regarding gases and
liquids. It aims to study the similarity and differences between the two states of matter and
reasons responsible for these. The objective of the practicals is to develop skills for working
in physical chemistry laboratory. The student will perform experiments based on the concepts
learnt in Physical chemistry-I course.

Learning outcomes

By the end of the course, the students will be able to:

• Derive mathematical expressions for different properties of gas and liquid and
understand their physical significance.
• Apply the concepts of gas equations and liquids while studying other chemistry
courses and every-day life.
• Handle stalagmometer and Ostwald viscometer properly.
• Determine the density of aqueous solutions.
• Dilute the given solutions as per required concentrations.
• Data reduction using numerical and graphical methods.

102
SYLLABUS OF DSC-3

UNIT – I (24 Hours)

Gaseous state
Kinetic t heory o f g ases- postulates and derivation of kinetic gas equation, Maxwell
distribution of molecular velocities and its use in evaluating average, root mean square and
most probable velocities and average kinetic energy. Definition, expression, applications and
temperature and pressure dependence of each one of the following properties of ideal gases:
Collision frequency, Collision diameter, Mean free path. Coefficient of viscosity, definition,
units and origin of viscosity of gases, relation between mean free path and coefficient of
viscosity, temperature and pressure dependence of viscosity of a gas, calculation of molecular
diameter from viscosity
Barometric distribution law, its derivation and applications, alternative forms of barometric
distribution law in terms of density and number of molecules per unit volume, effect of
height, temperature and molecular mass of the gas on barometric distribution

Behaviour of real gases- Compressibility factor, Z , Variation of compressibility factor with

pressure at constant temperature (plot of Z vs P) for different gases ( H2, CO2, CH4 and NH3),
Cause of deviations from ideal gas behaviour and explanation of the observed behaviour of
real gases in the light of molecular interactions

van der Waals (vdW) equation of state, Limitations of ideal gas equation of state and its
modifications in the form of derivation of van der Waal equation, Physical significance of
van der Waals constants, application of van der Waal equation to explain the observed
behaviour of real gases.

Isotherms of real gases- Critical state, relation between critical constants and van der Waals
constants, correlation of critical temperature of gases with intermolecular forces of attraction,
Continuity of states, Limitations of van der Waals equation, Reduced equation of state and
law of corresponding states (statement only).

Virial equation of state-Physical significance of second and third virial coefficients, van der
Waals equation expressed in virial form, Relations between virial coefficients and van der
Waals constants

UNIT – II (6 Hours)
Liquid state
Nature of liquid state, qualitative treatment of the structure of the liquid state

103
Physical properties of liquids-vapour pressure, its origin and definition, Vapour pressure of
liquids and intermolecular forces, and boiling point

Surface tension, its origin and definition, Capillary action in relation to cohesive and adhesive
forces, determination of surface tension by (i) using stalagmometer (drop number and drop
mass method both) and (ii) capillary rise method, Effects of addition of sodium chloride,
ethanol and detergent on the surface tension of water and its interpretation in terms of
molecular interactions, Role of surface tension in the cleansing action of detergents

Coefficient of viscosity and its origin in liquids, Interpretation of viscosity data of pure
liquids (water, ethanol, ether and glycerol) in the light of molecular interactions, Effects of
addition of sodium chloride, ethanol and polymer on the viscosity of water, relative viscosity,
specific viscosity and reduced viscosity of a solution, comparison of the origin of viscosity of
liquids and gases, effect of temperature on the viscosity of a liquid and its comparison with
that of a gas.

Practical component
Practicals 60 Hours
(Laboratory periods: 15 classes of 4 hours each)
1. Gases
a. To verify the Charles law using Charles law apparatus
b. To determine the value of universal gas constant R using the reaction
Mg(s) + 2HCl (aq)  MgCl2 (aq) + H2 (g)

2. Surface tension measurements using stalagmometer

a. Determine the surface tension of a liquid by drop number method.
b. Determine the surface tension of a liquid by drop weight method.
c. Study the variation of surface tension with different concentration of detergent
solutions. Determine CMC.
d. Study the effect of the addition of solutes on the surface tension of water at room
temperature and explain the observations in terms of molecular interactions:
(i) sugar
(ii) ethanol
(iii) sodium chloride
e. Study the variation of surface tension with different concentration of sodium
chloride solutions.

3. Viscosity measurement using Ostwald’s viscometer

a. Determination of co-efficient of viscosity of two unknown aqueous solution.
b. Study the variation of viscosity with different concentration of sugar solutions.
c. Study the effect of the addition of solutes such as (i) polymer (ii) ethanol (iii)
sodium chloride on the viscosity of water at room temperature and explain the
observations in terms of molecular interactions

104
 d. Study the variation of viscosity of water with the amounts of a solute and calculate
the intrinsic viscosity at room temperature.
e. Determine the viscosity average molecular mass of the polymer (PVA) using
viscosity measurements.

Essential/recommended readings
References:
Theory:
1. Atkins, P.W.; Paula, J.de. (2014), Atkin’s P hysical C hemistry E d., 10th Edition,
Oxford University Press.
2. Ball, D. W. (2017), Physical Chemistry, 2nd Edition, Cengage Learning, India.
3. Castellan, G. W. (2004), Physical Chemistry, 4th Edition, Narosa.
4. Kapoor, K.L. (2015), A T extbook of P hysical C hemistry, Vol 1, 6th Edition,
McGraw Hill Education.

Practical:
• Khosla, B.D.; Garg, V.C.; Gulati, A. (2015), Senior Practical Physical Chemistry,
R. Chand & Co, New Delhi.
• Kapoor, K.L. (2019), A T extbook of P hysical C hemistry, Vol.7, 1st Edition,
McGraw Hill Education.
• Garland, C. W.; Nibler, J. W.; Shoemaker, D. P. (2003), Experiments i n P hysical
Chemistry, 8th Edition, McGraw-Hill, New York.

Suggestive readings

Additional Resources:
1. Moore, W.J. (1972), Physical Chemistry, 5th Edition, Longmans Green & Co. Ltd.
Glasstone, S. (1948), Textbook of P hysical C hemistry, D. Van Nostrand company, New
York.

105
 BSc. Life Sciences
Multidisciplinary

DISCIPLINE SPECIFIC CORE COURSE (DSC-1): Basic Concepts of Organic

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course t itle & Credits Credit distribution of the course Eligibility Pre-requisite
Code Lecture Tutorial Practical/ criteria of the course
Practice (if any)
Basic Concepts 04 02 - 02 12th Pass NIL
of Organic
Chemistry

Learning Objectives

The Learning Objectives of this course are as follows:

• The course is infused with the recapitulation of fundamentals of organic chemistry
and the introduction of the concept of visualizing the organic molecules in a three-
dimensional space.
• To establish the applications of these concepts, a study of diverse reactions through
mechanisms is included.
• The constitution of the course strongly aids in the paramount learning of the basic
concepts and their applications

Learning outcomes

The Learning Outcomes of this course are as follows:

• Understand and explain the differential behavior of organic compounds based on

fundamental concepts learned.
• Understand the fundamental concepts of stereochemistry.
• Formulate the mechanism of organic reactions by recalling and correlating the
fundamental properties of the reactants involved.
• Learn and identify many organic reactions and their mechanisms including
electrophilic addition, nucleophilic addition, nucleophilic substitution, electrophilic
substitution and rearrangement reactions.

SYLLABUS OF DSC-1

UNIT – I Fundamentals of organic chemistry (6 Hours)

Types of Electronic displacements: Inductive effect, Resonance effect, Hyperconjugation,
Electromeric Effect. Reactive intermediates and their stability: carbocations, free radicals,
carbanions, benzyne, carbenes. Acidity and basicity in organic compounds (comparison of

119
carboxylic acids, alcohols, phenols, primary, secondary and tertiary aliphatic amines, aniline
and its derivatives)

UNIT – II Stereochemistry (6 Hours)

Types of projection formulae: Flying Wedge Formula, Newmann, Sawhorse and Fischer
representations and their interconversion.
Stereoisomerism: Concept of chirality (upto two carbon atoms). Configurational isomerism:
geometrical and optical isomerism; enantiomerism, diastereomerism and meso compounds).
Threo and erythro; D and L; Cis-trans nomenclature; CIP Rules: R/ S (for upto 2 chiral
carbon atoms) and E/Z nomenclature (for upto two C=C systems).
Conformational isomerism with respect to ethane, butane and cyclohexane.

UNIT – III Types of Organic Reactions (Including reactions of alkenes, alkyl and aryl
halides, alcohols, aldehydes, ketones) (18 Hours)
Electrophilic addition reactions
Electrophilic addition reaction (with respect to propene, propyne, 3,3-dimethyl-1-butene):
Hydration, Addition of HX in the absence and presence of peroxide, Hydroboration
oxidation, Addition of bromine (with stereochemistry).

Nucleophilic addition reactions

Nucleophilic addition reaction of carbonyl compounds: Addition of HCN, ammonia
derivatives (Hydroxylamine, Hydrazine, Semicarbazide and 2,4-DNP), the addition of
carbanion (Aldol condensation, Claisen Schmidt, Benzoin condensation, Perkin reaction,
reactions involving Grignard reagent).

Elimination and Nucleophilic substitution reactions

Nucleophilic substitution reaction (SN1 and SN2) in alkyl halides (mechanisms with
stereochemical aspect), alcohols (with nucleophiles like ammonia, halides, thiols, ambident
nucleophiles (cyanide and nitrite ion)), ethers (Williamson ether synthesis), Elimination
reaction (E1 & E2), elimination vs substitution (w.r.t. potassium t-butoxide and KOH);
Nucleophilic aromatic substitution in aryl halides-elimination addition reaction w.r.t.
chlorobenzene, including the effect of nitro group (on the ring) on the reaction. relative
reactivity and strength of C-X bond in alkyl, allyl, benzyl, vinyl and aryl halides towards
substitution reactions

Electrophilic substitution reactions

Electrophilic Aromatic substitution with mechanism (benzene)- sulphonation, nitration,
halogenation, Friedel craft acylation :o-, m- and p- directive influence giving examples of
toluene/nitrobenzene/ phenol/ aniline/ chlorobenzene.

Reactive intermediates and Rearrangement Reactions

Free radicals (Birch Reduction); Carbocations (Pinacol-Pinacolone, Wagner-Meerwein,
Rearrangement, and Beckmann rearrangement); Carbanions (Michael Addition); Carbenes
(Reimer-Tiemann).

120
Practical component (60 Hours)

1. Purification of an organic compound by crystallization (from water and alcohol) and

distillation, Criteria of purity: Determination of M.P.
2. Determination of boiling point of liquid compounds. (Boiling point lower than and more
than 100 °C by distillation and capillary method)
3. Detection of extra element
4. Preparations: (Mechanism of various reactions involved to be discussed).

a. Bromination of phenol/aniline.
b. 2,4-Dinitrophenylhydrazone of aldehydes and ketones
c. Semicarbazone of aldehydes/ ketones
d. Aldol condensation reaction using green method.
e. Bromination of Stilbene.
f. Acetanilide to p-Bromoacetanilide.

The above derivatives should be prepared using 0.5-1g of the organic compound. The solid
samples must be collected and may be used for recrystallization and melting point.

Essential/recommended readings
Theory:
1. Sykes, P.(2003), A Guide B ook t o Mech anism i n O rganic C hemistry, 6th Edition
Pearson Education.
2. Eliel, E. L. (2001), Stereochemistry of Carbon Compounds, Tata McGraw Hill.
3. Morrison, R. N.; Boyd, R. N., Bhattacharjee, S.K. (2010), Organic C hemistry, 7th
Edition, Pearson Education.
Practical:
1. Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. (2012), Vogel's
Textbook of Practical Organic Chemistry, Pearson.
2. Mann, F.G.; Saunders, B.C. (2009), Practical O rganic C hemistry, Pearson
Education.
3. Dhingra, S; Ahluwalia V.K., (2017), Advanced Experimental Organic Chemistry,
Manakin Press.

Suggestive readings

Theory:
1. Bahl, A; Bahl, B. S. (2019), Advanced Organic Chemistry, 22nd Edition, S. Chand.

Practical:
1. Pasricha, S., Chaudhary, A. (2021), Practical O rganic C hemistry: Volume I , I K
International Publishing House Pvt. Ltd., New Delhi.

Note: Examination s cheme a nd m ode s hall be a s pr escribed by t he E xamination

Branch, University of Delhi, from time to time.

121
 BSc. Physical Sciences
DISCIPLINE SPECIFIC CORE COURSE (DSC-1): Basic Concepts of Organic
Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course t itle Credits Credit distribution of the course Eligibility Pre-requisite

& Code Lecture Tutorial Practical/ criteria of the course
Practice (if any)
Basic 04 02 - 02 12th Pass NIL
Concepts of
Organic
Chemistry

Learning Objectives

The Learning Objectives of this course are as follows:

• The course is infused with the recapitulation of fundamentals of organic chemistry
and the introduction of the concept of visualizing the organic molecules in a three-
dimensional space.
• To establish the applications of these concepts, a study of diverse reactions through
mechanisms is included.
• The constitution of the course strongly aids in the paramount learning of the basic
concepts and their applications

Learning outcomes

The Learning Outcomes of this course are as follows:

• Understand and explain the differential behavior of organic compounds based on

fundamental concepts learned.
• Understand the fundamental concepts of stereochemistry.
• Formulate the mechanism of organic reactions by recalling and correlating the
fundamental properties of the reactants involved.
• Learn and identify many organic reactions and their mechanisms including
electrophilic addition, nucleophilic addition, nucleophilic substitution, electrophilic
substitution and rearrangement reactions.

SYLLABUS OF DSC-1

UNIT – I Fundamentals of organic chemistry (6 Hours)

Types of Electronic displacements: Inductive effect, Resonance effect, Hyperconjugation,
Electromeric Effect. Reactive intermediates and their stability: carbocations, free radicals,
carbanions, benzyne, carbenes.
Acidity and basicity in organic compounds (comparison of carboxylic acids, alcohols,
phenols, primary, secondary and tertiary aliphatic amines, aniline and its derivatives)

122
UNIT – II Stereochemistry (6 Hours)
Types of projection formulae: Flying Wedge Formula, Newmann, Sawhorse and Fischer
representations and their interconversion.
Stereoisomerism: Concept of chirality (upto two carbon atoms). Configurational isomerism:
geometrical and optical isomerism; enantiomerism, diastereomerism and meso compounds).
Threo and erythro; D and L; Cis-trans nomenclature; CIP Rules: R/ S (for upto 2 chiral
carbon atoms) and E/Z nomenclature (for upto two C=C systems).
Conformational isomerism with respect to ethane, butane and cyclohexane.

UNIT – III Types of Organic Reactions (Including reactions of alkenes, alkyl and aryl
halides, alcohols, aldehydes, ketones) (18 Hours)
Electrophilic addition reactions
Electrophilic addition reaction (with respect to propene, propyne, 3,3-dimethyl-1-butene):
Hydration, Addition of HX in the absence and presence of peroxide, Hydroboration
oxidation, Addition of bromine (with stereochemistry).

Nucleophilic addition reactions

Nucleophilic addition reaction of carbonyl compounds: Addition of HCN, ammonia
derivatives (Hydroxylamine, Hydrazine, Semicarbazide and 2,4-DNP), the addition of
carbanion (Aldol condensation, Claisen Schmidt, Benzoin condensation, Perkin reaction,
reactions involving Grignard reagent).

Elimination and Nucleophilic substitution reactions

Nucleophilic substitution reaction (SN1 and SN2) in alkyl halides (mechanisms with
stereochemical aspect), alcohols (with nucleophiles like ammonia, halides, thiols, ambident
nucleophiles (cyanide and nitrite ion)), ethers (Williamson ether synthesis), Elimination
reaction (E1 & E2), elimination vs substitution (w.r.t. potassium t-butoxide and KOH);
Nucleophilic aromatic substitution in aryl halides-elimination addition reaction w.r.t.
chlorobenzene, including the effect of nitro group (on the ring) on the reaction. relative
reactivity and strength of C-X bond in alkyl, allyl, benzyl, vinyl and aryl halides towards
substitution reactions

Electrophilic substitution reactions

Electrophilic Aromatic substitution with mechanism (benzene)- sulphonation, nitration,
halogenation, Friedel craft acylation :o-, m- and p- directive influence giving examples of
toluene/nitrobenzene/ phenol/ aniline/ chlorobenzene.

Reactive intermediates and Rearrangement Reactions

Free radicals (Birch Reduction); Carbocations (Pinacol-Pinacolone, Wagner-Meerwein,
Rearrangement, and Beckmann rearrangement); Carbanions (Michael Addition); Carbenes
(Reimer-Tiemann).

Practical component (60 Hours)

123
1. Purification of an organic compound by crystallization (from water and alcohol) and
distillation, Criteria of purity: Determination of M.P.
2. Determination of boiling point of liquid compounds. (Boiling point lower than and
more than 100 °C by distillation and capillary method)
3. Detection of extra element
4. Preparations: (Mechanism of various reactions involved to be discussed).
a. Bromination of phenol/aniline.
b. 2,4-Dinitrophenylhydrazone of aldehydes and ketones
c. Semicarbazone of aldehydes/ ketones
d. Aldol condensation reaction using green method.
e. Bromination of Stilbene.
f. Acetanilide to p-Bromoacetanilide.

The above derivatives should be prepared using 0.5-1g of the organic compound. The solid
samples must be collected and may be used for recrystallization and melting point.

Essential/recommended readings
Theory:
1. Sykes, P.(2003), A Guide B ook t o Mech anism i n O rganic C hemistry, 6th Edition
Pearson Education.
2. Eliel, E. L. (2001), Stereochemistry of Carbon Compounds, Tata McGraw Hill.
3. Morrison, R. N.; Boyd, R. N., Bhattacharjee, S.K. (2010), Organic C hemistry, 7th
Edition, Pearson Education.
Practical:
1. Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. (2012), Vogel's
Textbook of Practical Organic Chemistry, Pearson.
2. Mann, F.G.; Saunders, B.C. (2009), Practical O rganic Chemistry, Pearson
Education.
3. Dhingra, S; Ahluwalia V.K., (2017), Advanced Experimental Organic Chemistry,
Manakin Press.

Suggestive readings
Theory:
1. Bahl, A; Bahl, B. S. (2019), Advanced Organic Chemistry, 22nd Edition, S. Chand.

Practical:
1. Pasricha, S., Chaudhary, A. (2021), Practical O rganic C hemistry: Volume I , I K
International Publishing House Pvt. Ltd., New Delhi.

Note: E xamination scheme a nd m ode s hall be a s pr escribed by t he E xamination

Branch, University of Delhi, from time to time.

124
 COMMON POOL OF GENERIC ELECTIVES (GE) COURSES
OFFERED BY DEPARTMENT OF CHEMISTRY FOR ODD SEMESTER

GE 1: Chemistry: Atomic Structure and Chemical Bonding

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course titl e & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice
Atomic 4 2 2 Basic
Structure and knowledge
Chemical of
Bonding (GE- Chemistry
1)

Learning Objectives

The Learning Objectives of this course are as follows:

• To discuss the structure of atom as a necessary pre-requisite in understanding the
nature of chemical bonding in compounds.
• To provide basic knowledge about ionic and covalent bonding.

Learning Outcomes

By the end of the course, the students will be able to:

• Solve the conceptual questions using the knowledge gained by studying the quantum
mechanical model of the atom, quantum numbers, electronic configuration, radial and
angular distribution curves, and shapes of s, p, and d orbitals
• Understand the concept of lattice energy and solvation energy.
• Draw the plausible structures and geometries of molecules using radius ratio rules,
VSEPR theory and MO diagrams (homo- & hetero-nuclear diatomic molecules).

SYLLABUS OF GE 1

Theory:
Unit – 1: Atomic Structure ( 14 Hours)

Review of: Bohr’s theory and its limitations, Heisenberg uncertainty principle, Dual
behaviour of matter and radiation, De-Broglie’s relation, Hydrogen atom spectra, need of a
new approach to atomic structure. Time independent Schrodinger equation and meaning of
various terms in it. Significance of ψ and ψ2, Schrödinger equation for hydrogen atom, radial

125
and angular parts of the hydrogen wave functions (atomic orbitals) and their variations for 1s,
2s, 2p, 3s, 3p and 3d orbitals (Only graphical representation), radial and angular nodes and
their significance, radial distribution functions and the concept of the most probable distance
with special reference to 1s and 2s atomic orbitals. Significance of quantum numbers, orbital
angular momentum and quantum numbers ml and ms. Shapes of s, p and d atomic orbitals,
nodal planes, discovery of spin, spin quantum number (s) and magnetic spin quantum number
(ms). Rules for filling electrons in various orbitals, electronic configurations of the atoms,
stability of half-filled and completely filled orbitals, concept of exchange energy, relative
energies of atomic orbitals, anomalous electronic configurations.

Unit – 2: Chemical Bonding and Molecular Structure (16 Hours)

Ionic Bonding: General characteristics of ionic bonding, energy considerations in ionic
bonding, lattice energy and solvation energy and their importance in the context of stability
and solubility of ionic compounds, statement of Born-Landé equation for calculation of
lattice energy (no derivation), Born Haber cycle and its applications, covalent character in
ionic compounds, polarizing power and polarizability, Fajan’s rules. Ionic character in
covalent compounds, bond moment, dipole moment and percentage ionic character. Covalent
bonding: VB Approach: Shapes of some inorganic molecules and ions on the basis of VSEPR
(H2O, NH3, PCl5, SF6, ClF3, SF4) and hybridization with suitable examples of linear, trigonal
planar, square planar, tetrahedral, trigonal bipyramidal and octahedral arrangements. Concept
of resonance and resonating structures in various inorganic and organic compounds. MO
Approach: Rules for the LCAO method, bonding and antibonding MOs and their
characteristics for ss, s-p and p-p combinations of atomic orbitals, nonbonding combination
of orbitals, MO treatment of homonuclear diatomic molecules of 1st and 2nd periods
(including idea of s-p mixing) and heteronuclear diatomic molecules such as CO, NO and
NO+.

Practicals: (60 Hours)

(Laboratory Periods: 60)

1. Acid-Base Titrations: Principles of acid-base titrations to be discussed.

(i) Estimation of sodium carbonate using standardized HCl.

(ii) Estimation of carbonate and hydroxide present together in a mixture.
(iii) Estimation of carbonate and bicarbonate present together in a mixture.
(iv) Estimation of free alkali present in different soaps/detergents

2. Redox Titrations: Principles of oxidation-reduction titrations (electrode potentials) to be

discussed.

(i) Estimation of oxalic acid by titrating it with KMnO4.

(ii) Estimation of Mohr’s salt by titrating it with KMnO4.
(iii) Estimation of oxalic acid and sodium oxalate in a given mixture.
(iv) Estimation of Fe (II) ions by titrating it with K2Cr2O7 using internal indicator
(diphenylamine/ N-phenylanthranilic acid).

References:
126
Theory:

1. Lee, J.D.; (2010), Concise Inorganic Chemistry, Wiley India.

2. Huheey, J.E.; Keiter, E.A.; Keiter; R. L.; Medhi, O.K. (2009), Inorganic C hemistry-
Principles of Structure and Reactivity, Pearson Education.
3. Douglas, B.E.; McDaniel, D.H.; Alexander, J.J. (1994), Concepts a nd Mo dels o f
Inorganic Chemistry, John Wiley & Sons.
4. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010),
Shriver and Atkins Inorganic Chemistry, 5th Edition, Oxford University Press.

Practicals:

• Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of
Quantitative Chemical Analysis, John Wiley and Sons.

Additional Resources:

1. Wulfsberg, G (2002), Inorganic Chemistry, Viva Books Private Limited.

2. Miessler, G.L.; Fischer P.J.; Tarr, D. A. (2014), Inorganic Chemistry, 5th Edition,
Pearson.

GE 3: Chemistry: Bioinorganic Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title Credits Credit distribution of the Eligibility Pre-

& Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice
Bioinorganic 4 2 2 Basic
Chemistry knowledge
(GE-3) of
Chemistry

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce students to bioinorganic chemistry, currently a frontier area of chemistry
providing an interface between organic chemistry, inorganic chemistry and biology.
• To make students learn about the importance of inorganic chemical species, especially
metals, in biological systems, through discussions on topics such as the sodium-
potassium pump, the applications of iron in physiology, including iron transport and
storage system, role of magnesium in energy production and chlorophyll, toxicity of
heavy metal ions and their antidotes.

127
Learning Outcomes

By the end of the course, the students will be able to:

● Classify metal ions in biological systems as essential, non-essential, trace & toxic.
● Diagrammatically explain the working of the sodium-potassium pump in organisms
and the factors affecting it
● Understand the role of metal ions such as Mg, Ca and Fe in biological systems.
● Understand the toxicity of heavy metal ions (Hg, Pb, Cd and As) in the physiological
system
● Explain the use of chelating agents in medicine

SYLLABUS OF GE-3

Theory:
Unit 1: Introduction (6 Hours)
A brief introduction to bio-inorganic chemistry. Metal ions present in biological systems and
their classification on the basis of action (essential, non-essential, trace & toxic).
Classification of metallobiomolecules (enzymes, transport and storage proteins and non-
proteins). Brief idea about membrane transport, channels, pumps.

Unit 2:Role of s-block Elements in Biological System (8 Hours)

Role of metal ions present in biological systems with special reference to Na+, K+ and Mg2+
and Ca2+ ions: Na/K pump; Ca pump, role of Mg2+ ions in energy production and chlor
ophyll. Role of calcium in bone formation.
Unit 3:Role of iron in Biological System (8Hours)
Role of iron in oxygen transport and storage (haemoglobin and myoglobin), Perutz
mechanism, Cooperative effect, Bohr effect, comparison of oxygen saturation curves of
haemoglobin and myoglobin, carbon monoxide. Storage and transport of iron in humans
(ferritin and transferrin).
Unit 4: Toxicity of Heavy Metal Ions (8 Hours)
Toxicity of heavy metal ions (Hg, Pb, Cd and As), reasons for toxicity and their antidotes

Practicals: (60 Hours)

WEEKS)
(Laboratory Periods: 60)

1. Spectrophotometric estimation:
(i) Verify Lambert-Beer’s law and determine the concentration of
CuSO4/KMnO4/K2Cr2O7/CoSO4 in a solution of unknown concentration
(ii) Spectrophotometric estimation of Fe2+ ions by using 1, 10- phenanthroline

128
(iii) Determination of the composition of the Fe3+ - salicylic acid complex in solution by
Job’s method.
2. Complexometric titrations using disodium salt of EDTA:
(i) Estimation of Zn2+ using EBT / Xylenol orange as indicator
(ii) Estimation of Mg2+
(iii) Estimation of Ca2+ by substitution method
(iv) To estimate the concentration of Ca in commercially available medicines.
(v) To estimate the Mg present in multivitamins.

References:
Theory:
1. Huheey, J.E.; Keiter, E.A., Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry-
Principles of Structure and Reactivity, Pearson Education.
2. Shriver, D.D.; Atkins, P.; Langford, C.H. (1994), Inorganic C hemistry 2nd Ed.,
Oxford University Press.
3. Cotton, F.A.; Wilkinson, G.; Gaus, P.L. Basic I norganic C hemistry, 3rd
Edition,Wiley India.
4. Crichton, R.R. (2008), Biological I norganic C hemistry: A n I ntroduction.
Amsterdam, Elsevier.
5. Kaim, W., B. Schwederski and A. Klein. (2014), Bioinorganic Chemistry: Inorganic
Elements i n t he C hemistry o f L ife: A n Introduction a nd G uide. 2nd Edition,
Wiley.

Practical:

1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of
Quantitative Chemical Analysis, John Wiley and Sons.

Additional Resources:
1. Lippard, S.J.; Berg, J.M. (1994), Principles o f B ioinorganic C hemistry, Panima
Publishing Company.
2. Greenwood, N.N.; Earnshaw, A. (1997), Chemistry o f t he E lements, 2nd Edition,
Elsevier

GE 4: Chemistry: Basic Concepts of Organic Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-
Code course criteria requisite
Lecture Tutorial Practical/ of th e
Practice course
Basic C oncepts 4 2 2
of O rganic
Chemistry
(GE-4)
129
Learning Objectives
The Learning Objectives of this course are as follows:

• To teach the fundamentals of organic chemistry and the introduction of a new concept
of visualizing the organic molecules in a three- dimensional space.
• To establish the applications of these concepts, different types of organic reactions are
introduced.

Learning Outcomes

By the end of the course, the students will be able to:

• Understand and explain the differential behavior of organic compounds based on

fundamental concepts learnt.
• Formulate the mechanism of organic reactions by recalling and correlating the
fundamental properties of the reactants involved.
• Learn and identify many organic reaction mechanisms including free radical substitution,
electrophilic addition and electrophilic aromatic substitution.
• Differentiate between various types of organic reactions possible on the basis of reaction
conditions

SYLLABUS OF GE-4

Theory:
Unit 1: Basic Concepts (6 Hours)

Electronic displacements and their applications: Inductive, electromeric, resonance and

mesomeric effects and hyperconjugation. Dipole moment, acidity and basicity.
Homolytic and heterolytic fissions with suitable examples. Types, shape and relative stability
of carbocations, carbanions and free radicals. Electrophiles and nucleophiles
Concept of Aromaticity: Huckel's rule

Unit 2: Stereochemistry (10 Hours)

Stereoisomerism: Optical activity and optical isomerism, asymmetry, chirality, enantiomers,

diastereomers. specific rotation; Configuration and projection formulae: Newmann,
Sawhorse, Fischer and their interconversion. Chirality in molecules with one and two
stereocentres; meso configuration.
CIP rules: Erythro/Threo, D/L and R/S designations.
Geometrical isomerism: cis-trans, syn-anti and E/Z notations.

Unit 3: Types of Organic Reactions (14 Hours)

Introduction to substitution, addition, elimination, isomerization, rearrangement, oxidation

and reduction reactions.
Free radical substitutions (Halogenation), concept of relative reactivity v/s selectivity. Free
radical reactions in the biological reactions
130
Mechanisms of E1, E2, Saytzeff, Hoffmann eliminations and Cope elimination. Biological
dehydration reactions
Electrophilic Additions reactions of alkenes and alkynes: mechanism with suitable examples,
(Markownikoff/Antimarkownikoff addition), syn and anti-addition; addition of H2, X2,
hydroboration-oxidation, ozonolysis, hydroxylation.
Nucleophilic substitution reactions – SN1 and SN2 mechanisms with stereochemical aspects
and effect of solvent; nucleophilic substitution vs. elimination. Biological methylating agents
Electrophilic aromatic substitution: halogenation, nitration, sulphonation, Friedel Crafts
alkylation/ acylation with their mechanism. Directing effects of groups in electrophilic
substitution.

Practicals: (60 Hours)

(Laboratory Periods: 60)

1. Calibration of a thermometer and determination of the melting points of the organic
compounds (Kjeldahl method, electrically heated melting point apparatus and
BODMEL)
2. Purification of the organic compounds by crystallization using the following solvents:
3. a. Water b. Alcohol c. Alcohol-Water
4. Determination of boiling point of liquid compounds. (Boiling point lower than and more
than 100 °C by distillation, capillary method and BODMEL)
5. Acetylation of one of the following compounds: amines (aniline, o-, m-, p- toluidines and
o-, m-, p-anisidine) and phenols (β-naphthol, salicylic acid) either by conventional or
green method.
6. Bromination of acetanilide/aniline/phenol either by conventional or green method.
7. Nitration of chlorobenzene/nitrobenzene.

References:
Theory:
1. Sykes, P. (2005), A Guide B ook t o Mech anism i n O rganic C hemistry, Orient
Longman.
2. Eliel, E. L. (2000), Stereochemistry of Carbon Compounds, Tata McGraw Hill.
3. Morrison, R. N.; Boyd, R. N., Bhattacharjee, S.K. (2010), Organic C hemistry,
7th Edition, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).
4. Mehta B.; Mehta M. (2015), Organic Chemistry, PHI Learning Private Limited
5. Bahl, A; Bahl, B. S. (2012), Advanced Organic Chemistry, S. Chand.

Practicals:

1. Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. (2012), Vogel's Textbook
of Practical Organic Chemistry, Pearson.
2. Mann, F.G.; Saunders, B.C. (2009), Practical Organic Chemistry, Pearson Education.

131
 GE 7: Chemistry: States of Matter

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course Credits Credit distribution of the Eligibility Pre-requisite
title & course criteria of the course
Code Lecture Tutorial Practical/
Practice
States of 4 2 2
Matter
(GE-7)

Learning Objectives

The Learning Objectives of this course are as follows:

• To make students learn about the properties of ideal and real gases deviation from
ideal behaviour, properties of liquid, types of solids with details about crystal structure.
• To make student learn about the reaction rate, order, activation energy and theories of
reaction rates.

Learning Outcomes

By the end of the course, the students will be able to:

• Derive ideal gas law from kinetic theory of gases and explain why the real gases
deviate from ideal
• behaviour.
• Explain Maxwell-Boltzmann distribution, critical constants and viscosity of gases.
• Explain the properties of liquids especially surface tension and viscosity.
• Explain symmetry elements, crystal structure specially NaCl, KCl and CsCl
• Define rate of reactions and the factors that affect the rates of reaction.
• Understand the concept of rate laws e.g., order, molecularity, half-life and their
determination
• Learn about various theories of reaction rates and how these account for experimental
observations.

SYLLABUS OF GE-7

Theory:
Unit 1: Kinetic Theory of Gases (12 Hours)
Postulates of kinetic theory of gases and derivation of the kinetic gas equation, deviation of
real gases from ideal behaviour, compressibility factor, causes of deviation, van der Waals

132
equation of state for real gases. Boyle temperature (derivation not required), critical
phenomena, critical constants and their calculation from van der Waals equation, Andrews
isotherms of CO2, Maxwell Boltzmann distribution laws of molecular velocities and
molecular energies (graphic representation – derivation not required) and their importance.
Temperature dependence of these distributions, most probable, average and root mean square
velocities (no derivation), collision cross section, collision number, collision frequency,
collision diameter and mean free path of molecules, viscosity of gases and effect of
temperature and pressure on coefficient of viscosity (qualitative treatment only).

Unit 2: Liquids State (6 Hours)

Surface tension and its determination using stalagmometer, Viscosity of a liquid and
determination of coefficient of viscosity using Ostwald viscometer, effect of temperature on
surface tension and coefficient of viscosity of a liquid (qualitative treatment only). Effect of
addition of various solutes on surface tension and viscosity. Explanation of cleansing action
of detergents.
Unit 3: Solid State (12 Hours)

Forms of solids, symmetry elements, unit cells, crystal systems, Bravais lattice types and
identification of lattice planes. Laws of crystallography - law of constancy of interfacial
angles. Law of rational indices, Miller indices. X–ray diffraction by crystals, Bragg’s law and
powder XRD. Powder diffraction patterns of NaCl, CsCl and KCl (qualitative treatment
only), defects in crystals. Glasses and liquid crystals.

Practicals: (60 Hours)

(Laboratory periods: 60)
1. Surface tension measurement (use of organic solvents excluded): Determination of the
surface tension of a liquid or a dilute solution using a stalagmometer.
2. Viscosity measurement (use of organic solvents excluded):
a) Determination of the relative and absolute viscosity of a liquid or dilute solution using an
Ostwald viscometer.
b) Study of the variation of viscosity of an aqueous solution with concentration of solute.
3. Solid State: Powder XRD
c) Differentiate and classify the given set of the diffraction pattern as crystalline materials
or amorphous (Glass) substance.
d) Carry out analysis of a given set of powder XRD and determine the type of the cubic
crystal structure
e) Determination of approximate crystal size from a given set of powder XRD

References:

Theory:
1. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010),
Shriver and Atkin’s Inorganic Chemistry, Oxford.
2. Miessler, G. L.; Tarr, D.A. (2014), Inorganic Chemistry, Pearson.
3. Castellan, G. W. (2004), Physical Chemistry, Narosa.
133
4. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, Vol.1, 6th Edition, McGraw
Hill Education.
5. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, Vol.5, 3rd Edition, McGraw
Hill Education.

Practicals:

1. Khosla, B.D.; Garg, V.C.;Gulati, A.(2015),Senior Practical Physical Chemistry, R.

Chand & Co.

GE 9: Chemistry: Conductance and Electrochemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-
Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
Conductance 4 2 2 Basic
and knowledge
Electrochemistry of
(GE-9) Chemistry

Learning Objectives
The Learning Objectives of this course are as follows:
• To make students learn about conductance, its measurement and applications.
• To make students learn the principles of electrochemical cells: Electrolytic and
Galvanic cell, measurement of, measurement of emf and its applications.

Learning outcomes

By the end of the course, the students will be able to:

• Explain the factors that affect conductance, migration of ions and application of
conductance measurement.
• Understand different types of galvanic cells, their Nernst equations, measurement of
emf, calculations of thermodynamic properties and other parameters from the emf
measurements.
• Understand applications of Emf measurements in relation to determination of activity
coefficients, pH of a solution and Potentiometric titrations.

SYLLABUS OF GE-9

Theory:

Unit 1: Conductance (10 Hours)

134
Quantitative aspects of Faraday’s laws of electrolysis. Arrhenius theory of electrolytic
dissociation. Conductivity: equivalent and molar conductivity and their variation with
dilution for weak and strong electrolytes, Kohlrausch Law of independent migration of ions.
Wein Effect and Debye–Falkanhegan Effect.

Transference number and its experimental determination using Hittorf and moving boundary
methods, Ionic mobility, applications of conductance measurements: determination of degree
of ionization of weak electrolytes, solubility and solubility products of sparingly soluble salts,
ionic product of water, hydrolysis constant of a salt. Conductometric titrations (only acid-
base).

Unit 2: Electrochemistry (20 Hours)

Reversible and irreversible cells with Examples, concept of EMF of a cell, measurement of
EMF of a cell, Nernst equation and its importance, types of electrodes, standard electrode
potential (reduction Potential) and its application to Gas–ion half-cell. Electrochemical series.
Thermodynamics of a reversible cell, calculation of thermodynamic properties: G, H and S
from EMF data. Calculation of equilibrium constant from EMF data. Concentration cells with
transference and without transference, liquid junction potential; determination of activity
coefficients and salt bridge, pH determination using hydrogen electrode. Potentiometric
titrations-qualitative treatment (acid-base and oxidation-reduction only).

Practicals: (60 Hours)

(Laboratory periods: 60)
1. Conductance
(i) Determination of cell constant.
(ii) Determination of equivalent conductance, degree of dissociation and dissociation
constant of a weak acid.
(iii) Perform the following conductometric titrations:
a) Strong acid vs strong base
b) Weak acid vs strong base.

2. Potentiometry
Perform the potentiometric titrations of (i) Strong acid vs strong base, (ii) Weak acid vs
strong base and (iii) Mohr’s salt vs KMnO4.

References:

Theory:
1. Castellan, G.W. (2004), Physical Chemistry, Narosa.
2. Kapoor, K.L. (2015), A Textbook of Physical Chemistry,Vol 1, 6th Edition, McGraw
Hill Education.
3. Kapoor, K.L. (2013), A Textbook of Physical Chemistry,Vol 3, 3rd Edition, McGraw
Hill Education.

Practicals:
1. Khosla, B.D.; Garg, V.C.;Gulati, A.(2015), Senior Practical Physical Chemistry, R.
Chand & Co.

135
 GE 11: Chemistry: Chemistry of Food Nutrients

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course Credits Credit distribution of the Eligibility Pre-requisite
title & course criteria of the course
Code Lecture Tutorial Practical/
Practice
Chemistry 4 2 2
of Food
Nutrients
(GE-11)

Learning Objectives
The Learning Objective of this course is as follows:

• To help the students develop a basic understanding of the components of food, their
source, properties and interactions as well as changes that occur during processing,
storage, and utilization.

Learning Outcomes
On completion of the course, the student will be able to:
● Build a strong understanding of chemistry of food: composition of food, role of each
component.
● Understand some of the reactions and changes in individual food components which
occur during processing, handling and storage

SYLLABUS OF GE-11

Theory:
Unit 1: Carbohydrates (6 Hours)
Introduction, sources, functions, classification: monosaccharide, oligosaccharide and
polysaccharide, structure and importance of polysaccharides in food chemistry (pectin,
cellulose, starch, gums), chemical reactions of sugar: mutarotation, caramelisation; non
enzymic browning and its prevention, role of carbohydrates as sweeteners in food.

Unit 2: Lipids (8 Hours)

Introduction, sources, classification (fatty acids, phospholipids, fats & oils, waxes), common
fatty acids present in oils and fats, Omega- 3&6 fatty acids, trans fats, chemical properties-
Reichert Meissel value, Polenski value, iodine value, peroxide value, saponification value,

136
effect of frying on fats, changes in fats and oils- rancidity, lipolysis, flavor reversion, auto-
oxidation and its prevention.

Unit 3: Proteins (8 Hours)

Introduction, sources, classification (simple, conjugated, derived), structure of protein

(primary, secondary and tertiary), physico-chemical & functional properties of proteins,
protein denaturation.

Unit 4: Vitamins & Minerals (8 Hours)

Vitamins: Introduction, classification: fat-soluble vitamins & water-soluble vitamins.
Minerals: Introduction, classification: macrominerals (Ca, P, Mg) & microminerals (Se, Fe, I,
Co, Zn, Cu, Se, Cr).
Physiological importance of vitamins and minerals, effect of food processing on vitamins and
minerals.

Practicals: (60 Hours)

(Laboratory periods: 60)
1. Determination of moisture in food products by hot air oven-drying method.

2. Colorimetric determination of Iron in vitamin / dietary tablets.

4. 2, 6-Dichlorophenol indophenol method for estimation of vitamin C in a given solution/

lemon Juice/chillies.

5. Estimation of total soluble sugar content by ferricyanide method (volumetric analysis).

6. Determination of saponification value of the given fat/oil.

7. Determination of iodine value of the given fat/oil.

8. Qualitative tests for proteins and carbohydrates.

9. Qualitative estimation of cholesterol by Liebermann Burchard method.

References:
Theory:
1. deMan, J.M., Finley, J.W., Hurst, W.J., Lee, C.Y. (2018), Principles o f F ood
Chemistry, 4th Edition, Springer.
2. Msagati, T.A.M. (2013), Chemistry of F ood A dditives an d P reservatives, Wiley-
Blackwell.
3. Fennema, O.R. (2017), Food Chemistry, 5th Edition, CRC Press.
4. Attokaran, M. (2017), Natural Food Flavors an d C olorants, 2nd Ed., Wiley-
Blackwell.
5. Potter, N.N., Hotchkiss, J.H, (1995) Food Science, 5th Ed., Chapman & Hall.

137
 6. Brannen, D., Davidsin, P.M., Salminen, T. Thorngate III, J.H. (2002), Food
Additives, 2nd Edition, CRC Press.
7. Coultate, T. (2016), Food: T he C hemistry o f i ts C omponents, 6th Edn., Royal
Society of Chemistry.
8. Belitz, H. D.; Grosch, W. (2009), Food Chemistry, Springer.
10. Course: FOOD CHEMISTRY (iasri.res.in)

Practical:
1. Ranganna, S. (2017). Handbook of an alysis a nd q uality c ontrol f or f ruits an d
vegetable products, 2nd Edn., McGraw Hill Education
2. Sawhney, S.K., Singh, R. (2001), Introductory P ractical B iochemistry, Narosa
Publishing House

GE 12: Chemistry: Statistical Methods and Data Analysis

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title Credits Credit distribution of the Eligibility Pre-
& Code course criteria requisite
Lecture Tutorial Practical/ of th e
Practice course
Chemistry: 4 2 2
Statistical
Methods and
Data Analysis
(GE-12)

Learning Objectives
The Learning Objectives of this course are as follows:

• To give the students insight about the statistical treatment on the chemical analysis data
along with illustration about the analysis of collected analytical data that will help them
to take up a job of technician, scientist and laboratory manager.
• To explain the presentation of data in different form such as “Table, Graph, Bar
Diagram, Pie Chart, Venn diagram” along with their reliability and validity.

Learning Outcomes
At the end of this course student will be:
• Familiar with interpretation and use of analytical data collected by different techniques,
significance of different analytical techniques and their applications, reliability and
presentation of data for reporting to different forum.

138
SYLLABUS OF GE-12

Theory:
Unit 1: Basics of Chemical Analysis ( 4 Hours)
Analytical Chemistry, Qualitative and quantitative analysis, Analytical methodology.
Calibration of glass wares, recording laboratory data.

Unit 2: Different Methods of Chemical Analysis (8 Hours)

Titrimetric method: volumetric titremetry, standard solution, titrimetric curve, calculation;
Gravimetric method: precipitation gravimetry, calculation and applications of gravimetry;
and Spectrometric methods: introduction, principle and instrument, working quantitative
aspects absorbance, applications in chemical analysis

Unit 3: Statistical Method of Chemical Analysis (8 Hours)

Accuracy and Precision, Comparison of precision, Errors, Distribution of random errors,
propagation of errors, measurement of errors, significant figure, inter laboratory error,
methods of least square analysis of variance, Q test, Z test, T test, statistical treatment of
finite sample, recommendations for treating outliers. Minimising errors in analytical
procedure.

Unit 4: Data Analysis and Validation (4 Hours)

Confidence interval, Testing of hypothesis, plotting of data, least square method, Figures of
merit: sensitivity, detection limit, linear dynamic range, control test, upper control limit and
lower control limit, Validation, reporting analytical results and significant figures

Unit 5: Sampling, Standardisation, Labelling and Calibration (6 Hours)

Analytical samples, sample size, constituent sample, real samples, sample, sample handling,
preparing laboratory samples, automated sample handling, lab on chip and General laboratory
principles, recording laboratory data, standards, comparison of standards, internal standard,
external standards calibration, least square method, and multivariant calibration.

Practicals: (60 Hours)

(Laboratory periods: 60)
1. Calibrate the volume of laboratory glass wares i.e. volumetric flask, beaker, burette and
calibration constant.
2. Demonstrate the good laboratory practices like effect of dilution, temperature, taking
observation, personal and apparatus safety.
3. Determine the quantitative presence of heavy metals like copper, chromium and iron in
natural and laboratory samples using volumetric and gravimetric titration.
4. Determine the presence of magnesium ion in heavy water by EDTA method and prepare
calibration curve.
5. Evaluate the absolute and method errors in a set of data collected during determination of
nitrogen in an organic compound.
6. Calculate the standard deviation and predict precision of analytical results.

139
7. Determine the concentration of pollutant in natural sample after using external standards
methods.
8. Compare the inter laboratory error of a spectroscopic results.
9. Evaluate the limit of detection for colorimetric analysis of dyes and coloured metals in
wastes water samples.
10. Demonstrate the control of interference by masking by complexation.
11. Report the ten analytic results in significant numbers along with standard deviation.
12. Determine the confidence limit and interval for a laboratory instrument like breath
alcohol analyser
13. Demonstrate the internal standard method for calibration of metal estimation.
14. Estimate the comparative effectiveness of different types of graphs like line, pi chart and
bar graph.
15. Demonstrate the working of lab on chip like glucose sensor.

References:
1. Dey, R. A. and Underwood, A. L., Quantitative Analysis, 6th Edition, Pearson.
2. Skoog, D. A., West, D. M., Holler, F. J., Crouch, S. R., Fundamental an alytical
chemistry, Thomson Asia Ltd.
3. Encyclopaedia of analytical chemistry: Applications, Theory, and Instrumentation, R
A Meyor (Eds) Wiley and Sons (2000).

GE 13: Chemistry: Medicines in Daily Life

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course Credits Credit distribution of the Eligibility Pre-requisite
title & course criteria of the course
Code Lecture Tutorial Practical/
Practice
Medicines 4 2 2
in Daily
Life
(GE-13)

Learning Objectives

The Learning Objectives of this course are as follows:

• To make students study the basic details about various medicines of general uses,
which are crucial for the various diseases.
• To make students learn about the active pharmaceutical ingredient in some medicines,
their synthesis; therapeutic effect and side effects on human physiology.

140
 • To make students aware about the positive and negative effects of medicines those are
essential for a healthy day-to-day life.

Learning Outcomes
By the end of the course, the students will be able to:
● Understand the role of different medicines on human physiology.
● Gain the knowledge of active pharmaceutical ingredient and their roles in different
disease.
● Learn the proper use of different medicines and their effect and side effects.
● Learn the techniques of administering blood group, pulse rate, blood pressure and
may other general diagnostic applications.

SYLLABUS OF GE-13

Theory:
Unit 1: General Introduction (8 Hours)

Introduction-Health, disease, drugs, chemotherapy, approaches in drug designing,

classification of drugs and their origin.

Unit 2: Different class of medicines (22 Hours)

Structure of active ingredients, uses, dosage, side effects and their natural remedies:
Analgesics and antipyretics- Aspirin, paracetamol, ibuprofen, morphine, codeine
Antibiotics- Amoxicillin, norfloxacin, ciprofloxacin
Antihistamines or antiallergics- Cetrizine and Levocetrizine (role of stereoisomers)
Antiparasitic- Albendazole
Antidiabetics- Insulin, Glipizide and metformin
Antihypertensive – Amlodipine and its natural remedies- Rauwolfia.
Diuretic- Lasix
Antidepressant-Zoloft and its natural treatment
Antifungal – fluconazole, Itraconazole
Antacids- Ideal properties of antacids, combinations of antacids, Sodium 40 Bicarbonate,
rantidine, milk of magnesia, aluminium hydroxide gel
Anticoagulants/antiplatelet drugs- Warfarin, heparin and Ecosprin
Anaesthetics- Atracurium, Desflurane
Poison and Antidote: Sodium thiosulphate, Activated charcoal, Sodium nitrite
Astringents: Zinc Sulphate, Potash Alum
Supplements- zinc and calcium, vitamins
Synthesis of small molecule drugs like aspirin and paracetamol
Practicals: (60 Hours)
(Laboratory periods: 60)
1. Determination of heart rate and pulse rate, blood pressure and discussion on
medicines affecting them.
2. Identification test- Magnesium hydroxide, Sodium bicarbonate, Calcium gluconate.

141
 3. Preparation of inorganic pharmaceuticals- Boric acid Potash alum
4. Determination of sugar content in the given solution.
5. Estimation of zinc and calcium in a given solution.
6. Qualitative analysis of carbohydrates (Glucose, Fructose, Lactose, Maltose, Sucrose).
7. Qualitative tests for Proteins
8. Qualitative analysis of vitamin C.
9. Isolation of paracetamol (API) from a commercial tablet
10. Isolation of aspirin (API) from tablet and recording of melting point (synthesis needs
discussion)
References:
Theory:
1. Patrick, G. L. (2001) Introduction t o Med icinal C hemistry, Oxford University
Press.
2. Lemke, T. L. & William, D. A. (2002), Foye’s Principles of Medicinal Chemistry,
5th Ed., USA,
3. Singh H.; Kapoor V.K. (1996), Medicinal and Pharmaceutical Chemistry, Vallabh
Prakashan.
4. Chatwal, G.R. (2010), Pharmaceutical ch emistry, inorganic (vol. 1), Himalayan
publishing house
5. https://go.drugbank.com./

Practicals:
1. Jeffery, G.H., Bassett, J., Mendham, J., Denney, R.C. (1989), Vogel’s Textbook of
Quantitative Chemical Analysis, John Wiley and Sons.
2. Ahluwalia, V.K., Dhingra, S. (2004), Comprehensive Practical Organic
Chemistry: Qualitative Analysis, University Press.
3. Munwar, S., Ammaji, S.(2019), Comprehensive Practical Manual of
Pharmaceutical Chemistry, Educreation Publishing.
4. Mondal, P., Mondal, S.(2019), Handbook of Practical Pharmaceutical Organic,
Inorganic and Medicinal chemistry, Educreation Publishing.

GE 15: Chemistry and Society

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course Credits Credit distribution of the Eligibility Pre-requisite

title & course criteria of the course
Code Lecture Tutorial Practical/
Practice
Chemistry 4 2 2
and
Society
(GE-15)

142
Learning Objectives

The Learning Objectives of this course are as follows:

• To expand the literacy of chemistry, and increase general awareness, background of
chemistry and its importance among the non-chemistry student even arts as well as
commerce.
• To make a common student understand the importance and role of chemistry in
development of civilization, societal issues related to chemistry and their expected
solutions.

Learning Outcomes

At the end of this course the student will be able to:

• Increase the literacy of chemistry even in non-science students
• Understand the basic concept, principle and importance of chemistry
• Realize the importance of chemistry in daily life and future requirement

SYLLABUS OF GE-15

Theory:
Unit 1: Basics of chemistry (4 Hours)
Periodic table, Atom and molecules, chemical bonding, properties and chemical reactions
with simple examples and illustration.

Unit 2: Chemistry in Heritage (8 Hours)

Extraction and uses of metals like iron and stone in ancient times, metals in ornaments,
medicines, weapons and chemistry for preservatives, basics of preservation and few examples
of preservatives.
Unit 3: Chemistry in Life (10 Hours)

Edible and non- edible molecules, biochemistry of foods and medicine with examples:
Aspirin, Paracetamol. Ibuprofen and Penicillin, Cephalosporin, Chemistry for industry:
Artificial sweeteners, Soaps and detergents and cosmetics, Polymer and Plastics: Uses and
environmental issues.

Unit 4: Chemical pollution and Toxicity (2 Hours)

Chemical source of water, air and soil pollution, biomagnification and metal toxicity with
example and illustrations. monitoring of air pollution.

Unit 5: Testing of chemicals (2 Hours)

Flame test, solubility test, qualitative and quantitative identification of ions in natural samples
like metal copper, iron and chromium ores and adulterant in foods.

Unit 6: Future of chemistry (4 Hours)

Basics of green chemistry, Reuse and recycling of by-products, zero waste chemistry and
Alternate fuel and energy providing chemicals: biodiesel, natural gas and hydrogen.

143
Practicals/Hands-on Training: (60 Hours)
(Laboratory periods: 60)
1. Determine the calcium and magnesium contents in water samples using EDTA
methods.
2. Determine the organic contents and pH of soil sample.
3. Estimate the food adulterants in edible items
4. Quantify the presence metals by flame test method
5. Demonstrate the conversion of PET into bottle into value added products.
6. Determine the quantitative presence of heavy metals like copper and chromium in
natural sample like ore.
7. Demonstrate the exothermic and endothermic reaction in laboratory
8. Preparation aspirin and paracetamol as well as identify.
9. Compare the fuel efficiency of biodiesel and petrol.
10. Preparation of representative compound using microwave
11. Demonstrate the biodegradability of natural and synthetic plastics.
12. Demonstrate the protection of rusting of iron after surface spray coating.
13. Estimate the protein contents in edible samples using chemical methods.
14. Small working project on heritage chemistry like bio compatibility of metals and
medicinal importance of metals like iron, gold and silver.

References:
1. Lee, J. D., Concise Inorganic Chemistry, Wiley India Pvt. Ltd.
2. Sharma, B. K., Industrial chemistry, Goel Publishing House, India
3. Christian, Gary D., Dasgupta, Purnendu K., Schug, Kevin A., Analytical chemistry,
Wiley
4. V. Subramanian, A text book of Environmental chemistry, Wiley

GE 19: Radio-chemistry in Energy, Medicine and Environment

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE

COURSE
Course title Credits Credit distribution of the Eligibility Pre-
& Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice
Radio- 4 3 1
chemistry in
Energy,
Medicine and
Environment
(GE-19)

144
Learning Objectives

The Learning Objectives of this course is as follows:

• To give an introduction to nuclear and radiochemical concepts to the students.

• To help students gain fundamental knowledge about the radioisotopes and their real-
world applications in medicine, diagnostic techniques, energy, research and
environment.

Learning Outcomes

By the end of the course, the students will:

• Learn about radioisotopes, radioactive decay
• Use of radiochemistry in various fields
• Effect of radiations on health
• Learn about nuclear energy and nuclear pollution

SYLLABUS OF GE-19

Theory:
Unit 1: Introduction (9 Hours)
Atoms, composition of nucleus, mass number, isotopes, nuclear stability, radioactive decay,
radioactivity in nature: natural and artificial radioisotopes, elementary particles, radioactive
decay (α, β and γ decay), half-life period, types of nuclear reactions: nuclear fission and
nuclear fusion.

Unit 2: Nuclear power generation (6 Hours)

Nuclear Power generation from uranium ore (energy production and nuclear waste),
introduction to nuclear reactors for energy and nuclear weapons

Unit 3: Applications of radiochemistry (15 Hours)

C 14 decay and radioactive dating, irradiation of food, radiotracers for studying chemical
reactions (photosynthesis, metabolic studies of drugs, metabolism of organisms, fundamental
properties of genetic material), medicinal application of radio chemicals in radiotherapy (use
in cancer, hyperthyroidism, blood disorders), radio-pharmaceuticals, diagnostic procedures:
CT, PET

Unit 4: Environment radioactivity (6 Hours)

Natural radioactivity, natural process that release radioactive material in environment, man-
made events like Chernobyl disaster, bomb test, use of radiotracers in environmental studies.

Unit 5: Nuclear pollution and safety management (9 Hours)

145
Radiation protection standards, basics of radiation hazards, international guidelines on
radiation protection, disposal of nuclear waste, nuclear disaster and it's managements, Effect
of radiation on health: Biological effects of radiation, radiation monitors, dose limits for
workers and public,

Practicals: (30 Hours)

(Laboratory periods: 30)
1. Study the background radiation in different places and identify the probable source.
(Data to be provided).
2. Survey the diagnostic procedures involving radio-chemistry in different diagnostic
laboratories.
3. Write a report on the radio isotopes used in various diagnostic procedures.
4. Write a report on safety measures taken in diagnostic labs.
5. Write a report on any two nuclear and radiation accidents focusing on their impact on
human life, environment and economy.

References:
1. Nuclear and radiochemistry, Konya J., Nagy N. 2nd Edition, Elsevier
2. Radiochemistry and Nuclear Chemistry, 4th Edition, Choppin G., Lilijenzin J-O,
Rydberg J., Ekberg C. Elsevier.

GE 21: Chemistry in Indology and Physical & Mental Well Being

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course Credits Credit distribution of the Eligibility Pre-
title & course criteria requisite
Code Lecture Tutorial Practical/ of the
Practice course
Chemistry 4 3 1
in
Indology
and
Physical
& Mental
Well
Being
(GE-21)

Learning Objectives

The Learning Objectives of this course is as follows:

• To illuminate the students about the scientific basis and approaches related to the
practices that promote physical and mental health/balance, that includes meditation,

146
 sports, Yoga and nutrition. The chemical/biochemical mechanisms that underscore the
various states of the mind and body, which drives the general homeostasis or
anomalies thereof, shall also be illustrated.
• To make students aware about role of metals in ancient and medieval India
• To make students aware of how Alchemists used metals, chemicals, compounds and
ores in medicines
• To make students aware of the different types of instruments used in the ancient and
medieval India
• To make students aware of the life and work of ancient and medieval
scientists/chemists.

Learning Outcomes:
By the end of the course, the students will:
• Understand about the scientific basis and approaches that promote physical and
mental health.
• Know about the chemical/biochemical mechanisms that underline the states of the
mind and body
• Understand the role of metals in ancient and medieval India
• Understand how alchemists used metals and chemical compounds in medicines
• Know about the life and contributions of ancient scientists and chemists

SYLLABUS OF GE-21

Theory:

Unit 1: Physical Health Practices (9 Hours)

Principles of Physical Education, Body composition with respect to health and fitness and
different methods of body composition analysis, Calculation of energy expenditure (at rest
and during exercise), VO2 and calculation of VO2 max, respiratory exchange ratio, blood
pressure, Means of fitness development- aerobic and anaerobic exercises, yoga and physical
fitness, Exercises and their intensities related to heart rate zone, Different fitness levels for
different age groups and gender, Kinesiology, Physiology of Exercise

Unit 2: Mind-body Practices (6 Hours)

States of mind and types of brain waves, mindfulness meditation in clinical psychology and
psychiatry, Desbordes’ recent studies on brain activities (Harvard’s studies), MRI &
functional MRI studies.

147
Types of meditations- focused attention meditation (FA), open monitoring meditation (OM),
transcendental meditation (TM), loving–kindness meditation (LKM), mindfulness meditation
(MM) and body–mind meditation (B-M).
Biochemical alterations, such as changes in activity/production of hormones, cytokines,
chemokines, interferons, etc., oxygen saturation/desaturation, redox-condition and oxidative
balance, progression/regression of certain diseases/health conditions, in response to various
states of physical and mental well-being.

Unit 3: Nutrition for Mind/body Homeostasis (6 Hours)

Role of nutrition in physical and mental health. Nutrients: carbohydrates, Protein, Fat,
Vitamins, Minerals, Water-their functions, role of hydration (water balance) during exercise,
daily caloric requirement and expenditure.
Metabolism: An overview of ATP release in glycolysis, TCA cycle, electron transport chain.
basic concept of balanced diet vs. fad diet (Atkins, ketogenic etc.), Concept of BMI (Body
mass index) and BMR (Basal metabolic rate), Obesity and its hazard, Dieting versus exercise
for weight control.

Unit 4: Concepts of Atoms, Molecules and Laws of Motion (3 Hours)

Concepts of atoms and molecules, properties and categories of atoms and molecules, Laws of
motion.

Unit 5: Metallurgy (6 Hours)

Gold, Silver, Copper, Bronze and other alloys; Copper smelting blast furnace and copper
extraction; Tron and Steel; Iron smelting blast furnaces from Southern India; Ironworks in
Ancient and medieval India; Delhi Iron Pillar; Dhar and Kodachadri Iron pillars; Wootz steel;
Zinc and its extraction.

Unit 6: Chemicals (3 Hours)

Drugs, dyes, pigments, glass, cosmetics and perfumes, etc.

Unit 7: Drugs (6 Hours)

Eight categories of Gandhasara; Compounds of mercury (Hg) made and used by the Indian
Alchemists for medicinal purposes; Use of chemical, compounds and ores in medicines.

Unit 8: Life and work of Ancient Indian Scientists/Chemists (6 Hours)

(i) Maharshi Kanada (Ancient text and manuscripts), (ii) Nagarjuna (Ras Ratnakar,
Kakshaputtantra, Arogya Manjari, Yog Saar, Yoasthak), (iii) Vaagbhatt (Rasratna
Samuchchay), (iv) Govindacharya (Rasarnava), (v) Yashodhar (Ras Prakash Sudhakar), (vi)
Ramachandra (Rasendra Chintamani), (vii) Somdev (Rasendra Chudamani)

Practicals: (30 Hours )

148
(Laboratory periods: 30)
1. Extraction of essential oil from rose petal.
2. Extraction of casein from milk.
3. Determination of pulse rate/blood pressure/oxygen saturation before and after
exercise.
4. Determination of acid value of given oil sample.
5. Isolation of piperine from black pepper.
6. Determination of Copper in a brass turnings.
7. Extraction of Butea monosperma (Palash) dye for its use in coloration of cloth.
8. Determination of mass loss in mild steel in acidic/basic media.
9. Project on (Do any one):
Ayurveda as alternate medicine system,
Homeopathy in India,
Yogic Practices for mental wellness
Ancient Chemists of India
Other titles can also be suggested by the teacher.
10. Visit to
Iron Pillar, the metallurgical marvel and prepare a brief report.
Industries like Dabur India Ltd.
References:
1. Baer cites Kabat-Zinn, J. (1994): Wherever y ou g o, t here y ou a re: Mindfulness
meditation in everyday life. New York: Hyperion, p.4.
2. Buchholz L (October 2015). "Exploring the Promise of Mindfulness as Medicine".
JAMA. 314 (13): 1327–1329. doi:10.1001/jama.2015.7023. PMID 26441167.
3. Harrington A, Dunne JD (October 2015). "When m indfulness is t herapy: E thical
qualms, h istorical p erspectives". The American Psychologist. 70 (7): 621–631.
doi:10.1037/a0039460. PMID 26436312.
4. Blanck P, Perleth S, Heidenreich T, Kröger P, Ditzen B, Bents H, Mander J (March
2018). "Effects of mindfulness exercises as stand-alone intervention on symptoms
of an xiety an d d epression: S ystematic review an d m eta-analysis". Behaviour
Research and Therapy. 102: 25–35. doi:10.1007/s12671-014-0379-y. PMID
29291584.
5. Khoury B, Sharma M, Rush SE, Fournier C (June 2015). "Mindfulness-based stress
reduction f or he althy individuals: A m eta-analysis". Journal of Psychosomatic
Research. 78 (6): 519–528. doi:10.1016/j.jpsychores.2015.03.009. PMID 25818837.
6. Jain FA, Walsh RN, Eisendrath SJ, Christensen S, Rael Cahn B (2015). "Critical
analysis of t he e fficacy of m editation t herapies f or ac ute an d s ubacute p hase
treatment o f d epressive d isorders: a s ystematic rev iew". Psychosomatics. 56 (2):
140–152. doi:10.1016/j.psym.2014.10.007. PMC 4383597. PMID 25591492.
7. Reangsing C, Punsuwun S, Schneider JK (March 2021). "Effects o f m indfulness
interventions o n d epressive s ymptoms i n a dolescents: A m eta-analysis".
International Journal of Nursing Studies. 115: 103848.
doi:10.1016/j.ijnurstu.2020.103848. PMID 33383273. S2CID 229940390.

149
8. Sharma M, Rush SE (October 2014). "Mindfulness-based s tress red uction a s a
stress management i ntervention f or h ealthy i ndividuals: a s ystematic rev iew".
Journal of Evidence-Based Complementary & Alternative Medicine. 19 (4): 271–286.
doi:10.1177/2156587214543143. PMID 25053754.
9. Hofmann SG, Sawyer AT, Witt AA, Oh D (April 2010). "The effect of mindfulness-
based t herapy o n a nxiety a nd de pression: A meta-analytic rev iew". Journal of
Consulting and Clinical Psychology. 78 (2): 169–183. doi:10.1037/a0018555. PMC
2848393. PMID 20350028.
10. Chiesa A, Serretti A (April 2014). "Are mindfulness-based interventions ef fective
for substance use disorders? A systematic review of the evidence". Substance Use
& Misuse. 49 (5): 492–512. doi:10.3109/10826084.2013.770027. PMID 23461667.
S2CID 34990668.
11. Garland EL, Froeliger B, Howard MO (January 2014). "Mindfulness t raining
targets n eurocognitive mechanisms of ad diction at t he at tention-appraisal
emotion i nterface". Frontiers in Psychiatry. 4: 173. doi:10.3389/fpsyt.2013.00173.
PMC 3887509. PMID 24454293.
12. Sancho M, De Gracia M, Rodríguez RC, Mallorquí-Bagué N, Sánchez-González J,
Trujols J, et al. (2018). "Mindfulness-Based I nterventions f or t he T reatment o f
Substance an d B ehavioral A ddictions: A S ystematic R eview". Frontiers in
Psychiatry. 9 (95): 95. doi:10.3389/fpsyt.2018.00095. PMC 5884944. PMID
29651257.
13. Paulus MP (January 2016). "Neural B asis o f Mi ndfulness I nterventions t hat
Moderate the I mpact o f Stress on the Brain". Neuropsychopharmacology. 41 (1):
373. doi:10.1038/npp.2015.239. PMC 4677133. PMID 26657952.
14. Dunning DL, Griffiths K, Kuyken W, Crane C, Foulkes L, Parker J, Dalgleish T
(March 2019). "Research Review: The effects of mindfulness-based interventions
on c ognition a nd mental he alth i n c hildren a nd a dolescents - a metaanalysis o f
randomized co ntrolled t rials". Journal of Child Psychology and Psychiatry, and
Allied Disciplines. 60 (3): 244–258. doi:10.1111/jcpp.12980. PMC 6546608. PMID
30345511.
15. Sharman, J. R. (1964). Introduction to physical education. New York: A.S. Barnes
& Co.
16. William, J. F. (1964). The pr inciples o f physical e ducation. P hiladelphia: W.B.
Saunders Co
17. Bucher, C. A. (n.d.) Foundation of physical education. St. Louis: The C.V. Mosby
Co.
18. Sharkey, B. J. (1990). Physiology of fitness, Human Kinetics Book
19. Giam, C.K & The, K.C. (1994). Sport medicine ex ercise a nd f itness. Singapore:
P.G. Medical Book.
20. Kenney, W.L., Wilmore, J.H., Costill, D.L. (six edition) Physiology of sport an d
exercise.
21. Vedas: (i) Rig Veda, (ii) Yajur Veda, (iii) Atharva Veda, (iv) Sama Veda
22. Deb, B. M., The Peacock in Splendour, Visva Bharti University.
23. Ray, P. C., A History of Hindu Chemistry: from the Earliest Times to the Middle
of t he Si xteenth C entury A .D., Volume 1 – 1902, Volume 2 – 1908, The Bengal
Chemical and Pharmaceutical Works Ltd

150
24. “History of Chemistry in Ancient and Mideaval India” (Edited volume of Acharya
Ray’s “History of Hindu Chemistry”), Indian Chemical Society, Calcutta, 1956.
25. Harsha, N. M., Nagaraja, T. N., The History of Hindu Chemistry, Ancient Science
of Life, 2010, 30, 58 – 61.
26. Ray, P. C., Life and experiences of a Bengali chemist, Two Volume Set. Calcutta:
Chuckervertty, Chatterjee & Co. 1932 and 1935.
27. Ray, P. R., Chemistry i n A ncient I ndia, Journal of Chemical Education, 1948, 25
(6), 327.
28. Seal, B. N.(1915), The Positive Sciences of the Ancient Hindus, Longman Greens
and Co., Kolkata.

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 DEPARTMENT OF CHEMISTRY
Category-I

B.Sc. (H) Chemistry

DISCIPLINE SPECIFIC CORE COURSE -4 (DSC-4): CHEMISTRY OF S- AND P-BLOCK

ELEMENTS

Credit distribution, Eligibility and Pre-requisites of the Course

Course title & Credits Credit distribution of the Eligibility Pre-requisite

Code course criteria of the course
Lecture Tutorial Practical/ (if any)
Practice
Chemistry of s- 04 03 0 01 Class 12th ----
and p-Block Pass
Elements
(DSC-4:
Inorganic
Chemistry -II)

Learning objectives
The objectives of this course are as follows:
• To develop the general principles of metallurgy and s-, p-block elements.
• To introduce the terms minerals, ores, concentration, benefaction,
calcination, roasting, refining, etc. and explain the principles of oxidation and
reduction as applied to the extraction procedures.
• To make students ware of different methods of purification of metals, such as
electrolytic, oxidative refining, VanArkel-De Boer process and Mond’s process
are discussed and applications of thermodynamic concepts like that of Gibbs
energy and entropy to the extraction of metals.
• To familiarize students with the patterns and trends exhibited by s- and p-block
elements and their compounds with emphasis on synthesis, structure, bonding
and uses.
• To impart information about the fundamentals of internal and external redox
indicators, and iodometric/iodimetric titrations.

Learning outcomes
By studying this course, students will be able to:
● Learn the fundamental principles of metallurgy and understand the
importance of recovery of by-products during extraction.
● Applications of thermodynamic concepts like that of Gibbs energy and

96
 entropy to the principles of extraction of metals.
● Learn about the characteristics of s- and p- block elements as well as the
synthesis, structure, bonding and uses of their compounds
● Understand the concept and use of internal and external redox indicators
● Comprehend the theory and application of iodometric and iodimetric
titrimetric analysis

SYLLABUS OF DSC-4

UNIT – I: General Principles of Metallurgy (6 Hours)

Chief modes of occurrence of metals based on standard electrode potentials. Ellingham
diagrams for reduction of metal oxides using carbon and carbon monoxide as reducing agent.
Electrolytic Reduction, Hydrometallurgy with reference to cyanide process for silver and gold.
Methods of purification of metals: Electrolytic process, Van Arkel-De Boer process, Zone
refining. Brief discussion of metals and alloys used in ancient and medieval India.

UNIT – II: Chemistry of s- Block Elements (15 Hours)

General characteristics: melting point, flame colouration, reducing nature, diagonal
relationships and anomalous behavior of first member of each group. Reactions of alkali and
alkaline earth metals with oxygen, hydrogen, nitrogen and water.
Common features such as ease of formation, thermal stability, energetics of dissolution, and
solubility of the following alkali and alkaline earth metal compounds: hydrides, oxides,
peroxides, superoxides, carbonates, nitrates, sulphates.
Complex formation tendency of s-block elements; structure of the following complexes:
crown ethers and cryptates of Group I; basic beryllium acetate, beryllium nitrate, EDTA
complexes of calcium and magnesium.
Solutions of alkali metals in liquid ammonia and their properties

UNIT – III: Chemistry of p-Block Elements (9 Hours)

Electronic configuration, atomic and ionic size, metallic/non-metallic character, melting point,
ionization enthalpy, electron gain enthalpy, electronegativity, Catenation, Allotropy of C, P, S;
inert pair effect, diagonal relationship between B and Si and anomalous behaviour of first
member of each group.

UNIT – IV: Compounds of p-Block Elements (15 Hours)

Acidic/basic nature, stability, ionic/covalent nature, oxidation/reduction, hydrolysis, action of
heat on the following:
● Hydrides of Group 13 (only diborane), Group 14, Group 15 (EH3 where E = N, P,As,
Sb, Bi), Group 16 and Group 17.
● Oxoacids of phosphorus, sulphur and chlorine
● Interhalogen and pseudohalogen compound
● Clathrate compounds of noble gases, xenon fluorides (MO treatment of XeF2).

97
Practical component – 30 Hours

1. Redox Titrations
(i) Estimation of Fe(II) with K2Cr2O7 using diphenylamine as internal indicator.
(ii) Estimation of Fe(II) with K2Cr2O7 using N-phenyl anthranilic acid as
internal indicator.
(iii) Estimation of Fe(II) with K2Cr2O7 using external indicator.

2. Iodo/Iodimetric Titrations
(i) Estimation of Cu(II) using sodium thiosulphate solution (Iodometrically).
(ii) Estimation of K2Cr2O7 using sodium thiosulphate solution
(Iodometrically).
(iii) Estimation of antimony in tartaremetic iodimetrically.
(iv) Estimation of Iodine content in iodized salt.

Essential/recommended readings
Theory:
1. Lee, J. D.; (2010), Concise Inorganic Chemistry, Wiley India.
2. Huheey, J. E.; Keiter, E. A.; Keiter; R.L.; Medhi, O.K. (2009), Inorganic
Chemistry-Principles of Structure and Reactivity, Pearson Education.
3. Atkins, P. W.; Overton, T. L.; Rourke, J. P.; Weller, M. T.; Armstrong, F. A.
(2010), Shriver and Atkins Inorganic Chemistry, 5th Edition, Oxford
University Press.
4. Miessler, G. L.; Fischer P. J.; Tarr, D. A. (2014), Inorganic Chemistry, 5th
Edition, Pearson.
5. Housecraft, C. E.; Sharpe, A. G., (2018), Inorganic Chemistry, 5thEdition,
Pearson.
6. Canham, G. R., Overton, T. (2014), Descriptive Inorganic Chemistry, 6th
Edition, Freeman and Company.
7. Greenwood, N. N.; Earnsaw, A., (1997), Chemistry of Elements, 2nd Edition,
Elsevier.
Practicals:
1. Jeffery, G. H.; Bassett, J.; Mendham, J.; Denney, R. C. (1989), Vogel’s Text
book of Quantitative Chemical Analysis, John Wiley and Sons.
2. Harris, D. C.; Lucy, C. A. (2016), Quantitative Chemical Analysis, 9th Edition,
Freeman and Company.
3. Day, R. A.; Underwood, A. L. (2012), Quantitative Analysis, 6th Edition, PHI
Learning Private Limited.
Note: Examination scheme and mode shall be as prescribed by the Examination
Branch, University of Delhi, from time to time.

98
 DISCIPLINE SPECIFIC CORE COURSE – 5 (DSC-5): HALOALKANES, ARENES,
HALOARENES, ALCOHOLS, PHENOLS, ETHERS AND EPOXIDES

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutori Practical/ of the
al Practice course
(if any)
Haloalkanes, 04 02 0 02 Class 12th ---
Arenes, Pass
Haloarenes,
Alcohols,
Phenols, Ethers
and Epoxides
(DSC-5: Organic
Chemistry-II)

Learning Objectives

The Learning Objectives of this course are as follows:

• To impart understanding of the chemistry of organic functional groups, which
include haloalkanes, aromatic hydrocarbons, haloarenes and some oxygen
containing functional groups, along with their reactivity patterns.
• To develop understanding of detailed reactions and mechanistic pathways for
each functional group to unravel the spectrum of organic chemistry and the
extent of organic transformations.
• To aid in the paramount learning of the concepts and their applications.

Learning outcomes

On completion of the course, the student will be able to:

● Understand reactions of arenes, haloarenes and some oxygen containing
functional groups.
● Understand the concept of protection and deprotection
● Use the synthetic chemistry learnt in this course to do functional group
transformations.
● Propose plausible mechanisms for the reactions under study.

99
SYLLABUS OF DSC-5

Unit - 1: Haloalkanes ( 10 Hours)

Alkyl halides: Methods of preparation and properties, nucleophilic substitution
reactions – SN1, SN2 and SNi mechanisms with stereochemical aspects and effect of
solvent; nucleophilic substitution v/s elimination.
Organometallic compounds of Mg (Grignard reagent) – Use in synthesis of organic
compounds.

Unit - II: Aromatic Hydrocarbons (06 Hours)

Concept of Aromaticity and anti-aromaticity; Electrophilic aromatic substitution:
halogenation, nitration, sulphonation, Friedel Crafts alkylation/acylation with their
mechanism. Directing effects of groups in electrophilic substitution.

Unit - III: Aryl halides (04 Hours)

Preparation (including preparation from diazonium salts) and properties, nucleophilic
aromatic substitution; SNAr, Benzyne mechanism. Relative reactivity of alkyl, allyl,
benzyl, vinyl and aryl halides towards nucleophilic substitution reactions.

Unit - IV: Alcohols, Phenols, Ethers & Epoxides (10 Hours)

Alcohols: Relative reactivity of 1°, 2°, 3° alcohols, reactions of alcohols with sodium,
HX (Lucas test), esterification, oxidation (with PCC, alkaline KMnO4, acidic dichromate,
conc. HNO3). Oppenauer oxidation; Diols: oxidation of diols by periodic acid and lead
tetraacetate, Pinacol-Pinacolone rearrangement.
Phenols: Preparation using Cumene hydroperoxide, Acidity and factors affecting it,
Kolbe’s–Schmidt reactions, Riemer-Tiemann reaction, Houben–Hoesch condensation,
Schotten–Baumann reaction, Fries and Claisen rearrangements and their mechanism.
Ethers and Epoxides: Acid and Base catalyzed cleavage reactions.

Practical - 60 Hours
1. Acetylation of any one of the following compounds: amines (aniline, o-, m-, p-
toluidines and o-, m-, p-anisidine) and phenols (β-naphthol, salicylic acid) by any
one method:
i. Using conventional method ii. Using green approach
2. Benzolyation of one of the following amines (aniline, o-, m-, p-toluidines and o,
m-, p-anisidine) or one of the following phenols (β-naphthol, resorcinol, p-
cresol) by Schotten-Baumann reaction.
3. Bromination of acetanilide/aniline/phenol by anyone of the following:
(a) Green method b) Conventional method
4. Nitration of nitrobenzene/chlorobenzene.
5. Haloform reaction of ethanol.
6. Oxidation of benzyl alcohol to benzoic acid
7. Estimation of the given sample of phenol/amine by:

100
 a) Acetylation b) Bromate-Bromide method
8. Functional group tests for alcohols, phenols, carboxylic acids, phenols, carbonyl
compounds, esters.

Essential/recommended readings
Theory:
1. Morrison, R. N., Boyd, R. N., Bhattacharjee, S.K. (2010), Organic
Chemistry, 7th Edition, Dorling Kindersley (India) Pvt. Ltd., Pearson
Education.
2. Finar, I.L. (2002), Organic Chemistry, Volume 1, 6th Edition, Dorling Kindersley
(India) Pvt. Ltd., Pearson Education.
3. Ahluwalia, V.K.; Bhagat, P.; Aggarwal, R.; Chandra, R. (2005), Intermediate for
Organic Synthesis, I.K. International.
4. Solomons, T.W.G., Fryhle, C.B., Snyder, S.A. (2017), Organic Chemistry, 12th
Edition, Wiley.
Practical:
1. Mann, F.G., Saunders, B.C. (2009), Practical Organic Chemistry, 4th Edition,
Pearson Education.
2. Furniss, B.S., Hannaford, A.J., Smith, P.W.G., Tatchell, A.R. (2005), Vogel's
Textbook of Practical Organic Chemistry, Pearson.
3. Ahluwalia, V.K., Aggarwal, R. (2004), Comprehensive Practical Organic
Chemistry: Preparation and Quantitative Analysis, University Press.
4. Ahluwalia, V.K., Dhingra, S. (2004), Comprehensive Practical Organic
Chemistry: Qualitative Analysis, University Press.
5. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–I, I K
International Publishing house Pvt. Ltd, New Delhi
6. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–II, I K
International Publishing house Pvt. Ltd, New Delhi

Suggestive readings
1. Carey, F.A., Sundberg, R. J. (2008), Advanced Organic Chemistry: Part B:
Reaction and Synthesis, Springer.
2. Bruice, P.Y. (2020), Organic Chemistry, 3rd Edition, Pearson.
3. Patrick, G. (2012), BIOS Instant Notes in Organic Chemistry, Viva Books.
4. Parashar, R.K., Ahluwalia, V.K. (2018), Organic Reaction Mechanism, 4th
Edition, Narosa Publishing House.

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

101
 DISCIPLINE SPECIFIC CORE COURSE – 6 (DSC-6): Thermodynamics and its
Applications
Credit distribution, Eligibility and Pre-requisites of the Course

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chemical 04 03 - 01 Class XII ----
Thermodynamics Pass
and its
Applications
(DSC – 6: Physical
Chemistry – II)

Learning Objectives

The Learning Objectives of this course are as follows:

• To make students understand thermodynamic concepts, terminology,
properties of thermodynamic systems, laws of thermodynamics and their
correlation with other branches of physical chemistry and make them able to
apply thermodynamic concepts to the system of variable compositions,
equilibrium and colligative properties.

Learning outcomes
On completion of the course, the student will be able to:
• Understand the three laws of thermodynamics, concept of State and Path functions,
extensive and intensive properties.
• Derive the expressions of ΔU, ΔH, ΔS, ΔG, ΔA for an ideal gas under different
conditions.
• Explain the concept of partial molar properties.

SYLLABUS OF DSC-6

UNIT – I: Basic Concepts of Chemical Thermodynamics (06 Hours)

Intensive and extensive variables; state and path functions; isolated, closed and open
systems.

102
Mathematical treatment - Exact and inexact differential, Partial derivatives, Euler's
reciprocity rule, cyclic rule.
UNIT – II: First law and Thermochemistry (15 Hours)
Concept of heat, Q, work, W, internal energy, U, and statement of first law; enthalpy,
H, relation between heat capacities, Joule Thompson Porous Plug experiment, Nature
of Joule Thompson coefficient, calculations of Q, W, ΔU and ΔH for reversible,
irreversible and free expansion of gases (ideal and van der Waals) under isothermal
and adiabatic conditions.
Enthalpy of reactions: standard states; enthalpy of neutralization, enthalpy of
hydration, enthalpy of formation and enthalpy of combustion and its applications,
bond dissociation energy and bond enthalpy; effect of temperature (Kirchhoff’s
equations) on enthalpy of reactions.
UNIT – III: Second Law (15 Hours)
Concept of entropy; statement of the second law of thermodynamics, Carnot cycle.
Calculation of entropy change for reversible and irreversible processes (for ideal
gases). Free Energy Functions: Gibbs and Helmholtz energy; variation of S, G, A with T,
V, P; Free energy change and spontaneity (for ideal gases). Relation between Joule-
Thomson coefficient and other thermodynamic parameters; inversion temperature;
Gibbs-Helmholtz equation; Maxwell relations; thermodynamic equation of state.
UNIT – IV Third Law (03 Hours)
Statement of third law, unattainability of absolute zero, calculation of absolute
entropy of molecules, concept of residual entropy, calculation of absolute entropy of
solid, liquid and gases.
UNIT – V Systems of Variable Composition (06 Hours)
Partial molar quantities, dependence of thermodynamic parameters on composition;
Gibbs Duhem equation, chemical potential of ideal mixtures, Change in
thermodynamic functions on mixing of ideal gases.

Practical – 30 Hours
Thermochemistry:
(a) Determination of heat capacity of a calorimeter for different volumes using
change of enthalpy data of a known system (method of back calculation of heat
capacity of calorimeter from known enthalpy of solution of sulphuric acid or
enthalpy of neutralization).
(b) Determination of heat capacity of a calorimeter for different volumes using
heat gained equal to heat lost by cold water and hot water.
(c) Determination of enthalpy of neutralization of hydrochloric acid with sodium
hydroxide.

103
 (d) Determination of the enthalpy of ionization of ethanoic acid.
(e) Determination of integral enthalpy solution of endothermic salts.
(f) Determination of integral enthalpy solution of exothermic salts.
(g) Determination of basicity of a diprotic acid by the thermochemical method in
terms of the changes of temperatures observed in the graph of temperature
versus time for different additions of a base. Also calculate the enthalpy of
neutralization of the first step.
(h) Determination of enthalpy of hydration of salt.
(i) Study of the solubility of benzoic acid in water and determination of ΔH.
Any other experiment carried out in the class.
Essential/recommended readings
Theory
1. Peter, A.; Paula, J. de. (2011), Physical Chemistry, 9th Edition, Oxford University
Press.
2. Castellan, G. W. (2004), Physical Chemistry, 4th Edition, Narosa.
3. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, Vol 2, 6th Edition,
McGraw Hill Education.
4. Kapoor, K.L., A Textbook of Physical Chemistry, Vol 3, 5th Edition, McGraw Hill
Education.
5. McQuarrie, D. A.; Simon, J. D. (2004), Molecular Thermodynamics, Viva Books
Pvt. Ltd.
Practical:
1. Khosla, B.D.; Garg, V.C.; Gulati, A. (2015), Senior Practical Physical Chemistry,
R. Chand & Co, New Delhi.
2. Kapoor, K.L. (2019), A Textbook of Physical Chemistry, Vol.7, 1st Edition,
McGraw Hill Education.
3. Garland, C. W.; Nibler, J. W.; Shoemaker, D. P. (2003), Experiments in Physical
Chemistry, 8th Edition, McGraw-Hill, New York.

Suggestive readings
1. Levine, I.N. (2010), Physical Chemistry, Tata Mc Graw Hill.
2. Assael, M. J.; Goodwin, A. R. H.; Stamatoudis, M.; Wakeham, W. A.; Will, S.
(2011), Commonly asked Questions in Thermodynamics. CRC Press.

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

104
 Category II
BSc. Life Science with Chemistry as one of the Core Discipline

DISCIPLINE SPECIFIC CORE COURSE – 4:

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice (if any)
4 2 0 2 Class XII ----
Chemical Pass
Bonding and
Elements in
Biological
System
CHEM-DSC-
02

Learning Objectives

The Learning Objectives of this course are as follows:

• Students gain basic knowledge of chemical bonding in compounds which is a
necessary pre-requisite in understanding the general properties of the compound.
• Unit 2 reviews the importance of inorganic chemical species, especially metals in
biological systems, their classification and detailed discussion of toxic metals.
• The discussions also provide them the details of sodium-potassium pump, role of
some metal ions such as calcium, magnesium and the role of iron in transport and
storage system

Learning outcomes

By the end of the course, the students will be able to:

• Understand the concept of lattice energy using Born-Landé and Born Haber Cycle and
their applications
• Rationalize the conductivity of metals, semiconductors and insulators based on the
Band theory.
• Understand the importance and application of chemical bonds, inter-molecular and
intramolecular weak chemical forces and their effect on melting points, boiling points,
solubility and energetics of dissolution.
• Know about the essential, non-essential, trace and toxic metal ions and their role in
biological system and effects of their deficiency. They will also learn their dose response
relationship curves.
• Understand active and Passive transport and diagrammatically explain the working of

105
 the sodium-potassium pump in organisms and the factors affecting it
• Explain the sources and consequences of excess and deficiency of trace metals and
learn about the toxicity of certain metal ions, the reasons for toxicity
• Storage and transport of iron in bio-systems

SYLLABUS OF DSC-4

Unit I: Chemical Bonding (18 Hours)

Ionic Bonding: General characteristics of ionic bonding, Lattice Enthalpy and Solvation
Enthalpy and their relation to stability and solubility of ionic compounds, Born-Lande
equation for calculation of Lattice Enthalpy (no derivation), Born-Haber cycle and its
applications, polarizing power and polarizability, Fajan's rules, ionic character in covalent
compounds, bond moment, dipole moment and percentage ionic character.
Covalent Bonding: Valence Bond Approach, Hybridization and VSEPR Theory with suitable
examples, Concept of resonance and resonating structures in various inorganic and organic
compounds, Molecular Orbital Approach: Rules for the LCAO method, bonding, nonbonding
and antibonding MOs and their characteristics for s-s, s-p and p-p combinations of atomic
orbitals, MO treatment of homonuclear diatomic molecules of 1st and 2nd periods (including
idea of s-p mixing) and heteronuclear diatomic molecules such as CO, NO and NO+.
Brief introduction to Metallic Bonding, Hydrogen Bonding, van der Waals forces

Unit II: Elements in Biological System (12 Hours)

Classification of elements in biological system, Geochemical effect on the distribution of
metals, Metal ions present in biological systems with special reference to Na+, K+, Ca2+, Mg2+,
Fe2+, Cu2+ and Zn2+, Sodium / K-pump, Role of Ca2+ (blood clotting and structural), Role of Mg2+
in chlorophyll and energy production, Excess and deficiency of some trace metals, Toxicity of
metal ions (Hg, Pb, Cd and As), reasons for toxicity, Dose response relationship curves of metal
ions, Iron and its application in bio-systems, Storage and transport of iron.

PRACTICALS: 60 Hours
1. Preparation of standard solutions.
2. Estimation of Sodium carbonate using HCl by acid base titration.
3. Estimation of carbonate and hydroxide present together in a mixture.
4. Estimation of carbonate and bicarbonate present together in a mixture.
5. Estimation of free alkali present in different soaps/detergents
6. Estimation of oxalic acid using KMnO4 by redox titration.
7. Estimation of Mohr’s salt using KMnO4 by redox titration.
8. Determination of dissolved oxygen in water.
9. Estimation of Fe (II) ions by titrating it with K2Cr2O7 using internal and external
indicators.
10. Estimation of Cu (II) ions iodometrically using Na2S2O3
11. Paper Chromatographic separation of mixture of metal ions

106
 a. Cu2+, Cd2+
b. Ni2+, Co2+.

12. Any suitable experiment (other than the listed ones) based upon
neutralisation/redox reactions.

References:
Theory:
1. Lee, J.D.; (2010), Concise Inorganic Chemistry, Wiley India.
2. Huheey, J.E.; Keiter, E.A.; Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry-
Principles of Structure and Reactivity, Pearson Education.
3. Douglas, B.E.; McDaniel, D.H.; Alexander, J.J. (1994), Concepts and Models of
Inorganic Chemistry, John Wiley & Sons.
4. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010), Shriver
and Atkins Inorganic Chemistry, 5th Edition, Oxford University Press.
5. Crichton, R.; (2019), Biological inorganic chemistry: a new introduction to
molecular structure and function, third edition, Elsevier, Academic Press.
6. Kaim, W; Schwederski, B.; Klein, A. (2013), Bioinorganic Chemistry - Inorganic
Elements in the Chemistry of Life: An Introduction and Guide, 2nd Edition, Wiley.

Practical:

1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of
Quantitative Chemical Analysis, John Wiley and Sons.

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

107
 Category II
BSc. Physical Science with Chemistry as one of the Core Disciplines

DISCIPLINE SPECIFIC CORE COURSE – 4:

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title Credits Credit distribution of the Eligibility Pre-

& Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
4 2 0 2 Class 12th ----
Periodic Pass
Properties
and Chemical
Bonding DSC-
4
Chemistry-II

Learning Objectives

The Learning Objectives of this course are as follows:

• The course discusses the periodicity in properties with reference to the s, p and d block,
which is necessary in understanding their group chemistry.
• It provides basic knowledge about ionic, covalent and metallic bonding underlining the fact
that chemical bonding is best regarded as a continuum between the three cases.
• It provides an overview of hydrogen bonding and van derWaal’s forces which influence the
melting points, boiling points, solubility and energetics of dissolution of compounds

Learning outcomes

By the end of the course, the students will be able to:

• Understand periodicity in ionization enthalpy, electron gain enthalpy,
electronegativity and enthalpy of atomization.
• Understand variability in oxidation state, colour, metallic character, magnetic and
catalytic properties and ability to form complexes
• Understand the concept of lattice energy using Born-Landé expression.
• Draw Born Haber Cycle and analyse reaction energies.
• Draw the plausible structures and geometries of molecules using VSEPR theory.
• Understand and draw MO diagrams (homo- & hetero-nuclear diatomic molecules).
Understand the importance and applications of hydrogen and van der Wall bonding

108
SYLLABUS OF DSC-4

Unit I: Periodic Properties (12 Hours)

Electronic configurations of the atoms. Stability of half-filled and completely filled orbitals,
concept of exchange energy, inert pair effect.
General group trends of s, p and d block elements with special reference to Ionization Enthalpy,
Electron Gain Enthalpy, Electronegativity, Enthalpy of Atomization, oxidation state, colour,
metallic character, magnetic and catalytic properties, ability to form complexes
UNIT II: Chemical Bonding (18 Hours)
Ionic Bonding: General characteristics of ionic bonding, Lattice Enthalpy and Solvation
Enthalpy and their relation to stability and solubility of ionic compounds, Born-Lande equation
for calculation of Lattice Enthalpy (no derivation), Born-Haber cycle and its applications,
polarizing power and polarizability, Fajan's rules, ionic character in covalent compounds, bond
moment, dipole moment and percentage ionic character.
Covalent Bonding: Valence Bond Approach, Hybridization and VSEPR Theory with suitable
examples, Concept of resonance and resonating structures in various inorganic and organic
compounds, Molecular Orbital Approach: Rules for the LCAO method, bonding, nonbonding
and antibonding MOs and their characteristics for s-s, s-p and p-p combinations of atomic
orbitals, MO treatment of homonuclear diatomic molecules of 1st and 2nd periods (including
idea of s-p mixing) and heteronuclear diatomic molecules such as CO, NO and NO+.
Brief introduction to Metallic Bonding, Hydrogen Bonding, van der Waal’s Forces

PRACTICALS: 60 Hours
1. Preparation of standard solutions.
2. Estimation of Sodium carbonate with HCl
3. Estimation of oxalic acid by titrating it with KMnO4.
4. Estimation of Mohr’s salt by titrating it with KMnO4.
5. Estimation of water of crystallization in Mohr’s salt by titrating with KMnO4.
6. Estimation of Fe (II) ions by titrating it with K2Cr2O7 using internal and external indicators.
7. Estimation of Cu (II) ions iodometrically using Na2S2O3.
8. Chromatographic separation of mixture of metal ions Cu2+, Cd2+ or Ni2+, Co2+.
9. Estimation of Fe (II) ions by titrating it with K2Cr2O7 using
a). internal indicator
b). external indicator
10. Estimation of Cu (II) ions iodometrically using Na2S2O3 .
11. Paper Chromatographic separation of mixture of metal ions
a). Cu 2+ , Cd 2+
b). Ni 2+ , Co 2+
12. Any suitable experiment (other than the listed ones) based upon neutralisation/redox
reactions.

References:
Theory:

109
 1. Huheey, J.E.; Keiter, E.A., Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry-
Principles of Structure and Reactivity, Pearson Education
2. Shriver, D.D.; Atkins, P.; Langford, C.H. (1994), Inorganic Chemistry 2nd Ed.,
Oxford University Press.
3. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010),
Inorganic Chemistry, 5th Edition, W. H. Freeman and Company.
4. Lee, J.D.; (2010), Concise Inorganic Chemistry, Wiley India
5. Douglas, B.E.; McDaniel, D.H.; Alexander, J.J. (1994),Concepts and Models of
Inorganic Chemistry, John Wiley & Sons.
6. Wulfsberg, G (2002), Inorganic Chemistry, Viva Books Private Limited.
7. Miessler, G.L.; Fischer P.J.; Tarr, D. A. (2014), Inorganic Chemistry, 5th Edition,
Pearson.

Practical:
• Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of
Quantitative Chemical Analysis, John Wiley and Sons.

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

110
 COMMON POOL OF GENERIC ELECTIVES
OFFERED BY DEPARTMENT OF CHEMISTRY

GENERIC ELECTIVES -12: Coordination and Organometallic Compounds

Credit distribution, Eligibility and Pre-requisites of the Course

Course title & Credits Credit distribution of the Eligibility Pre-
Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice
Coordination and 4 2 0 2 Class XII ---
Organometallic Pass
Compounds
(GE-2)

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce students to some important d-block metals and their compounds which they
are likely to come across.
• To make students learn about organometallic compounds, a frontier area of chemistry
providing an interface between organic and inorganic chemistry.
• To familiarize students with coordination compounds which find manifold applications
in diverse fields.

Learning outcomes

By the end of the course, the students will be able to:

● Familiarize with different types of organometallic compounds, their structures and

bonding involved.
● Understand the nature of Zeise’s salt and compare its synergic effect with that of
carbonyls.
● Identify important structural features of tetrameric methyl lithium and understand
the concept of multicenter bonding in these compounds
● Apply 18-electron rule to rationalize the stability of metal carbonyls and related
species
● Use IR data to explain the extent of back bonding in carbonyl complexes
● Understand the terms, ligand, denticity of ligands, chelate, coordination number and
use standard rules to name coordination compounds
● Use Valence Bond Theory to predict the structure and magnetic behaviour of metal
complexes and understand the terms inner and outer orbital complexes
● Understand the properties of coordination compounds and VBT and CFT for bonding
in coordination compounds

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 ● Explain the meaning of the terms ∆o, ∆t, pairing energy, CFSE, high spin and low spin
and how
● CFSE affects thermodynamic properties like lattice enthalpy and hydration enthalpy

Theory:
Unit 1: Coordination Chemistry 4 Hours

Brief discussion with examples of types of ligands, denticity and concept of chelate. IUPAC
system of nomenclature of coordination compounds (mononuclear and binuclear) involving
simple monodentate and bidentate ligands.

Unit 2:Bonding in coordination compounds 14 Hours

Valence Bond Theory (VBT): Salient features of theory, concept of inner and outer orbital
complexes of Cr, Fe, Co and Ni. Drawbacks of VBT.

Crystal Field Theory: Splitting of d orbitals in octahedral symmetry. Crystal field effects for
weak and strong fields. Crystal field stabilization energy (CFSE), concept of pairing energy.
Factors affecting the magnitude of ∆o.

Spectrochemical series. Splitting of d orbitals in tetrahedral symmetry. Comparison of CFSE

for octahedral and tetrahedral fields, tetragonal distortion of octahedral geometry. Jahn-
Teller distortion, square planar coordination.

Unit 3: Organometallic Compounds 12 Hours

Definition and classification with appropriate examples based on nature of metal-carbon

bond (ionic, s, p and multicentre bonds). Structure and bonding of methyl lithium and Zeise’s
salt. Structure and physical properties of ferrocene. 18-electron rule as applied to carbonyls.
Preparation, structure, bonding and properties of mononuclear and polynuclear carbonyls of
3d metals. π-acceptor behaviour of carbon monoxide (MO diagram of CO to be discussed),
synergic effect and use of IR data to explain extent of back bonding.

Practicals: 60 Hours

1. Gravimetry

Discuss basic principles of gravimetry (precipitation, co-precipitation and post precipitation,

digestion, washing etc)

(i) Estimation of Ni(II) using dimethylglyoxime (DMG).

(ii) Estimation of copper as CuSCN.
(iii) Estimation of Al(III) by precipitating with oxine and weighing as Al(oxine)3 (aluminium
oxinate).

2. Inorganic Preparations

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(i) Schiff’s base involving ethylenediamine and salicylaldehyde (or any other amine and
aldehyde/ketone) and to check its purity using TLC.
(ii) Nickel/ Copper complex of the above prepared Schiff’s base and its characterisation
using UV/Vis spectrophotometer. The IR spectra also to be interpreted
(iii) tetraamminecopper (II) sulphate
(iv) potassium trioxalatoferrate (III) trihydrate.
(v) tetraamminecarbonatocobalt(III) nitrate

References:
Theory:

1. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010), Shriver
and Atkins Inorganic Chemistry, W. H. Freeman and Company.
2. Miessler, G. L.; Fischer P.J.; Tarr, D.A. (2014), Inorganic Chemistry, Pearson.
3. Huheey, J.E.; Keiter, E.A., Keiter; R.L., Medhi, O.K. (2009), Inorganic Chemistry-
Principles of Structure and Reactivity, Pearson Education.
4. Pfennig, B. W. (2015), Principles of Inorganic Chemistry. John Wiley & Sons.
5. Cotton, F.A.; Wilkinson, G. (1999), Advanced Inorganic Chemistry Wiley-VCH.

Practicals:

1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of
Quantitative Chemical Analysis, John Wiley and Sons.
2. Schiff Base Complex of Cu (II) with Antibacterial and Electrochemical Study, Arjun C.
Bhowmick, Majharul I. Moim, Miththira Balasingam , American Journal of Chemistry
2020, 10(2): 33-37, DOI: 10.5923/j.chemistry.20201002.03

Keywords: Organometallic compounds, metal carbonyls, synergistic effect, Coordination

compounds, VBT, Crystal field theory, Splitting of d levels, Dq

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

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 GENERIC ELECTIVES -13: – CHEMISTRY OF OXYGEN CONTAINING
FUNCTIONAL GROUPS AND THEIR APPLICATIONS TO BIOLOGY

Credit distribution, Eligibility and Pre-requisites of the Course

Course title & Credits Credit distribution of the course Eligibility Pre-requisite
Code Lecture Tutorial Practical/ criteria of the course
Practice
Chemistry of 4 2 0 2 Class XII ----
Oxygen containing Pass
Functional Groups
and their
Applications to
Biology
(GE-5)

Learning Objectives
• To teach the fundamental chemistry of oxygen containing functional groups.
• To establish these concepts typical reactions of alcohols, phenols, aldehydes, ketones,
carboxylic acids and their derivatives.
• To make students understand the relevance of oxygen containing functional groups to
biology and the importance of these compounds in real world.

Learning outcomes

By the end of the course, the students will be able to:

• Understand and explain the differential behavior of organic compounds based on

reaction chemistry.
• Formulate the mechanism of organic reactions by recalling and correlating the
fundamental properties of the reactants involved.
• Understand the applications of functional group chemistry to biology.

Syllabus - Theory:

Unit 1: Alcohols (upto 5 Carbon) 5 Hours

Structure and classification of alcohols as 1⁰, 2⁰ & 3⁰, Reactions: Acidic character of alcohols
and reaction with sodium, with HX (Lucas Test), esterification, oxidation (with PCC, alkaline
KMnO4, acidic K2Cr2O7 and conc. HNO3), Oppeneauer Oxidation, Biological oxidation
Reactions

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Unit 2: Phenols 4 Hours

Acidity of phenols and factors affecting their acidity, Reactions: Electrophilic substitution
reactions, viz. nitration, halogenation, sulphonation, Reimer-Tiemann reaction, Gattermann–
Koch reaction, Houben-Hoesch condensation; Reaction due to OH group: Schotten-Baumann
reaction

Unit 3: Aldehydes and Ketones (Aliphatic and Aromatic) 12 Hours

Reactions: Nucleophilic addition, nucleophilic addition-elimination reaction including

reaction with HCN, ROH, NaHSO3, NH2-G derivatives. Iodoform test, Aldol condensation and
its biological application, Cannizzaro’s reaction, Wittig reaction, Benzoin condensation,
Clemmensen reduction, Wolff Kishner reduction, Meerwein-Pondorff Verley reduction,
enzyme-catalyzed additions to α,β-unsaturated carbonyl compounds.

Unit 4: Carboxylic acids and their derivatives (Aliphatic and Aromatic) 9 Hours

Reactions: Hell-Volhard Zelinsky reaction, acidity of carboxylic acids, effect of substitution on

acid strength, Claisen condensation and its biological applications, decarboxylation in
biological systems, relative reactivities of acid derivatives towards nucleophiles, activation of
carboxylate ions for nucleophilic acyl substitution reactions in biological systems,
Reformatsky reaction, Perkin condensation.

Practicals: : 60 Hours

Preparations: (Mechanism of various reactions involved to be discussed) (Recrystallization,

determination of melting point and calculation of quantitative yields to be done in all cases)

1. Oxime of aldehydes and ketones

2. 2,4-Dinitrophenylhydrazone of aldehydes and ketones

3. Aldol condensation using green method.

4. Benzoin condensation using Thiamine Hydrochloride as a catalyst.

5. Alkaline hydrolysis of amide/ester.

6. Benzoylation of one of the following amines (aniline, o-, m-, p-toluidines and o-, m-, p-
anisidine) or one of the following phenols (β-naphthol, resorcinol, p-cresol) by Schotten-
Baumann reaction.

7. Identification of functional group for monofunctional organic compounds (Alcohols,

phenols, aldehydes, ketones, carboxylic acids).

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References:
Theory:

1. Sykes, P. (2005), A Guide Book to Mechanism in Organic Chemistry, Orient Longman.

2. Eliel, E. L. (2000), Stereochemistry of Carbon Compounds, Tata McGraw Hill.
3. Morrison, R. N.; Boyd, R. N., Bhattacharjee, S.K. (2010), Organic Chemistry, 7th
Edition, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).
4. Mehta B.; Mehta M. (2015), Organic Chemistry, PHI Learning Private Limited Bahl,
5. Bahl, A., Bahl, B. S. (2012), Advanced Organic Chemistry, S. Chand.
6. Bruice, Paula Y. (2020), Organic Chemistry, 8th Edition, Pearson.

Practicals:
1. Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. (2012), Vogel's Textbook
of Practical Organic Chemistry, Pearson.
2. Mann, F.G.; Saunders, B.C. (2009), Practical Organic Chemistry, Pearson Education.

Keywords: Alcohols, Lucas Test, Phenol, Aldehydes, Ketones, Nucleophilic addition,

nucleophilic addition – elimination, Cannizzaro’s reaction, Wittig reaction, Benzoin
condensation, Enzyme-catalysed reaction, Carboxylic acid, Claisen condensation

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

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 GENERIC ELECTIVES-14: MOLECULES OF LIFE

Credit distribution, Eligibility and Pre-requisites of the Course

Course title & Credits Credit distribution of the course Eligibility Pre-requisite
Code Lecture Tutorial Practical/ criteria of the course
Practice
Molecules of 4 2 0 2 Class XII ----
Life Pass

(GE-6)

Learning Objectives
• To deliver information about the chemistry of carbohydrates, proteins & enzymes and
its relevance in the biological system using suitable examples.
• To place key emphasis on understanding the structural principles that govern
reactivity/physical /biological properties of biomolecules as opposed to learning
structural details.

Learning outcomes

By the end of the course, the students will be able to:

● Learn and demonstrate how the structure of biomolecules determines their chemical
properties, reactivity and biological uses.
● Gain an insight into the mechanism of enzyme action and inhibition.
● Understand the basic principles of drug-receptor interaction and SAR.

Syllabus - Theory:
Unit 1: Carbohydrates 12 Hours
Classification of carbohydrates, reducing and non-reducing sugars, biological functions,
general properties and reactions of glucose and fructose, their open chain structure, epimers,
mutarotation and anomers, reactions of monosaccharides, determination of configuration of
glucose (Fischer proof), cyclic structure of glucose. Haworth projections. Cyclic structure of
fructose. Linkage between monosaccharides: structure of disaccharides (sucrose, maltose,
lactose) and polysaccharides (starch and cellulose) excluding their structure elucidation.

Unit 2: Amino Acids, Peptides and Proteins 10 Hours

Classification of amino acids and biological uses of amino Acids, peptides and proteins.
Zwitterion structure, isoelectric point and correlation to acidity and basicity of amino acids.
Determination of primary structure of peptides, determination of N-terminal amino acid (by

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Edman method) and C– terminal amino acid (with carboxypeptidase enzyme). Synthesis of
simple peptides (up to dipeptides) by N-protection (t-butyloxycarbonyl) & C-activating groups
(only DCC) and Merrifield solid phase synthesis, Overview of primary, secondary, tertiary and
quaternary structure of proteins, denaturation of proteins.

Unit 3: Enzymes and correlation with drug action 08 Hours

Classification of enzymes and their uses (mention Ribozymes). Mechanism of enzyme action,
factors affecting enzyme action, Coenzymes and cofactors and their role in biological
reactions, specificity of enzyme action (including stereospecificity), enzyme inhibitors and
their importance, phenomenon of inhibition (Competitive and non-competitive inhibition
including allosteric inhibition). Drug action-receptor theory. Structure – activity relationships
of drug molecules, binding role of –OH group, -NH2 group, double bond and aromatic ring.

Practicals: (60 Hours)

1. Estimation of glucose by Fehling’s solution.

2. Determination of total sugar content by ferricyanide method (volumetric/colorimetric
method).
3. Study of the titration curve of glycine.
4. Estimation of proteins by Lowry’s method.
5. Study of the action of salivary amylase on starch under optimum conditions.
6. Qualitative tests for amino acids, proteins and carbohydrates.
7. Separation and identification of mixture of sugars by paper chromatography.

References:
Theory:
1. Finar, I. L. Organic Chemistry (Volume 1 & 2), Dorling Kindersley (India) Pvt. Ltd.
(Pearson Education).
2. Morrison, R. N.; Boyd, R. N., Bhattacharjee, S.K. (2010), Organic Chemistry, 7th
Edition, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).
3. Berg, J. M.; Tymoczko, J. L.; Stryer, L. (2019), Biochemistry, 9th Ed., W. H.
Freeman Co Ltd.

Practicals:
1. Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. (2012), Vogel's Textbook
of Practical Organic Chemistry, Pearson.
2. Manual of Biochemistry Workshop, 2012, Department of Chemistry, University of
Delhi.

Teaching Learning Process:

● Chalk and black board method. Along with pedagogy of flipped classroom

135
 ● Certain topics like mechanism of enzyme action and enzyme inhibition can be taught
through audio-visual aids.
● Students should be encouraged to participate actively in the classroom through
regular presentations on curriculum-based topics, peer assessment, designing games
based on specific topics etc.
● As the best way to learn something is to do it yourself, practicals are planned in such
a way so as to reinforce the topics covered in theory.

Assessment Methods:
● Graded assignments
● Class tests and Quizzes
● Class seminars by students on course topics with a view to strengthening the content
through width and depth
● Continuous evaluation for the practicals
● End semester university theory and practical examination.

Keywords: Carbohydrates, point, Amino acids, Enzymes, SAR, Drug Receptor Theory

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

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 GENERIC ELECTIVES -15 : CHEMICAL KINETICS AND PHOTOCHEMISTRY

Credit distribution, Eligibility and Pre-requisites of the Course

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice
Chemical 4 2 0 2 Class XII -----
Kinetics and Pass
Photochemistry
(GE-8)

Learning Objectives
• To make students learn about the fundamentals of chemical kinetics, rates of chemical
reactions, complex reactions, theories of reaction rate and the laws of photochemistry
aimed at understanding electronic transitions upon irradiation of electromagnetic
radiation in UV-Vis region.

Learning outcomes

By the end of the course, the students will be able to:

• Understand the concept of rate of a reaction, order and molecularity of a reaction,

various factors affecting the rate and theories of reaction rates.
• Students will be able to apply the learnt concepts in studying the reaction kinetics of
various reactions.
• Understand the basic concepts of photochemistry, photochemical and
photosensitized reactions and their role in biochemical systems.

Syllabus - Theory:
Unit 1: Chemical Kinetics 20 Hours
The concept of reaction rates, effect of temperature, pressure, catalyst and other factors on
reaction rates. Order and molecularity of a reaction, derivation of integrated rate equations
for zero, first and second order reactions (both for equal and unequal concentrations of
reactants), half–life of a reaction, general methods for determination of order of a reaction.
kinetics of complex reactions (integrated rate expressions up to first order only): (i) Opposing
reactions (ii) parallel reactions and (iii) consecutive reactions and their differential rate

137
equations (steady-state approximation in reaction mechanisms). Concept of activation
energy and its calculation from Arrhenius equation. Theories of reaction rates: Collision
theory and activated complex theory of bi-molecular reactions. Comparison of the two
theories (qualitative treatment only)

Unit 2: Photochemistry 10 Hours

Characteristics of electromagnetic radiation, Jablonski Diagram. Lambert-Beer’s law and its
limitations, physical significance of absorption coefficients. Laws of photochemistry, quantum
yield, actinometry, examples of low and high quantum yields, photochemical equilibrium and
the differential rate of photochemical reactions, photosensitized reactions, quenching. Role
of photochemical reactions in biochemical processes.

Practicals: (60 Hours)

Chemical Kinetics
Study the kinetics of the following reactions by integrated rate method:
a) Acid hydrolysis of methyl acetate with hydrochloric acid.
b) Compare the strength of HCl and H2SO4 by studying the kinetics of hydrolysis methyl
acetate.
c) Initial rate method: Iodide-persulphate reaction
d) Integrated rate method: Saponification of ethyl acetate.
e) Study the reaction kinetics of Iodination of acetone.

References:
Theory:
1. Castellan, G.W. (2004), Physical Chemistry, Narosa.
2. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, Vol 5, 6th Edition, McGraw Hill
Education.
3. Kapoor, K.L. (2013), A Textbook of Physical Chemistry, Vol 6, 3rd Edition, McGraw Hill
Education.

Practicals:
1. Khosla, B.D.; Garg, V.C.;Gulati, A.(2015), Senior Practical Physical Chemistry, R. Chand &
Co.

Teaching Learning Process:

• Teaching Learning Process for the course is visualized as largely student-focused
• Transaction through an intelligent mix of conventional and modern methods
• Engaging students in cooperative learning.
• Learning through quiz design.
• Problem solving to enhance comprehension.

Assessment Methods: Assessment will be done on the basis of regular class test, presentations
and assignments as a part of internal assessment during the course as per the curriculum. End
semester university examination will be held for both theory and practical. In practical,

138
assessment will be done based on continuous evaluation, performance in the experiment on the
date of examination and viva voce.
Keywords: Rate Law, Rate constant. Arrhenius Equation, Lambert-Beer’s law, Jablonski
Diagram

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

139
 GENERIC ELECTIVES -16: BASICS OF POLYMER CHEMISTRY

Credit distribution, Eligibility and Pre-requisites of the Course

Course title & Credits Credit distribution of the course Eligibility Pre-
Code Lecture Tutorial Practical/ criteria requisite of
Practice the course
Basics of Polymer 4 2 0 2 Class XII -----
Chemistry Pass

(GE-10)

Learning Objectives
• To help the student to know about the synthesis, properties and applications of
polymers.

Learning outcomes

By the end of the course, the students will be able to:

• Know about classification of polymeric material.
• Learn about different mechanisms of polymerization and polymerization techniques
• Evaluate kinetic chain length of polymers based on their mechanism
• Differentiate between polymers and copolymers
• Learn about different methods of finding out average molecular weight of polymer.
• Differentiate between glass transition temperature (Tg) and crystalline melting point
(Tm)
• Learn properties and applications of various useful polymers in our daily life

Syllabus Theory:

Unit 1: Introduction to polymers 10 Hours

Different schemes of classification of polymers, Polymer nomenclature, configuration and
conformation of polymers, Molecular forces and chemical bonding in polymers, Texture of
Polymers
Functionality and its importance:
Criteria for synthetic polymer formation, basic methods of polymerization processes and their
mechanism: addition, condensation, Relationships between functionality, extent of reaction
and degree of polymerization.

140
Unit 2: Properties of Polymers 10 Hours
Glass transition temperature (Tg) and determination of Tg, Free volume theory, WLF
equation, Factors affecting glass transition temperature (Tg).
Crystallization and crystallinity: Determination of crystalline melting point and degree of
crystallinity,
Morphology of crystalline polymers, Factors affecting crystalline melting point.
Molecular weight distribution and determination of molecular weight of polymers (Mn, Mw,
etc.) by end group analysis, viscometry and osmotic pressure methods. Molecular weight
distribution and its significance.

Unit 3: Preparation, properties and applications 10 Hours

Brief introduction to preparation, structure, properties and application of the following
polymers: polyolefins, polystyrene and styrene copolymers, poly(vinyl chloride), poly(vinyl
acetate), acrylic polymers, fluoro polymers, polyamides and related polymers. Phenol
formaldehyde resins (Bakelite, Novolac), polyurethanes, silicone polymers, polydienes,
Polycarbonates, Conducting Polymers: polyacetylene, polyaniline, poly(p-phenylene
sulphide, polypyrrole, polythiophene

Practicals: (60 Hours)

Polymer Synthesis

1. Free radical solution polymerization of styrene (St) / Methyl Methacrylate

(MMA)/MethylAcrylate (MA).
2. Preparation of nylon 6,6
3. Redox polymerization of acrylamide
4. Precipitation polymerization of acrylonitrile
5. Preparation of urea-formaldehyde resin
6. Preparations of novalac resin/resole resin.
7. Microscale Emulsion Polymerization of Poly(methylacrylate).

Polymer characterization

1. Determination of molecular weight of polyvinyl propylidene in water by viscometry.

2. Determination of the viscosity-average molecular weight of poly(vinyl alcohol) (PVOH)
and the fraction of head-to-head monomer linkages in the polymer.
3. Determination of molecular weight by end group analysis of polymethacrylic acid.

Polymer analysis

1. Estimation of the amount of HCHO in the given solution by sodium sulphite method.
2. Determine the melting point of crystalline polymer.
3. Measurement of glass transition temperature, Tg.s

141
References:
Theory:
1. Carraher,C. E. Jr. (2013), Seymour’s Polymer Chemistry, Marcel Dekker, Inc.
2. Odian, G. (2004), Principles of Polymerization, John Wiley.
3. Billmeyer, F.W. (1984), Text Book of Polymer Science, John Wiley.
4. Ghosh, P. (2001), Polymer Science & Technology, Tata Mcgraw-Hill.
5. Lenz, R.W. (1967), Organic Chemistry of Synthetic High Polymers, Intersecience
(Wiley).

Practical:
1. Allcock, H.R.; Lampe, F. W.; Mark, J. E. (2003), Contemporary Polymer Chemistry,
Prentice-Hall.
2. Fried, J.R. (2003), Polymer Science and Technology, Prentice-Hall.
3. Munk, P.; Aminabhavi, T. M. (2002), Introduction to Macromolecular Science, John
Wiley & Sons.
4. Sperling, L.H. (2005), Introduction to Physical Polymer Science, John Wiley & Sons.

Teaching Learning Process:

• Student centred teaching Learning process.
• Blend of conventional blackboard teaching and modern teaching learning tools
• Focus on real life applications of concepts
• Problem solving and quizzes for enhanced understanding of the concepts
• Engaging students in collaborative learning.
• Pre-lab learning of theoretical concept of the experiment.
• Performing the experiment, recording the data, calculating the result.
• Interpreting the result.
• Comparing the results of the class.
• Discussing the sources of error.

Assessment Methods:
• Class Tests at Periodic Intervals.
• Written assignment(s)
• Continuous evaluation of laboratory work and record file.
• Oral assessment, quizzes.
• Mock practical examination.
• Semester end University examination.

Keywords: Bonding, Texture, Polymerization, Crystallization, Properties, Applications.

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

142
 GENERIC ELECTIVES 17: CHEMISTRY: MOLECULAR MODELLING,
ARTIFICIAL INTELLIGENCE AND MACHINE LEARNING

Credit distribution, Eligibility and Pre-requisites of the Course

Course title & Code Credits Credit distribution of the course Eligibility Pre-
Lecture Tutorial Practical/ criteria requisite
Practice of the
course
Chemistry: Molecular 4 2 0 2 Class XII ----
Modelling, Artificial Pass
Intelligence and
Machine Learning
(GE-14)

Learning Objectives
• To make students familiar with modern scientific machine (programming) language
i.e., Python, Artificial Intelligence (AI) & Machine Learning (ML) and their potential
applications in chemistry.
• To provide elementary ideas of the techniques prevailing in the field of AI and ML and
their applications to research problems especially related to research and
development of new materials and pharmaceutical compounds with desired
properties.

Learning outcomes

By the end of the course, the students will be:

• Conversant with the Python Programming Language.
• Familiar with Elementary techniques of AI and ML
• Able to apply techniques of AI & ML in basic problems of research in some important
areas of research in Chemistry.

Syllabus Theory:
Part A: Molecular Modelling

Introduction to computational chemistry: 7 Hours

Overview of Computational Methods in Chemistry (Ab initio, DFT, Semi- empirical, Molecular
Mechanics

Potential Energy Surfaces 4 Hours

The concept of Potential energy surface, Intrinsic Reaction Coordinates, Stationary points,

143
Equilibrium points – Local and Global minima, Geometry optimization and energy
minimization.

Molecular Mechanics 4 Hours

Force Fields (A brief idea of a basic force field), Elementary idea of MM1, MM2, MM3, MM4,
MM+, AMBER etc. A brief Idea of Molecular Docking

Part B: Artificial Intelligence & Machine learning in Chemistry 15 Hours

An overview of computationally readable and processible representation of molecules, e.g.,
SMILES, mol files. Chemical space and access to chemical databases. Statistical treatment of
data: regression analysis andtypes of regression. Elementary Idea of Quantitative structure-
activity relationship (QSAR).

An insight into Artificial Intelligence & Machine learning and potentialareas of applications in
chemistry. Dimensional reduction; Principal Component Analysis (PCA) and the importance
and necessity of nonlinearity in Artificial Intelligence.

Genetic algorithm, basics of random mutation hill climbing (RMHC) and simulated annealing.

Practicals: (60 hours)

Molecular Modeling based Exercise
1) Write the Z-Matrix of a given set of molecules.

2) Carry out geometry optimisation on H2O, H2S, H2Se molecules and compare the
optimized bond angles and dipole moments from the results obtained. Obtain the
ESP-mapped density surfaces and interpret the results obtained with reference to
bonding in these molecules.
Suggestive: A comparative analysis of results of the above exercise may be carried out using
different quantum mechanicalmethods.
3) Calculate the energy of the following chemical species andarrange them in order
of increasing stability.
1-hexene, 2-methyl-2-pentene, (E)-3-methyl-2-pentene, (Z)-3- methyl-2-pentene, and 2,3-
dimethyl-2-butene in order of increasing stability.
4) Carry out the geometry optimisation on the following chemical species and compare
the shapes and dipole moments of the molecules.
1-butanol, 2-butanol, 2-methyl-1-propanol, and 2-methyl-2- propanol.
Correlate the computationally obtained values of the dipolemoments with the experimental
values of the boiling points: (118ºC, 100 ºC, 108 ºC, 82 ºC, of 1-butanol, 2-butanol, 2-
methyl-1- propanol, and 2-methyl-2- propanol respectively).
5) Based on the implicit electronic structure calculations, determine the heat of
hydrogenation of Ethene.
6) Based on the calculations of enthalpies of the participating chemical species on

144
 optimized geometry of the molecules, calculate the reaction enthalpy at 298 K for the
following,industrially important reactions:
𝐶𝐶𝐶𝐶4 + 𝐻𝐻2𝑂𝑂 → 𝐶𝐶𝐶𝐶 + 3𝐻𝐻2 (steam reforming of methane)

𝑁𝑁2 + 3 𝐻𝐻2 → 2𝑁𝑁𝑁𝑁3 (Haber-Bosch process)

7) Carry out geometry optimisation and determine the energy of the participating
chemical species in the following reactions Using these results calculate the resonance
energy of thiophene.
8) Carry out geometry optimization & energy calculations on the following species and
obtain Frontier Molecular Orbitals. Visualize the Molecular Orbitals of these species
and interpret the results for bonding in these molecules.
Benzene, Naphthalene, and Anthracene.
9) Compare the gas phase basicities of the methylamines by comparing the enthalpies
of the following reactions:
10) On the basis of results of geometry optimization and energy calculations, determine
the enthalpy of isomerization of cis andtrans 2-butene.
11) QSAR based exercise on problems of interest to chemist.
12) Perform a conformational analysis of butane. Plot the graph between the angle of
rotation and the energy of the conformers using spreadsheet software.
13) Compute the resonance energy of benzene by comparison of its enthalpy of
hydrogenation with that of cyclohexene.
14) Perform a geometry optimization followed by a frequency assessment (opt+freq
keyword) using the B3LYP method and 6- 31-G(d) basis set on a given set of small
molecules i.e. BH3, CH4.
Suggestive: A greater number of molecules may be studied as per instructions received from
the concerned teacher.
15) Based on the fundamentals of conceptual DFT calculate the ionization potential (IP),
electron affinity (EA), electronegativity and electron chemical potential of a given set
of molecules.
16) Perform molecular docking of Sulfonamide-type D-Glu inhibitor into MurD active site
using Argus lab.

Artificial Intelligence (AI) and Machine Learning (ML) based exercise on problems of
interest to chemist

17. Travelling salesman problem and electrical circuit design (minimization of path-
length).
18. Genetic algorithm, in solving matrix form of linear equations
19. Non-linear least-square fitting problem.
20. Particle Swarm Optimization on the sphere function.

Important Instruction Note on working approach:

145
 • A student is required to perform/investigate a minimum of 10 exercises in total.
• The exercises mentioned above will be performed by the student strictly in
accordance with the instructions received and only under the supervision of the
teacher concerned.
• Any other exercise may be carried out with prior permission, input, discussion and
instructions received from the teacher concerned.

References:
1. Lewars, E. (2003), Computational Chemistry, Kluwer academicPublisher.
2. Cramer, C.J. (2004), Essentials of Computational Chemistry, John Wiley & Sons.
3. Cartwright C.; Kharma N., (2008), Using artificial intelligence in chemistry and
biology, First Edition, CRC Press Taylor & Francis Group
4. Hippe; Z., Artificial Intelligence in Chemistry: Structure Elucidation and Simulation
of Organic Reactions, (1991) Academic Press, Elsevier
5. Soft Computing in Chemical and Physical Sciences A Shift in Computing Paradigm
(Kanchan Sarkar, Sankar Prasad Bhattacharyya) (z-lib.org)
6. Understanding Properties of Atoms, Molecules and Materials (PRANAB. SARKAR,
Sankar Prasad Bhattacharyya) (z-lib.org)

Web Resources:

1. https://www.afs.enea.it/software/orca/orca_manual_4_2_1.pdf
2. https://dasher.wustl.edu/chem430/software/avogadro/learning-avogadro.pdf
3. http://www.arguslab.com/arguslab.com/ArgusLab.html
4. https://barrett- group.mcgill.ca/tutorials/Gaussian%20tutorial.pdf
5. https://gaussian.com/techsupport/
6. https://gaussian.com/man/
7. https://gaussian.com/wp-content/uploads/dl/gv6.pdf
8. https://dasher.wustl.edu/chem478/software/spartan-manual.pdf
9. http://www.mdtutorials.com/gmx/
10. https://vina.scripps.edu/manual/

Teaching Learning Process: Hands-on laboratory exercises Conventional teaching learning

method. Engaging students in collaborative learning

Keywords: Molecular Modeling, Potential Energy Surface (PES), Geometry Optimization,

Frequency calculation, Artificial Intelligence, Machine Learning, Nural Networks, Genetic
Algorithm.

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

146
 GENERIC ELECTIVES 18: ROLE OF METALS IN MEDICINES
Credit distribution, Eligibility and Pre-requisites of the Course

Course Credits Credit distribution of the course Eligibility Pre-requisite

title & Lecture Tutorial Practical/ criteria of the course
Code Practice
Role of 4 2 0 2 Class XII ----
Metals in Pass
Medicines
(GE-16)

Learning Objectives

• To make the learners familiar about role of metal ions in some commercially available
medicines.

Learning outcomes
By the end of this course student will be able to learn:
• Role of metal ions in various biomolecules and their functions.
• Role of metals in commercially available medicines and their functions

Syllabus Theory:
Unit 1: Bio role of Metals 04 Hours
Brief introduction of following metals in biological system
Fe, Cu, Zn, Mn, Cr(III), V, Mo, W, Co, Ni, Na, K, Mg and Ca
Chemical structure, Commercial name, Name of the disease it is made for and its brief
mechanism of action shall be taught for all the mentioned metals below.

Unit 2: Diagnostic and therapeutic agents 08 Hours

Diagnostic and therapeutic agents with Pt (Cisplatin) and Ga for cancer, Au (auranofin) for
arthritis and V for diabetes.

Unit 3: Metals in drugs 06 Hours

Li2CO3 (Camcolit) for manic-depressive illness, NaHCO3 (Alka-seltzer) for heartburn, Al(OH)3
(Gaviscon) for heartburn, As (melarsoprol) for sleeping sickness, Bi subsalicylate (pepto-
Bismol) for heartburn and diarrhea, Bi subcitrate (De-nol) peptic ulcer, Zinc oxide with Fe2O3
(Calamine lotion) as antimicrobial agent.

147
Unit 4: Metals in Multivitamins 06 Hours
Cyanocobalamin (Co), Ferrous fumerate (Fe), Magnesium oxide (Mg), Zinc Sulfate (Zn),
Manganese sesulphate (Mn), Copper Sulfate (Cu), Sodium selenite (Se) and Chromium
trichloride (Cr).

Unit 5: Radiopharmaceuticals and MRI contrast agents 06 Hours

99mTcfor heart, brain and bone imaging, 123I radiopharmaceuticals, BaSO4for X-ray contrast
agent, Gd (III) for MRI contrast agents.

Practicals: (60 hours)

Volumetric titrations:
1. To estimate the acidity of commercially available antacids.
2. To estimate the concentration of Fe in commercially available medicines.
3. To estimate the concentration of Ca in commercially available medicines.
4. To estimate the strength of carbonate in tablets containing Li2CO3
5. To estimate the sodium bicarbonate in synthetic/commercially available drug.
6. To estimate the zinc and iron present in Calamine lotion.
7. To estimate the Mg present in multivitamins.
References:
1. Metals in Medicine, John Wiley & Sons Ltd, Nov 2009
2. Chapter-9, Metals in Medicine, Stephen J. Lippard
3. Jones, Chris and Thornback, John, Medicinal applications of coordination chemistry,
Cambridge, UK: Royal Society of Chemistry, 2007
Teaching Learning Process:
• Hands-on laboratory exercises
• Conventional teaching learning method. Engaging students in collaborative learning
Assessment Methods:
• Continuous evaluation of laboratory work and record file. Oral assessment, quizzes.
• Presentation on lab practices.
• Semester end examination.
Key words: Diagnostic, therapeutic agents, multivitamins, radiopharmaceuticals and MRI
contrast agents.

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

148
 GENERIC ELECTIVES -19: ENERGY AND THE ENVIRONMENT

Credit distribution, Eligibility and Pre-requisites of the Course

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice
Energy and the 4 3 0 1 Class XII ---
Environment Pass

(GE-17)

Learning Objectives

• To develop basic understanding of energy, issues related to energy, importance of

energy in terms of economy, health and the environment.
• To understand different sources of energies, renewable and non-renewable sources of
energy. To understand the importance of green fuels.
• To make the students understand the adverse effect of pollution, and possible
remediations.

Learning Outcomes
By the end of this course student will be able to learn:
• Describe basic energy concepts
• Account for conventional and renewable energy technologies and their application
• Reflect and evaluate the environmental impact of energy production and the
relationship between energy production, consumption and climate change
• Reflect on energy costs, analyse the consequences of today’s energy consumption
• Efficient use of energy, water and other resources, Use of renewable energy, such as
solar energy
• Pollution and waste reduction measures, and the enabling of re-use and recycling
• Good indoor environmental air quality, Use of materials that are non-toxic, ethical and
sustainable
• Consideration of the environment in design, construction and operation

149
Syllabus Theory:
Unit 1: 13 Hours

Introduction, chemistry and energy, conversion of chemical energy to electrical energy,

Carbon cycle, Greenhouse gases, Global warming and climate change, Carbon footprint, zero-
carbon or low-carbon energy. Electrical energy and steam energy, Energy Alternatives,
Hidden Costs of Energy.

Unit 2: 10 Hours

Production methods for electric power: Non-Renewable (conventional) sources of energy:

Fossil fuels: Coal, petroleum and Natural gas. Energy transformation. Renewable energy
sources: solar, hydropower, wind, geothermal, wave, ocean thermal, tidal, ocean currents,
nuclear energy, biomass.

Unit 3: 12 Hours

Production methods for electric power: Renewable (green) energy, conversion and storage
systems. Nuclear fusion, Hydrogen fuels, photovoltaic solar cells, hydroelectric. Sustainable
energy, biomass, Biofuels, production of biofuels, advantages, blending of biofuels with
conventional fuels, Carbon Capture and Reuse, Waste to Energy Technologies.

Unit 4: 10 Hours

Air Pollution, Urban and Indoor Air Pollution, Pollution and waste reduction measures,
chemical remediation of air pollution. Effect of pollution on health and economy.

Practicals: (30 Hours)

Tutorials

1. Conversion of biomass to biofuels (2-3 different biofuels)

2. Working on solar cell model.
3. Working on wind turbine model.
4. Working on geothermal energy model.
5. Working on hydroelectric plant model.
6. Presentations by students

References:
Theory

1. Rao, C S., Environment pollution control Engineering, New Age International reprint
2015, 2nd edition
2. Bharucha, E., Textbook of Environmental Studies, Universities Press (2005)
3. Wright, R.T., Environmental Science-Towards a sustainable Future, Prentice Hall
(2008) 9th edition.
4. Ahluwalia, V. K., Energy and Environment, The Energy and Resources Institute (TERI)
(2019).

150
References:
Practicals

• Challapalli Narayan Rao, Practical approach to implementation of Renewable Energy

Systems, Evincepub Publishing, 2022

Keywords: Energy, Renewable and non-renewable energy resources, Synthetic fuels,

Biofuels, Carbon footprint, air pollution, remediation, pollution related health and economy.

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

151
 GENERIC ELECTIVES -20 : CHEMISTRY OF FRAGRANCES AND FLAVOURS:
AN INDUSTRY’S PERSPECTIVE

Credit distribution, Eligibility and Pre-requisites of the Course

Course title & Code Credits Credit distribution of the course Eligibility Pre-
Lecture Tutorial Practical/ criteria requisite
Practice of the
course
Chemistry of 4 3 0 1 Class XII ----
Fragrances and Pass
Flavours: An
Industry’s Perspective
(GE-18)

Learning Objectives

• To make the students understand the applications of chemistry in the world of flavours
and fragrances. The use of fragrance is ubiquitous and is a global human phenomenon.
Over the course of time, countless numbers of flavors and fragrances have found their
way into everyday life, notably into foods, beverages and confectionery items; into
personal care products (soaps, toothpastes, mouthwashes, deodorants, bath lotions and
shampoos), perfumes, and other cosmetics as well as pharmaceutical formulations.
Indeed, flavors and aromas are added to make such products more attractive or to mask
the taste or smell of less pleasant ones.

Learning Outcomes
By the end of this course student will be able to learn:

• Synthesis of various fragrance and flavour ingredients

• Formulation methods, how different factors affects the formulation process in
Fragrance and Flavour industry
• Uphold safety regulation and execute quality processes
• Quality control in manufacturing process, legal aspects, classification of odour and
odorants.
• Different methods used for separation, purification and isolation of perfumes and
flavours like distillation, extraction, crystallization, etc.

152
Syllabus Theory:
Unit 1: Fragrances 18 Hours

• Introduction to fragrances, types of fragrances (Fragrance families and classification)

• History of perfumes, Perfumery raw materials, classification of odour, odour type and
odorants
• India in the context of Fragrance Industry
• ABCs of perfumery, odour aspects of perfumes, fragrance pyramid, fragrance families
• Some basic chemical knowledge to provide a better understanding of the structure of
molecules possessing a sensory power, The volatility and solubility of sensory
molecules
• Chemistry of aromatic compounds in perfume making, Composition of fragrances
• Current trends in fragrances, sensory analysis of different products
• Study of the raw materials used in perfumery (origin, extraction method, and
olfaction)
• Key chemical reactions for conversion of raw materials to fragrances
• Extraction of essential oils used in perfumery
• Difference between alcohol and oil-based perfumes
• Outline of health, safety and sustainability parameters in perfumer

Unit 2: Sustainable Fragrance by Design 4 Hours

• The challenges of sustainability and how it impacts the industry
• Sustainability charter
• Green chemistry principles
• Commitment to Biodiversity

Unit 3: Flavours 18 Hours

• Introduction to flavours, types of flavours, flavour raw materials
• Understanding of terms like, Flavour and Flavouring agents. Attributes of flavour,
taste, odour, odour stimulation, basic tastes and the human olfactory system.
• Stability of flavour in food, sensory evaluation of flavours in foods, Various flavour
formulation
• Systematic approach to understanding flavour formation during food processing, food
matrix, interaction of added flavours
• Flavour enhancers, modifiers, precursors, suppressors, solvents.
• Key chemical reactions for conversion of raw materials to flavours
• Forms of flavour and the manufacturing processes involving all types of flavours.
Aroma recovery during processing.
• Biogenesis of flavours in fruits and vegetables, reaction flavours, off flavours.
• Stability of flavor in food, sensory evaluation of flavours in foods
• Selection and application of flavours in foods and beverages
• Legal aspects (natural flavours and natural flavouring substances, nature identical
flavouring substances, artificial flavouring substances), and the FSSA act.

153
Unit 4: Extraction, Isolation and Purification of Perfumes and Flavour Compounds
05 Hours
• Extraction techniques for the separation of volatile oils from natural source-
including. Distillation, Evaporation, Crystallization and Adsorption, supercritical fluid
extraction methods of isolation of important ingredients

Practicals: (30 hours)

1. Extraction of D-limonene from orange peel using liquid CO2.
2. Extraction of caffeine from coffee beans using liquid CO2.
3. Extraction of essential oils from lemon using steam distillation
4. Extraction of essential oils from lemon using liquid CO2.
5. Extraction of essential oils from fragrant flowers.
6. Determination of esters by Thin Layer Chromatography
7. Memorisation of different raw materials used in perfumery, perfume language,
Memorisation of perfumes
8. Testing up of different flavours
9. Analysis of spectra of perfume formulations.

References:
1. Arctander, S. (2008), Perfume and flavour materials of Natural origin, Allured
Publishing Corporation, USA
2. Arctander, S. (2017), Volume I and II, Perfume and Flavour Chemicals, (Aroma
Chemicals), Allured Publishing Corporation, USA
3. Curtis,T.; Williams, D. C.(2001) 2nd Edition, An Introduction to Perfumery, Micelle
Press, USA.
4. Sell,C. (2008), Understanding Fragrance Chemistry, Allured Publishing Corporation,
USA
5. Calkin,R.R., Jellinek, J.S., Perfumery: Practice and Principles, John Wiley & Sons Inc.
6. Gimelli, S.P. (2001), Aroma Science, Micelle Press, USA
7. Arctander, S. (2019), Perfume and Flavour Materials of Natural Origin, Orchard
Innovations
8. https://www.beyondbenign.org/lessons/essential-oil-extraction-using-liquid-co2/

Keywords: Fragrances, Flavours, pharmaceutical formulation, distillation, extraction

techniques

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

154
 GENERIC ELECTIVES -21 : GREEN CHEMISTRY

Credit distribution, Eligibility and Pre-requisites of the Course

Course Credits Credit distribution of the course Eligibility Pre-requisite

title & Lecture Tutorial Practical/ criteria of the course
Code Practice
Green 4 2 0 2 Class XII ----
Chemistry Pass

(GE-20)

Learning Objectives
Huge rise in environmental pollution, depleting resources, climate change, ozone depletion,
heaps and heaps of landfills piling up has forced the society to become more and more
environmentally conscious. Future chemists and innovators are compelled to work towards
sustainable practices. Green chemistry has arisen from these concerns. It is not a new branch
of chemistry but helps to improve the creative and innovative thinking in undergraduate
students. Green chemistry is a way to boost profits, increase productivity and ensure
sustainability with absolute zero waste. Innovations and applications of green chemistry in
education have helped companies to gain environmental benefits as well as to achieve
economic and societal goals also. Undergraduate students are the ultimate scientific
community of tomorrow. Training them to practice chemistry in the safest way possible is key
towards safe working conditions in the laboratories as well as the chemical industry and
extends to society in a sustainable future for the planet.

Learning Outcomes:
By the end of this course, students will be able to:
● Understand the twelve principles of green chemistry and also build the basic
understanding of toxicity, hazard and risk related to chemical substances.
● Calculate atom economy, E-factor and relate them in all organic synthesis
● Appreciate the use of catalyst over stoichiometric reagents
● Learn to use green solvents, renewable feedstock and renewable energy
sources for carrying out safer chemistry
● Appreciate the use of green chemistry in problem solving skills and critical
thinking to innovate and find solutions to environmental problems.
● Learn to design safer processes, chemicals and products through
understanding of inherently safer design (ISD)
● Appreciate the success stories and real-world cases as motivation for them to
practice green chemistry

155
Syllabus :

Unit 1: Introduction 08 Hours

Definition of green chemistry and how it is different from conventional chemistry and
environmental chemistry.
• Need of green chemistry
• Importance of green chemistry in- daily life, Industries and solving human health problems
(four examples each).
• A brief study of Green Chemistry Challenge Awards (Introduction, award categories and
study about five last recent awards).

Unit 2: Twelve Principles of Green Chemistry 12 Hours

The twelve principles of the Green Chemistry with their explanation, Special emphasis on the
following:
• Prevention of waste / byproducts, pollution prevention hierarchy.
• Green metrics to assess greenness of a reaction: environmental impact factor, atom
economy and calculation of atom economy.
• Green solvents-supercritical fluids, water as a solvent for organic reactions, ionic liquids,
solvent less reactions, solvents obtained from renewable sources.
• Catalysis and green chemistry- comparison of heterogeneous and homogeneous catalysis,
biocatalysis, asymmetric catalysis and photocatalysis.
• Green energy and sustainability.
• Real-time analysis for pollution prevention.
• Prevention of chemical accidents, designing greener processes, inherent safer design,
principle of ISD “What you don’t have cannot harm you”, greener alternative to Bhopal Gas
Tragedy (safer route to carcarbaryl) and Flixiborough accident (safer route to cyclohexanol)
subdivision of ISD, minimization, simplification, substitution, moderation and limitation

Unit 3: 10 Hours
The following Real-world Cases in green chemistry should be discussed: Surfactants for
carbon dioxide – replacing smog producing and ozone depleting solvents with CO2 for
precision cleaning and dry cleaning of garments. Designing of environmentally safe marine
antifoulant. Rightfit pigment: Synthetic azo pigments to replace toxic organic and inorganic
pigments. An efficient, green synthesis of a compostable and widely applicable plastic
(polylactic acid) made from corn.

Practical: (60 Hours)

Characterization by melting point, UV-Visible spectroscopy, IR spectroscopy and any other
specific method should be done (wherever applicable).
1. Preparation and characterization of nanoparticles of gold using tea leaves/silver
nanoparticles using plant extracts.

156
 2. Preparation of biodiesel from waste cooking oil and characterization (TLC, pH, solubility,
combustion test, density, viscosity, gel formation at low temperature and IR can be
provided).
3. Benzoin condensation using thiamine hydrochloride as a catalyst instead of cyanide.
4. Extraction of D-limonene from orange peel using liquid CO2 prepared from dry ice.
5. Mechanochemical solvent free, solid-solid synthesis of azomethine using p-toluidine
and o-vanillin/p-vanillin.
6 Microwave-assisted Knoevenagel reaction using anisaldehyde, ethylcyanoacetate and
ammonium formate.
7. Photoreduction of benzophenone to benzopinacol in the presence of sunlight.
8. Photochemical conversion of dimethyl maleate to dimethyl fumarate (cis-trans
isomerisation)
9. Benzil- Benzilic acid rearrangement: Preparation of benzilic acid in solid state under
solvent-free condition.

References:
Theory:
1. Anastas, P.T., Warner, J.C. (2014), Green Chemistry, Theory and Practice, Oxford
University Press.
2. Lancaster, M. (2016), Green Chemistry: An Introductory Text, 3rd Edition, RSC
Publishing.
3. Cann, M. C., Connely, M.E. (2000), Real-World cases in Green Chemistry, American
Chemical Society, Washington.
4. Matlack, A.S. (2010), Introduction to Green Chemistry, 2nd Edition, Boca Raton: CRC
Press/Taylor & Francis Group publisher.
5. Alhuwalia, V.K., Kidwai, M.R. (2005), New Trends in Green chemistry, Anamalaya
Publishers.
6. Sidhwani, I.T, Sharma, R.K. (2020), An Introductory Text on Green Chemistry, Wiley
India Pvt Ltd.

Practical:

1. Kirchoff, M.; Ryan, M.A. (2002), Greener approaches to undergraduate chemistry

experiment, American Chemical Society, Washington DC.
2. Sharma, R.K.; Sidhwani, I.T.; Chaudhari, M.K. (2013), Green Chemistry Experiments: A
monograph, I.K. International Publishing House Pvt Ltd. New Delhi.
3. Pavia, D.L.; Lamponam, G.H.; Kriz, G.S.W. B. (2012), Introduction to organic
Laboratory Technique- A Microscale approach, 4th Edition, Brooks-Cole Laboratory
Series for Organic chemistry.
4. Sidhwani I.T. (2015), Wealth from Waste: A green method to produce biodiesel from
waste cooking oil and generation of useful products from waste further generated.
DU Journal of Undergraduate Research and Innovation, 1(1),131-151. ISSN: 2395-
2334.
5. Sidhwani, I.T; Sharma, R.K. (2020), An Introductory Text on Green Chemistry, Wiley
India Pvt Ltd.

157
 6. Monograph on Green Chemistry Laboratory Experiments, Green Chemistry Task
Force Committee, Department of Science and Technology, Government of India.

Keywords: Green chemistry, Twelve principles of green chemistry, Atom economy, Waste
minimization, green metric, green solvents, Solvent free, Catalyst, Bio-catalyst, Renewable
energy sources, Hazardous, Renewable feedstock, Ionic liquids, Supercritical fluids, Inherent
safer design, green synthesis, combinatorial, Sustainable development, Presidential green
chemistry awards.
Note: Examination scheme and mode shall be as prescribed by the Examination
Branch, University of Delhi, from time to time.

158
 DEPARTMENT OF CHEMISTRY
Category-I
B Sc. (Hons) Chemistry

DISCIPLINE SPECIFIC CORE COURSE -7 (DSC-7): Chemistry of d- and f-

block Elements & Quantitative Inorganic Analysis
CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course Credits Credit distribution of the Eligibility Pre-requisite

title & course criteria of the course
Code Lecture Tutorial Practical/ (if any)
Practice
Chemistry of 04 02 0 02 Passed Class NIL
d- and f- 12th with
Elements & Physics,
quantitative Chemistry,
Inorganic Mathematics
Analysis (DSC-
7)

Learning Objectives

The Objectives of this course are as follows:

● To provide thorough knowledge about the d- and f- block elements with respect to
the general group trends, physical and chemical properties of these elements.
● To familiarize the students with the d- and f-block elements and get an idea about
horizontal similarity in a period in addition to vertical similarity in a group.
● To impart the knowledge about inorganic polymer
● To give an idea about the principles of gravimetric analysis.

Learning outcomes
By studying this course, the students will be able to:

● List the important properties of transition metals, lanthanoids, and actinoids

● Use Latimer diagrams to predict and identify species which are reducing, oxidizing
and tend to disproportionate and calculate skip step potentials.
● Describe the classification, structure and applications of Inorganic Polymers.
● List and use the principles of gravimetric analysis for quantitative analysis

SYLLABUS OF DSC-7

UNIT – 1: Transition Elements (12 Hours)

89
General group trends with special reference to electronic configuration, colour, variable
valency, magnetic properties, catalytic properties, and ability to form complexes. Stability of
various oxidation states and e.m.f. (Latimer diagrams), Frost diagrams of Mn and Cr.
A brief discussion of differences between the first, second and third transition series

UNIT – 2: Lanthanoids and Actinoids (8 Hours)

A brief discussion of electronic configuration, oxidation states, colour, spectral and magnetic
properties. Lanthanoid contraction (causes and effects) separation of lanthanoids by ion
exchange method.

UNIT – 3: Inorganic Polymer (8 Hours)

Comparison with organic polymers, classification, structure and applications of following

inorganic polymers:
● Borates
● Silicates, silicones
● Phosphates
● Phosphazenes (for cyclic polymers, only trimer is to be discussed)

UNIT – 4: Principles of gravimetric analysis (2 Hours)

Particle size, Precipitation, Coagulation, Peptization, Co-precipitation, Digestion, Filtration
and washing the precipitate, Drying and ignition the precipitate

Practical component (60 Hours)

(Laboratory periods:15 classes of 4 hours each)

(A) Gravimetry
1. Estimation of Ni(II) using dimethylglyoxime (DMG).
2. Estimation of copper as CuSCN.
3. Estimation of iron as Fe2O3 by precipitating iron as Fe(OH)3. (by homogeneous and
heterogeneous method)
4. Estimation of Al(III) by precipitating with oxime and weighing as Al(oxime)3
(aluminiumoxinate).

(B) Inorganic Preparations

1. Potassium aluminium sulphate KAl(SO4)2.12H2O (potash alum) or Potassium
chromium sulphate KCr(SO4)2.12H2O (chrome alum).
2. Manganese phosphate and
3. Sodium peroxoborate

(C ) Paper chromatographic separation of following metal ions (minimum two should be

done):
1. Ni(II) and Co(II)

90
 2. Cu(II) and Cd(II)
3. Fe(III) and Al(III)

Essential/recommended readings

Theory:

1. Lee, J.D.(2010),ConciseInorganicChemistry,WileyIndia.
2. Huheey,J.E.;Keiter,E.A.;Keiter;R.L.;Medhi,O.K.(2009),InorganicChemistry-
PrinciplesofStructureandReactivity,PearsonEducation.
3. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010),
Shriver and Atkins Inorganic Chemistry, 5th Edition, Oxford University Press.
4. Miessler, G.L.; Fischer P.J.; Tarr, D. A. (2014), Inorganic Chemistry, 5th Edition,
Pearson.
5. Pfennig, B. W. (2015), Principles of Inorganic Chemistry. John Wiley & Sons.
6. Cotton, F.A.; Wilkinson, G. (1999), Advanced Inorganic Chemistry, Wiley-VCH.
7. Das, A. K.; Das, M. (2014), Fundamental Concepts of Inorganic Chemistry, 1st
Edition, Volume 1-3, CBS Publishers & Distributors Pvt. Ltd.
8. Chandrashekhar,V. (2005), Inorganic and Organometallic Polymers , 5th Edition,
Springer Publications

Practical:
1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of
Quantitative Chemical Analysis, John Wiley and Sons,
2. Harris, D. C.; Lucy,C. A.(2016), Quantitative Chemical Analysis, 9th Edition, Freeman
and Company.
3. Day, R. A.; Underwood, A. L. (2012), Quantitative Analysis, Sixth Edition, PHI
Learning Private Limited.
4. Marr, G.; Rockett, B.W. (1972), Practical Inorganic Chemistry, Van Nostrand
Reinhold.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

91
 DISCIPLINE SPECIFIC CORE COURSE -8 (DSC-8): Carbonyls, Carboxylic
acids, Amines, Nitro compounds, Nitriles, Isonitriles and Diazonium salts

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Code Credits Credit distribution of the Eligibility Pre-
course criteria requisite of
Lecture Tutorial Practical/ the course
Practice (if any)
Carbonyls, 04 03 0 01 Passed Class NIL
Carboxylic Acids, 12 th
with
Amines, Nitro Physics,
Compounds, Chemistry,
Nitriles, Isonitriles Mathematics
and Diazonium
salts
(DSC-8)

Learning objectives

The objectives of this course are as follows:

● To infuse students with the details of the chemistry of aldehydes, ketones, carboxylic
acids and their derivatives, nitro, amines and diazonium salts.
● To make students aware of the chemical synthesis, properties, reactions and key
applications of the listed classes of compounds and develop understanding of detailed
mechanistic pathways for each functional group to unravel the spectrum of organic
chemistry and the extent of organic transformations.
● To aid in the paramount learning of the concepts and their applications.

Learning outcomes

By studying this course, students will be able to:

● Explain the chemistry of oxygen and nitrogen containing compounds.
● Use the synthetic chemistry learnt in this course to do functional group
transformations.
● Propose plausible mechanisms for the reactions under study.

SYLLABUS OF DSC-8

UNIT – 1: Carbonyls, Carboxylic acid & their derivatives (27 Hours)

Carbonyl Compounds: Reaction of carbonyl compounds with ammonia derivatives, Aldol and
Benzoin condensation, Knoevenagel condensation, Claisen-Schmidt, Perkin, Cannizzaro and

92
Wittig reaction, Beckmann and Benzil-Benzilic acid rearrangements, haloform reaction and
Baeyer Villiger oxidation, α-substitution reactions, oxidations and reductions (Clemmensen,
Wolff Kishner, LiAlH4, NaBH4, MPV, PDC), addition reactions of α,β-unsaturated carbonyl
compounds: Michael addition.
Carboxylic acids and derivatives: Effect of substituents on acidic strength on carboxylic acids,
HVZ reaction, typical reactions of dicarboxylic acids and hydroxy acids. Comparative study of
nucleophilic acyl substitution for acid chlorides, anhydrides, esters and amides, Mechanism of
acidic and alkaline hydrolysis of esters, Dieckmann and Reformatsky reactions, Hoffmann-
bromamide degradation and Curtius rearrangement.
Active methylene compounds: Keto-enol tautomerism. Preparation and synthetic applications
of diethyl malonate and ethyl acetoacetate.

UNIT – 2: Nitro Compounds, Amines, Diazonium salts, Nitriles and Isonitriles (18 Hours)

Nitro compounds: General methods of preparation: from alkyl halides, alkanes, oxidation of
amines and oximes. Henry reaction, Nef reaction, Reduction-electrolytic reduction, reaction
with nitrous acid, reduction in acidic, basic and neutral medium (for aromatic compounds)

Amines: Preparation, chirality in amines (pyramidal inversion), Basicity of amines: Effect of

substituents, solvent and steric effects, distinction between Primary, secondary and tertiary
amines using Hinsberg’s method and nitrous acid, Gabriel Phthalimide synthesis, Carbylamine
reaction, Mannich reaction, Hoffmann’s exhaustive methylation, Hofmann-elimination
reaction and Cope elimination.

Diazonium Salts: Synthetic applications of diazonium salts including preparation of arenes,

haloarenes, phenols, cyano and nitro compounds; Coupling reactions of diazonium salts
(preparation of azo dyes).

Nitriles: Preparation using following reactions: Dehydration of amides and aldoximes,

substitution reaction in alkyl halides and tosylates, from Grignard reagents and from
dehydrogenation of primary amines. Properties: Physical properties, discussion on the
following reactions with mechanism: Reaction with Grignard reagent, hydrolysis, addition
reaction with HX, NH3, reaction with aqueous ROH, Reduction reactions-catalytic reduction
and Stephen’s reaction, Condensation reactions-Thorpe Nitrile Condensation.
Isonitriles: Preparation from the following reactions: Carbylamine reaction, substitution in
alkyl halides and dehydrogenation of N-substituted formamides. Properties: Physical
properties, discussion on the following reactions with mechanism: Hydrolysis, reduction,
addition of– HX, X2 and sulphur, Grignard reaction, oxidation and rearrangement.

Practical component (30 Hours)

(Laboratory periods:15 classes of 2 hours each)

93
 1. Preparation of oximes for aldehydes/ketones (like benzaldehyde, ethyl methyl ketone,
cyclohexanone etc.)
2. Preparation of semicarbazone derivatives for aldehydes/ketones (like benzaldehyde,
ethyl methyl ketone, cyclohexanone etc.)
3. Hydrolysis of amides/esters.
4. Selective reduction of m-dinitrobenzene to m-nitroaniline.
5. Preparation of S-benzylisothiouronium salts for water soluble and water insoluble
carboxylic acids.
6. Systematic qualitative analysis of the given organic compounds containing
monofunctional groups (aromatic hydrocarbons, alcohols, phenol) and preparation of
one suitable derivative.

Students should be exposed to preparative routes for the synthesis of 3,5-dinitrobenzoate,

benzoates, acetate derivatives.

Note: The above derivatives should be prepared using 0.5-1.0 g of the organic compound. The
solid samples must be collected and may be used for recrystallization, melting point and
compound analysis.

Essential/recommended readings
Theory:
1. Morrison, R. N., Boyd, R. N., Bhattacharjee, S.K. (2010), Organic Chemistry, 7th
Edition, Dorling Kindersley (India) Pvt. Ltd., Pearson Education.
2. Finar, I.L. Organic Chemistry Volume 1, Dorling Kindersley (India) Pvt. Ltd., Pearson
Education.
3. Finar, I.L. Organic Chemistry Volume 2, Dorling Kindersley (India) Pvt. Ltd., Pearson
Education.
4. Solomons, T.W.G., Fryhle, C.B.; Snyder, S.A. (2017), Organic Chemistry, 12th Edition,
Wiley.

Practical:
1. Vogel, A.I. (2012), Quantitative Organic Analysis, Part 3, Pearson Education.
2. Mann, F.G., Saunders, B.C. (2009), Practical Organic Chemistry, Pearson Education.
3. Furniss, B.S., Hannaford, A.J., Smith, P.W.G., Tatchell, A.R. (2012), Vogel's Textbook
of Practical Organic Chemistry, 5th Edition, Pearson.
4. Ahluwalia, V.K., Dhingra, S. (2004), Comprehensive Practical Organic Chemistry:
Qualitative Analysis, University Press.
5. Ahluwalia, V.K., Aggarwal, R. (2004), Comprehensive Practical Organic Chemistry:
Preparation and Quantitative Analysis, University Press.
6. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–I, I K
International Publishing house Pvt. Ltd, New Delhi.
7. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–II, I K
International Publishing house Pvt. Ltd, New Delhi.

94
Suggestive Readings
1. Mukherji, S.M., Singh, S.P. (2017), Reaction Mechanism in Organic Chemistry,
Trinity Press.
2. Singh,J., Awasthi, S. K., Singh, Jaya, Fundamentals of Organic Chemistry-III, Pragati
Prakashan (2023)
3. Carey, F.A., Sundberg, R. J. (2008), Advanced Organic Chemistry: Part B: Reaction
and Synthesis, Springer.
4. Bruice, P.Y. (2015), Organic Chemistry, 3rd Edition, Pearson.
5. Patrick, G. (2003), BIOS Instant Notes in Organic Chemistry, Viva Books.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

95
 DISCIPLINE SPECIFIC CORE COURSE – 9 (DSC-9): Chemical equilibrium,
Ionic equilibrium, conductance and solid state

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chemical 04 03 0 01 Passed Class NIL
equilibrium, XII with
Ionic Physics,
equilibrium, Chemistry
conductance and
Mathematics
and solid state
(DSC-9)

Learning Objectives:

The Learning Objectives of this course are as follows:

● To make students understand the concept of chemical equilibrium and ionic equilibrium.
● To introduce the concept of electrolytes, ionization of various electrolytes, pH.
● To explain the applications of ionization in buffer, hydrolysis, acid-base titrations and
indicators.
● To introduce the concept of electrolytic conductance with respect to strong and weak
electrolytes and then extend it to understand concepts like ionic mobility, transference
and related properties.
● To develop the advance concept of solid state with emphasis on crystal structures in
general and cubic crystals in details.

Learning Outcomes:

By studying this course, students will be able to:

● Apply the concept of equilibrium to various physical and chemical processes.
● Derive and express the equilibrium constant for various reactions at equilibrium.
● Use Le Chatelier’s principle to predict the thermodynamic conditions required to get
maximum yield of a reaction
● Apply the concept of equilibrium to various ionic reactions.
● List different types of electrolytes and their properties related to conductance in aqueous
solutions.
● Use conductance measurements for calculating many properties of the electrolytes.

96
● Prepare buffer solutions of appropriate pH.
● Explain the crystal properties and predict the crystal structures of cubic systems form the
XRD.
● Use the instruments like pH-meter and conductivity meters.

SYLLABUS OF DSC-9

UNIT – 1: Chemical Equilibrium (6 Hours)

Criteria of thermodynamic equilibrium, degree of advancement of reaction, Chemical
equilibria in ideal gases, Thermodynamic derivation of relation between Gibbs free energy of
a reaction and reaction quotient, Equilibrium constants and their dependence on
temperature, pressure and concentration, Le Chatelier’s Principle (Quantitative treatment),
Free energy of mixing and spontaneity (qualitative discussion).

UNIT – 2: Ionic equilibrium (12 Hours)

Strong, moderate and weak electrolytes, Arrhenius theory of electrolytic dissociation, degree
of ionization, factors affecting degree of ionization, ionization constant and ionic product of
water. Ionization of weak acids and bases, pH scale, common ion effect; dissociation constants
of mono and diprotic acids. Salt hydrolysis-calculation of hydrolysis constant, degree of
hydrolysis and pH for different salts. Buffer solutions; derivation of Henderson equation and
its applications. Solubility and solubility product of sparingly soluble salts – applications of
solubility product principle. Qualitative treatment of acid – base titration curves. Theory of
acid–base indicators; selection of indicators and their limitations.

UNIT – 3: Conductance (12 Hours)

Quantitative aspects of Faraday’s laws of electrolysis, Conductivity, equivalent and molar

conductivity and their variation with dilution for weak and strong electrolytes. Molar
conductivity at infinite dilution. Kohlrausch’s law of independent migration of ions. Debye-
Huckel-Onsager equation, Wien effect, Debye-Falkenhagen effect, Walden’s rule. Ionic
velocity, mobility and their determination, transference number and its relation to ionic
mobility, determination of transference number using Moving Boundary methods.
Applications of conductance measurement: (i) degree of dissociation of weak electrolytes, (ii)
ionic product of water (iii) solubility and solubility product of sparingly soluble salts, (iv)
conductometric titrations (v) hydrolysis constants of salts.

UNIT – 4: Solid state (15 Hours)

Nature of the solid state, law of constancy of interfacial angles, law of rational indices, Miller
indices, elementary idea of symmetry, seven crystal systems and fourteen Bravais lattices; X-
ray diffraction, Bragg’s law, a simple account of rotating crystal method and powder pattern
method. Analysis of powder diffraction patterns of NaCl, CsCl and KCl.

97
Practical component (30 Hours)
(Laboratory periods: 15 classes of 2 hours each)
pH metry:
1. Study the effect of addition of HCl/NaOH on pH to the solutions of acetic acid, sodium
acetate and their mixtures.
2. Preparation of buffer solutions of different pH values
a. Sodium acetate-acetic acid
b. Ammonium chloride-ammonium hydroxide
3. pH metric titration of
a. Strong acid with strong base
b. Weak acid with strong base. Determination of dissociation constant of a weak acid.
Conductometry:
1. Determination of cell constant
2. Determination of conductivity, molar conductivity, degree of dissociation and
dissociation constant of a weak acid.
3. Perform the following conductometric titrations:
a. Strong acid vs. strong base
b. Weak acid vs. strong base
c. Mixture of strong acid and weak acid vs. strong base
d. Strong acid vs. weak base

p-XRD (p-XRD crystal pattern to be provided to the students)

1. Differentiate and classify the given set of the diffraction pattern as crystalline materials
or amorphous (Glass) substance.
2. Carry out analysis of a given set of p-XRD and determine the type of the cubic crystal
structure
a. NaCl
b. CsCl
c. KCl
3. Determination of approximate crystal size from a given set of p-XRD

Essential/recommended readings
Theory
1. Peter, A.; Paula, J. de. (2011), Physical Chemistry, 9th Edition, Oxford University Press.
2. Castellan, G. W. (2004), Physical Chemistry, 4th Edition, Narosa.
3. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, Vol 2, 6th Edition, McGraw Hill
Education.
4. McQuarrie, D. A.; Simon, J. D. (2004), Molecular Thermodynamics, Viva Books Pvt.
Ltd.
5. Kapoor, K.L. (2015),A Textbook of Physical Chemistry, Vol 1, 6th Edition, McGraw Hill
Education.

Practical:

98
 1. Khosla, B.D.; Garg, V.C.; Gulati, A. (2015), Senior Practical Physical Chemistry, R.
Chand & Co, New Delhi.
2. Kapoor, K.L. (2019), A Textbook of Physical Chemistry, Vol.7, 1st Edition, McGraw Hill
Education.
3. Garland, C. W.; Nibler, J. W.; Shoemaker, D. P. (2003), Experiments in Physical
Chemistry, 8th Edition, McGraw-Hill, New York.

Suggestive readings

1. Levine, I.N. (2010), Physical Chemistry, Tata Mc Graw Hill.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

99
 POOL OF DISCIPLINE SPECIFIC ELECTIVE COURSE

DISCIPLINE SPECIFIC ELECTIVE COURSE -1 (DSE-1): Nuclear and

Environmental Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE

COURSE
Course title & Credits Credit distribution of the Eligibility Pre-
Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Nuclear and 04 03 0 01 Passed Class NIL
Environmental 12th with
Chemistry Physics,
(DSE-1) Chemistry

Learning Objectives

The Objectives of this course are as follows:

● To make students know more about nuclear chemistry

● To familiarise the students about environmental chemistry, especially with respect to
air and water

Learning outcomes

By studying this course, the students will be able to:

● Gain knowledge about Nuclear chemistry, radioactive decay, nuclear disasters, and
nuclear waste and their disposal.
● Describe the composition of air, various air pollutants, effects and control measures of
air pollutants.
● List different sources of water, water quality parameters, impacts of water pollution,
water treatment.
● Identify different industrial effluents and their treatment methods.

SYLLABUS OF DSE-1

Unit-1 : Nuclear Chemistry (21 Hours)

100
The nucleus: subatomic particles, e liquid drop model; forces in nucleus-mesons; stability of
nucleus-n/p ratio, binding energy; radioactive elements.
Radioactive decay- α-decay, β-decay, γ-decay; neutron emission, positron emission; unit of
radioactivity (curie); half life period; radioactive displacement law, radioactive series.
Measurement of radioactivity: ionization chamber, Geiger Counters, Scintillation counters.
Nuclear reactions: Nuclear fission-theory of nuclear fission; chain reaction; nuclear fusion;
nuclear reactors-fast breeder reactors, fuels used in nuclear reactors, separation of isotopes,
moderators, coolants; nuclear reactors in India.
Applications: Dating of rocks and minerals, carbon dating, neutron activation analysis, isotopic
labeling studies, nuclear medicine- 99mTc radio pharmaceuticals.
Nuclear disasters – Chernobyl disaster, Three Mile Island Disaster, Disposal of nuclear waste
and its management.

UNIT – 2: Air Pollution (12 Hours)

Major regions of atmosphere, chemical and photochemical reactions in atmosphere. Air

pollutants: types, sources, particle size and chemical nature, Major sources of air pollution,
Pollution by SO2, CO2, CO, NOx, H2S and other foul-smelling gases, methods of estimation of
CO, NOx, SOx and control procedures.

Chemistry and environment impact of the following: Photochemical smog, Greenhouse effect,
Ozone depletion

Air pollution control, Settling Chambers, Venturi Scrubbers, Electrostatic Precipitators (ESPs).

UNIT – 3 : Water Pollution: (12 Hours)

Hydrological cycle, water resources, aquatic ecosystems, Sources and nature of water
pollutants, Techniques for measuring water pollution, Impacts of water pollution on
hydrological cycle and ecosystems. Water purification methods. Effluent treatment plants
(primary, secondary and tertiary treatment).

Sludge disposal. Industrial waste management, incineration of waste. Water treatment and
purification (reverse osmosis, electro dialysis, ion-exchange). Water quality parameters for
wastewater, industrial water and domestic water.

Practical component (30 Hours)

(Laboratory periods:15 classes of 2 hours each)
(At least four experiments to be performed)

1. Determination of dissolved oxygen in a given sample of water.

2. Determination of Chemical Oxygen Demand (COD) in a given sample of water.
3. Determination of Biological Oxygen Demand (BOD) in a given sample of water.

101
4. Measurement of chloride, sulphate and salinity of water samples by simple titration
method (AgNO3 and potassium chromate).
5. Estimation of total alkalinity of water samples (CO32-, HCO3-) using double titration
method.
6. Measurement of dissolved CO2 in a given sample of water.
7. Determination of hexavalent Chromium Cr(VI) concentration in tannery wastes/ waste
water sample using UV-Vis spectrophotometry technique.

Essential/recommended readings

Theory:
1. Stanley E. Manahan, 10th edition, Environmental chemistry, CRC Press, Taylor and
Francis Group, US, 2017
2. Baird, C. and Cann,M., Environmental Chemistry,(2012), Fifth Edition, W. H.
Freemann & Company, New York, US.
3. VanLoon, G.W. and Duffy, J.S.( 2018) Environmental Chemistry - A global
perspective, Fourth Edition, Oxford University Press
4. Brusseau, M.L.; Pepper,I.L. and Gerba, C., (2019) Environmental and Pollution
Science, Third Edition, Academic Press.
5. Masters, G.M., (1974) Introduction to Environmental Science and Technology, John
Wiley & Sons.
6. Masters, G.M., (2015) Introduction to Environmental Engineering and Science.
JPrentice Hall India Learning Private Limited.
1. 7.Arnikar, H.J., (1987), Second Edition, Essentials of Nuclear Chemistry, Wiley
Blackwell Publishers
7. Arnikar, H.J.; Rajurkar, N. S.,(2016) Nuclear Chemistry through Problems, New Age
International Pvt. Ltd.
8. De, A.K.(2012), Environmental Chemistry, New Age International Pvt., Ltd.
9. Khopkar, S.M.(2010), Environmental Pollution Analysis, New Age International
Publisher.
10. Das, A. K. (2010), Fundamentals of Inorganic Chemistry, Volume 1, Second Edition,
CBS Publishers & Distributors Pvt Ltd.
11. Das, A. K. (2012), Environment Chemistry with Green chemistry, Books and Allied (P)
Ltd.
Practical:
1. Vowles, P.D.; Connell, D.W. (1980),Experiments in Environmental
Chemistry: A Laboratory Manual, Vol.4, Pergamon Series in Environmental
Science.
2. Gopalan, R.; Anand, A.; Sugumar R.W. (2008),A Laboratory Manual for
Environmental Chemistry, I. K. International.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

102
 DISCIPLINE SPECIFIC ELECTIVE COURSE - 2 (DSE-2): Inorganic
materials of industrial importance

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE

COURSE
Course title & Credits Credit distribution of the course Eligibility Pre-requisite of
Code Lecture Tutorial Practical/ criteria the course
Practice (if any)
Inorganic 04 03 0 01 Passed Class NIL
Materials of 12th with
Industrial Physics,
Importance Chemistry
(DSE-2)

Learning Objectives
The objectives of this course are as follows:
● To make students understand the diverse roles of inorganic materials in the industry
and to give an insight into how these raw materials are converted into products used in
day-to-day life.
● To make students learn about silicates, fertilizers, surface coatings,
batteries, engineering materials for mechanical construction.
● To develop the interest of students in the frontier areas of inorganic and material
chemistry.
Learning outcomes
By studying this course, the students will be able to:

● State the composition and applications of the different kinds of glass.

● State the composition of cement and discuss the mechanism of setting of cement.
● Defend the suitability of fertilizers for different kinds of crops and soil.
● Explain the process of formulation of paints and the basic principle behind the
protection offered by the surface coatings.
● Describe the principle, working and applications of different batteries.
● Evaluate the synthesis and properties of nano-dimensional materials, various
semiconductor and superconductor oxides.

SYLLABUS OF DSE-2

Unit 1: Silicate Industries ( 6 Hours)

Glass: Glassy state and its properties, classification (silicate and non-silicate glasses).
Manufacture and processing of glass. Composition and properties of the following types of

103
glasses: Soda lime glass, lead glass, armoured glass, different types of safety glass, borosilicate
glass, fluorosilicate glass, coloured glass, photosensitive glass, photochromic glass, glass wool
and optical fibre.

Cement: Manufacture of Portland cement and the setting process, Different types of
cements: quick setting cements, eco-friendly cement (slag cement), pozzolana cement.

Unit 2: Fertilizers (6 Hours)

Different types of fertilizers (N, P and K). Importance of fertilizers, chemistry involved in the
manufacture of the following fertilizers: urea, calcium ammonium nitrate, ammonium
phosphates, superphosphate of lime and potassium nitrate.

Unit 3: Surface Coatings (18 Hours)

Brief introduction to and classification of surface coatings, paints and pigments: formulation,
composition and related properties, pigment volume concentration (PVC)and critical pigment
volume concentration (CPVC), fillers, thinners, enamels and emulsifying agents. Special
paints: heat retardant, fire retardant, eco-friendly paints, plastic paints, water and oil paints.
Preliminary methods for surface preparation, metallic coatings (electrolytic and electroless
with reference to chrome plating and nickel plating), metal spraying and anodizing.

Contemporary surface coating methods like physical vapor deposition, chemical vapor
deposition, galvanising, carburizing, sherardising, boriding, nitriding and cementation.

Unit 4: Batteries (9 Hours)

Primary and secondary batteries, characteristics of an Ideal Battery, principle, working,
applications and comparison of the following batteries: Pb- acid battery, Li-metal batteries, Li-
ion batteries, Li-polymer batteries, solid state electrolyte batteries, fuel cells, solar cells and
polymer cells.
Unit 5: Nano dimensional materials (6 Hours)
Introduction to zero, one and two-dimensional nanomaterial: Synthesis, properties and
applications of fullerenes, carbon nanotubes, carbon fibres, semiconducting and
superconducting oxides.

Practical component (30 Hours)

(Laboratory periods:15 classes of 2 hours each)
(At least four experiments to be performed)

1. Detection of constituents of Ammonium Sulphate fertilizer (Ammonium and Sulphate ions)

by qualitative analysis and determine its free acidity.

2. Detection of constituents of CAN fertilizer (Calcium, Ammonium and Nitrate ions)

fertilizer and estimation of Calcium content.

104
3. Detection of constituents of Superphosphate fertilizer (Calcium and Phosphate ions) and
estimation of phosphoric acid content.

4. Analysis of (Cu, Ni) in alloy or synthetic samples (methods involving Gravimetry and
Spectrophotometry).

5. Analysis of (Cu, Zn) in alloy or synthetic samples (Multiple methods involving Iodometry,
and Potentiometry).

6. Synthesis of pure ZnO and Cu doped ZnO nanoparticles.

7. Synthesis of silver nanoparticles by green and chemical approach methods and its
characterization using UV-visible spectrophotometer

Essential/recommended readings
Theory:

1. West, A. R. (2014),Solid State Chemistry and Its Application, Wiley

2. Smart, L. E.; Moore, E. A. (2012),Solid State Chemistry An Introduction, CRC Press
Taylor & Francis.
3. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong,
F.A.(2010),Shriver and Atkins Inorganic Chemistry, W. H. Freeman and Company.
4. Kent, J. A. (ed) (1997), Riegel’s Handbook of Industrial Chemistry, CBS Publishers,
New Delhi.
5. Poole Jr.; Charles P.; Owens, Frank J.(2003), Introduction to Nanotechnology, John
Wiley and Sons.

Practical:

1. Svehla, G.(1996),Vogel’s Qualitative Inorganic Analysis, Prentice Hall.

2. Banewicz, J. J.; Kenner, C.T. Determination of Calcium and Magnesium in
Limestones and Dolomites, Anal. Chem., 1952, 24 (7), 1186–1187.
3. Ghorbani, H. R.; Mehr, F.P.; Pazoki, H.; Rahmani B. M. Synthesis of ZnO
Nanoparticles by Precipitation Method. Orient J Chem 2015;31(2).
4. Orbaek, W.; McHale, M.M.; Barron, A.R. Synthesis and characterization of silver
nanoparticles for an undergraduate laboratory, J. Chem. Educ. 2015, 92,
339−344.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

105
 DISCIPLINE SPECIFIC ELECTIVE COURSE – 3 (DSE-3): Green Chemistry
in Organic Synthesis
CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE
COURSE

Course Credits Credit distribution of the Eligibility Pre-requisite

title & course criteria of the course
Code Lecture Tutorial Practical/ (if any)
Practice
Green 04 03 0 01 Passed Class Basic
Chemistry in 12th with knowledge
Organic Physics, of organic
Synthesis Chemistry reactions
(DSE-3)

Learning objectives

The objectives of this course are as follows:

● To create awareness about the chemistry that is not harmful for human health and the
environment.
● To provide thorough knowledge of the green chemistry principles that can be used to
develop chemistry in greener way.
● To familiarize students with new remediation technologies for the cleaning up of
hazardous substances.
● To use green chemistry for boosting profits, increase productivity and ensure
sustainability with absolute zero waste.
● To learn about innovations and applications of green chemistry in education that helps
companies to gain environmental benefits as well as to achieve economic and societal
goals also
● The objective of the practical component is to develop basic skills to be able to design,
develop and run chemical processes in a sustainable way.

Learning outcomes

By studying this course, students will be able to:

● List the twelve principles of green chemistry and build the basic understanding of
toxicity, hazard and risk related to chemical substances.
● Calculate atom economy, E-factor and relate them in all organic synthesis
● State the uses of catalyst over stoichiometric reagents
● Debate and use green solvents, renewable feedstock, and renewable energy sources for
carrying out safer chemistry
● Use green chemistry for problem solving, innovation and finding solutions to
environmental problems.
● Design safer processes, chemicals, and products through understanding of inherently
safer design (ISD)

106
 ● Discuss the success stories and use real-world cases to practice green chemistry

SYLLABUS OF DSE-3

UNIT – 1: Introduction (3 Hours)

Introduction to Green Chemistry, some important environmental laws, pollution prevention Act
of 1990, emergence of green chemistry, need for Green Chemistry. Goals of Green Chemistry.
Limitations/ Obstacles in the pursuit of the goals of Green Chemistry. Green chemistry in
sustainable development.

UNIT – 2: Application of Green Chemistry Principles (36 Hours)

Principles of Green Chemistry and designing a chemical synthesis

Concept familiarization and application of green chemistry principles using specific examples
1. Prevention of waste/ by products; waste or pollution prevention hierarchy
2. Green metrics to assess greenness of a reaction: Calculation of atom economy of the
rearrangement, addition, substitution, and elimination reactions; calculation of E-factor
for industrial processes
3. Prevention/ minimization of hazardous/ toxic products
4. Safer Solvent and Auxiliaries: Problems associated with conventional reaction media
Some Common Green solvents: Introduction, application, advantages, and disadvantages
of green solvents in organic synthesis (taking suitable examples). Special emphasis on the
following:
i. Super Critical Fluids (with special reference to carbon dioxide)
ii. Water: Concept of In-water, and on-water reactions (with special reference to synthesis
of terpinol and linalool in water, Benzoin condensation, Heck reaction)
iii. Ionic Liquids: Physical properties and classification of Ionic Liquids (with special
reference to Diels Alder reaction and Coumarin synthesis in ionic liquids)
iv. Biomass derived Solvents: Physicochemical properties, Use of glycerol and its
derivatives (Mizoroki–Heck reaction) and 2-methyltetrahydrofuran (Suzuki–Miyaura
reaction).
5. Design for energy efficiency: Phenomenon of accelerating organic reactions by using the
following Green Chemistry tools (taking suitable examples) and its advantages:
i. Mechanochemistry
ii. Ultrasound assisted reactions: Taking examples like Simmons Smith reaction, Diels–
Alder reaction,
iii. Microwave assisted reactions: Special emphasis on solvent-free synthesis- copper
phthalocyanine and aspirin, In-water reactions-Hofmann Elimination, methyl benzoate to
benzoic acid and Decarboxylation reaction;
iv. Electrocatalysis: Taking examples like adiponitrile synthesis, synthesis of 3-
bromothiophene.
v. Visible light induced Reactions: with examples such as, syntheses of caprolactam and
vitamin D3, cis-trans isomerization of alkenes
6. Use of renewable starting materials: Illustrate with few examples such as biodiesel,
bioethanol, polymers from renewable resources (PLA from corn), Synthesis and
properties of 2-Methyltetrahydrofuran, furfural and 5-Aminolevulinic acid (DALA)
from levulinic acid

107
 7. Avoidance of unnecessary derivatization – careful use of blocking/protecting groups
(taking specific examples like selective oxidation of aldehydic group and synthesis of
6-Aminopenicillanic Acid (6-APA) from penicillin G
8. Catalysis and green chemistry
Introduction to Catalysis (including concept of selectivity, turnover frequency and
turnover number), Types of Catalysts: Heterogeneous catalysis and homogeneous
catalysis (H-beta and zeolites in organic synthesis), General catalytic cycle for
heterogeneous catalysis; Asymmetric catalysis (Monsanto route to L-dopa via
asymmetric hydrogenation, synthesis of carbapenhem via Asymmetric reduction);
Photocatalysis (with special reference to TiO2); Biocatalysis (Synthesis of adipic
acid/catechol using biocatalyst) and Nanocatalysis (oxazole synthesis using
nanocatalyst)
9. Design for degradation: (Illustrate with the help of examples: soaps and detergents,
pesticides, polymers)
10. Real Time monitoring of chemical processes using inline, offline, and online techniques
11. Inherently safer design/chemistry:
Principle and subdivision of ISD, Bhopal Gas Tragedy (safer route to carbaryl) and
Flixiborough accident (safer route to cyclohexanol, Asahi Process)

UNIT – 3: Industrial Applications and Success Stories (6 Hours)

● Vitamin C Synthesis using enzymes (Hoffman La Roche)
● Zoloft -Presidential Chemistry Award Winning Innovation (Pfizer)
● Methyl Methacrylate syngas process (Eastman Chemicals)
● Synthesis of herbicide disodium iminodiacetate
● Rightfit pigments azo dyes synthesis and their applications
● Healthier Fats and oils by Green Chemistry: Enzymatic Interesterification for
production of No Trans-Fats and Oils.
● Synthesis of anti-tuberculosis drug Paramycin from waste water stream

Practical component (30 Hours) (Laboratory periods:15 classes of 2 hours each)

Note: Characterization by melting point, UV-Visible spectroscopy, IR spectroscopy and any

other specific method should be done (wherever applicable).
1. Preparation and characterization of nanoparticles of gold using tea leaves/silver
nanoparticles using plant extracts.
2. Preparation of biodiesel from waste cooking oil and characterization (TLC, pH,
solubility, combustion test, density, viscosity, gel formation at low temperature and IR
can be provided).
3. Benzoin condensation using thiamine hydrochloride as a catalyst instead of cyanide.
4. Extraction of D-limonene from orange peel using liquid CO2 prepared from dry ice.
5. Mechanochemical solvent free, solid-solid synthesis of azomethine using p-toluidine
and o-vanillin/p-vanillin.
6. Microwave-assisted Knoevenagel reaction using anisaldehyde, ethylcyanoacetate and
ammonium formate.
7. Photoreduction of benzophenone to benzopinacol in the presence of sunlight.
8. Photochemical conversion of dimethyl maleate to dimethyl fumarate (cis-trans
isomerisation)

108
 9. Benzil- Benzilic acid rearrangement: Preparation of benzilic acid in solid state under
solvent-free condition.
10. Preparation of dibenzalacetone by cross aldol condensation reaction using base
catalysed green method.

Essential/recommended readings
Theory:
1. Anastas, P.T., Warner, J.C. (2014), Green Chemistry, Theory and Practice, Oxford
University Press.
2. Lancaster, M. (2016), Green Chemistry: An Introductory Text, 3rd Edition, RSC
Publishing.
3. Cann, M. C., Connely, M.E. (2000), Real-World cases in Green Chemistry,
American Chemical Society, Washington.
4. Matlack, A.S. (2010), Introduction to Green Chemistry, 2nd Edition, Boca Raton:
CRC Press/Taylor & Francis Group publisher.
5. Alhuwalia,V.K., Kidwai, M.R. (2005), New Trends in Green chemistry, Anamalaya
Publishers.
6. Sidhwani, I.T, Sharma, R.K. (2020), An Introductory Text on Green Chemistry,
Wiley India Pvt Ltd.

Practicals:
1. Kirchoff, M.; Ryan, M.A. (2002), Greener approaches to undergraduate chemistry
experiment, American Chemical Society, Washington DC.
2. Sharma, R.K.; Sidhwani, I.T.; Chaudhari, M.K. (2013), Green Chemistry
Experiments: A monograph, I.K. International Publishing House Pvt Ltd. New Delhi.
3. Pavia, D.L.; Lamponam, G.H.; Kriz, G.S.W. B. (2012), Introduction to organic
Laboratory Technique- A Microscale approach, 4th Edition, Brooks-Cole
Laboratory Series for Organic chemistry.
4. Sidhwani I.T. (2015), Wealth from Waste: A green method to produce biodiesel from
waste cooking oil and generation of useful products from waste further generated. DU
Journal of Undergraduate Research and Innovation, 1(1),131-151. ISSN: 2395-
2334.
5. Sidhwani, I.T; Sharma, R.K. (2020), An Introductory Text on Green Chemistry,
Wiley India Pvt Ltd.
6. Monograph on Green Chemistry Laboratory Experiments, Green Chemistry Task
Force Committee, Department of Science and Technology, Government of India.
7. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–I, I K
International Publishing house Pvt. Ltd, New Delhi
8. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–II, I K
International Publishing house Pvt. Ltd, New Delhi

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

109
 DISCIPLINE SPECIFIC ELECTIVE COURSE – 4 (DSE-4): Reactions,
Reagents and Chemical Process

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course Credits Credit distribution of the Eligibility Pre-requisite

title & course criteria of the course
Code Lecture Tutorial Practical/ (if any)
Practice
Reactions, 04 03 0 01 Passed Class Basic
Reagents and 12th with knowledge
Chemical Physics, of organic
Process Chemistry reactions
(DSE-4)

Learning objectives

The objectives of this course are as follows:

● To study the important organic name and rearrangement reactions that are crucial for
the synthesis of valuable organic compounds.
● To give the knowledge belonging to the role of reagents in organic reactions for the
synthesis of chemo-, diastereo- and enantio-selective products.
● To impart the knowledge of process chemistry that is a key part of the large-scale
synthesis of chemical products essential for day-to-day life

Learning outcomes

By studying this course, students will be able to:

● Explain the reaction mechanism of various name and rearrangement reactions
● Discuss the role of the reagents in organic synthesis and apply these reagents for the
bulk chemical synthesis
● Debate and use oxidizing and reducing reagents for selective synthesis organic products
● Apply the learnt techniques to chemical processes
● Acquire skills for human resource building especially in the chemical industry.

SYLLABUS OF DSE-4

UNIT – 1: Name Reactions (15 Hours)

Application, scope and mechanism of following reactions: Prevost Reaction, Chugaev
Reaction, Maukaiyama Aldol Reaction, Mozingo Reaction, Ramberg Backlund Reaction,
Shapiro Reaction, Barbier Reaction, Clark- Eschweiler Reaction, Darzen’s Reaction, Julia-
Olifination Reaction, Tiffeneaus Damjanov Reaction, Darkin West Reaction, Bischler-
Napieralaski Reaction, Birch reduction of aromatic compounds, Appel Reaction, Mitsunobu
Reaction, Corey Kim Oxidation, Azide-alkyne 1,3-dipolar cycloaddition reaction, Olefin
metathesis: Grubbs reaction, Heck Reaction, Suzuki coupling and Wittig reaction.

110
UNIT – 2: Reducing Reagents (9 Hours)

Reactions, mechanism and applications of following reducing agents: Sodium borohydride,

Lithium aluminium hydride, NaBH3CN, DIBALH, lithium-tri-tert-butoxyaluminum hydride,
Red-Al Na[AlH2(OCH2OCH2OCH3)2], Zinc borohydride, L and K selectrides, LiBHEt3 and
KBHEt3, Luche Reagent NaBH4-CeCl3, K[BH(OAc)3], bis-Boric Acid (BBA),
Catecholborane, DEMS (Diethoxymethylsilane), 3-Mercapto propionic acid,
Polymethylhydrosiloxane (PMHS), Schwartz’s Reagent (Zirconocene chloride hydride).

UNIT – 3: Oxidizing Reagents (9 Hours)

Reactions, mechanism and applications of following oxidizing agents: Jones Reagent (CrO3,
H2SO4, H2O), Swern Reagent (DMSO, oxalyl chloride), Dess Martin, TEMPO, TPAP
(Tetrapropyl ammonium perruthenate), Fetizon’s Reagent, Fenton’s Reagent [H2O2 + Fe(II)
ion], Sodium perborate NaH2BO4, Sodium Bismuthate NaBiO3, ABNO (9-
OPO(OEt)2
Azabicyclo[3.3.1]nonane N-oxyl), DEAP (Diethyl allyl phosphate, ),
AZADO (2-Azaadamantane N-oxyl], Wacker oxidation.

UNIT – 4: Process Chemistry (12 Hours)

1. Process chemistry a) Introduction, stages of scale up process: Bench, pilot, and large-
scale process with at least two examples of scale up process of API. b) In-process control
and validation of large-scale process.
2. Unit Processes: The following unit processes should be studied with mechanism and one
example of each process Nitration: Nitrating agents, process equipment for technical
nitration. Halogenation: Types of halogenations, catalytic halogenations. Reduction:
Catalytic hydrogenation, hydrogen transfer reactions, metal hydrides. Oxidation: Types
of oxidative reactions, and non-metallic oxidizing agents such as H, sodium hypochlorite,
oxygen gas, ozonolysis.

Practical component (30 Hours)

(Laboratory periods:15 classes of 2 hours each)

1. Oxidation of alcohols to acid using Jones reagent.

2. Reduction of acetophenone and its derivatives to 1-phenyl ethanol derivatives by
NaBH4.
3. Reduction of 4-tert-butyl-cyclohexanone to cis and trans 4-tert-butyl-cyclohexanol.
4. Synthesis of 2,5-dimethyl-2,5-hexanediol from tert-butanol using Fenton’s reagents.
5. Wittig reaction of benzyltriphenylphosphonium chloride and 4-bromobenzaldehyde
using potassium phosphate (tribasic).
6. Substitution (SN2) reaction of 1-iodobutane and 2-naphthol.
7. Aldol condensation reaction: solventless synthesis of chalcones.
9. Borohydride reduction of a ketone: hydrobenzoin from benzil.
10. Visit to chemical industry for the demonstration of pilot scale.

111
Essential/recommended readings

Theory:
1. Clayden, J. Greeves, N., Warren, S. Organic Chemistry, South Asian Edition,
Oxford University Press, USA
2. Gadamasetti K., Process Chemistry in the Pharmaceutical Industry: Challenges in
an Ever- Changing Climate-An Overview, Vol-2, CRC Press, London.
3. Murphy R.M., Introduction to Chemical Processes: Principles, Analysis, Synthesis,
McGraw-Hill Education, New York.
4. Harrington P. J., Pharmaceutical Process Chemistry for Synthesis: Rethinking the
Routes to Scale up, John Wiley and Sons, Inc, New Jersey.
5. Parashar, R.K.; Ahluwalia, V.K. (2018), Organic Reaction Mechanism, 4th Edition,
Narosa Publishing House.
6. Singh J., S. K. Awasthi, Singh Jaya (2023) Fundamental of Organic Chemistry, Paper
III, Pragati Prakashan.

Practical:
1. Mann F.G, Saunders, B.C., Practical Organic Chemistry, Dorling Kindersley
(India) Pvt. Ltd. (Pearson Education Ltd.), Singapore.
2. Vogel A.I., Elementary Practical Organic Chemistry, Dorling Kindersley (India)
Pvt. Ltd. (Pearson Education Ltd.), Singapore.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

DISCIPLINE SPECIFIC ELECTIVE COURSE -5(DSE-5): Solutions,

Colligative properties, Phase Equilibria and adsorption

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Solutions, 04 03 0 01 Class 12 th
NIL
Colligative with Physics,
properties, Phase Chemistry
Equilibria and
adsorption
(DSE-5)

Learning Objectives

The Learning Objectives of this course are as follows:

● To make the students understand the various properties of dilute solutions.

112
 ● To make the students understand the thermodynamic basis of colligative properties.
● To explain the concept of phase, co-existence of phases, phase diagram for various
types of system, CST and distribution law.
● To introduce the concept of adsorption, its dependence on various conditions and
applications

Learning outcomes

By studying this course, students will be able to:

● Explain different types of phase equilibrium, draw a well labelled phase diagram.
● Predict the existence of a substance in a given phase under different conditions of
temperature and pressure
● Apply the concepts of phase, solutions and distribution law while studying other
chemistry courses and every-day life processes.
● Explain the type of adsorption that can take place in different systems and predict the
conditions to get maximum adsorption.

SYLLABUS OF DSE-5

UNIT-1: Solutions and Colligative Properties (12 Hours)

Dilute solutions; lowering of vapour pressure, Raoult’s law, Henry’s law. Thermodynamic
basis of the colligative properties - lowering of vapour pressure, elevation of Boiling Point,
Depression of Freezing point and Osmotic pressure and derivation of expressions for these
using chemical potential. Application of colligative properties in calculating molar masses of
normal, dissociated and associated solutes in solutions, van’t Hoff factor and its applications.
Concept of activity and activity coefficients.

UNIT-2: Phase Equilibria (24 Hours)

Concept of phases, components and degrees of freedom, derivation of Gibbs Phase Rule for
nonreactive and reactive systems; Clausius-Clapeyron equation and its applications to solid-
liquid, liquid-vapour and solid-vapour equilibria, phase diagram for one component systems
(H2O and S), with applications. A comparison between the phase diagram of CO2 and H2O.
Phase diagrams for systems of solid-liquid equilibria involving eutectic, congruent and
incongruent melting points, solid solutions (excluding partial miscibility). Binary solutions:
Gibbs-Duhem-Margules equation, its derivation and applications to fractional distillation of
binary miscible liquids (ideal and non-ideal), Konovalov’s laws, azeotropes, lever rule, partial
miscibility of liquids, CST, miscible pairs, steam distillation. Nernst distribution law: its
derivation and applications.
Three component systems, water-chloroform-acetic acid system, triangular plots.

UNIT-3: Surface chemistry (9 Hours)

Physical adsorption, chemisorption, adsorption isotherms (Langmuir and Freundlich). Nature

of adsorbed state. Multilayer adsorption, BET equation derivation, thermodynamic treatment
of adsorption-Gibbs equation.

113
Practical component (30 Hours)
(Laboratory periods: 15 classes of 2 hours each)
Practical

Phase Equilibrium

1. Determination of critical solution temperature and composition at CST of the phenol

water system
2. To study the effect of impurities of sodium chloride and succinic acid on the CST of
phenol-water system.
3. To study the cooling curves for the following systems:
(i) simple eutectic
(ii) congruently melting systems.
Adsorption

Verify the Freundlich and Langmuir isotherms for adsorption of acetic acid on activated
charcoal.

Essential/recommended readings
Theory:
1. Peter, A.; Paula, J. de. (2011), Physical Chemistry, 9th Edition, Oxford University
Press.
2. Castellan, G. W. (2004), Physical Chemistry, 4th Edition, Narosa.
3. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, Vol 3, 6th Edition, McGraw
Hill Education.
4. Kapoor, K.L. (2015),A Textbook of Physical Chemistry, Vol 5, 6th Edition, McGraw
Hill Education.
5. Ball, D. W. (2017), Physical Chemistry, 2nd Edition, Cengage Learning, India.

Practical:
4. Khosla, B.D.; Garg, V.C.; Gulati, A. (2015), Senior Practical Physical Chemistry, R.
Chand & Co, New Delhi.
5. Garland, C. W.; Nibler, J. W.; Shoemaker, D. P. (2003), Experiments in Physical
Chemistry, 8th Edition, McGraw-Hill, New York.

Suggestive readings

1. Levine, I.N. (2010), Physical Chemistry, Tata Mc Graw Hill.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

114
 DISCIPLINE SPECIFIC ELECTIVE COURSE- 6 (DSE-6): Applications of
computers in Chemistry
CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Applications of 04 03 0 01 Class 12 NIL
th

with
computers in
Physics,
Chemistry Chemistry
(DSE 6)

Learning Objectives

The Learning Objectives of this course are as follows:

To make the students learn the working of computer and its applications in chemistry via
programming language, C language and use of software as a tool to understand chemistry and solve
chemistry-based problems.

Learning outcomes

By studying this course, students will be able to:

● Use commands and library functions in programming in C language.

● Develop algorithm to solve problems and write corresponding programs in C language
for performing calculations involved in laboratory experiments.
● Use various spreadsheet software to perform theoretical calculations and plot graphs

SYLLABUS OF DSE-6

UNIT 1: Introduction to Basic Computer System (6 Hours)

Hardware and Software; Input devices, Storage devices, Output devices, Central Processing
Unit (Control Unit and Arithmetic Logic Unit); Number system (Binary, Octal and
Hexadecimal Operating System); Computer Codes (BCD and ASCII); Numeric/String
constants and variables. Operating Systems (DOS, WINDOWS, and Linux); Software
languages: Low level and High-Level languages (Machine language, Assembly language;
QBASIC, C, C++, FORTRAN 90&95); Compiled versus interpreted languages. Debugging
Software Products (Office, chemsketch, scilab, matlab, and hyperchem), internet application

115
UNIT 2: Commands and Library functions in C language (18 Hours)
C language for solving some of the basic and complicated chemistry problems). QB4 version
of C language can be used.
Numeric constants, variables & its declaration, Arithmetic expressions, hierarchy of
operations, inbuilt functions and header files. Syntax and use of the following commands in C
language: scanf, printf, fscanf and fprintf; goto, relational operators, if-else statement; while,
for and do while loops, switch-break statements; header files (<stdio.h>, <stdlib.h>, <math.h>,
<ctype.h>, <malloc.h>, <string.h>), arrays & pointers, library functions (abs & fabs, int, float,
double, ceil, char, exp, log, rand, sqrt, \t, \v, \n and trigonometric Functions), defining and
accessing functions, gnuplot- syntax and commands
Simple programs using C commands, Matrix addition and multiplication

UNIT 3: Use of C language for solving problems in Chemistry (21 Hours)

Solution of quadratic equation, polynomial equations (formula, iteration, Newton – Raphson
methods and binary bisection) with examples of polynomial equations used in chemistry;
Numerical differential, Numerical integration (Trapezoidal and Simpson’s rule), Calculation
of area under the curves for chemistry problems, e.g., entropy calculations, Simultaneous
equations, Statistical analysis-mean, variance, standard deviation, error, least square method.
Plotting linear graphs using experimental data, plotting (i)trigonometric functions-particle in a
one-dimensional box(ii) exponential function (iii) Ideal gas isotherms. Plotting van der Waals
Isotherms, and observe whether van der Waal gas equation is valid at temperatures lower than
critical temperature where we require to solve a cubic equation.

Practical Component (30 Hours)

(Laboratory periods: 15 classes of 2 hours each)
Computer programs using C language based on numerical methods
1. Simple programs to calculate numerical values of chemistry problems.
2. Roots of equations: (e.g. volume of gas using Van der Waals equation and comparison
with ideal gas, pH of a weak acid).
3. Solving polynomial equation using iterative method. (Van der Waal’s equation of state,
pH of a weak acid using exact expression)
4. Solving polynomial equation using Newton-Raphson’s method. (Van der Waal’s
equation of state, pH of a weak acid using exact expression)
5. Matrix operations: addition, multiplication and transpose
6. Numerical differentiation (e.g., change in pressure for small change in volume of a van
der Waals gas, potentiometric titrations).
7. Numerical integration using trapezoidal method. (e.g. entropy/ enthalpy change from
heat capacity data).

116
 8. Numerical integration using Simpson’s rule
9. Mean, standard deviation
10. Least square curve fitting method for linear equation.
11. Calculate the relative intensities of peaks of a proton obtained after spin-spin coupling
with 4 equivalent neighbouring protons in a high-resolution NMR spectrum using
GOSUB RETURN.
Computer programs using C language for plotting graphs
1. Van der Waals isotherm
2. Compressibility versus pressure curves
3. Maxwell distribution curves
4. Concentration-time graph using kinetics data
5. pH metric titration curve
6. Conductometric titration curves for strong acid-strong base titrations.
7. Calibration curve using Lambert Beer’s law
8. Particle in a one-dimensional box.
Note: Minimum 12 exercises is to be performed relating to C language
Plotting graphs using spreadsheet
1. Particle in a one-dimensional box.
2. van der Waals isotherms below critical temperature, at critical temperature and above
critical temperature.
3. Radial plots and radial distribution functions for orbitals of hydrogen atom.
4. Plotting characteristics graphs of zero, first and second order reactions using
concentration time data and determine the order of the reaction.
Essential/recommended readings
Theory:
1. McQuarrie, D. A. (2008), Mathematics for Physical Chemistry, University Science
Books.
2. Mortimer, R. (2005), Mathematics for Physical Chemistry,3rd Edition, Elsevier.
3. Steiner, E. (1996), The Chemical Maths Book, Oxford University Press.
4. Yates, P. (2007), Chemical Calculations, CRC Press.
5. Harris, D. C. (2007), Quantitative Chemical Analysis,6th Edition, Freeman, Chapters
3-5.
6. Rajaraman, V., Computer Programming in C, PHI Learning Private Limited.
7. Gottfried, B., Programming with C, Tata McGraw Hills Education Pvt. Ltd., 3rd Edition.
Practical:

117
 1. Levie, R.D. (2001), How to use Excel in analytical chemistry and in general
scientific data analysis, Cambridge University Press.
2. Kapoor, K.L. (2019), A Textbook of Physical Chemistry, Vol.7, 1st Edition, McGraw
Hill Education.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

118
 Bachelor of Sciences (Life Sciences)
Category II
BSc (Life Sciences) with Chemistry as one of the Core Discipline

DISCIPLINE SPECIFIC CORE COURSE -7: Chemistry -III Chemical

Energetics and Equilibria

Credit distribution, Eligibility and Pre-requisites of the Course

Course Credits Credit distribution of the Eligibility Pre-requisite

title & course criteria of the course
Code Lecture Tutorial Practical/ (if any)
Practice
Chemical 04 02 00 02 Passed Class NIL
Energetics and 12 th
with
Equilibria
Physics,
(DSC-7: Chemistry,
Chemistry 03:
Mathematics

Learning objectives

The objectives of this course are as follows:

● To develop basic understanding of the chemical energetics, laws of thermodynamics
and ionic equilibrium.
● to provides basic understanding of the behaviour of electrolytes and their solutions.
● To make students learn about the properties of ideal and real gases and deviation
from ideal behavior

Learning outcomes
By studying this course, students will be able to:
● Explain the laws of thermodynamics, thermochemistry and equilibria.
● Use the concept of pH and its effect on the various physical and chemical properties
of the compounds.
● Use the concepts learnt to predict feasibility of chemical reactions and to study
the behaviour of reactions in equilibrium

SYLLABUS

UNIT-1: Chemical Energetics (16 Hours)

Recapitulation of Intensive and extensive variables; state and path functions; Isolated, closed
and open systems

143
First law

Concept of heat (Q), work (W), internal energy (U), and statement of first law; enthalpy (H),
relation between heat capacities for ideal gas, Joule’s experiment, calculations of Q, W, ΔU
and ΔH for reversible expansion of ideal gases under isothermal conditions.

Thermochemistry

Enthalpy of reactions: standard states; enthalpy of neutralization, enthalpy of ionization

enthalpy of hydration, enthalpy of formation and enthalpy of combustion, Integral enthalpy of
solution, bond dissociation energy and bond enthalpy; Hess’s law, Born Haber’s cycle (NaCl/
KCl).

Second Law

Concept of entropy; statements of the second law of thermodynamics (Kelvin and Clausius).
Calculation of entropy change for reversible processes (for ideal gases). Free Energy Functions:
Gibbs and Helmholtz energy (Non-PV work and the work function); Free energy change and
concept of spontaneity (for ideal gases).

Third Law

Statement of third law, qualitative treatment of absolute entropy of molecules (examples of NO, CO),
concept of residual entropy

UNIT-2: Chemical Equilibrium (4 Hours)

Criteria of thermodynamic equilibrium. Free energy change in a chemical reaction and

equilibrium constant, exergenic and endergenic reactions with examples such conversion of
ATP to ADP or vice verca,, Le Chatelier’s principle, relationship between Kp, Kc and Kx for
reactions involving ideal gases.

UNIT-3: Ionic Equilibria (10 Hours)

Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of
ionization, Ostwald’s dilution law, ionization constant and ionic product of water, ionization
of weak acids and bases, Degree of ionization, pH scale, common ion effect, Buffer solutions,
Henderson-Hasselbach equation. Solubility and solubility product of sparingly soluble salts –
applications of solubility product principle

Practical Component: 60 Hours

(Laboratory periods: 15 classes of 4 hours each)
Chemical Energetics:
1. Determination of heat capacity of calorimeter.
2. Determination of enthalpy of neutralization of hydrochloric acid with sodiumhydroxide.
3. Determination of the enthalpy of ionization of acetic acid.
4. Determination of enthalpy of neutralization of acetic acid and ammonium hydroxide using Hess’s law.

144
5. Determination of integral enthalpy of solution (both endothermic and exothermic) of salts.
6. Determination of enthalpy of hydration of Copper sulphate.

Ionic equilibria:
7. Preparation of buffer solutions: (i) Sodium acetate-acetic acid or (ii) Ammonium chloride-ammonium
acetate. Measurement of the pH of buffer solutions and comparison of the values with theoretical values.

8. Study the effect of addition of HCl/NaOH on pH of the buffer solutions (acetic acid, and sodium acetate).
9. pH metric titration of strong acid with strong base,
10. pH metric titration of weak acid with strong base

References:
Theory:
1. Castellan, G. W. (2004),Physical Chemistry,Narosa.
2. Kapoor, K. L. (2015),A Textbook of Physical Chemistry,Vol 1, 6th Edition, McGraw Hill
Education.

3. Kapoor, K. L. (2015), A Textbook of Physical Chemistry, Vol 2, 6thEdition, McGraw Hill

Education.

4. Puri, B. R., Sharma, L. R. and Pathania M. S. (2020), Principles of Physical Chemistry, Vishal
PublishingCo.

Practical:
1. Khosla,B. D.;Garg,V. C.; Gulati,A.(2015), SeniorPracticalPhysicalChemistry,R.Chand&Co.
2. Kapoor, K. L. (2019), A Textbook of Physical Chemistry, Vol 7, 1st Edition, McGraw Hill
Education.

3. Batra, S. K., Kapoor, V and Gulati, S. (2017) 1st Edition, Experiments in Physical Chemistry,
Book Age series.

Additional Resources:
1. Mahan, B. H.(2013), University Chemistry,Narosa.

2. Barrow, G. M. (2006), Physical Chemistry, 5thEdition, McGrawHill.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

145
 Pool of DISCIPLINE SPECIFIC ELECTIVES (DSEs) for BSc. Life Science

DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -1:

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE-1: 04 02 00 02 Passed NIL
Chemistry of Class XII
Major and with
Minor Science
Biogenic
Elements

Learning Objectives

The Learning Objectives of this course are as follows:

● To review periodic properties of main group elements and their role in the biological
systems.
● To discuss the patterns and trends exhibited by main group elements and their
compounds with emphasis on synthesis, structure, bonding and their diverse
applications in the environment, industry and in the biological system.
● To get an insight into how these compounds such as oxides of N and S affect our day-
to-day life.
● To learn about inorganic polymeric compounds borazine, silicates, silicones,
phosphonitrilic compounds and their applications.
● To develop the interest of students in the frontier areas of inorganic and material
chemistry.

Learning outcomes

By studying this course, students will be able to:

● Explain the periodicity in atomic and ionic radii, electronegativity, ionization
enthalpy, electron gain enthalpy of elements of the periodic table.
● Explain oxidation states with reference to the existence of elements in unusual and
rare oxidation states in alkalides, carbides and nitrides.
● Explain vital role of sodium, potassium, calcium and magnesium ions etc. in
biological systems and the role of oxides of N and S in our environment.
● Predict distribution of major and minor biogenic elements in human beings

146
SYLLABUS OF CHEM-DSE 1

UNIT-1: Periodic Properties (6 Hours)

Electronic configurations of the atoms. Stability of half-filled and completely filled orbitals,
the concept of exchange energy, inert pair effect.
General group trends of main group elements with special reference to size (atomic and ionic),
Ionization Enthalpy, Electron Gain Enthalpy, Electronegativity, oxidation states (including rare
oxidation states of alkali metals, carbides and nitrides), melting and boiling points, flame
colour, metallic character and complex formation tendency (crown ethers and cryptates), Alkali
metal solutions in liquid ammonia
Distribution of major and minor biogenic elements in human beings

UNIT 2: Structure, Bonding and Properties (16 Hours)

Structure, bonding and properties: Acidic/Basic nature, stability, ionic/covalent nature,
oxidation/reduction, hydrolysis, thermal stability of the following:
Hydrides: hydrides of Group 13 (only diborane), Group 14, Group 15 (EH where E = N, P, 3

As, Sb, Bi), Group 16 and Group 17.

Oxides: Oxides of nitrogen, phosphorus and sulphur
Oxoacids: oxoacids of phosphorus, sulphur and chlorine
Halides of phosphorus
Relevance of above compounds in industrial/environmental/biological systems wherever
applicable

UNIT 3: Preparation, Properties, Structure and Uses (8 Hours)

Preparation, properties, structure and uses of the following compounds: Borazine, Silicates,
silicones, Phosphonitrilic halides {(PNCl ) where n = 3 and 4} 2 n

Practical component 60 Hours

(Laboratory periods: 15 classes of 4 hours each)
Qualitative semi-micro analysis of mixtures containing 2 anions and 2 cations (preferably 7-8
mixtures). Emphasis should be given to the understanding of the chemistry of different
reactions. The following radicals are suggested: CO , NO , S , SO , SO , S O , CH COO , 3
2-
2
- 2-
3
2-
4
2-
2 3
2-
3
-

F, Cl , Br , I- ,
- -

NO , BO , C O , PO , NH , K , Pb , Cu , Cd , Bi , Sn , Sb , Fe , Al , Cr , Zn , Mn ,
3
-
3
3-
2 4
2-
4
3-
4
+ + 2+ 2+ 2+ 3+ 2+ 3+ 3+ 3+ 3+ 2+ 2+

Co , Ni , Ba , Sr , Ca , Mg .
2+ 2+ 2+ 2+ 2+ 2+

The mixtures may contain combination of anions/one interfering anion.

Spot tests should be preferred wherever applicable.

References:
Theory:
1. Lee, J.D.; (2010), Concise Inorganic Chemistry, Wiley India.
2. Huheey, J.E.; Keiter, E.A.; Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry-
Principles of Structure and Reactivity, Pearson Education.
3. Douglas, B.E.; McDaniel, D.H.; Alexander, J.J. (1994), Concepts and Models of
Inorganic Chemistry, John Wiley & Sons.

147
 4. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010),
Shriver and Atkins, Inorganic Chemistry, 5 Edition, Oxford University Press.
th

5. Housecraft, E. H.; Sharpe, A.G. (2018), Inorganic Chemistry, 5 Edition, Pearson.

th

Practicals:
1. Vogel, A.I. (1972), Qualitative Inorganic Analysis, Longman.
2. Svehla, G. (1996), Vogel’s Qualitative Inorganic Analysis, Prentice Hall

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -2:

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Chem-DSE-2: 04 02 00 02 Passed Class NIL
XII with
Polynuclear Science
Hydrocarbons,
Pharmaceutical
Compounds,
UV- Visible &
IR
Spectroscopy

Learning Objectives

The Learning Objectives of this course are as follows:

● To introduce the chemistry and applications of polynuclear hydrocarbons and
heterocyclic compounds.
● Introduction to spectroscopy, an important analytical tool which allows identification
of organic compounds by correlating their spectra to structure.

Learning outcomes
By studying this course, students will be able to:
● Understand the fundamentals of polynuclear hydrocarbons and heterocyclic compounds
through the study of methods of preparation, properties and chemical reactions with
underlying mechanism.
● Gain insight into the basic fundamental principles of IR and UV-Vis spectroscopic
techniques.
● Use basic theoretical principles underlying UV-visible and IR spectroscopy as a tool for
functional group identification in organic molecules.

148
SYLLABUS OF CHEM-DSE-2

UNIT-1: Polynuclear Hydrocarbons (6 Hours)

Introduction, classification, uses, aromaticity of polynuclear compounds, Structure elucidation
of naphthalene, preparation and properties of naphthalene and anthracene.

UNIT-2: Pharmaceutical Compounds (12 Hours)

Introduction, classification, general mode of action of antipyretics and analgesics, aspirin;
Synthesis, uses and side effects of the following drugs:
Antipyretics - Paracetamol (with synthesis and mode of action); Analgesics- Ibuprofen (with
synthesis and overview of the mode of action); Antimalarials - Chloroquine (synthesis and
mode of action).
An elementary treatment of Antibiotics and detailed study of chloramphenicol including mode
of action. Medicinal values of curcumin (haldi), azadirachtin (neem), vitamin C and antacid
(ranitidine).

UNIT-3: UV-Visible and IR Spectroscopy (12 Hours)

UV-Visible and IR Spectroscopy and their application to simple organic molecules.
Electromagnetic radiations and their properties; double bond equivalence and hydrogen
deficiency. UV-Visible spectroscopy (electronic spectroscopy): General electronic transitions,
λ & ε , chromophores &auxochromes, bathochromic & hypsochromic shifts. Application of
max max

Woodward rules for the calculation of λ for the following systems: conjugated dienes -
max

alicyclic, homoannular and heteroannular; α, β-unsaturated aldehydes and ketones, charge

transfer complex.

Infrared (IR) Spectroscopy: Infrared radiation and types of molecular vibrations, the
significance of functional group & fingerprint region. IR spectra of alkanes, alkenes, aromatic
hydrocarbons (effect of conjugation and resonance on IR absorptions), simple alcohols (inter
and intramolecular hydrogen bonding and IR absorptions), phenol, carbonyl compounds,
carboxylic acids and their derivatives (effect of substitution on >C=O stretching absorptions).

Practical component 60 Hours

(Laboratory periods: 15 classes of 4 hours each)

1. Isolation and estimation of the amount of aspirin in a commercial tablet.

2. Preparation of Aspirin.
3. Synthesis of ibuprofen.
4. Systematic qualitative identification and derivative preparation of organic compounds
(Aromatic hydrocarbons, Aryl halides)
5. Detection of simple functional groups through examination of IR spectra (spectra to be
provided). IR spectra of simple compounds like phenols, aldehydes, ketones, carboxylic
acids may be given.
6. Differentiation between of o-/p-hydroxybenzaldehyde by IR spectroscopy (Spectra to
be provided).
7. Differentiation between benzoic acid and cinnamic acid by UV spectroscopy.
8. Diel’s Alder reaction using Anthracene and Maleic anhydride.

149
 9. Partial Reduction of m-dinitrobenzene to m-nitroaniline and then analysing the IR
spectra of reactant and Product.
10. Laboratory preparation of Paraacetamol.

References:
Theory:
1. Finar, I. L. Organic Chemistry (Volume 1 & 2), Dorling Kindersley (India) Pvt. Ltd.
(Pearson Education).
2. Morrison, R. N.; Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt.
Ltd. (Pearson Education).
3. Bahl, A; Bahl, B. S. (2012), Advanced Organic Chemistry, S. Chand.
4. Pavia, D.L. Introduction to Spectroscopy, Cengage learning (India) Pvt. Ltd.
2. Kemp, W. (1991), Organic Spectroscopy, Palgrave Macmillan.

Practicals:

1. Ahluwalia, V.K.; Dhingra, S.; Gulati, A. (2005), College Practical Chemistry,

University Press (India) Ltd.
2. Ahluwalia, V.K.; Dhingra, S. (2004), Comprehensive Practical Organic Chemistry:
Qualitative Analysis, University Press.
3. Vogel, A.I. (1972), Textbook of Practical Organic Chemistry, Prentice-Hall.
4. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I, I K
International Publishing House Pvt. Ltd., New Delhi.
5. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I, I K
International Publishing House Pvt. Ltd., New Delhi.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

150
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 3:

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 3: 04 02 0 02 Passed NIL
Computer Class XII
Applications with
in Chemistry Science

Learning Objectives

The Learning Objectives of this course are as follows:

● To introduce the students to basic computer skills that will help them in solving
chemistry problems using spreadsheets and BASIC language.
● To acquaint the students with different software for data tabulation, calculation, graph
plotting, data analysis and document preparation.
● To expose the students to the concept of molecular modelling, its applications to various
molecular systems, energy minimization techniques, analysis of Mulliken Charge and
ESP Plots.

Learning outcomes

By studying this course, students will be able to:

● Have knowledge of most commonly used commands and library functions used in
programming in C language.
● Develop algorithm to solve problems and write corresponding programs in C language
for performing calculations involved in laboratory experiments.
● Use various spreadsheet software to perform theoretical calculations and plot graphs

SYLLABUS OF CHEM-DSE-3

UNIT-1: Programming using BASIC (20 Hours)

Programming Language – Elements of BASIC language, Numeric and string Constants and
Variables, arithmetic expressions, hierarchy of operations, inbuilt functions. Syntax and use of
the various QBASIC commands: REM, CLS, INPUT, PRINT, GOTO, IF, IF…THEN,
IF..THEN..ELSE, IF and END IF, FOR and NEXT etc., DIM, READ, DATA, GOSUB,

151
RETURN, RESTORE, DEF FNR and Library Functions, Simple programs based on usage of
the commands mentioned above.
Statistical analysis using BASIC: Mean, Least square fit - Linear regression, variance, standard
deviation.

UNIT-2: Handling of Numerical Data (4 Hours)

Spreadsheet software: MS Excel. Creating a spreadsheet, entering and formatting information,
applying basic functions and formulae to the data, drawing charts, tables and graphs, displaying
the equation of graph along with the R2 value, incorporating tables and graphs in Word files,
graphical solution of equations, plotting pressure-volume curves of van der Waals gases,
Maxwell-Boltzmann distribution, concentration versus time graphs, spectral data, titration
curves, etc.

UNIT-3: Molecular Modelling (6 Hours)

Introduction to molecular modelling, overview of classical and quantum mechanical methods
(molecular mechanics, semi empirical, ab initio and DFT), general considerations and
comparison of these methods.

Practical component 60 Hours

(Laboratory periods: 15 classes of 4 hours each)
Exercises of Programing
1. Calculate pressure of a real gas using Van der Waal’s Equation.
2. Calculate the most probable speed, average speed and root men square velocity of an
ideal gas.
3. Roots of quadratic equations
4. Binomial coefficient using GOSUB statement.
5. Mean, standard deviation
6. Least square curve fitting method for linear equation.
Plotting graphs using a spreadsheet
1. van der Waals isotherms
2. Maxwell-Boltzmann distribution curves as function of temperature and molecular
weight
3. Plot the conductometric titration curve for
a) strong acid vs strong base and b) weak acid vs strong base
0. Plot the pH metric titration curve for
a) strong acid vs strong base and b) weak acid vs strong base and determine the pKa of
the weak acid
0. Plot the graphs for the kinetics of first order reaction and determine the rate constant
1. Plot the UV-vis absorbance spectra and determine the molar absorption coefficient.

152
Molecular Modelling
1. Optimize and compare the geometry parameters of H2O and H2S using Argus Lab.
2. Compare the basicities of N atom in ammonia, methylamine, dimethylamine and
trimethylamine using Argus Lab by comparing Mulliken charges and ESP map in Argus
Lab.
3. Compare C-C bond lengths and bond order in ethane, ethene and ethyne using Argus
Lab.
4. Determine enthalpy of isomerization of cis and trans-2-butene in Argus Lab.
5. Compare the HAH bond angles for the second row hydrides (BeH2, CH4, NH3, H2O) and
compare with the results from qualitative MO theory.

References:
Theory:
1. Levie, R. de. (2001), How to use Excel in analytical chemistry and in general
scientific data analysis, Cambridge Univ. Press.
2. Venit, S.M. (1996),Programming in BASIC: Problem solving with structure and
style. Jaico Publishing House.
3. Lewars, E. (2003), Computational Chemistry, Kluwer academic Publisher.
4. Cramer, C.J.(2004), Essentials of Computational Chemistry, John Wiley & Sons.
5. Hinchcliffe, A. (1996), Modelling Molecular Structures, John Wiley & Sons.
6. Leach, A.R.(2001), Molecular Modelling, Prentice-Hall.

Practicals:
1. Lewars, E. (2003), Computational Chemistry, Kluwer academic Publisher.
2. Cramer, C.J. (2004), Essentials of Computational Chemistry, John Wiley & Sons.
3. Hinchcliffe, A. (1996), Modelling Molecular Structures, John Wiley & Sons.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

153
 Bachelor of Sciences (Physical Sciences)
Category II
BSc (Physical Sciences) with Chemistry as one of the Core Discipline

DISCIPLINE SPECIFIC CORE COURSE -7: Chemistry -III Chemical

Energetics and Equilibria

Credit distribution, Eligibility and Pre-requisites of the Course

Course Credits Credit distribution of the Eligibility Pre-requisite

title & course criteria of the course
Code Lecture Tutorial Practical/ (if any)
Practice
Chemical 04 02 0 02 Passed Class NIL
Energetics and 12 th
with
Equilibria
Physics,
(DSC-7: Chemistry,
Chemistry 03:
Mathematics

Learning objectives

The objectives of this course are as follows:

● To develop basic understanding of the chemical energetics, laws of thermodynamics
and ionic equilibrium.
● to provides basic understanding of the behaviour of electrolytes and their solutions.
● To make students learn about the properties of ideal and real gases and deviation
from ideal behavior

Learning outcomes
By studying this course, students will be able to:
● Explain the laws of thermodynamics, thermochemistry and equilibria.
● Use the concept of pH and its effect on the various physical and chemical properties
of the compounds.
● Use the concepts learnt to predict feasibility of chemical reactions and to study
the behaviour of reactions in equilibrium

SYLLABUS

UNIT-1: Chemical Energetics (16 Hours)

154
Recapitulation of Intensive and extensive variables; state and path functions; Isolated, closed
and open systems

First law

Concept of heat (Q), work (W), internal energy (U), and statement of first law; enthalpy (H),
relation between heat capacities for ideal gas, Joule’s experiment, calculations of Q, W, ΔU
and ΔH for reversible expansion of ideal gases under isothermal conditions.

Thermochemistry

Enthalpy of reactions: standard states; enthalpy of neutralization, enthalpy of ionization

enthalpy of hydration, enthalpy of formation and enthalpy of combustion, Integral enthalpy of
solution, bond dissociation energy and bond enthalpy; Hess’s law, Born Haber’s cycle (NaCl/
KCl).

Second Law

Concept of entropy; statements of the second law of thermodynamics (Kelvin and Clausius).
Calculation of entropy change for reversible processes (for ideal gases). Free Energy Functions:
Gibbs and Helmholtz energy (Non-PV work and the work function); Free energy change and
concept of spontaneity (for ideal gases).

Third Law

Statement of third law, qualitative treatment of absolute entropy of molecules (examples of NO, CO),
concept of residual entropy

UNIT-2: Chemical Equilibrium (4 Hours)

Criteria of thermodynamic equilibrium. Free energy change in a chemical reaction and

equilibrium constant, exergenic and endergenic reactions with examples such conversion of
ATP to ADP or vice verca,, Le Chatelier’s principle, relationship between Kp, Kc and Kx for
reactions involving ideal gases.

UNIT-3: Ionic Equilibria (10 Hours)

Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of
ionization, Ostwald’s dilution law, ionization constant and ionic product of water, ionization
of weak acids and bases, Degree of ionization, pH scale, common ion effect, Buffer solutions,
Henderson-Hasselbach equation. Solubility and solubility product of sparingly soluble salts –
applications of solubility product principle

Practical Component: 60 Hours

(Laboratory periods: 15 classes of 4 hours each)
Chemical Energetics:
1. Determination of heat capacity ofcalorimeter.
2. Determination of enthalpy of neutralization of hydrochloric acid with sodiumhydroxide.
3. Determination of the enthalpy of ionization of acetic acid.

155
4. Determination of enthalpy of neutralization of acetic acid and ammonium hydroxide using Hess’s law.
5. Determination of integral enthalpy of solution (both endothermic and exothermic) of salts.
6. Determination of enthalpy of hydration of Copper sulphate.

Ionic equilibria:
7. Preparation of buffer solutions: (i) Sodium acetate-acetic acid or (ii) Ammonium chloride-ammonium
acetate. Measurement of the pH of buffer solutions and comparison of the values with theoretical values.

8. Study the effect of addition of HCl/NaOH on pH of the buffer solutions (acetic acid, and sodium acetate).
9. pH metric titration of strong acid with strong base,
10. pH metric titration of weak acid with strong base

References:
Theory:
1. Castellan, G. W. (2004),Physical Chemistry,Narosa.
2. Kapoor, K. L. (2015),A Textbook of Physical Chemistry,Vol 1, 6th Edition, McGraw Hill
Education.

3. Kapoor, K. L. (2015), A Textbook of Physical Chemistry, Vol 2, 6thEdition, McGraw Hill

Education.

4. Puri, B. R., Sharma, L. R. and Pathania M. S. (2020), Principles of Physical Chemistry, Vishal
PublishingCo.

Practical:
1. Khosla,B. D.;Garg,V. C.; Gulati,A.(2015), SeniorPracticalPhysicalChemistry,R.Chand&Co.
2. Kapoor, K. L. (2019), A Textbook of Physical Chemistry, Vol 7, 1st Edition, McGraw Hill
Education.

3. Batra, S. K., Kapoor, V and Gulati, S. (2017) 1st Edition, Experiments in Physical Chemistry,
Book Age series.

Additional Resources:
1. Mahan, B. H.(2013), University Chemistry,Narosa.

2. Barrow, G. M. (2006), Physical Chemistry, 5thEdition, McGrawHill.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

156
Pool of DISCIPLINE SPECIFIC ELECTIVES (DSEs) for BSC (Physical Science)

DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -1:

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credit Credit distribution of the Eligibilit Pre-

Code s course y criteria requisite
of the
Lectur Tutoria Practical/
course (if
e l
Practice any)

Chem-DSE-1: 04 02 0 02 Passed NIL

Class XII
Main Group with
Chemistry Science

Learning Objectives
The Learning Objectives of this course are as follows:

● To provide basic understanding of the fundamental principles of metallurgy through

study of the different methods of extraction and refining of metals.
● To illustrate the diversity and fascination of inorganic chemistry through
the study of structure, properties and utilities of s- and p-block elements
and their compounds.

Learning outcomes

By studying this course, students will be able to:

● Understand the basis of occurrence of metals in nature and the methods that can
be applied on minerals to extract the metals from them.
● Explain the importance of free energy of formation of oxides with the choice of
reducing agent for extracting the metals.
● Understand and explain the importance of refining of metals and the choice of a
refining procedure
● Explain the group trends observed for different properties of s and p block
elements
● Explain the structures and the bonding basis of compounds of s- and p- block
elements
● Explain the uniqueness observed in alkali metals and some other main group
elements
● Understand and explain the polymerization of inorganic ions to generate
inorganic polymers and the difference between organic and inorganic polymers.

157
Syllabus
Unit 1: General Principles of Metallurgy (6 Hours)

Chief modes of occurrence of metals based on standard electrode potentials. Ellingham

diagrams for reduction of metal oxides using carbon and carbon monoxide as reducing agent.
Electrolytic Reduction, Hydrometallurgy with reference to cyanide process for silver and gold.
Methods of purification of metals: Electrolytic process, Van Arkel-De Boer process, Zone
refining.

Unit 2: General Properties (4 Hours)

General group trends of s- and p-block elements with special reference to melting and boiling
points, flame colour, metallic character and complex formation tendency, diagonal relationship
and anomalous behaviour of first member of each group, Alkali metal solutions in liquid
ammonia
Unit 3: Structure, Bonding, Properties and Applications (16 Hours)

Structure, bonding, properties (Acidic/Basic nature, stability, ionic/covalent nature,

oxidation/reduction, hydrolysis, thermal stability) and applications of the following:
Crown Ethers and cryptates of Alkali metals
Hydrides: hydrides of Group 13 (only diborane), Group 14, Group 15 (EH3 where E = N, P, As,
Sb, Bi), Group 16 and Group 17.
Oxides: Oxides of nitrogen, phosphorus and sulphur.
Oxoacids: oxoacids of phosphorus, sulphur and chlorine
Halides of phosphorus

Unit 4: Inorganic Polymers (4 Hours)

Preparation, properties, structure and uses of the following:

Borazine, Silicates and Silicones

Practicals (60 Hours)

(Laboratory periods:60)

Qualitative semi-micro analysis of mixtures containing 2 anions and 2 cations (preferably

7-8 mixtures). Emphasis should be given to the understanding of the chemistry of different
reactions. The following radicals are suggested:

CO32-, NO2- , S2-, SO32-, SO42- , S2O32-, CH3COO-, F-, Cl-, Br-, I- , NO3- , BO33-, C2O4 2-, PO4 3-,
NH4 +, K+, Pb2+ , Cu2+, Cd2+, Bi3+, Sn2+, Sb3+, Fe3+, Al3+, Cr3+, Zn2+, Mn2+, Co2+, Ni2+, Ba2+, Sr2+,
Ca2+, Mg2+
The mixtures may contain combination of anions/one interfering anion.

158
 Spot tests should be preferred wherever applicable.

References:

Theory:

1. Lee, J.D.; (2010), Concise Inorganic Chemistry, Wiley India.

2. Huheey, J.E.; Keiter, E.A.; Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry- Principles of
Structure and Reactivity, Pearson Education.
3. Douglas, B.E.; McDaniel, D.H.; Alexander, J.J. (1994), Concepts and Models of Inorganic
Chemistry, John Wiley & Sons.
4. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010), Shriver and
Atkins Inorganic Chemistry, 5th Edition, Oxford University Press.
5. Housecraft, E. H.; Sharpe, A.G. (2018), Inorganic Chemistry, 5th Edition, Pearson.
6. F.A. Cotton & G. Wilkinson (1999), Advanced Inorganic Chemistry, 6th Edition, John Wiley &
Sons.

Practicals:

1. Vogel, A.I. (1972), Qualitative Inorganic Analysis, Longman.

2. Svehla, G. (1996), Vogel’s Qualitative Inorganic Analysis, Prentice Hall.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University
of Delhi, from time to time.

159
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -2:

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Chem-DSE-2: 04 02 0 02 Passed Class NIL
XII with
Polynuclear Science
Hydrocarbons,
Pharmaceutical
Compounds,
UV- Visible &
IR
Spectroscopy

Learning Objectives

The Learning Objectives of this course are as follows:

● To introduce the chemistry and applications of polynuclear hydrocarbons and
heterocyclic compounds.
● Introduction to spectroscopy, an important analytical tool which allows identification
of organic compounds by correlating their spectra to structure.

Learning outcomes
By studying this course, students will be able to:
● Understand the fundamentals of polynuclear hydrocarbons and heterocyclic compounds
through the study of methods of preparation, properties and chemical reactions with
underlying mechanism.
● Gain insight into the basic fundamental principles of IR and UV-Vis spectroscopic
techniques.
● Use basic theoretical principles underlying UV-visible and IR spectroscopy as a tool for
functional group identification in organic molecules.

SYLLABUS OF CHEM-DSE-2

UNIT-1: Polynuclear Hydrocarbons (6 Hours)

160
Introduction, classification, uses, aromaticity of polynuclear compounds, Structure elucidation
of naphthalene, preparation and properties of naphthalene and anthracene.

UNIT-2: Pharmaceutical Compounds (12 Hours)

Introduction, classification, general mode of action of antipyretics and analgesics, aspirin;
Synthesis, uses and side effects of the following drugs:
Antipyretics - Paracetamol (with synthesis and mode of action); Analgesics- Ibuprofen (with
synthesis and overview of the mode of action); Antimalarials - Chloroquine (synthesis and
mode of action).
An elementary treatment of Antibiotics and detailed study of chloramphenicol including mode
of action. Medicinal values of curcumin (haldi), azadirachtin (neem), vitamin C and antacid
(ranitidine).

UNIT-3: UV-Visible and IR Spectroscopy (12 Hours)

UV-Visible and IR Spectroscopy and their application to simple organic molecules.
Electromagnetic radiations and their properties; double bond equivalence and hydrogen
deficiency. UV-Visible spectroscopy (electronic spectroscopy): General electronic transitions,
λ & ε , chromophores &auxochromes, bathochromic & hypsochromic shifts. Application of
max max

Woodward rules for the calculation of λ for the following systems: conjugated dienes -
max

alicyclic, homoannular and heteroannular; α, β-unsaturated aldehydes and ketones, charge

transfer complex.

Infrared (IR) Spectroscopy: Infrared radiation and types of molecular vibrations, the
significance of functional group & fingerprint region. IR spectra of alkanes, alkenes, aromatic
hydrocarbons (effect of conjugation and resonance on IR absorptions), simple alcohols (inter
and intramolecular hydrogen bonding and IR absorptions), phenol, carbonyl compounds,
carboxylic acids and their derivatives (effect of substitution on >C=O stretching absorptions).

Practical component 60 Hours

(Laboratory periods: 15 classes of 4 hours each)

1. Isolation and estimation of the amount of aspirin in a commercial tablet.

2. Preparation of Aspirin.
3. Synthesis of ibuprofen.
4. Systematic qualitative identification and derivative preparation of organic compounds
(Aromatic hydrocarbons, Aryl halides)
5. Detection of simple functional groups through examination of IR spectra (spectra to be
provided). IR spectra of simple compounds like phenols, aldehydes, ketones, carboxylic
acids may be given.
6. Differentiation between of o-/p-hydroxybenzaldehyde by IR spectroscopy (Spectra to
be provided).
7. Differentiation between benzoic acid and cinnamic acid by UV spectroscopy.
8. Diel’s Alder reaction using Anthracene and Maleic anhydride.
9. Partial Reduction of m-dinitrobenzene to m-nitroaniline and then analysing the IR
spectra of reactant and Product.
10. Laboratory preparation of Paraacetamol.

References:
Theory:
1. Finar, I. L. Organic Chemistry (Volume 1 & 2), Dorling Kindersley (India) Pvt. Ltd.

161
 (Pearson Education).
2. Morrison, R. N.; Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt.
Ltd. (Pearson Education).
3. Bahl, A; Bahl, B. S. (2012), Advanced Organic Chemistry, S. Chand.
4. Pavia, D.L. Introduction to Spectroscopy, Cengage learning (India) Pvt. Ltd.
3. Kemp, W. (1991), Organic Spectroscopy, Palgrave Macmillan.

Practicals:

1. Ahluwalia, V.K.; Dhingra, S.; Gulati, A. (2005), College Practical Chemistry,

University Press (India) Ltd.
2. Ahluwalia, V.K.; Dhingra, S. (2004), Comprehensive Practical Organic Chemistry:
Qualitative Analysis, University Press.
3. Vogel, A.I. (1972), Textbook of Practical Organic Chemistry, Prentice-Hall.
4. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I, I K
International Publishing House Pvt. Ltd., New Delhi.
5. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I, I K
International Publishing House Pvt. Ltd., New Delhi.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

162
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 3:

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 3: 04 02 0 02 Passed NIL
Computer Class XII
Applications with
in Chemistry Science

Learning Objectives

The Learning Objectives of this course are as follows:

● To introduce the students to basic computer skills that will help them in solving
chemistry problems using spreadsheets and BASIC language.
● To acquaint the students with different software for data tabulation, calculation, graph
plotting, data analysis and document preparation.
● To expose the students to the concept of molecular modelling, its applications to various
molecular systems, energy minimization techniques, analysis of Mulliken Charge and
ESP Plots.

Learning outcomes

By studying this course, students will be able to:

● Have knowledge of most commonly used commands and library functions used in
programming in C language.
● Develop algorithm to solve problems and write corresponding programs in C language
for performing calculations involved in laboratory experiments.
● Use various spreadsheet software to perform theoretical calculations and plot graphs

SYLLABUS OF CHEM-DSE-3

UNIT-1: Programming using BASIC (20 Hours)

Programming Language – Elements of BASIC language, Numeric and string Constants and
Variables, arithmetic expressions, hierarchy of operations, inbuilt functions. Syntax and use of
the various QBASIC commands: REM, CLS, INPUT, PRINT, GOTO, IF, IF…THEN,
IF..THEN..ELSE, IF and END IF, FOR and NEXT etc., DIM, READ, DATA, GOSUB,

163
RETURN, RESTORE, DEF FNR and Library Functions, Simple programs based on usage of
the commands mentioned above.
Statistical analysis using BASIC: Mean, Least square fit - Linear regression, variance, standard
deviation.

UNIT-2: Handling of Numerical Data (4 Hours)

Spreadsheet software: MS Excel. Creating a spreadsheet, entering and formatting information,
applying basic functions and formulae to the data, drawing charts, tables and graphs, displaying
the equation of graph along with the R2 value, incorporating tables and graphs in Word files,
graphical solution of equations, plotting pressure-volume curves of van der Waals gases,
Maxwell-Boltzmann distribution, concentration versus time graphs, spectral data, titration
curves, etc.

UNIT-3: Molecular Modelling (6 Hours)

Introduction to molecular modelling, overview of classical and quantum mechanical methods
(molecular mechanics, semi empirical, ab initio and DFT), general considerations and
comparison of these methods.

Practical component 60 Hours

(Laboratory periods: 15 classes of 4 hours each)
Exercises of Programing
1. Calculate pressure of a real gas using Van der Waal’s Equation.
2. Calculate the most probable speed, average speed and root men square velocity of an
ideal gas.
3. Roots of quadratic equations
4. Binomial coefficient using GOSUB statement.
5. Mean, standard deviation
6. Least square curve fitting method for linear equation.
Plotting graphs using a spreadsheet
1. van der Waals isotherms
2. Maxwell-Boltzmann distribution curves as function of temperature and molecular
weight
3. Plot the conductometric titration curve for
a) strong acid vs strong base and b) weak acid vs strong base
4. Plot the pH metric titration curve for
a) strong acid vs strong base and b) weak acid vs strong base and determine the pKa of
the weak acid
5. Plot the graphs for the kinetics of first order reaction and determine the rate constant
6. Plot the UV-vis absorbance spectra and determine the molar absorption coefficient.
Molecular Modelling

164
 1. Optimize and compare the geometry parameters of H2O and H2S using Argus Lab.
2. Compare the basicities of N atom in ammonia, methylamine, dimethylamine and
trimethylamine using Argus Lab by comparing Mulliken charges and ESP map in Argus
Lab.
3. Compare C-C bond lengths and bond order in ethane, ethene and ethyne using Argus
Lab.
4. Determine enthalpy of isomerization of cis and trans-2-butene in Argus Lab.
5. Compare the HAH bond angles for the second row hydrides (BeH2, CH4, NH3, H2O) and
compare with the results from qualitative MO theory.

References:
Theory:
1. Levie, R. de. (2001), How to use Excel in analytical chemistry and in general
scientific data analysis, Cambridge Univ. Press.
2. Venit, S.M. (1996),Programming in BASIC: Problem solving with structure and
style. Jaico Publishing House.
3. Lewars, E. (2003), Computational Chemistry, Kluwer academic Publisher.
4. Cramer, C.J.(2004), Essentials of Computational Chemistry, John Wiley & Sons.
5. Hinchcliffe, A. (1996), Modelling Molecular Structures, John Wiley & Sons.
6. Leach, A.R.(2001), Molecular Modelling, Prentice-Hall.

Practicals:
1. Lewars, E. (2003), Computational Chemistry, Kluwer academic Publisher.
2. Cramer, C.J. (2004), Essentials of Computational Chemistry, John Wiley & Sons.
3. Hinchcliffe, A. (1996), Modelling Molecular Structures, John Wiley & Sons.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

165
 UNIVERSITY OF DELHI

CNC-II/093/1(28)/2023-24/283
Dated: 08.11.2023

NOTIFICATION

Sub: Amendment to Ordinance V

[E.C Resolution No. 14-1-6/-(6) dated 09.06.2023 and 27-1-1/-(7) dated

25.08.2023]

Following addition be made to Appendix-II-A to the Ordinance V (2-A) of the

Ordinances of the University;

Add the following:

Syllabi of Semester-IV, V and VI of the following Programmes of Department of

Chemistry under Faculty of Science based on Under Graduate Curriculum
Framework -2022 implemented from the Academic Year 2022-23 :
(i) BSc. (Hons.) Chemistry
(ii) BSc. (Physical Science) with Chemistry as one of Core Discipline
(iii) BSc. (Life Science) with Chemistry as one of the Core Discipline
(iv) BSc. (Industrial Chemistry) – Chemistry Component
(v) BSc (Hons.) Applied Life Sciences with Agrochemicals and Pest
Management.

1
 DEPARTMENT OF CHEMISTRY

SEMESTER _IV

B Sc. (Hons) Chemistry

DISCIPLINE SPECIFIC CORE COURSE - 10(DSC-10): Coordination Chemistry

and Reaction Mechanism

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title Credits Credit distribution of the course Eligibility Pre-

& Code Lecture Tutorial Practical/ criteria requisite
Practice
of the
course
(if any)
Coordination 04 03 -- 01 Class 12th --
Chemistry with
and Reaction Physics,
Mechanism Chemistry,
(DSC-10: Mathematics
Inorganic
Chemistry -
IV)
Learning Objectives

The Objectives of this course are as follows:

• To familiarize the students with coordination compounds which find manifold

applications in diverse areas.
• To acquaint the student with the concept of Inorganic reaction mechanism.
Learning Outcomes

By studying this course, the students will be able to:

• Explain the terms- ligand, denticity of ligands, chelate, coordination number and use
standard rules to name coordination compounds.
• Discuss the various types of isomerism possible in such compounds.
• Use Valence Bond Theory to predict the structure and magnetic behaviour of metal
complexes and understand the terms inner and outer orbital complexes.

2
 • Explain the meaning of the terms ∆o, ∆t, pairing energy, CFSE, high spin and low spin
complexes and how CFSE affects thermodynamic properties like lattice enthalpy and
hydration enthalpy.
• Explain magnetic properties and colour of complexes on the basis of Crystal Field
Theory.
• Explain the reaction mechanism of coordination compounds and differentiate between
kinetic and thermodynamic stability.

SYLLABUS OF DSC-10
Unit-1: Coordination Chemistry (Hours: 28)

Werner’s Coordination theory, simple problems based on this theory

IUPAC nomenclature of coordination compounds, isomerism in coordination compounds
(coordination numbers 4 and 6). Valence bond theory and its application to complexes of
coordination numbers 4 and 6.
Crystal field theory, measurement of ∆o. Calculation of CFSE in weak and strong fields,
concept of pairing energies, factors affecting the magnitude of ∆o. Octahedral vs. tetrahedral
coordination, tetragonal distortions from octahedral geometry: Jahn-Teller theorem, square
planar geometry. Qualitative aspect of Ligand field and MO Theory (for octahedral σ-donor,
π- acceptor and π- donor complexes).
Unit-2: Stability of complexes and Inorganic Reaction Mechanism: (Hours: 17)
Brief discussion of thermodynamic and kinetic stability, Factors affecting stability of
complexes, such as chelate effect, macrocyclic effect, resonance effect etc., trends in step
wise formation constant, interpretation of lability and inertness based on VBT and CFT.
Introduction to inorganic reaction mechanisms, concept of reaction pathways, transition state,
intermediate and activated complex. Substitution reactions in square planar complexes,
factors affecting the rate of Substitution reactions in square planar complexes- such as charge
effect, solvent effect and Trans- effect (Theories of trans-effect).
Practical component
Practical: Credits: 01
(Laboratory periods: 15 classes of 2 hours each)
(A) Argentometry
Estimation of Cl ̅
(i) By Mohr’s method
(ii) By Vohlard’s method and
(iii) By Fajan’s method
(B) Complexometric Titrations:
(i) Complexometric estimation of Mg2+/ Zn2+ using EDTA
(ii) Estimation of total hardness of water samples

3
(iii) Estimation of Ca2+ in solution by substitution method
(iv) Estimation of Ca/Mg in drugs or biological samples.
(C) Properties of Complexes
Synthesis of ammine complexes of Ni(II) and its ligand exchange reactions (e.g. bidentate
ligands like acetylacetone, dimethyl glyoxime, glycine) by substitution method.
Essential/recommended readings

Theory:
1. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010),
Shriver and Atkins Inorganic Chemistry, 5th Edition, Oxford University Press.
2. Miessler, G.L.; Fischer P.J.; Tarr, D. A. (2014), Inorganic Chemistry, Fifth Edition,
Pearson.
3. Huheey, J.E.; Keiter, E.A.; Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry-
Principles of Structure and Reactivity, Pearson Education.
4. Pfennig, B. W. (2015), Principles of Inorganic Chemistry, John Wiley & Sons.
5. Cotton, F.A.; Wilkinson, G.(1999), Advanced Inorganic Chemistry, Wiley-VCH.
6. Sodhi G.S. (2018), Principles of Inorganic Chemistry, Viva Books India.

Practicals:
1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of
Quantitative Chemical Analysis, John Wiley and Sons,
2. Harris, D. C.; Lucy, C. A. (2016), Quantitative Chemical Analysis, 9th Edition,
Freeman and Company.
3. Day, R. A.; Underwood, A. L. (2012), Quantitative Analysis, Sixth Edition, PHI
Learning Private Limited.
4. Marr, G.; Rockett, B.W. (1972), Practical Inorganic Chemistry, Van Nostrand
Reinhold.

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

4
 DISCIPLINE SPECIFIC CORE COURSE -11 (DSC-11): Carbohydrates, Lipids and
Heterocyclic Compounds

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title Credits Credit distribution of the Eligibility Pre-

& Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice (if any)
Carbohydra 04 03 -- 01 Class 12th --
tes, Lipids with
and Hetero Physics,
cyclic Chemistry
Compounds
(DSC-11,
Organic
Chemistry
IV)
Learning Objectives

The Objectives of this course are as follows:

• To familiarize students with the chemistry of carbohydrates, lipids, and heterocyclic
compounds
• To enable students to develop novel, efficient, convenient, selective and
environmentally benign synthetic methods for synthesis of heterocyclic compounds.

Learning outcomes

By studying this course, the students will be able to:

• Describe uses and applications carbohydrates, lipids and heterocycles
• Use the knowledge gained from study of carbohydrates, lipids and heterocycles to
propose greener and better synthetic routes.
• Use the chemistry and biology of carbohydrates, lipids and heterocycles to better serve
the mankind.

5
SYLLABUS OF DSC-11

Unit-1: Carbohydrates & Lipids (Hours: 24)

Monosaccharides: Constitution and absolute configuration of glucose and fructose, epimers
and anomers, mutarotation, determination of ring size of glucose and fructose, Haworth
projection and conformational structures; Interconversion of aldoses and ketoses; Killiani-
Fischer synthesis and Ruff degradation; Linkage between monosaccharides: Comparative
study of the structure of disaccharides (sucrose, maltose, lactose) and polysaccharides (starch,
cellulose and glycogen) excluding their structure elucidation. Reactions of disaccharides-
reducing property, hydrolysis, methylation and acetylation.
Lipids: Introduction to lipids, classification. Oils and fats: Common fatty acids present in oils
and fats, Omega-3&6 fatty acids, trans fats, hydrogenation, hydrolysis, acid value,
saponification value, iodine number. Biological importance of triglycerides, phospholipids,
glycolipids, and steroids (cholesterol).
Unit-2: Heterocyclic Compounds (Hours:21)
Classification and nomenclature of heterocyclic compounds (containing only one hetero atom).
Structure, aromaticity in 5-membered and 6-membered rings containing one heteroatom;
Basicity and relative reactivity towards electrophilic substitution reactions (amongst five
membered and six membered rings.
General methods of synthesis for: furan, thiophene, pyrrole (Paal-Knorr synthesis, Hantzsch
synthesis), pyridine (Hantzsch synthesis), indole (Fischer Indole synthesis), quinoline (Skraup
synthesis, Friedlander’s synthesis, Knorr quinoline synthesis, Doebner-Miller synthesis)
Properties: Physical properties, discussion on the following reaction (with mechanism) for
furan, pyrrole, thiophene, pyridine, indole and quinoline: Electrophilic substitution- nitration,
sulphonation, halogenation, formylation, acylation, mercuration and carboxylation. Oxidation,
reduction, addition, reactions showing acidic /basic character, reaction with diazonium salts,
ring opening, ring expansion and nucleophilic substitution reaction wherever applicable should
be discussed.
Practical: Credits: 01
(Laboratory periods: 15 classes of 2 hours each)
1. Estimation of sugars by using Fehling solution.
2. Functional group tests for amine, nitro and amides.
3. Determination of saponification value of the given oil.
4. Determination of iodine number of the given oil.
5. Systematic qualitative analysis of the given organic compounds containing monofunctional
groups (carboxylic acids, carbonyl compounds, carbohydrates and esters) and preparation
of one suitable derivative.
Essential/recommended readings

6
Theory:
1. Berg, J.M., Tymoczko, J.L., Stryer, L. (2019), Biochemistry, 9th Edition W.H. Freeman
and Co.
2. Nelson, D.L., Cox, M.M., Lehninger, A.L. (2017), Principles of Biochemistry. W.H.
Freeman and Co., International Edition.
3. Morrison, R. N., Boyd, R. N., Bhattacharjee, S.K. (2010), Organic Chemistry, 7th
Edition, Dorling Kindersley (India) Pvt. Ltd., Pearson Education.
4. Parashar, R.K., Negi, B. (2016) Chemistry of Heterocyclic Compounds, Ane Books
Pvt Ltd.
5. Kuashik, S., Singh, A. (2023), Biomolecules: From Genes to Proteins, Ist Edition,
Berlin, Boston: De Gruyter.
6. Finar, I.L., (2012), Organic Chemistry Volume 1, 6th Edition, Pearson Education.
7. Singh J, Awasthi S K, Singh J, Fundamentals of Organic Chemistry, Pragati
Prakashan Meerut.
Practical:

1. Vogel, A.I. (2012), Quantitative Organic Analysis, Part 3, Pearson Education.

2. Mann, F.G., Saunders, B.C. (2009), Practical Organic Chemistry, Pearson Education.
3. Ahluwalia, V.K., Dhingra, S. (2004), Comprehensive Practical Organic Chemistry:
Qualitative Analysis, University Press.
4. Ahluwalia, V.K., Aggarwal, R. (2004), Comprehensive Practical Organic
Chemistry: Preparation and Quantitative Analysis, University Press
5. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–I, I K
International Publishing house Pvt. Ltd, New Delhi
6. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–II, I K
International Publishing house Pvt. Ltd, New Delhi
Note: Examination scheme and mode shall be as prescribed by the Examination
Branch, University of Delhi, from time to time.

7
 DISCIPLINE SPECIFIC CORE COURSE-12 (DSC-12): Electrochemical Cells,
Chemical Kinetics and Catalysis

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Electrochemical 04 03 -- 01 Class 12th --
Cells, Chemical with
Kinetics and Physics,
Catalysis Chemistry,
(DSC-12, Mathematics
Physical
Chemistry IV)
Learning Objectives
The Objectives of this course are as follows:
• To provide a detailed understanding about galvanic cells and their types
• To explain the applications of galvanic cells and EMF measurements.
• To get an understanding of the kinetics of simple and complex chemical reactions
• To give basic concept about catalysts and enzymes.
• To teach the working of potentiometer and different electrodes for performing
potentiometric titrations
• To explain the experimental study of kinetics of simple reactions
Learning outcomes
By studying this course, the students will be able to:

• Explain the working of electrochemical cells and different types of galvanic cell.
• Devise a spontaneous galvanic cell using various combinations of half-cells.
• Understand the concept of concentration cell
• Use the appropriate galvanic cell to measure pH, calculate thermodynamic parameters
and perform potentiometric titrations.
• Write rate law and derive rate equations for simple and complex reactions and
understanding of theories of reaction rates.
• Understand different types of catalysts and mechanism of enzyme catalysis.
• Perform potentiometric titrations using appropriate electrodes for quantitative analysis.
• Set up experiments to study the kinetics of simple reactions.
SYLLABUS OF DSC-12
Unit-1: Electrochemical Cells (Hours: 21)

8
Rules of oxidation/reduction of ions based on half-cell potentials, Chemical cells, reversible
and irreversible cells with examples. Electromotive force of a cell and its measurement,
Nernst equation; Standard electrode (reduction) potential and its application to different kinds
of half-cells. Application of EMF measurements in determining (i) free energy, enthalpy and
entropy of a cell reaction, (ii) equilibrium constants, and (iii) pH values, using hydrogen,
quinone-hydroquinone, glass and SbO/Sb2O3 electrodes. Concentration cells with and
without transference, liquid junction potential; determination of activity coefficients and
transference numbers. Qualitative discussion of potentiometric titrations (acid-base, redox,
precipitation). Structure of electric double layer (qualitative aspects only).

Unit-2: Chemical Kinetics (Hours: 18)

Order and molecularity of a reaction, rate laws in terms of the advancement of a reaction,
differential and integrated form of rate expressions up to second order reactions, experimental
methods for determination of rate laws, kinetics of complex reactions (integrated rate
expressions up to first order only): (i) Opposing reactions (ii) parallel reactions and (iii)
consecutive reactions and their differential rate equations (steady-state approximation in
reaction mechanisms) (iv) chain reactions.
Temperature dependence of reaction rates; Arrhenius equation; activation energy. Collision
theory of reaction rates, Lindemann mechanism, qualitative treatment of the theory of
absolute reaction rates, introduction to electrode kinetics (qualitative aspects only).
Unit-3: Catalysis: (Hours: 6)
Types of catalyst, specificity and selectivity, mechanisms of catalyzed reactions at solid
surfaces. Enzyme catalysis, Michaelis-Menten mechanism, acid-base catalysis.
Practical: Credits: 01
(Laboratory periods: 15 classes of 2 hours each)
(A) Potentiometry:
Perform the following potentiometric titrations:
1. Strong acid vs. strong base
2. Weak acid vs. strong base
3. Dibasic acid vs. strong base
4. Mixture of strong and weak acid vs strong base
5. Potassium dichromate vs. Mohr's salt
(B) Chemical Kinetics:
Study the kinetics of the following reactions
1. Iodide-persulphate reaction by Initial rate method
2. Acid hydrolysis of methyl acetate with hydrochloric acid.
3. Saponification of ethyl acetate by conductometric measurements.
Suggested experiments

9
 1. To study the kinetics of Iodide-persulphate reaction using integrated rate method.
2. Comparison of the strengths of HCl and H2SO4 by studying kinetics of hydrolysis of
methyl acetate.
Essential/recommended readings
Theory:
1. Atkins, P.W.; Paula, J.de. (2014), Atkin’s Physical Chemistry Ed., 10th Edition,
Oxford University Press.
2. Ball, D. W. (2017), Physical Chemistry, 2nd Edition, Cengage Learning, India.
3. Castellan, G. W. (2004), Physical Chemistry, 4th Edition, Narosa.
4. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, Vol 3, 6th Edition, McGraw
Hill Education.
5. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, Vol 5, 3rd Edition, McGraw
Hill Education.
6. Laidler K.J. (2003), Chemical Kinetics, 3rd Edition, Pearson Education India.
Practical:
1. Khosla, B.D.; Garg, V.C.; Gulati, A. (2015), Senior Practical Physical Chemistry, R.
Chand & Co, New Delhi.
2. Kapoor, K.L. (2019), A Textbook of Physical Chemistry, Vol.7, 1st Edition, McGraw
Hill Education.
3. Garland, C. W.; Nibler, J. W.; Shoemaker, D. P. (2003), Experiments in Physical
Chemistry, 8th Edition, McGraw-Hill, New York
Note: Examination scheme and mode shall be as prescribed by the Examination
Branch, University of Delhi, from time to time.

10
 SEMESTER-V
BSC. (HONS.) CHEMISTRY

DISCIPLINE SPECIFIC CORE COURSE -13 (DSC-13): Basics of Organometallic

Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Basics of 04 03 -- 01 Class 12th -
Organometallic with
Chemistry (DSC- Physics,
13)-Inorganic Chemistry,
Chemistry-V Mathematics
Learning Objectives

The Objectives of this course are as follows:

• To familiarize the students with the interactions of metal atom with organic molecules
(or not so typical organic molecule), which is in an entirely different fashion as
compared to coordination compounds.
• To familiarize the students with the structure and bonding in organometallic compounds
• To familiarize the student with how organometallic compounds can act as good
catalysts for organic transformations and hencehave industrial importance associated
with medicines, bioorganic synthesis, and energy production.
Learning Outcomes

By studying this course, the students will be able to:

• Identify and classify organometallic compounds of different types.

• Explain the stability of organometallic compounds and hence the requirement of special
experimental conditions for their synthesis.
• Explain the bonding modes through VBT and MOT in these compounds.
• Explain the chemical nature of these compounds through various reactions thus
acquiring skills to understand their applications.
• Explain the mechanism of catalysis by these compounds. This may prepare the student
to predict the catalytic pathways for new reactions

SYLLABUS OF DSC-13
Unit-1: Introduction to Organometallic Chemistry (Hours: 6)

11
Definition, brief history, classification of organometallic compounds on the basis of bond
type. Common notation used in organometallic chemistry, concept of hapticity of organic
ligands, importance of organometallic chemistry, organometallic compounds as reagents,
additives, and catalysts. Introduction to the 18-electron rule or effective atomic number rule,
electron count of mononuclear, polynuclear and substituted metal carbonyls of 3d series and
finding metal-metal bonds.
Unit-2: Structure and Bonding in Organometallic Compounds ( Hours : 12)
Structures of mononuclear and binuclear carbonyls of Cr, Mn, Fe, Co and Ni using VBT.
Molecular orbital theory applied to organometallic compounds, description of bonding of two
electron ligands to transition metals. π-acceptor behavior of CO (MO diagram of CO to be
discussed), π-bonding of CO with metal (synergic effect) and use of IR data to explain extent
of back bonding, bonding modes of CO, symmetry of metal carbonyls.
Bonding between metal atoms and organic π- systems: linear (ethylene, allyl, butadiene) and
cyclic (cyclopentadiene, benzene), Zeise’s salt and comparison of synergic effect with that in
carbonyls.
Metal alkyls and Metal-carbene complexes
Unit-3: Synthesis, Reactions and Applications of Organometallic Compounds (Hours:
16)
General methods of synthesis of metal carbonyls: direct carbonylation, reductive
carbonylation, thermal and photochemical decomposition, of mono and binuclear carbonyls
of 3d series.
Reaction of metal carbonyls: reduction, oxidation, photochemical substitution, migratory
insertion of carbonyls, and nucleophilic addition of CO.
Synthesis of metal-alkene complexes through ligand addition, reduction and substitution and
reaction of metal bound alkenes, Zeise’s salt
Metal–sandwich compounds: Ferrocene: synthesis, physical properties and reactions:
acylation, sulfonation, alkylation metallation, acetylation, chloromercuration, Mannich
reaction, comparison of aromaticity and reactivity of ferrocene with that of benzene.
Synthesis and reactions of Metal alkyls and Metal-carbenes
Unit-4: Catalysis by Organometallic Compounds (Hours: 11)
General principles of catalysis, properties of catalysts, homogeneous and heterogeneous
catalysis. (Catalytic steps, examples and industrial applications), deactivation and
regeneration of catalysts, (catalytic poisons and promoter).
Organometallic catalysis of the following reactions of commercial importance and their
mechanism:
1. Alkene hydrogenation (using Wilkinson’s Catalyst)
2. Synthetic gasoline preparation (Fischer Tropsch reaction)
3. Polymerisation of ethene using Ziegler-Natta catalyst
4. Wacker oxidation process (Smidth process)
5. Hydroformylation reaction (Oxo-process)
6. Monsanto Acetic Acid process
Theoretical aspects of enlisted practicals are also to be included in the theory paper.
Practical component
Practical: Credits: 01
(Laboratory periods: 15 classes of 2 hours each)

12
 1. To study and compare the UV-Vis spectrum of ferrocene (in methanol or acetonitrile)
and potassium ferrocyanide (in water).
2. To study the cyclic voltammogram of ferrocene.
3. Preparation of Bis(acetylacetonato)copper(II) complex and characterisation through
UV-Visible spectrum of its aqueous solution..
4. Preparation of tris(acetylacetonato)manganese(III) complex.
5. Preparation of Potassium tris(oxalato)ferrate(III) complex.
6. Preparation of Tetraamminecopper(II) sulphate monohydrate complex.
7. Preparation of Pentaamminechloridocobalt(III) chloride.
8. Preparation of Hexaamminecobalt(III) chloride
9. Determination of number of chloride ions in ionisation sphere to confirm the formula
of complexes prepared in (6) and (7) through potentiometric titration or conductance
measurements. (See reference 5 & 6 of Practicals)
10. Compare and interpret the visible spectrum of complexes prepared in (6) and (7) for
shifts in wavelength maxima.

Any other organometallic compounds synthesised from time to time may also be
included.

Essential/recommended readings
Theory:

1. Gary L Miesler, Paul J Ficsher, and Donald A Tarr, Inorganic Chemistry 5th Edition
, Pearson.
2. Shriver & Atkins Inorganic Chemistry, Edn V, W.H. Freeman and Company.
3. F.A. Cotton & G. Wilkinson, Advanced Inorganic Chemistry, 5th Edition.
4. William W. Porterfield, Inorganic Chemistry, Ist Edition.
5. Huheey, J.E.; Keiter, E.A., Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry-
Principles of Structure and Reactivity, Pearson Education.
6. Principles of Organometallic Chemistry by M.L.H Green, Coward, G.E Coates and
K.Wade 3rd Edition.
7. Cotton, F.A.; Wilkinson, G.; Gaus, P.L. Basic Inorganic Chemistry, 3rd Edition, Wiley
India.
8. Greenwood, N.N.; Earnshaw, A. (1997), Chemistry of the Elements, 2nd Edition,
Elsevier.
9. Gupta, B. D., Elias, A. J., (2013) Basic Organometallic Chemistry: Concepts,
Syntheses and Applications, 2nd Edition, Universities Press.
Practicals:
1. ChemTexts (2020) 6:22, https://doi.org/10.1007/s40828-020-00119-6
2. J. Chem Education: 1971, Volume 48(2), 133
3. Front. Chem. Sci. Eng. 2013, 7(3): 329–337, DOI 10.1007/s11705-013-1339-0
4. Orbital: Electron. J. Chem. 2019, 11 (6): 348-354

13
 6. Vogel’s text book of quantitative chemical analysis. Edn V

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

14
DISCIPLINE SPECIFIC CORE COURSE - 14 (DSC-14): Nucleic Acids, Amino Acids,
Proteins and Enzymes

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the course Eligibility Pre-requisite
Code Lecture Tutorial Practical/ criteria of the course
Practice (if any)
Nucleic Acids, 04 02 -- 02 Class 12th --
Amino Acids, with
Proteins and Physics,
Enzymes Chemistry
(DSC-14,
Organic
Chemistry- V)
Learning Objectives
The objectives of this course are as follows:
• To familiarize students with the fascinating chemistry and biology of biomolecules,
i.e., nucleic acids and proteins etc..
• To develop the interest of students in the basic concepts of heredity, which are
imparted through replication, transcription, and translation processes.
• To discuss basic fundamentals of enzyme action and inhibition, which forms the basis
of drug action.

Learning outcomes

By studying this course, the students will be able to:

• Demonstrate how structure of biomolecules determines their reactivity and biological
role.
• Gain insight into concepts of heredity through the study of genetic code, replication,
transcription, and translation
• Demonstrate basic understanding of enzyme action and role of inhibitors
• Use knowledge gained to solve real world problems.

SYLLABUS OF DSC-14

Unit-1: Nucleic Acids (Hours: 8)

Structure of components of nucleic acids: Bases, Sugars, Nucleosides and Nucleotides.

Nomenclature of nucleosides and nucleotides, structure of polynucleotides (DNA and RNA)
and factors stabilizing them, biological roles of DNA and RNA; Concept of heredity: Genetic
Code, Replication, Transcription and Translation.

15
Unit-2: Amino Acids, Peptides and Proteins (Hours: 14)
Amino acids and their classification; α-amino acids - Synthesis, ionic properties, and
reactions. zwitterions, pKa values, isoelectric point, and electrophoresis; Study of peptides:
determination of their primary structure-end group analysis; Synthesis of peptides using N-
protecting, C-protecting and C-activating groups, Solid-phase synthesis; Overview of
primary, secondary and tertiary structures of proteins, protein denaturation.
Unit-3: Enzymes (Hours: 8)
Introduction, classification, and characteristics of enzymes. Salient features of active site of
enzymes. Mechanism of enzyme action (taking trypsin as an example), factors affecting
enzyme action, coenzymes, and cofactors (including ATP, NAD, FAD), specificity of enzyme
action (including stereospecificity). Enzyme inhibitors and their importance, phenomenon of
inhibition (competitive, uncompetitive, and non-competitive inhibition including allosteric
inhibition).
Practical component
Practical: Credits: 02
(Laboratory periods: 15 classes of 4 hours each)
1. Study of the titration curve of glycine.
2. Estimation of glycine by Sorenson Formol Titration
3. Qualitative analysis of proteins- Ninhydrin test, Biuret test, Millon’s reagent test,
Xanthoproteic test.
4. Estimation of proteins by Lowry’s method.
5. Study of the action of salivary amylase on starch at room temperature.
6. Effect of temperature on the action of salivary amylase.
7. Effect of pH on the action of salivary amylase
8. Study the inhibition of α-Amylase by copper sulphate
9. Isolation and estimation of DNA using cauliflower/onion.

Essential/recommended readings
Theory:
1. Berg, J.M., Tymoczko, J.L., Stryer, L. (2019), Biochemistry, Nineth Edition W.H.
Freeman and Co.
2. Nelson, D.L., Cox, M.M., Lehninger, A.L. (2017), Principles of Biochemistry. W.H.
Freeman and Co., International Edition.
3. Murray, R.K., Granner, D.K., Mayes, P.A., Rodwell, V.W. (2009), Harper’s Illustrated
Biochemistry. Lange Medical Books/McGraw-Hill.
4. Brown, T.A. (2018), Biochemistry, (First Indian Edition) Viva Books.
5. Kuashik, S., Singh, A. (2023), Biomolecules: From Genes to Proteins, First Edition,
Berlin, Boston: De Gruyter.
6. Voet, D., Voet, J.G. (2010), Biochemistry, Fourth Edition, Wiley.

16
 7. Singh J, Awasthi S K, Singh J, Fundamentals of Organic Chemistry, Pragati
Prakashan Meerut.

Additional Resources:
1. Finar, I.L. (2008), Organic Chemistry, Volume 2, Fifth Edition, Pearson Education.
2. Bruice, P.Y. (2020), Organic Chemistry, Egighth Edition, Pearson Education.

Practicals:
1. Manual of Biochemistry Workshop (2012), Department of Chemistry, University of
Delhi.
2. Kumar, A., Garg, S., Garg, N. (2015), Biochemical Tests: Principles and Protocols.
Viva Books.
3. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–II, I K
International Publishing house Pvt. Ltd, New Delhi
Note: Examination scheme and mode shall be as prescribed by the Examination
Branch, University of Delhi, from time to time.

17
 DIS

DISCIPLINE SPECIFIC CORE COURSE-15 (DSC-15): Quantum Chemistry and

Organic Chemistry IV Covalent bonding

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the course Eligibility Pre-requisite
Code Lecture Tutorial Practical/ criteria of the course
Practice (if any)
Quantum 04 03 -- 01 Class 12th
Chemistry and with Physics,
Covalent Chemistry,
bonding Mathematics
(DSC-15,
Physical
Chemistry V)
Learning objectives
The objectives of this course are as follows:
• To make students understand the limitations of classical mechanics and the need of
quantum chemistry
• To familiarize the students with the postulates of quantum chemistry
• To explain how to apply the postulates to derive equations for various models and
extend to hydrogen atom and hydrogen like atoms.
• To explain the valence bond and molecular orbital theories and their applications to
simple molecules
• To explain the use of some computational software
Learning outcomes
By studying this course, students will be able to:
• Explain the limitations of classical mechanics and solution in terms of quantum
mechanics for atomic/molecular systems.
• Develop an understanding of quantum mechanical operators, quantization, probability
distribution, uncertainty principle
• Set up Schrodinger equations for different types of systems
• Explain the concept of covalent bonding based on valence bond theory and molecular
orbital theory.
• Perform calculations using different software and plot different wavefunctions and
probability distribution curves.
• Perform simple calculations using appropriate quantum mechanical methods in
different computational software
SYLLABUS OF DSC-15
Unit-1: Quantum Chemistry (Hours: 22)

18
Postulates of quantum mechanics, quantum mechanical operators and commutation rules,
Schrödinger equation and its application to free particle and particle in a box rigorous
treatment), quantization of energy levels, zero-point energy and Heisenberg Uncertainty
principle; wave functions, probability distribution functions, nodal properties, Extension to
two and three- dimensional boxes, separation of variables, degeneracy.
Qualitative treatment of simple harmonic oscillator model of vibrational motion: Setting up
of Schrödinger equation and discussion of solution and wave functions. Vibrational energy
of diatomic molecules and zero-point energy.
Angular momentum. Rigid rotator model of rotation of diatomic molecule. Schrödinger
equation in Cartesian and spherical polar coordinates (derivation not required). Separation of
variables. Spherical harmonics. Discussion of solution (Qualitative).
Unit-2: Hydrogen atom (Hours: 08)
Qualitative treatment of hydrogen atom and hydrogen-like ions: setting up of Schrödinger
equation in spherical polar coordinates, radial part and quantization of energy (only final
energy expression). Average and most probable distances of electron from nucleus. Zeeman
effect, Introduction of spin quantum number and magnetic spin quantum number Setting up
of Schrödinger equation for many electron atoms (He, Li), Indistinguishability of electrons
and Pauli exclusion principle, Need for approximation methods. Statement of variation
theorem and application to simple systems (particle-in-a-box, harmonic oscillator, hydrogen
atom).
Unit-3: Covalent bonding (Hours: 15)
Setting up of Schrödinger equation, Born-Openheimer approximation, LCAO-MO treatment
of H2+ and its qualitative extension to H2, Valence bond (VB) treatment of H2, Comparison of
LCAO-MO and VB wave functions of H2 and their refinements, Qualitative description of
LCAO-MO of homonuclear and heteronuclear diatomic molecules-HF and LiH.
Practical component
Practical: Credits: 01
(Laboratory periods: 15 classes of 2 hours each)
1. Plot the radial wavefunctions and probability distribution for H atom's 1s, 2s, 2p orbital
using software like EXCEL.
2. Using a software such as ArgusLab, plot HOMO, LUMO and ESP maps of various
molecules.
3. Draw probability plots for a particle in a 1-dimensional box for different values of
quantum number n - commenting on the number of points of zero probability and then
correlate them with the correspondence principle.
4. Plot the electron density contour maps of sigma molecular orbitals for diatomic
homonuclear molecules.
5. Plotting of the wave function and probability curve for simple harmonic motion and
interpret the results for first two levels.

19
 6. Plotting energy as a function of distance for simple harmonic motion - parabolic curve.
7. Using software such as ArgusLab calculate properties such as dipole moment and
Mulliken charges using quantum mechanical methods.
Note: Any other suitable software may also be used .
Essential/recommended readings
Theory:
1. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, McGraw Hill Education,
Vol 4, 5th Edition, McGraw Hill Education.
2. House, J.E. (2004), Fundamentals of Quantum Chemistry, 2nd Edition, Elsevier.
3. McQuarrie, D.A. (2016), Quantum Chemistry, Viva Books.
4. Chandra, A. K. (2001), Introductory Quantum Chemistry, Tata McGraw-Hill.
5. House, J.E. (2004), Fundamentals of Quantum Chemistry, 2nd Edition, Elsevier
Suggested Readings
1. Atkins, P.W.; Friedman, R. (2010), Molecular Quantum Mechanics, 5th Edition,
Oxford University Press.
Practical:
1. McQuarrie, D. A. Mathematics for Physical Chemistry University Science Books
(2008).
2. Mortimer, R. Mathematics for Physical Chemistry. 3rd Ed. Elsevier (2005).
3. Steiner, E. The Chemical Maths Book Oxford University Press (1996).
4. Yates, P. Chemical Calculations. 2nd Ed. CRC Press (2007).
5. Levie, R. de, How to use Excel in analytical chemistry and in general scientific
data analysis, Cambridge Univ. Press (2001) 487 pages.
6. Noggle, J. H. Physical Chemistry on a Microcomputer. Little Brown & Co. (1985).
Note: Examination scheme and mode shall be as prescribed by the Examination
Branch, University of Delhi, from time to time.

20
 SEMESTER-VI

BSC. (HONS.) CHEMISTRY

DISCIPLINE SPECIFIC CORE COURSE -16 (DSC-16): Principles in Qualitative

Analysis and Bioinorganic Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the course Eligibility Pre-
Code criteria requisite

Lecture Tutorial Practical/ of the

course
Practice
(if any)

Principles in 04 02 -- 02 Class 12th --

Qualitative with
Analysis and Physics,
Bioinorganic Chemistry,
Chemistry Mathematics

(DSC-16:
Inorganic
Chemistry -VI)

Learning Objectives

The Objectives of this course are as follows:

• To discuss the principles of qualitative analysis

• To understand the concept of solubility products and the common ion effect on the
separation of cations.
• To discuss the importance of metal ions in biological systems.
• To discuss the applications of iron in physiology, including iron transport and storage.

Learning Outcomes:

21
By the end of the course, the students will be able to:

• Explain the basic principles of qualitative inorganic analysis.

• Discuss the influence of solubility products and the common ion effect on the separation
of cations.
• Discuss the identification of interfering anions and their removal.
• Explain and discuss the importance of metal ions in biological systems, through
discussions on
metal-containing enzymes, the sodium-potassium pump.
• Discuss the applications of iron in physiology, including iron transport and storage
system.

Unit-1: Theoretical Principles in Qualitative Analysis (Hours: 12)

Basic principles involved in analysis of cations and anions. Solubility product, common-ion
effect. Principles involved in separation of cations into groups and choice of group reagents.
Interfering anions (fluoride, borate, oxalate and phosphate), need to remove them after Group
II and methods of removal. Analysis of insoluble substances.

Unit-2: Bioinorganic Chemistry (Hours: 18)

Metal ions present in biological systems, classification of elements according to their action in
biological system. Geochemical effect on the distribution of metals. Sodium / potassium pump,
conduction of nerve impulses, Ca-pump, carbonic anhydrase and carboxypeptidase. Excess and
deficiency of some trace metals. Toxicity of metal ions (Hg, Pb, Cd and As), reasons for
toxicity, Use of chelating agents in medicine, Cisplatin as an anti-cancer drug.

Iron and its application in bio-systems, Haemoglobin, Myoglobin, cytochrome-C-oxidase ;

Storage and transfer of iron.

Practical: Credits: 02

(Laboratory periods: 15 classes of 4 hours each)

(A) Qualitative semi-micro analysis of mixtures containing 3 anions and 3 cations.

Emphasis should be given to the understanding of the chemistry of different reactions.
The following radicals are suggested:
CO32-, NO2-, S2-, SO32-, SO42-, S2O32-, CH3COO-, F-, Cl-, Br-, I-, NO3-, BO33-, C2O42-,
PO43-, NH4+, K+, Pb2+, Cu2+, Cd2+, Bi3+, Sn2+, Sb3+, Fe3+, Al3+, Cr3+, Zn2+, Mn2+, Co2+,
Ni2+, Ba2+, Sr2+, Ca2+, Mg2+

(B) Mixtures should preferably contain one interfering anion, or insoluble component
(BaSO4, SrSO4, PbSO4, CaF2 or Al2O3) or combination of anions e.g. CO32- and SO32-,
NO2- and NO3-, Cl-and Br-, Cl- and I-, Br- and I-, NO3- and Br-, NO3- and I-. Spot tests
should be done whenever possible.

22
Essential/recommended readings

1. Svehla, G. (1996), Vogel’s Qualitative Inorganic Analysis,7th Edition, Prentice Hall.

2. Huheey, J.E.; Keiter, E.A., Keiter; R. L.; Medhi, O. K. (2009), Inorganic Chemistry
Principles of Structure and Reactivity, Pearson Education.
3. Lippard, S.J.; Berg, J.M. (1994), Principles of Bioinorganic Chemistry, Panima
Publishing Company.
4. Biological Inorganic Chemistry by RR Crichton in additional books
5. Bioinorganic Chemistry- Inorganic Elements in the Chemistry of Life: An Introduction
and Guide, 2nd Edition by Wolfgang Kaim, Brigitte Schwederski, Alex Klein
6. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010), 5th
Edition, Oxford University Press.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

DISCIPLINE SPECIFIC CORE COURSE – 17 (DSC-17): Polynuclear Hydrocarbons,

Photochemistry, Pericyclic Reactions, and Spectroscopy of Organic Compounds

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Code Credits Credit distribution of the Eligibility Pre-
course criteria requisite of
the course
(if any)
Lecture Tutorial Practical/

Practice

Polynuclear 04 03 -- 01 Class 12th -

Hydrocarbons, with
Photochemistry, Physics,
Pericyclic Reactions, Chemistry
and Spectroscopy of
Organic Compounds
(DSC-17, Organic
Chemistry-VI)

23
Learning objectives

The objectives of this course are as follows:

• To provide thorough knowledge of the chemistry of polynuclear hydrocarbons .

• To detail the basic principles and applications of pericyclic reactions and
photochemistry
• To familiarize students with the various tools and techniques for identifying and
characterizing the organic compounds through their interactions with electromagnetic
radiations viz. UV-Visible, IR and NMR spectroscopy.

Learning outcomes
By studying this course, students will be able to:

• Discuss and use the chemistry of polynuclear hydrocarbons for application in real world
problems.
• Discuss and use the pericyclic reactions and photochemistry for research and other
applications.
• Use spectroscopic techniques to determine structure and stereochemistry of known and
unknown compounds.

SYLLABUS OF DSC-17
Unit-1: Polynuclear Hydrocarbons (Hours: 6)

Introduction, classification, structure, nomenclature and uses. Aromaticity of polynuclear

hydrocarbons, structure elucidation of Naphthalene and general methods of preparation of
naphthalene and anthracene (including Haworth method, Friedel Craft acylation, Diels Alder
reaction, Elbs reaction). Relative reactivity of naphthalene and anthracene in comparison to
benzene.

Discussion on the following reactions (with mechanism) for Naphthalene and Anthracene:
Addition reactions, Oxidation, Electrophilic substitution- Friedel Craft reaction,
Chloromethylation, Halogenation, Formylation, Nitration and sulphonation. Reduction reaction
and Diels Alder reaction.

Unit-2: Photochemistry and Pericyclic reactions (Hours: 12)

Photochemistry

Introduction and basic principles of photochemistry, photochemical energy, photolytic

cleavage, photochemistry of carbonyl compounds (Norrish type 1, Norrish type 2 and Peterno
Buchi reactions)

24
Pericyclic Reactions

Introduction: Types of pericyclic reactions (Electrocyclic, Cycloaddition and Sigmatropic

Rearrangements), Symmetry in σ and π molecular orbitals, Frontier Molecular Orbitals.

Electrocyclic Reactions: Conrotatory and Disrotatory motion in ring opening and ring closing
reactions in (4n) and (4n+2) π electron systems, FMO method, Woodward Hoffmann rule.

Cycloaddition Reactions: [2+2] and [4+2] π cycloaddition reactions, Diels Alder reaction
(electron rich and electron poor dienes and dienophiles, Stereochemistry, Alder rule of endo
addition).

Sigmatropic Reactions: [1,3], [1,5] and [3,3] sigmatropic rearrangements, Cope rearrangement,
Claisen Rearrangements.

Unit-3: Spectroscopy of Organic Compounds (Hours: 27)

UV-Visible Spectroscopy: Types of electronic transitions, λmax, chromophores and

Auxochromes, bathochromic and hypsochromic shifts, intensity of absorption, factors
affecting λmax values, application of Woodward Rules for calculation of λmax for the following
systems: α, β-unsaturated aldehydes, ketones, carboxylic acids and esters; conjugated dienes:
alicyclic, homoannular and heteroannular; Extended conjugated systems (aldehydes, ketones
and dienes); distinction between cis and trans isomers by UV; Colour concept, Theory of colour
and constitution-Witt’s theory, valence bond and molecular orbital theory.

IR Spectroscopy: Fundamental and non-fundamental molecular vibrations; IR absorption

positions of O and N containing functional groups; effect of H-bonding, conjugation, resonance
and ring size on IR absorptions; fingerprint region and its significance, application of IR in
functional group analysis.
1
H-NMR Spectroscopy: Basic principles of proton magnetic resonance, chemical shift and
factors, influencing it; equivalent and non-equivalent protons (chemical and magnetic
equivalence), Spin–Spin coupling and coupling constant; Anisotropic effects in alkene, alkyne,
aldehydes and aromatics. Interpretation of NMR spectra of simple compounds containing AX,
AX2, AX3, A2X3 spin systems, special case of 1-nitropropane.

Applications of IR, UV and 1H-NMR Spectroscopy for identification of simple organic

compounds (spectra to be provided for some representative compounds).

Practical component

Practical: Credits: 01

(Laboratory periods: 15 classes of 2 hours each)

1. Systematic qualitative analysis of the given organic compounds containing

monofunctional groups (Aryl halides, nitro compounds, amines and amides) and simple

25
 bifunctional compounds like salicylic acid, cinnamic acid, p-nitro phenol etc. and
preparation of one suitable crystalline derivative.
2. Differentiation between of o-/p-hydroxybenzaldehyde by IR spectroscopy (Spectra to
be provided).
3. Differentiation between of benzoic acid and cinnamic acid by UV spectroscopy
(Spectra to be provided).

Essential/recommended readings

Theory:
1. Morrison, R. N., Boyd, R. N., Bhattacharjee, S.K. (2010), Organic Chemistry, 7th
Edition, Dorling Kindersley (India) Pvt. Ltd., Pearson Education.
2. Finar, I.L. Organic Chemistry Volume 1, Dorling Kindersley (India) Pvt. Ltd.,
Pearson Education.
3. Finar, I.L. Organic Chemistry Volume 2, Dorling Kindersley (India) Pvt. Ltd.,
Pearson Education.
4. Solomons, T.W.G., Fryhle, C.B.; Snyder, S.A. (2017), Organic Chemistry, 12th
Edition, Wiley.
5. Silverstein R.M. (2005), Spectrometric Identification of organic compounds, 7th
edition, John Wiley and Sons,
6. Kemp W. (2019), Organic Spectroscopy, Third Edition, MacMillan.
7. Pavia, D. (2015), Introduction to Spectroscopy, Fifth Edition, Cengage Learning
India Pvt. Learning.
8. Scheinmann, F., Introduction to spectroscopic methods for identification of organic
compounds, Volume 2, Pergamon Press.
9. Ahluwalia, V.K., Parashar, R.K. (2011), Organic Reaction Mechanisms, 4th Edition,
Narosa Publishing House.
10. Horspool, W.M. (1976) Aspects of Organic Photochemistry, Academic Press.
11. Singh J, Awasthi S K, Singh J, Fundamentals of Organic Chemistry, Pragati
Prakashan Meerut.

Practical:
1. Vogel, A.I. (2012), Quantitative Organic Analysis, Part 3, Pearson Education.
2. Mann, F.G., Saunders, B.C. (2009), Practical Organic Chemistry, Pearson Education.
3. Furniss, B.S., Hannaford, A.J., Smith, P.W.G., Tatchell, A.R. (2012), Vogel's
Textbook of Practical Organic Chemistry, Fifth Edition, Pearson.
4. Ahluwalia, V.K., Dhingra, S. (2004), Comprehensive Practical Organic Chemistry:
Qualitative Analysis, University Press.
5. Ahluwalia, V.K., Aggarwal, R. (2004), Comprehensive Practical Organic
Chemistry: Preparation and Quantitative Analysis, University Press
6. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–I, I K
International Publishing house Pvt. Ltd, New Delhi
7. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–II, I K
International Publishing house Pvt. Ltd, New Delhi

26
 DISCIPLINE SPECIFIC CORE COURSE-18 (DSC-18): Photochemistry and
Spectroscopy

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
of the
course (if
Lecture Tutorial Practical/
any)
Practice

Photochemistry 04 02 - 02 Class XII

and Spectroscopy with Physics,
Chemistry
(DSC-18, and
Physical Mathematics
Chemistry VI)

Learning Objectives:

The Learning Objectives of this course are as follows:

• To make students understand the laws of photochemistry and their applications

• To understand the basis of molecular spectroscopy
• To study different types of spectroscopic techniques and their applications

Learning Outcomes:

By studying this course, students will be able to:

• Explain low and high quantum yield

• Explain photosensitized reactions
• Apply the concept of quantization to spectroscopy.
• Interpret various types of spectra and know about their application in structure
elucidation
SYLLABUS OF DSC-18

Unit-1: Introduction to Molecular Spectroscopy and Photochemistry (Hours: 6)

Interaction of electromagnetic radiation with molecules and various types of spectra; Born
Oppenheimer approximation.

27
Characteristics of electromagnetic radiation. Lambert-Beer’s law and its limitations, physical
significance of absorption coefficients. Laws of photochemistry, quantum yield, actinometry,
examples of low and high quantum yields, photochemical equilibrium and the differential rate
of photochemical reactions, photosensitized reactions, quenching. Role of photochemical
reactions in biochemical processes, photostationary states, chemiluminescence.

Unit-2: Rotational, Vibrational , Raman and Electronic Spectroscopy (Hours: 14)

Rotational spectroscopy: Selection rules, intensities of spectral lines, determination of bond

lengths of diatomic molecules, isotopic substitution, classification of molecules based on
moment of inertia, applications of rotation spectroscopy (e.g. microwave appliances)

Vibrational spectroscopy: Classical equation of vibration, computation of force constant,

amplitude of diatomic molecular vibrations, anharmonicity, Morse potential, dissociation
energies, fundamental frequencies, overtones, hot bands, degrees of freedom for polyatomic
molecules, modes of vibration, concept of group frequencies.

Vibration-rotation spectroscopy: diatomic vibrating rotator, P, Q, R branches.

Raman spectroscopy: Qualitative treatment of Rotational Raman effect; effect of nuclear spin,
Vibrational Raman spectra, Stokes and anti-Stokes lines; their intensity difference, rule of
mutual exclusion.

Electronic spectroscopy

Franck-Condon principle, electronic transitions, singlet and triplet states, Jablonski diagrams,
fluorescence and phosphorescence, dissociation and predissociation, calculation of electronic
transitions of polyenes using free electron model.

Unit-3: NMR and ESR (Hours: 10)

Nuclear Magnetic Resonance (NMR) spectroscopy: Principles of NMR spectroscopy, Larmor

precession, chemical shift and low-resolution spectra, different scales (δ and Ƭ), spin-spin
coupling and high resolution spectra, interpretation of PMR spectra of simple organic
molecules like methanol, ethanol and acetaldehyde.

Principles of ESR spectroscopy, hyperfine structures, ESR of simple radicals

Practical component

Practical: Credits: 02

(Laboratory periods: 15 classes of 4 hours each)

(A) Colorimetry :

1. Verify Lambert-Beer’s law and determine the concentration of (i) CuSO4 (ii) KMnO4
(iii) K2Cr2O7 in a solution of unknown concentration

28
 2. Determine the concentrations of KMnO4 and K2Cr2O7in a mixture.
3. Study the kinetics of iodination of propanone in acidic medium.
4. Determine the amount of iron present in a sample using 1,10-phenathroline.
5. Determine the dissociation constant of an indicator (phenolphthalein).
6. Study the kinetics of interaction of crystal violet/ phenolphthalein with sodium
hydroxide
(B) UV/Visible spectroscopy:

1. Study the 200-500 nm absorbance spectra of KMnO4 and K2Cr2O7 (in 0.1 M H2SO4)
and determine the λmax values. Calculate the energies of the two transitions in different
units (J molecule-1, kJ mol-1, cm-1, eV).
2. Study the pH-dependence of the UV-Vis spectrum (200-500 nm) of K2Cr2O7.
3. Record the 200-350 nm UV spectra of the given compounds (acetone, acetaldehyde,
2- propanol, acetic acid) in water. Comment on the effect of structure on the UV spectra
of organic compounds.
(C) Analysis of the given vibration-rotation spectrum of HCl(g)
Essential/recommended readings

Theory:

1. Banwell, C.N.; McCash, E.M. (2006), Fundamentals of Molecular Spectroscopy,

Tata McGraw- Hill.
2. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, McGraw Hill Education,
Vol 4, 5th Edition, McGraw Hill Education.
3. Kakkar, R. (2015), Atomic & Molecular Spectroscopy, Cambridge University Press.

Suggested Readings:

1. Engel, T.; Reid, P. (2013), Quantum Chemistry and Spectroscopy, Pearson

Practical:

1. Khosla, B.D.; Garg, V.C.; Gulati, A. (2015), Senior Practical Physical Chemistry,
R. Chand & Co, New Delhi.
2. Garland, C. W.; Nibler, J. W.; Shoemaker, D. P. (2003), Experiments in Physical
Chemistry, 8th Edition, McGraw-Hill, New York
3. Kapoor, K.L. (2019), A Textbook of Physical Chemistry, Vol.7, 1st Edition,
McGraw Hill Education.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

29
 POOL OF DSE FOR III/IV/V/VI SEMESTER

DISCIPLINE SPECIFIC ELECTIVE COURSE - 1 (DSE-1): Inorganic

Materials of Industrial Importance
CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE
COURSE
Course title Credits Credit distribution of the course Eligibility Pre-requisite
& Code Lecture Tutorial Practical/ criteria of the course
Practice (if any)
Inorganic 04 03 -- 01 Class 12th --
Materials with
of Physics,
Industrial Chemistry
Importance
(DSE-1)

Learning Objectives
The objectives of this course are as follows:
• To make students understand the diverse roles of inorganic materials in the industry
and to give an insight into how these raw materials are converted into products used in
day-to-day life.
• To make students learn about silicates, fertilizers, surface coatings,
batteries, engineering materials for mechanical construction.
• To develop the interest of students in the frontier areas of inorganic and material
chemistry.

Learning outcomes
By studying this course, the students will be able to:

• State the composition and applications of the different kinds of glass.

• State the composition of cement and discuss the mechanism of setting of cement.
• Defend the suitability of fertilizers for different kinds of crops and soil.
• Explain the process of formulation of paints and the basic principle behind the
protection offered by the surface coatings.
• Describe the principle, working and applications of different batteries.
• Evaluate the synthesis and properties of nano-dimensional materials, various
semiconductor and superconductor oxides.

SYLLABUS OF DSE-1

Unit 1: Silicate Industries ( 6 Hours

30
Glass: Glassy state and its properties, classification (silicate and non-silicate glasses).
Manufacture and processing of glass. Composition and properties of the following types of
glasses: Soda lime glass, lead glass, armoured glass, different types of safety glass, borosilicate
glass, fluorosilicate glass, coloured glass, photosensitive glass, photochromic glass, glass wool
and optical fibre.

Cement: Manufacture of Portland cement and the setting process, Different types of
cements: quick setting cements, eco-friendly cement (slag cement), pozzolana cement.

Unit 2: Fertilizers ( 6 Hours)

Different types of fertilizers (N, P and K). Importance of fertilizers, chemistry involved in the
manufacture of the following fertilizers: urea, calcium ammonium nitrate, ammonium
phosphates, superphosphate of lime and potassium nitrate.

Unit 3: Surface Coatings ( 18 Hours

Brief introduction to and classification of surface coatings, paints and pigments: formulation,
composition and related properties, pigment volume concentration (PVC)and critical pigment
volume concentration (CPVC), fillers, thinners, enamels and emulsifying agents. Special
paints: heat retardant, fire retardant, eco-friendly paints, plastic paints, water and oil paints.
Preliminary methods for surface preparation, metallic coatings (electrolytic and electroless
with reference to chrome plating and nickel plating), metal spraying and anodizing.

Contemporary surface coating methods like physical vapor deposition, chemical vapor
deposition, galvanising, carburizing, sherardising, boriding, nitriding and cementation.

Unit 4: Batteries (9 Hours)

Primary and secondary batteries, characteristics of an Ideal Battery, principle, working,
applications and comparison of the following batteries: Pb- acid battery, Li-metal batteries, Li-
ion batteries, Li-polymer batteries, solid state electrolyte batteries, fuel cells, solar cells and
polymer cells.
Unit 5: Nano dimensional materials (6 Hours)
Introduction to zero, one and two-dimensional nanomaterial: Synthesis, properties and
applications of fullerenes, carbon nanotubes, carbon fibres, semiconducting and
superconducting oxides.

Practical component

Practicals: Credits:
01 (Laboratory periods:15 classes of 2 hours each)

(At least four experiments to be performed)

1. Detection of constituents of Ammonium Sulphate fertilizer (Ammonium and Sulphate ions)

by qualitative analysis and determine its free acidity.

31
2. Detection of constituents of CAN fertilizer (Calcium, Ammonium and Nitrate ions)
fertilizer and estimation of Calcium content.

3. Detection of constituents of Superphosphate fertilizer (Calcium and Phosphate ions) and

estimation of phosphoric acid content.

4. Analysis of (Cu, Ni) in alloy or synthetic samples (methods involving Gravimetry and
Spectrophotometry).

5. Analysis of (Cu, Zn) in alloy or synthetic samples (Multiple methods involving Iodometry,
and Potentiometry).

6. Synthesis of pure ZnO and Cu doped ZnO nanoparticles.

7. Synthesis of silver nanoparticles by green and chemical approach methods and its
characterization using UV-visible spectrophotometer

Essential/recommended readings
Theory:

1. West, A. R. (2014),Solid State Chemistry and Its Application, Wiley

2. Smart, L. E.; Moore, E. A. (2012),Solid State Chemistry An Introduction, CRC Press
Taylor & Francis.
3. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong,
F.A.(2010),Shriver and Atkins Inorganic Chemistry, W. H. Freeman and Company.
4. Kent, J. A. (ed) (1997), Riegel’s Handbook of Industrial Chemistry, CBS Publishers,
New Delhi.
5. Poole Jr.; Charles P.; Owens, Frank J.(2003), Introduction to Nanotechnology, John
Wiley and Sons.

Practical:

1. Svehla, G.(1996),Vogel’s Qualitative Inorganic Analysis, Prentice Hall.

2. Banewicz, J. J.; Kenner, C.T. Determination of Calcium and Magnesium in
Limestones and Dolomites, Anal. Chem., 1952, 24 (7), 1186–1187.
3. Ghorbani, H. R.; Mehr, F.P.; Pazoki, H.; Rahmani B. M. Synthesis of ZnO
Nanoparticles by Precipitation Method. Orient J Chem 2015;31(2).
4. Orbaek, W.; McHale, M.M.; Barron, A.R. Synthesis and characterization of silver
nanoparticles for an undergraduate laboratory, J. Chem. Educ. 2015, 92, 339−344.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

32
 DISCIPLINE SPECIFIC ELECTIVE COURSE – 2 (DSE-2): Green Chemistry in Organic
Synthesis

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE

COURSE

Course Credits Credit distribution of the Eligibility Pre-requisite

title & course criteria of the course
Code Lecture Tutorial Practical/ (if any)
Practice
Green 04 03 -- 01 Class 12th Basic
Chemistry with Physics, knowledge
in Organic Chemistry of organic
Synthesis reactions
(DSE-2)

Learning objectives

The objectives of this course are as follows:

• To create awareness about the chemistry that is not harmful for human health and the
environment.
• To provide thorough knowledge of the green chemistry principles that can be used to
develop chemistry in greener way.
• To familiarize students with new remediation technologies for the cleaning up of
hazardous substances.
• To use green chemistry for boosting profits, increase productivity and ensure
sustainability with absolute zero waste.
• To learn about innovations and applications of green chemistry in education that helps
companies to gain environmental benefits as well as to achieve economic and societal
goals also
• The objective of the practical component is to develop basic skills to be able to design,
develop and run chemical processes in a sustainable way.

Learning outcomes

By studying this course, students will be able to:

• List the twelve principles of green chemistry and build the basic understanding of
toxicity, hazard and risk related to chemical substances.
• Calculate atom economy, E-factor and relate them in all organic synthesis
• State the uses of catalyst over stoichiometric reagents
• Debate and use green solvents, renewable feedstock, and renewable energy sources for
carrying out safer chemistry
• Use green chemistry for problem solving, innovation and finding solutions to
environmental problems.

33
 • Design safer processes, chemicals, and products through understanding of inherently
safer design (ISD)
• Discuss the success stories and use real-world cases to practice green chemistry

SYLLABUS OF DSE-2

UNIT – 1: Introduction (3 Hours

Introduction to Green Chemistry, some important environmental laws, pollution prevention Act
of 1990, emergence of green chemistry, need for Green Chemistry. Goals of Green Chemistry.
Limitations/ Obstacles in the pursuit of the goals of Green Chemistry. Green chemistry in
sustainable development.

UNIT – 2: Application of Green Chemistry Principles (36 Hours

Principles of Green Chemistry and designing a chemical synthesis

Concept familiarization and application of green chemistry principles using specific examples
1. Prevention of waste/ by products; waste or pollution prevention hierarchy
2. Green metrics to assess greenness of a reaction: Calculation of atom economy of the
rearrangement, addition, substitution, and elimination reactions; calculation of E-factor
for industrial processes
3. Prevention/ minimization of hazardous/ toxic products
4. Safer Solvent and Auxiliaries: Problems associated with conventional reaction media
Some Common Green solvents: Introduction, application, advantages, and disadvantages
of green solvents in organic synthesis (taking suitable examples). Special emphasis on the
following:
i. Super Critical Fluids (with special reference to carbon dioxide)
ii. Water: Concept of In-water, and on-water reactions (with special reference to synthesis
of terpinol and linalool in water, Benzoin condensation, Heck reaction)
iii. Ionic Liquids: Physical properties and classification of Ionic Liquids (with special
reference to Diels Alder reaction and Coumarin synthesis in ionic liquids)
iv. Biomass derived Solvents: Physicochemical properties, Use of glycerol and its
derivatives (Mizoroki–Heck reaction) and 2-methyltetrahydrofuran (Suzuki–Miyaura
reaction).
5. Design for energy efficiency: Phenomenon of accelerating organic reactions by using the
following Green Chemistry tools (taking suitable examples) and its advantages:
i. Mechanochemistry
ii. Ultrasound assisted reactions: Taking examples like Simmons Smith reaction, Diels–
Alder reaction,
iii. Microwave assisted reactions: Special emphasis on solvent-free synthesis- copper
phthalocyanine and aspirin, In-water reactions-Hofmann Elimination, methyl benzoate to
benzoic acid and Decarboxylation reaction;
iv. Electrocatalysis: Taking examples like adiponitrile synthesis, synthesis of 3-
bromothiophene.
v. Visible light induced Reactions: with examples such as, syntheses of caprolactam and
vitamin D3, cis-trans isomerization of alkenes
6. Use of renewable starting materials: Illustrate with few examples such as biodiesel,
bioethanol, polymers from renewable resources (PLA from corn), Synthesis and

34
 properties of 2-Methyltetrahydrofuran, furfural and 5-Aminolevulinic acid (DALA)
from levulinic acid
7. Avoidance of unnecessary derivatization – careful use of blocking/protecting groups
(taking specific examples like selective oxidation of aldehydic group and synthesis of
6-Aminopenicillanic Acid (6-APA) from penicillin G
8. Catalysis and green chemistry
Introduction to Catalysis (including concept of selectivity, turnover frequency and
turnover number), Types of Catalysts: Heterogeneous catalysis and homogeneous
catalysis (H-beta and zeolites in organic synthesis), General catalytic cycle for
heterogeneous catalysis; Asymmetric catalysis (Monsanto route to L-dopa via
asymmetric hydrogenation, synthesis of carbapenhem via Asymmetric reduction);
Photocatalysis (with special reference to TiO2); Biocatalysis (Synthesis of adipic
acid/catechol using biocatalyst) and Nanocatalysis (oxazole synthesis using
nanocatalyst)
9. Design for degradation: (Illustrate with the help of examples: soaps and detergents,
pesticides, polymers)
10. Real Time monitoring of chemical processes using inline, offline, and online techniques
11. Inherently safer design/chemistry:
Principle and subdivision of ISD, Bhopal Gas Tragedy (safer route to carbaryl) and
Flixiborough accident (safer route to cyclohexanol, Asahi Process)

UNIT – 3: Industrial Applications and Success Stories (6 Hours)

• Vitamin C Synthesis using enzymes (Hoffman La Roche)

• Zoloft -Presidential Chemistry Award Winning Innovation (Pfizer)
• Methyl Methacrylate syngas process (Eastman Chemicals)
• Synthesis of herbicide disodium iminodiacetate
• Rightfit pigments azo dyes synthesis and their applications
• Healthier Fats and oils by Green Chemistry: Enzymatic Interesterification for
production of No Trans-Fats and Oils.
• Synthesis of anti-tuberculosis drug Paramycin from waste water stream

Practical component Credits:

01 (Laboratory periods:15 classes of 2 hours each)

Note: Characterization by melting point, UV-Visible spectroscopy, IR spectroscopy and any

other specific method should be done (wherever applicable).
1. Preparation and characterization of nanoparticles of gold using tea leaves/silver
nanoparticles using plant extracts.
2. Preparation of biodiesel from waste cooking oil and characterization (TLC, pH,
solubility, combustion test, density, viscosity, gel formation at low temperature and IR
can be provided).
3. Benzoin condensation using thiamine hydrochloride as a catalyst instead of cyanide.
4. Extraction of D-limonene from orange peel using liquid CO2 prepared from dry ice.
5. Mechanochemical solvent free, solid-solid synthesis of azomethine using p-toluidine
and o-vanillin/p-vanillin.
6. Microwave-assisted Knoevenagel reaction using anisaldehyde, ethylcyanoacetate and
ammonium formate.

35
 7. Photoreduction of benzophenone to benzopinacol in the presence of sunlight.
8. Photochemical conversion of dimethyl maleate to dimethyl fumarate (cis-trans
isomerisation)
9. Benzil- Benzilic acid rearrangement: Preparation of benzilic acid in solid state under
solvent-free condition.
10. Preparation of dibenzalacetone by cross aldol condensation reaction using base
catalysed green method.

Essential/recommended readings
Theory:
1. Anastas, P.T., Warner, J.C. (2014), Green Chemistry, Theory and Practice, Oxford
University Press.
2. Lancaster, M. (2016), Green Chemistry: An Introductory Text, 3rd Edition, RSC
Publishing.
3. Cann, M. C., Connely, M.E. (2000), Real-World cases in Green Chemistry,
American Chemical Society, Washington.
4. Matlack, A.S. (2010), Introduction to Green Chemistry, 2nd Edition, Boca Raton:
CRC Press/Taylor & Francis Group publisher.
5. Alhuwalia,V.K., Kidwai, M.R. (2005), New Trends in Green chemistry, Anamalaya
Publishers.
6. Sidhwani, I.T, Sharma, R.K. (2020), An Introductory Text on Green Chemistry,
Wiley India Pvt Ltd.

Practicals:
1. Kirchoff, M.; Ryan, M.A. (2002), Greener approaches to undergraduate chemistry
experiment, American Chemical Society, Washington DC.
2. Sharma, R.K.; Sidhwani, I.T.; Chaudhari, M.K. (2013), Green Chemistry
Experiments: A monograph, I.K. International Publishing House Pvt Ltd. New Delhi.
3. Pavia, D.L.; Lamponam, G.H.; Kriz, G.S.W. B. (2012), Introduction to organic
Laboratory Technique- A Microscale approach, 4th Edition, Brooks-Cole Laboratory
Series for Organic chemistry.
4. Sidhwani I.T. (2015), Wealth from Waste: A green method to produce biodiesel from
waste cooking oil and generation of useful products from waste further generated. DU
Journal of Undergraduate Research and Innovation, 1(1),131-151. ISSN: 2395-
2334.
5. Sidhwani, I.T; Sharma, R.K. (2020), An Introductory Text on Green Chemistry,
Wiley India Pvt Ltd.
6. Monograph on Green Chemistry Laboratory Experiments, Green Chemistry Task
Force Committee, Department of Science and Technology, Government of India.
7. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–I, I K
International Publishing house Pvt. Ltd, New Delhi
8. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume–II, I K
International Publishing house Pvt. Ltd, New Delhi

36
 DISCIPLINE SPECIFIC ELECTIVE COURSE -3(DSE-3): Solu�ons, Colliga�ve proper�es,
Phase Equilibria and adsorp�on

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE

COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
th
Solutions, 04 03 - 01 Class 12
Colligative with
properties, Phase Physics,
Equilibria and Chemistry
adsorption
(DSE-3)

Learning Objectives

The Learning Objectives of this course are as follows:

• To make the students understand the various properties of dilute solutions.
• To make the students understand the thermodynamic basis of colligative properties.
• To explain the concept of phase, co-existence of phases, phase diagram for various
types of system, CST and distribution law.
• To introduce the concept of adsorption, its dependence on various conditions and
applications

Learning outcomes

By studying this course, students will be able to:

• Explain different types of phase equilibrium, draw a well labelled phase diagram.
• Predict the existence of a substance in a given phase under different conditions of
temperature and pressure
• Apply the concepts of phase, solutions and distribution law while studying other
chemistry courses and every-day life processes.
• Explain the type of adsorption that can take place in different systems and predict the
conditions to get maximum adsorption.

SYLLABUS OF DSE-3

UNIT-1: Solutions and Colligative Properties (12 Hours

37
Dilute solutions; lowering of vapour pressure, Raoult’s law, Henry’s law. Thermodynamic basis
of the colligative properties - lowering of vapour pressure, elevation of Boiling Point,
Depression of Freezing point and Osmotic pressure and derivation of expressions for these
using chemical potential. Application of colligative properties in calculating molar masses of
normal, dissociated and associated solutes in solutions, van’t Hoff factor and its applications.
Concept of activity and activity coefficients.

UNIT-2: Phase Equilibria (24 Hours)

Concept of phases, components and degrees of freedom, derivation of Gibbs Phase Rule for
nonreactive and reactive systems; Clausius-Clapeyron equation and its applications to solid-
liquid, liquid-vapour and solid-vapour equilibria, phase diagram for one component systems
(H2O and S), with applications. A comparison between the phase diagram of CO2 and H2O.
Phase diagrams for systems of solid-liquid equilibria involving eutectic, congruent and
incongruent melting points, solid solutions (excluding partial miscibility). Binary solutions:
Gibbs-Duhem-Margules equation, its derivation and applications to fractional distillation of
binary miscible liquids (ideal and non-ideal), Konovalov’s laws, azeotropes, lever rule, partial
miscibility of liquids, CST, miscible pairs, steam distillation. Nernst distribution law: its
derivation and applications.
Three component systems, water-chloroform-acetic acid system, triangular plots.

UNIT-3: Surface chemistry (9 Hours

Physical adsorption, chemisorption, adsorption isotherms (Langmuir and Freundlich). Nature

of adsorbed state. Multilayer adsorption, BET equation derivation, thermodynamic treatment
of adsorption-Gibbs equation.

Practical component Credit: 01

(Laboratory periods: 15 classes of 2 hours each)
Practical

Phase Equilibrium

1. Determination of critical solution temperature and composition at CST of the phenol

water system
2. To study the effect of impurities of sodium chloride and succinic acid on the CST of
phenol-water system.
3. To study the cooling curves for the following systems:
(i) simple eutectic
(ii) congruently melting systems.

Adsorption

Verify the Freundlich and Langmuir isotherms for adsorption of acetic acid on activated
charcoal.

Essential/recommended readings

38
Theory:
1. Peter, A.; Paula, J. de. (2011), Physical Chemistry, 9th Edition, Oxford University
Press.
2. Castellan, G. W. (2004), Physical Chemistry, 4th Edition, Narosa.
3. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, Vol 3, 6th Edition, McGraw
Hill Education.
4. Kapoor, K.L. (2015),A Textbook of Physical Chemistry, Vol 5, 6th Edition, McGraw
Hill Education.
5. Ball, D. W. (2017), Physical Chemistry, 2nd Edition, Cengage Learning, India.

Practical:
1. Khosla, B.D.; Garg, V.C.; Gulati, A. (2015), Senior Practical Physical Chemistry, R.
Chand & Co, New Delhi.
2. Garland, C. W.; Nibler, J. W.; Shoemaker, D. P. (2003), Experiments in Physical
Chemistry, 8th Edition, McGraw-Hill, New York.

Suggestive readings

1. Levine, I.N. (2010), Physical Chemistry, Tata Mc Graw Hill.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

39
 DISCIPLINE SPECIFIC ELECTIVE COURSE -4 (DSE-4): Nuclear and
Environmental Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE

COURSE
Course title & Credits Credit distribution of the Eligibility Pre-
Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Nuclear and 04 03 -- 01 Class 12th --
Environmental with
Chemistry Physics,
(DSE-4) Chemistry

Learning Objectives

The Objectives of this course are as follows:

• To make students know more about nuclear chemistry

• To familiarise the students about environmental chemistry, especially with respect to
air and water

Learning outcomes

By studying this course, the students will be able to:

• Gain knowledge about Nuclear chemistry, radioactive decay, nuclear disasters, and
nuclear waste and their disposal.
• Describe the composition of air, various air pollutants, effects and control measures of
air pollutants.
• List different sources of water, water quality parameters, impacts of water pollution,
water treatment.
• Identify different industrial effluents and their treatment methods.

SYLLABUS OF DSE-4

Unit-1 : Nuclear Chemistry (21 Hours

40
The nucleus: subatomic particles, e liquid drop model; forces in nucleus-mesons; stability of
nucleus-n/p ratio, binding energy; radioactive elements.
Radioactive decay- α-decay, β-decay, γ-decay; neutron emission, positron emission; unit of
radioactivity (curie); half life period; radioactive displacement law, radioactive series.
Measurement of radioactivity: ionization chamber, Geiger Counters, Scintillation counters.
Nuclear reactions: Nuclear fission-theory of nuclear fission; chain reaction; nuclear fusion;
nuclear reactors-fast breeder reactors, fuels used in nuclear reactors, separation of isotopes,
moderators, coolants; nuclear reactors in India.
Applications: Dating of rocks and minerals, carbon dating, neutron activation analysis, isotopic
labeling studies, nuclear medicine- 99mTc radio pharmaceuticals.
Nuclear disasters – Chernobyl disaster, Three Mile Island Disaster, Disposal of nuclear waste
and its management.

UNIT – 2: Air Pollution (12 Hours

Major regions of atmosphere, chemical and photochemical reactions in atmosphere. Air

pollutants: types, sources, particle size and chemical nature, Major sources of air pollution,
Pollution by SO2, CO2, CO, NOx, H2S and other foul-smelling gases, methods of estimation of
CO, NOx, SOx and control procedures.

Chemistry and environment impact of the following: Photochemical smog, Greenhouse effect,
Ozone depletion

Air pollution control, Settling Chambers, Venturi Scrubbers, Electrostatic Precipitators (ESPs).

UNIT – 3 : Water Pollution: (12

Hours)

Hydrological cycle, water resources, aquatic ecosystems, Sources and nature of water
pollutants, Techniques for measuring water pollution, Impacts of water pollution on
hydrological cycle and ecosystems. Water purification methods. Effluent treatment plants
(primary, secondary and tertiary treatment).

Sludge disposal. Industrial waste management, incineration of waste. Water treatment and
purification (reverse osmosis, electro dialysis, ion-exchange). Water quality parameters for
wastewater, industrial water and domestic water.

Practical component
Practical: Credits: 01
(Laboratory periods:15 classes of 2 hours each)
(At least four experiments to be performed)

1. Determination of dissolved oxygen in a given sample of water.

2. Determination of Chemical Oxygen Demand (COD) in a given sample of water.
3. Determination of Biological Oxygen Demand (BOD) in a given sample of water.

41
4. Measurement of chloride, sulphate and salinity of water samples by simple titration
method (AgNO3 and potassium chromate).
5. Estimation of total alkalinity of water samples (CO32-, HCO3-) using double titration
method.
6. Measurement of dissolved CO2 in a given sample of water.
7. Determination of hexavalent Chromium Cr(VI) concentration in tannery wastes/ waste
water sample using UV-Vis spectrophotometry technique.

Essential/recommended readings

Theory:

1. Stanley E. Manahan, 10th edition, Environmental chemistry, CRC Press, Taylor and
Francis Group, US, 2017
2. Baird, C. and Cann, M., Environmental Chemistry,(2012), Fifth Edition, W. H.
Freemann & Company, New York, US.
3. VanLoon, G.W. and Duffy, J.S.( 2018) Environmental Chemistry - A global
perspective, Fourth Edition, Oxford University Press
4. Brusseau, M.L.; Pepper,I.L. and Gerba, C., (2019) Environmental and Pollution
Science, Third Edition, Academic Press.
5. Masters, G.M., (1974) Introduction to Environmental Science and Technology, John
Wiley & Sons.
6. Masters, G.M., (2015) Introduction to Environmental Engineering and Science.
JPrentice Hall India Learning Private Limited.
1. 7.Arnikar, H.J., (1987), Second Edition, Essentials of Nuclear Chemistry, Wiley
Blackwell Publishers
7. Arnikar, H.J.; Rajurkar, N. S.,(2016) Nuclear Chemistry through Problems, New Age
International Pvt. Ltd.
8. De, A.K.(2012), Environmental Chemistry, New Age International Pvt., Ltd.
9. Khopkar, S.M.(2010), Environmental Pollution Analysis, New Age International
Publisher.
10. Das, A. K. (2010), Fundamentals of Inorganic Chemistry, Volume 1, Second Edition,
CBS Publishers & Distributors Pvt Ltd.
11. Das, A. K. (2012), Environment Chemistry with Green chemistry, Books and Allied (P)
Ltd.
Practical:
1. Vowles, P.D.; Connell, D.W. (1980), Experiments in Environmental
Chemistry: A Laboratory Manual, Vol.4, Pergamon Series in Environmental
Science.
2. Gopalan, R.; Anand, A.; Sugumar R.W. (2008), A Laboratory Manual for
Environmental Chemistry, I. K. International.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

42
 DISCIPLINE SPECIFIC ELECTIVE COURSE – 5 (DSE-5): Reac�ons, Reagents and
Chemical Process

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE

COURSE

Course Credits Credit distribution of the Eligibility Pre-requisite

title & course criteria of the course
Code Lecture Tutorial Practical/ (if any)
Practice
Reactions, 04 03 -- 01 Class 12th Basic
Reagents with Physics, knowledge
and Chemistry of organic
Chemical reactions
Process
(DSE-5)

Learning objectives

The objectives of this course are as follows:

• To study the important organic name and rearrangement reactions that are crucial for
the synthesis of valuable organic compounds.
• To give the knowledge belonging to the role of reagents in organic reactions for the
synthesis of chemo-, diastereo- and enantio-selective products.
• To impart the knowledge of process chemistry that is a key part of the large-scale
synthesis of chemical products essential for day-to-day life

Learning outcomes
By studying this course, students will be able to:
● Explain the reaction mechanism of various name and rearrangement reactions
● Discuss the role of the reagents in organic synthesis and apply these reagents for the
bulk chemical synthesis
● Debate and use oxidizing and reducing reagents for selective synthesis organic products
● Apply the learnt techniques to chemical processes
● Acquire skills for human resource building especially in the chemical industry.

SYLLABUS OF DSE-5

UNIT – 1: Name Reactions (15 Hours)

Application, scope and mechanism of following reactions: Prevost Reaction, Chugaev
Reaction, Maukaiyama Aldol Reaction, Mozingo Reaction, Ramberg Backlund Reaction,
Shapiro Reaction, Barbier Reaction, Clark- Eschweiler Reaction, Darzen’s Reaction, Julia-
Olifination Reaction, Tiffeneaus Damjanov Reaction, Darkin West Reaction, Bischler-
Napieralaski Reaction, Birch reduction of aromatic compounds, Appel Reaction, Mitsunobu

43
Reaction, Corey Kim Oxidation, Azide-alkyne 1,3-dipolar cycloaddition reaction, Olefin
metathesis: Grubbs reaction, Heck Reaction, Suzuki coupling and Wittig reaction.

UNIT – 2: Reducing Reagents (9 Hours)

Reactions, mechanism and applications of following reducing agents: Sodium borohydride,

Lithium aluminium hydride, NaBH3CN, DIBALH, lithium-tri-tert-butoxyaluminum hydride,
Red-Al Na[AlH2(OCH2OCH2OCH3)2], Zinc borohydride, L and K selectrides, LiBHEt3 and
KBHEt3, Luche Reagent NaBH4-CeCl3, K[BH(OAc)3], bis-Boric Acid (BBA),
Catecholborane, DEMS (Diethoxymethylsilane), 3-Mercapto propionic acid,
Polymethylhydrosiloxane (PMHS), Schwartz’s Reagent (Zirconocene chloride hydride).

UNIT – 3: Oxidizing Reagents (9 Hours

Reactions, mechanism and applications of following oxidizing agents: Jones Reagent (CrO3,
H2SO4, H2O), Swern Reagent (DMSO, oxalyl chloride), Dess Martin, TEMPO, TPAP
(Tetrapropyl ammonium perruthenate), Fetizon’s Reagent, Fenton’s Reagent [H2O2 + Fe(II)
ion], Sodium perborate NaH2BO4, Sodium Bismuthate NaBiO3, ABNO (9-
OPO(OEt)2
Azabicyclo[3.3.1]nonane N-oxyl), DEAP (Diethyl allyl phosphate, ),
AZADO (2-Azaadamantane N-oxyl], Wacker oxidation.

UNIT – 4: Process Chemistry (12 Hours)

1. Process chemistry a) Introduction, stages of scale up process: Bench, pilot, and large-
scale process with at least two examples of scale up process of API. b) In-process control
and validation of large-scale process.
2. Unit Processes: The following unit processes should be studied with mechanism and one
example of each process Nitration: Nitrating agents, process equipment for technical
nitration. Halogenation: Types of halogenations, catalytic halogenations. Reduction:
Catalytic hydrogenation, hydrogen transfer reactions, metal hydrides. Oxidation: Types
of oxidative reactions, and non-metallic oxidizing agents such as H, sodium hypochlorite,
oxygen gas, ozonolysis.

Practical component Credits:

01 (Laboratory periods:15 classes of 2 hours each)

1. Oxidation of alcohols to acid using Jones reagent.

2. Reduction of acetophenone and its derivatives to 1-phenyl ethanol derivatives by NaBH4.
3. Reduction of 4-tert-butyl-cyclohexanone to cis and trans 4-tert-butyl-cyclohexanol.
4. Synthesis of 2,5-dimethyl-2,5-hexanediol from tert-butanol using Fenton’s reagents.
5. Wittig reaction of benzyltriphenylphosphonium chloride and 4-bromobenzaldehyde using
potassium phosphate (tribasic).
6. Substitution (SN2) reaction of 1-iodobutane and 2-naphthol.
7. Aldol condensation reaction: solventless synthesis of chalcones.
8. Borohydride reduction of a ketone: hydrobenzoin from benzil.
9. Visit to chemical industry of the demonstration of pilot scale.

44
Essential/recommended readings

Theory:
2. Clayden, J. Greeves, N., Warren, S. Organic Chemistry, South Asian Edition,
Oxford University Press, USA
3. Gadamasetti K., Process Chemistry in the Pharmaceutical Industry: Challenges in
an Ever- Changing Climate-An Overview, Vol-2, CRC Press, London.
4. Murphy R.M., Introduction to Chemical Processes: Principles, Analysis, Synthesis,
McGraw-Hill Education, New York.
5. Harrington P. J., Pharmaceutical Process Chemistry for Synthesis: Rethinking the
Routes to Scale up, John Wiley and Sons, Inc, New Jersey.
6. Parashar, R.K.; Ahluwalia, V.K. (2018), Organic Reaction Mechanism, 4th Edition,
Narosa Publishing House.

Practical:
1. Mann F.G, Saunders, B.C., Practical Organic Chemistry, Dorling Kindersley
(India) Pvt. Ltd. (Pearson Education Ltd.), Singapore.
2. Vogel A.I., Elementary Practical Organic Chemistry, Dorling Kindersley (India)
Pvt. Ltd. (Pearson Education Ltd.), Singapore.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

45
 DISCIPLINE SPECIFIC ELECTIVE COURSE - 6 (DSE- 6): Polymers,
Colloids, Surfaces and Interfaces

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course Credits Credit distribution of the course Eligibility Pre-requisite

title & Lecture Tutorial Practical/ criteria of the course
Code Practice (if any)
Polymers, 04 03 -- 01 Class 12th --
Colloids, with
Surfaces Physics,
and Chemistry
Interfaces
(DSE- 6)

Learning Objectives
The objectives of this course are as follows:
• To give students a comprehensive coverage of important physical aspects of polymers
chemistry, colloids, emulsions, surfaces and interfaces.
• to study the applications of these aspects.

Learning outcomes
By studying this course, the students will be able to:
• Explain the types of polymers, kinetics of polymerization and polymer properties.
• Understand and apply the concepts of properties of polymer solutions and their
thermodynamics.
• Comprehend the basic concepts of surface chemistry specifically in relation to colloids.
• Have a thorough understanding of applications of colloids in various areas.
SYLLABUS OF DSE-6

UNIT 1: Introduction to polymers (Hours: 6)

Recapitulation of basic concepts of polymers. Types of polymerizations and their mechanism

and kinetics: Free radical, ionic, step-growth, coordination, copolymerization. Polymerization
techniques: Bulk, solution, suspension, and emulsion.

UNIT 2: Polymer solution (Hours: 9)

46
Polymer solution – solubility parameter, properties of dilute solutions and their criteria,
Thermodynamics of polymer solutions, entropy, enthalpy, and free energy change. Flory
Huggins theory.

UNIT 3: Introduction to Colloid Chemistry (Hours: 9)

Recapitulation of basic concepts of Adsorption, Distinction among true solutions, colloids and
suspensions, Components of Colloids, classification of colloids - lyophilic, lyophobic;
Preparation methods and properties of lyophobic solutions, Hydrophile-lyophile balance
(HLB), multi molecular, macromolecular and associated colloids (micelles formation),
preparation and properties of colloids - Tyndall effect, Brownian movement, electrophoresis,
dialysis, coagulation and flocculation; Charge on Colloidal particles and Electrical double layer
concept, Suspensions and their characteristics, Emulsions and their characteristics.

UNIT 4: Surface chemistry in relation to colloids (Hours: 12)

Surface film on liquid surface, surface potential, monomolecular films, Langmuir Blodgett
layers. Emulsions, foams and aerosols; electrical aspects of surface chemistry; Surface of
solids, solid-liquid interface, stability of dispersions, stabilization of suspensions

UNIT 5: Application of colloids (Hours: 9)

Characterization of colloidal particles, Role of colloid chemistry in Nanotechnology (wet
colloid chemical approach, “bottom up” fabrication of nanoparticles and nanostructured
materials), applications of colloid chemistry in petroleum recovery, coating and painting, food,
pharmaceuticals and cosmetic industry, medicinal chemistry (use in drug formulations),
Sewage disposal, Purification of water, cleansing action of soap, Formation of Delta, Smoke
precipitation, Photography, Artificial rain

Practical component

Practicals: Credits: 01
(Laboratory periods:15 classes of 2 hours each)

1. Free radical solution polymerization of styrene (St) / Methyl Methacrylate

(MMA)/MethylAcrylate (MA).
2. Preparation of nylon 6,6
3. Determination of molecular weight of polyvinyl propylidene in water by viscometry.
4. Determination of the viscosity-average molecular weight of poly(vinyl alcohol)
(PVOH) and the fraction of head-to-head monomer linkages in the polymer.
5. Determination of molecular weight by end group analysis of polymethacrylic acid.
6. Estimation of the amount of HCHO in the given solution by sodium sulphite method.
7. Preparation of Colloidal Sols of following
A. Arsenic sulphide,

47
 B. Antimony sulphide
C. Ferric chloride
D. Aluminium hydroxide
8. To find out the precipitation values of arsenious sulphide sol by using monovalent,
bivalent and trivalent cations.
9. To determine the nature of charge on particle in given colloidal solution and their
electrophoretic velocity and zeta potential.
10. To prepare lyophilic sol of starch.
Essential/recommended readings
Theory:
1. Carraher,C. E. Jr. (2013), Seymour’s Polymer Chemistry, Marcel Dekker, Inc.
2. Odian, G. (2004), Principles of Polymerization, John Wiley.
3. Billmeyer, F.W. (1984), Text Book of Polymer Science, John Wiley
4. Myers D.,Surface, interfaces and colloids Principles and Applications, 2nd Edition,
Wiley-VCH
5. V.R. Gowarikar (2010), Polymer Science, New Age International Publishers Ltd.
Practical:
1. Sperling, L.H. (2005), Introduction to Physical Polymer Science, John Wiley & Sons

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

48
 DISCIPLINE SPECIFIC ELECTIVE COURSE -7 (DSE-7): Novel Inorganic
Solids

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course Credits Credit distribution of the course Eligibility Pre-requisite

title & Lecture Tutorial Practical/ criteria of the course
Code Practice (if any)
Novel 04 03 -- 01 Class 12th --
Inorganic with
Solids Physics,
(DSE-7) Chemistry

Learning Objectives

The Objectives of this course are as follows:

• To familiarize the students with the characterization techniques of inorganic solids

• To familiarize the students with use and manifold applications of composites, carbon
or high-tech ceramics

Learning Outcomes:

By studying this course, the students will be able to:

• Explain the mechanism of solid-state synthesis.

• Explain about the different characterization techniques and their principle.
• Explain the importance of composites and their applications.
• Discuss and explain the usage of solid materials in various instruments, batteries, etc.
which would help them to appreciate the real-life importance of these materials

SYLLABUS OF DSE- 7

Unit 1: Synthesis of inorganic solids (Hours: 5)

Conventional heat and beat method, Co-precipitation method, Sol-gel method, Hydrothermal
method, Chemical vapor deposition (CVD), Ion-exchange and Intercalation method.

Unit 2: Characterization techniques of inorganic solids (Hours: 10)

49
Powder X-ray Diffraction, UV-visible spectroscopy, Scanning Electron Microscopy (SEM),
Transmission Electron Microscopy (TEM), Fourier-Transform Infrared (FTIR) spectroscopy,
Brunauer–Emmett–Teller (BET) surface area analyser, Dynamic Light Scattering (DLS)

Unit 3: Pigments (Hours: 10)

Cationic, anionic and mixed solid electrolytes and their applications. Inorganic pigments –
coloured, white and black pigments.

One-dimensional metals, molecular magnets, inorganic liquid crystals.

Unit 4: Composite materials (Hours: 10)

Introduction, limitations of conventional engineering materials, role of matrix in composites,

classification, matrix materials, reinforcements, metal-matrix composites, polymer-matrix
composites, fibre-reinforced composites, bio-nanocomposites, environmental effects on
composites, applications of composites.

Unit 5: Speciality polymers (Hours: 10)

Speciality polymers: Conducting polymers - Introduction, conduction mechanism,

polyacetylene, polyparaphenylene, polyaniline. and polypyrrole, applications of conducting
polymers, ion-exchange resins and their applications.

Ceramic & Refractory: Introduction, classification, properties, manufacturing and

applications of ceramics, refractory and superalloys as examples.

Practicals Credits: 01
(Laboratory periods: 15 classes of 2 hours each)

1. Preparation of polyaniline and its characterization using UV-visible spectrophotometer.

2. Intercalation of hydrogen in tungsten trioxide and its conductivity measurement using
conductometer.
3. Synthesis of the following inorganic pigments:

(i) PbCrO4 / chrome yellow

(ii) Barium white

(iii) Prussian Blue

(iv) Malachite

. 4. Preparation of zeolite A and removal of Mg and Ca ions from water samples quantitatively
using zeolite.

5. Determination of exchange capacity of cation exchange resins and anion exchange

resins.

50
 6. Determination of a mixture of cobalt and nickel (UV-visible spectroscopy).
7. Preparation of a disc of a ceramic compound using ball milling, pressing and sintering,
and study its XRD.

Essential/recommended readings

Theory:

1. West, A. R. (2014), Solid State Chemistry and Its Application, Wiley.

2. Smart, L. E.; Moore, E. A., (2012),Solid State Chemistry: An Introduction CRC
Press Taylor & Francis.
3. Rao, C. N. R.; Gopalakrishnan, J. (1997),New Direction in Solid State Chemistry,
Cambridge University Press.
4. Poole Jr.; Charles P.; Owens, Frank J. (2003), Introduction to Nanotechnology, John
Wiley and Sons.

Practicals:

1. Orbaek, W.; McHale, M.M.; Barron, A. R.; Synthesis and Characterization of Silver
Nanoparticles for An Undergraduate Laboratory,J. Chem. Educ. 2015, 92,
339−344.
2. MacDiarmid, G.; Chiang, J.C.; Richter, A.F.; Somasiri, N.L.D.(1987), Polyaniline:
Synthesis and Characterization of the Emeraldine Oxidation State by Elemental
Analysis, L. Alcaeer (ed.), Conducting Polymers, 105-120, D. Reidel Publishing.
3. Cheng, K.H.; Jacobson, A.J.; Whittingham, M.S. (1981),Hexagonal Tungsten
Trioxide and Its Intercalation Chemistry, Solid State Ionics, 5, 1981, 355-358.
4. Ghorbani H.R.; Mehr, F.P; Pazoki, H; Rahmani, B.M.; Synthesis of ZnO
Nanoparticles by Precipitation Method, Orient J Chem 2015, 31(2).

Note: Examination scheme and mode shall be as prescribed by the Examination

Branch, University of Delhi, from time to time.

51
 DISCIPLINE SPECIFIC ELECTIVE COURSE – 8 (DSE-8): Applied Organic
Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course Credits Credit distribution of the course Eligibility Pre-requisite

title & Lecture Tutorial Practical/ criteria of the course
Code Practice (if any)
Applied 04 03 -- 01 Class 12th --
Organic with
Chemistry Physics,
(DSE-8) Chemistry

Learning Objectives
The objectives of this course are as follows:
• To make students aware of the importance of organic compounds in daily life.
• To familiarize students with the chemistry and uses of dyes, polymers, terpenoids,
alkaloids, steroids and pharmaceutical compounds and their direct or indirect effect on
human life and health

Learning outcomes

By the end of this course the students will be able to:

● Discuss and demonstrate the chemistry and uses of commercially important and
naturally occurring compounds like dyes, polymers, terpenoids, alkaloids, steroids and
pharmaceuticals.
● Appreciate the chemistry of biodegradable and conducting polymers and their
importance to human life and society.
● Comprehend the chemistry of dyeing and dyes. Explain why some dyes are better than
others. Describe the applications of various types of dyes including those in foods and
textiles.
● Comprehend the synthetic routes and mode of action of some selected pharmaceutical
compounds

● Use the knowledge gained to solve real world problems

52
SYLLABUS OF DSE-8

Unit 1: Dyes (Hours: 7)

Nomenclature of commercial dyes with at least one example. Suffixes - G, O, R, B, 6B, L, S;
colour index and colour index number. Classification of dyes based on structure and
application; Chemistry of dyeing.
Synthesis and applications of the following types of dyes: Azo dyes - Methyl orange, Congo
red; Triphenyl methane dyes-Malachite green, Rosaniline and Crystal violet; Phthalein Dyes -
Phenolphthalein; Natural dyes - Structure elucidation and synthesis of Alizarin and Indigotin;
Edible Dyes (natural and synthetic) with examples and effect of synthetic food colours on
health.

Unit 2: Polymers (Hours:12)

Introduction and classification based on origin, monomer units, thermal response, mode of
formation, structure, application and tacticity; di-block, tri-block and amphiphilic polymers;
Weight average molecular weight, number average molecular weight, glass transition
temperature (Tg) of polymers; Polymerisation Reactions-Addition and condensation.
Mechanism of cationic, anionic and free radical addition polymerization; Ziegler-Natta
polymerisation of alkenes.
Preparation and applications of: Plastics -thermosetting (phenol-formaldehyde, Polyurethanes)
and thermosoftening (PVC, polythene); Fabrics -natural (cellulose and synthetic derivatives of
cellulose like rayon and viscose); synthetic (acrylic, polyamide, polyester); Rubbers-natural
and synthetic: Buna-N, Buna-S, Neoprene, silicon rubber; Vulcanization; Polymer additives;
Introduction to Specialty Polymers: electroluminescent (Organic light emitting diodes),
Conducting, biodegradable polymers and liquid crystals.

Unit 3: Natural Product Chemistry- An Introduction to Terpenoids, Alkaloids

and Steroids (Hours: 12)
Terpenes: Introduction, occurrence, classification, uses, isoprene and special isoprene rule;
structure elucidation, synthesis and industrial application of citral.
Alkaloids: Introduction, occurrence, classification, uses, general structural features, general
methods for structure elucidation including Hoffmann’s exhaustive methylation and Emde’s
method. Structure elucidation, synthesis and physiological action of Nicotine.
Steroids: Introduction, occurrence, structure, Diel’s hydrocarbon, nomenclature of steroid
hydrocarbons, structure and biological functions of the following steroids- Cholesterol, Sex
Hormones (Estrogen, androgen and progesterone), Adrenocortical hormones (Cortisone and
cortisol) and Ergosterol (antirachitic effect).

53
Unit 4: Pharmaceutical Compounds (Hours:14)
Introduction, classification; Synthesis, uses, mode of action and side effects of the following
drugs:
Antipyretics -Paracetamol; Analgesics- Ibuprofen; Antimalarials - Chloroquine; Antitubercular
drugs - Isoniazid.
An elementary treatment of Antibiotics and detailed study of chloramphenicol including mode
of action. Structure and medicinal uses of curcumin (haldi), azadirachtin (neem), vitamin C
and antacid (ranitidine).

Practical component
Practical: Credits: 01
(Laboratory periods:15 classes of 2 hours each)
(At least five experiments to be performed)

1. Synthesis of urea formaldehyde resin and test the solubility.

2. Preparation of Starch-PVA Film.
3. Preparation of Methyl orange.
4. Separation of a mixture of dyes by Thin Layer Chromatography (TLC).
5. Isolation and estimation of the content of aspirin in a commercial tablet.
6. Synthesis of 4-methyl-7-hydroxycoumarin by condensation of resorcinol with ethyl
acetoacetate.
7. Synthesis of 3,5-dimethyl pyrazole by condensation of acetylacetone and hydrazine.
8. Synthesis of benzimidazole.
9. Synthesis of 2,3-diphenylquinoxaline.
10. Synthesis of paracetamol

Essential/recommended readings

Theory:
1. Finar, I.L. Fifth Edition Organic Chemistry, Volume 2, Pearson Education, 2008.
2. Saunders, K. J., (1988), Organic Polymer Chemistry, Second Edition Chapman &
Hall, London.
3. Campbell, Ian M., (2000), Introduction to Synthetic Polymers, Second Edition,
Oxford University Press, USA.
4. Bahadur, P. and Sastry, N.V. (2002) Principles of Polymer Science Narosa, New Delhi
5. Patrick, G. An Introduction to Medicinal Chemistry (2013), Fourth Edition, Oxford
University Press.
6. Beale J.M. Block J., (2010) Wilson and Gisvold's Textbook of Organic Medicinal
and Pharmaceutical Chemistry, Twelfth Edition, Lippincott Williams and Wilkins.
7. Alagarsamy, V. (2010), Textbook of Medicinal Chemistry, Volume II, Second
Edition, Reed Elsevier India Private Limited.

54
Practical:
1. Sciam, A.J. TLC of mixture of dyes; J. Chem. Educ., 1985, 62(4), 361.
https://pubs.acs.org/doi/10.1021/ed062p361.
2. McKone, H.T.; Nelson, G.J. Separation, and identification of some FD &C dyes by
TLC. An undergraduate laboratory experiment, J. Chem. Educ., 1976, 53(11), 722.
DOI: 10.1021/ed053p722.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

55
DISCIPLINE SPECIFIC ELECTIVE COURSE- 9 (DSE-9): Applica�ons of Computers in
Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE

COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Applications of 04 03 - 01 Class 12 th

with
Computers in
Physics,
Chemistry Chemistry
(DSE 9)

Learning Objectives

The Objectives of this course are as follows:

• To familiarize the students with the fundamental building blocks and syntax of coding
in Python with
• To apply python programming to solve simple Chemistry problems by thinking
algorithmically and coding structurally

Learning outcomes
By studying this course, the students will be able to:

• Understand the importance of python programming in chemistry and its applications in

the field of AI and ML
• Perform simple computations in python after learning the basic syntax, loop structure,
string data manipulation etc.
• Solve chemistry problems such as finding pKa of a weak acid, solving Schrodinger’s
equation etc.
• Plot experimental data and perform regression analysis

SYLLABUS OF DSE-9

UNIT–1: Basic Computer system (Hours: 3)

Hardware and Software; Input devices, Storage devices, Output devices, Central Processing
Unit (Control Unit and Arithmetic Logic Unit); Number system (Binary, Octal and

56
Hexadecimal Operating System); Computer Codes (BCD and ASCII); Numeric/String
constants and variables. Operating Systems (DOS, WINDOWS, and Linux); Software
languages: Low level and High-Level languages (Machine language, Assembly language;
QBASIC, C, C++, FORTRAN 90&95); Compiled versus interpreted languages. Debugging
Software Products (Office, chemsketch, scilab, matlab, and hyperchem), internet application

UNIT-2: Introduction to Python (Hours: 3)

Why Python? Python coding environment setup, Python as an interpreted language, Brief
history of Python, Uses of Python (including artificial intelligence and machine learning),
Applications of Python in Chemistry

UNIT-3: Coding in Python (Hours: 18)

(i) Basic syntax including constants and variables, Operators, Data Types, Declaring and using
Numeric data types: int, float, string etc. (ii) Program Flow Control Conditional blocks: if, else
and else if, simple FOR loops, FOR loop using ranges, string, list and dictionaries. Use of while
loops, Loop manipulation using pass, continue, break and else. (iii) Complex data types: String,
List, Arrays, Tuples and Dictionary, String operations and manipulation methods, List
operations including slicing, in-built Python Functions. (iv) Python packages - usage of numpy
and scipy for mathematical computations.

UNIT-4: Plotting graphs (Hours: 9)

Matplotlib for Plotting - Simple plots, formatting of plots, multiple plots, histograms, bar
graphs, distributions, curve fitting – linear regression.

UNIT-5: Numerical Methods in Chemistry (Hours: 12)

Solution of quadratic equation, polynomial equations (formula, iteration, Newton – Raphson
methods and binary bisection) with examples of polynomial equations used in chemistry;
Numerical differentiation – finite difference method (backward, central and forward),
Numerical integration - Trapezoidal and Simpson’s rule to calculate area under the curves for
chemistry problems, e.g., entropy calculations, Simultaneous equations, Statistical analysis-
mean, variance, standard deviation, error, Curve fitting – linear regression, Solving
Schrödinger’s equation using Python packages.

Practical component

Practicals: Python Programming for Chemists Credits: 01

4. Writing simple programs using scipy and numpy

a. syntax, data types
b. loop structure, conditional loops

57
 c. To learn string data manipulation
d. Array and lists
e. Sorting, matrix manipulations

5. Plotting graphs using matplotlib

a. Planck’s distribution law
b. Maxwell-Boltzmann distribution curves as a function of temperature and mass
c. Radial distribution curves for hydrogenic orbitals
d. Gas law Isotherms – Ideal and Real
e. Data from phase equilibria studies
f. Wavefunctions and Probabilities as multiplots
g. Kinetics data with linear fitting

6. Numerical Methods in Chemistry

a. Solving equations involved in chemical equilibria such as pH of a weak acid at
a given concentration, cubic equation obtained from solving van der Waals
equation of real gases using Iteration, Newton-Raphson, and Binary Bisection
Method
b. Numerical Differentiation – finding equivalence point given pH metric and
potentiometric titrations data by finding the first and the second derivative using
the finite difference method
c. Numerical Integration – Trapezoidal and Simpson’s 1/3 rule to calculate
enthalpy and entropy of an ideal gas
d. Statistical Analysis – Calculating Mean, Variance, Standard Deviation
e. Solving Schrodinger’s Equation

Essential/recommended readings

Theory:

7. Dr. M. Kanagasabapathy(2023), Python for Chemistry: An introduction to Python

algorithms, Simulations, and Programing for Chemistry (English Edition), BPB
Publications
8. Robert Johansson (2021), Numerical Python: Scientific Computing and Data
Science Applications with Numpy, SciPy and Matplotlib, 2nd Edition, Apress

Practical

1. Urban M., Murach J., Murach’s Python programming, 2nd Indian reprint 2018,
Shroff publishers and distributors
2. Gaddis T., Starting out with python plus My programming Lab with Pearson e-
text-Access card package, 3rd ed.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

58
 DISCIPLINE SPECIFIC ELECTIVE COURSE - 10(DSE-10): Analytical
Methods in Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title Credits Credit distribution of the course Eligibility Pre-

& Code Lecture Tutorial Practical/ criteria requisite of
Practice the course
(if any)
04 03 -- 01 Class 12th -
Analytical with
Methods in Physics,
Chemistry
Chemistry
(DSE-10)

Learning Objectives

The Objectives of this course are as follows:

• To familiarize the students with concept of sampling, Accuracy, Precision, Statistical

test data-F, Q and t test.
• To familiarize the students with the laws of spectroscopy and selection rules governing
the possible transitions in the different regions of the electromagnetic spectra.
• To familiarize the students with important separation methods like solvent extraction
and chromatography

Learning Outcomes:

By studying this course, the students will be able to:

• Perform experiment with accuracy and precision.

• Develop methods of analysis for different samples independently.
• Test contaminated water samples.
• Use basic principle of instrument like Flame Photometer, UV-Visible
spectrophotometer learnt for practical applications.
• Apply knowledge of geometrical isomers and keto-enol tautomers to analysis.
• Determine composition of soil.
• Estimate macronutrients using Flame photometry.

59
SYLLABUS OF DSE-10

Unit 1: Qualitative and Quantitative Aspects of Analysis: (Hours: 5)

Sampling, evaluation of analytical data, errors, accuracy and precision, methods of their
expression.

Normal law of distribution of indeterminate errors, statistical test of data; F, Q and t test,
rejection of data, and confidence intervals.

Unit 2: Optical Methods of Analysis (Hours: 25)

Origin of spectra, interaction of radiation with matter, fundamental laws of spectroscopy and
selection rules

UV-Visible Spectrometry: Basic principles of instrumentation (choice of source,

monochromator and detector) for single and double beam instrument; Transmittance.
Absorbance and Beer-Lambert law

Basic principles of quantitative analysis: estimation of metal ions from aqueous solution,
geometrical isomers, keto-enol tautomers.

Flame Atomic Absorption and Emission Spectrometry: Basic principles of instrumentation

(choice of source, monochromator, detector, choice of flame and Burner designs). Techniques
of atomization and sample introduction; Method of background correction, sources of chemical
interferences and their method of removal, Techniques for the quantitative estimation of trace
level of metal ions from water samples.

Unit 3: Thermal methods of analysis (Hours: 5)

Theory of thermogravimetry (TG) and basic principle of instrumentation of thermal analyser.

Techniques for quantitative estimation of Ca and Mg from their mixture.

Unit 4: Separation techniques (Hours:10)

Solvent extraction: Classification, principle and efficiency of the technique.

Mechanism of extraction: extraction by solvation and chelation, Technique of extraction: batch,

continuous and counter current extractions, Qualitative and quantitative aspects of solvent
extraction: extraction of metal ions from aqueous solution, extraction of organic species from
the aqueous and non-aqueous media.

Chromatography: Classification, principle and efficiency of the technique, Mechanism of

separation: adsorption, partition & ion-exchange

Practicals Credits 01

60
(Laboratory periods: 15 classes of 2 hours each)

1. Separation of constituents of leaf pigments by Thin Layer Chromatography

2. Solvent Extractions

(i) To separate a mixture of Ni2+ & Fe2+ by complexation with DMG and extracting the
Ni2+ DMG complex in chloroform, and determine its concentration by
spectrophotometry.

3. Analysis of soil:

(i) Total soluble salt

(ii) Estimation of exchangeable calcium and magnesium
(iii) Estimation of carbonate and bicarbonate
(iv) Qualitative detection of nitrate and phosphate
4. Separation of amino acids from organic acids by ion exchange chromatography.
5. Spectrophotometry

(i) Verification of Lambert-Beer’s law and determination of concentration of a coloured

species (CuSO4 / KMnO4 /CoCl2 / CoSO4)
(ii) Spectrophotometric analysis of caffeine and benzoic acid in a soft drink
(iii) Determination of concentration of coloured species via following methods;
(a) Graphical method, (b) Epsilon method, (c) Ratio method, (iv) Standard addition
method
6. Flamephotomerty
(i) Estimation of potassium, calcium and magnesium using flame photometry

Essential/recommended readings

Theory:

1. Willard, H.H.(1988),Instrumental Methods of Analysis, 7th Edition, Wardsworth

Publishing Company.
2. Christian, G.D.(2004),Analytical Chemistry, 6th Edition, John Wiley & Sons, New
York.
3. Harris, D. C.(2007),Quantitative Chemical Analysis,6th Edition, Freeman.
4. Khopkar, S.M. (2008), Basic Concepts of Analytical Chemistry, New Age
International Publisher.
5. Skoog, D.A.; Holler F.J.; Nieman, T.A. (2005), Principles of Instrumental Analysis,
Thomson Asia Pvt. Ltd.

Practicals:

1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C.(1989),Vogel’s Textbook of

Quantitative Chemical Analysis,John Wiley and Sons.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

61
 DISCIPLINE SPECIFIC ELECTIVE COURSE - 11 (DSE-11): Basic Principles
of Food Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course Credits Credit distribution of the course Eligibility Pre-requisite

title & Lecture Tutorial Practical/ criteria of the course
Code Practice (if any)
Basic 04 03 -- 01 Class 12th --
Principles with
of Food Physics,
Chemistry Chemistry
(DSE-11)

Learning Objectives
The objectives of this course are as follows:
• To make students understand the sources, importance, stability and transformations of
food components during handling and processing.
• To make students aware about nature and importance of additives in food chemistry.

Learning outcomes
By studying this course, the students will be able to:
• Develop a strong understanding of basic fundamentals of food chemistry
• Discuss and demonstrate how alterations /transformations during processing and
handling affect the quality and stability of food
• Develop an elementary idea on the nature and importance of additives in food
chemistry.
• Apply the knowledge gained to real world problems

SYLLABUS OF DSE-11
Unit 1: Introduction (Hours:3)
What is food chemistry; An overview of the following: alterations during handling or
processing (texture, flavour, colour), chemical and biochemical reactions leading to alteration
in food quality (browning, oxidation, hydrolysis, protein denaturation), cause and effect
relationship pertaining to food handling; factors governing stability of food (chemical and
environmental factors) and role of food chemists.
Unit 2: Water (Hours:3)

62
Definition of water in food, structure of water and ice, types of water, sorption phenomenon,
water activity and packaging, water activity and shelf-life.
Unit 3: Carbohydrates (Hours:6)
Introduction, sources, functions, deficiencies, structure and importance of polysaccharides in
food chemistry (Agar and Agarose, Pectin, Hemicellulose, Cyclodextrins, Gums, Alginate,
Starches, modified starches), Non-enzymatic browning and its prevention, caramelisation,
formation of acrylamide in food, role of carbohydrates as sweeteners and comparison with
artificial sweeteners.
Unit 4: Proteins (Hours:6)
Introduction, sources, classification, functions, deficiencies, physico-chemical & functional
properties of proteins, nature of food proteins (plant and animal proteins).
Unit 5: Lipids (Hours:6)
Introduction, sources, classification and physical properties, functions, deficiencies, effect of
frying on fat, reaction of lipids: hydrogenation, interesterification, hydrolysis, auto-oxidation
and its prevention; flavour reversion, fat replacers: fat mimetics and fat substitutes.
Unit 6: Vitamins and Minerals (Hours:6)
Vitamins: Introduction, sources, classification: water soluble and water insoluble vitamins,
essential vitamins, physiological function, deficiencies, causes of variation and loss in foods,
vitamin like compounds, effect of food processing.
Minerals: Introduction, sources, classification: major minerals and trace elements,
physiological function, deficiencies, factors affecting mineral content of food, fortification and
enrichment of foods with minerals, effect of food processing.
Unit 7: Food Additives (Hours:15)
Additives: Introduction, importance, classification, antioxidants, emulsifiers, stabilizers,
gelling agents, gums, thickeners, sweeteners, acidulants, preservatives, humectants, food toxins
Colouring Agents and Pigments: Introduction, natural food colourants: anthocyanins,
carotenoids, chlorophyll, caramel, betalains; examples of pigments in common food; Nature-
identical colourants: β-Carotene, canthaxanthin and riboflavin; artificial colouring agents;
artificial/synthetic colourants: Azo dyes (e.g. amaranth dye, tatrazine, citrous red, Allura red);
quinoline (e.g. quinoline yellow); phthalein (e.g. erythrosine); triarylmethanes and indigoid
(e.g. indigo carmine), FD&C Dyes and lakes; properties of certified dyes, colours exempt from
certification.
Food Flavor: Sensation of taste and odour, chemical dimension of basic types of taste (Salty,
Sweet, Bitter, Sour, Umami taste), other sensations like astringency, coolness,
pungency/pungency); non-nutritive sweeteners (aspartame, saccharin, sucralose, cyclamate)
and nutritive sweeteners, molecular mechanism of flavour perception, biogenesis of fruits and
vegetable flavors, taste inhibition, modification and enhancement, common vegetable and
spice flavors.

63
Practical component
Practical: Credits: 01
(Laboratory periods:15 classes of 2 hours each)
(At least four experiments to be performed)
1. Determination of moisture in food products by hot air oven-drying method.
2. Paper chromatography of synthetic food dyes.
3. Quantitative determination of food dyes in powdered drink mixes by
spectrophotometric method.
4. Colorimetric determination of Iron in vitamin / dietary tablets.
5. Determination of rancidity of edible oils by Kriess Test.
6. Estimation of Vitamin C in a given solution/ lemon Juice/chillies by 2, 6-
dichlorophenol by Indophenol Method.
7. Isolation of casein from milk.
8. Qualitative estimation of cholesterol by Liebermann-Burchard method.
9. Detecting the presence of Vanaspati and rancidity in the given Ghee sample through
qualitative tests.

Essential/recommended readings
Theory:
1. DeMan, J.M., Finley, J.W., Hurst, W.J., Lee, C.Y. (2018), Principles of Food
Chemistry, Fourth Edition, Springer.
2. Msagati, T.A.M. (2013), Chemistry of Food Additives and Preservatives, Wiley-
Blackwell.
3. Fennema, O.R. (2017), Food Chemistry, Fifth Edition, CRC Press.
4. Attokaran, M. (2017), Natural Food Flavors and Colorants, Second Edition, Wiley-
Blackwell.
5. Potter, N.N., Hotchkiss, J.H, (1995) Food Science, Fifth Edition, Chapman & Hall.
6. Brannen, D., Davidsin, P.M., Salminen, T. Thorngate III, J.H. (2002), Food Additives,
Second Edition, CRC Press.
7. Coultate, T. (2016), Food: The Chemistry of its Components, Sixth Edition, Royal
Society of Chemistry.
8. Belitz, H. D.; Grosch, W. (2009), Food Chemistry, Springer.
9. Course: Food Chemistry (iasri.res.in)
Practical:
1. Ranganna, S. (2017). Handbook of analysis and quality control for fruits and vegetable
products, Second Edition, McGraw Hill Education
2. Sawhney, S.K., Singh, R. (2001), Introductory Practical Biochemistry, Narosa
Publishing House

64
Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

DISCIPLINE SPECIFIC ELECTIVE COURSE -12 (DSE-12): Computational

Methods & Molecular Modelling

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Computational 04 03 -- 01 Class 12th --
Methods & with
Molecular Physics,
Modelling Chemistry
(DSE-12) and
Mathematics

Learning Objectives

The Objectives of this course are as follows:

• To make students learn the theoretical background of computational techniques in

molecular modelling.
• To give the different flavours of computational chemistry by the end of this course.
• To provide hands-on experience in molecular modelling on various software

Learning outcomes

By studying this course, the students will be able to:

• Explain the theoretical background of computational techniques and selective
application to various molecular systems.
• Compare computational and experimental results and explain deviations.
• Perform Optimization of geometry parameters of a molecule (such as shape, bond
length and bond angle) through the use of software like Chem Sketch and Argus Lab in
interesting hands-on exercises.
• Perform analysis of molecular properties using various software.

65
SYLLABUS OF DSE-12

UNIT-1 : Introduction (Hours: 6)

Introduction to computational chemistry: Overview of Classical and Quantum Mechanical

Methods (Ab initio, DFT, Semi-empirical, Molecular Mechanics, Molecular Dynamics, and
Monte Carlo)

UNIT – 2: Potential Energy Surfaces (Hours: 6)

Intrinsic Reaction Coordinates, Stationary points, Equilibrium points – Local and Global
minima, Geometry optimization and energy minimization, the concept of transition state with
examples, Hessian matrix

UNIT – 3 : Molecular Mechanics & Molecular Dynamics (Hours: 9)

Molecular Mechanics

Force Fields (A brief explanation of all the terms of a basic force field), the basic idea of MM1,
MM2, MM3, MM4, MM+, AMBER, BIO+, OPLS.

Molecular Dynamics

The concept of the periodic box, ensembles (microcanonical, canonical, isothermal – isobaric),
steps in a typical MD simulation.

UNIT-4: Huckel Molecular Orbital Theory (Hours: 6)

Huckel MO with examples: ethene and propenyl systems, Properties calculated – energy,
charges, bond order, electronic energies, resonance energies.

UNIT- 5: Computational Methods (Hours: 18)

Ab-initio methods
Antisymmetry principle, Slater determinants, SCF method, Hartree-Fock method.
Basis sets, Basis functions, STOs and GTOs, diffuse and polarization functions. Minimal basis
sets, Basis set superposition error (BSSE) - Effective core potentials (ECP)
Advantages of ab initio calculations.

Density Functional Theory

A brief description of Density Functional Theory (DFT). Calculation of Electronic Properties
in ground and Excited states

Semi-empirical methods
Basic idea about Zero differential overlap (ZDO) approximation

66
Some important concepts
Concepts of atomic charges, electrostatic potential maps, computation of thermodynamic
properties and spectroscopic observables

Practical component
Practical: Credits: 01
(Laboratory periods:15 classes of 2 hours each)

1) Write the Z-Matrix of a given set of molecules.

2) Carry out geometry optimisation on H2O, H2S, H2Se molecules compare the optimized
bond angles and dipole moments from the results obtained. Obtain the ESP-mapped
density surfaces and interpret the results obtained with reference to bonding in these
molecules.

Suggestive: A comparative analysis of results of the above exercise may be carried out
using different quantum mechanical methods.

3) Calculate the energy of the following chemical species and arrange them in order of
increasing stability.

1-hexene, 2-methyl-2-pentene, (E)-3-methyl-2-pentene, (Z)-3-methyl-2-pentene, and

2,3- dimethyl-2-butene in order of increasing stability.

4) Carry out geometry optimisation on the following chemical species and compare the
shapes and dipole moments of the molecules.

1-pentanol, 2-pentanol, 3-pentanol, 2-methylbutan-1-ol, 3-methylbutan-1-ol, 2-

methylbutan-2-ol, 2-methylbutan-3-ol and 2,2-dimethylpropanol.

Correlate the computationally obtained values of the dipole moments with the
experimental values of the boiling points: (118 ºC, 100 ºC, 108 ºC, 82 ºC, of 1-butanol,
2-butanol, 2-methyl-1-propanol, and 2-methyl-2- propanol respectively).

5) Based on the implicit electronic structure calculations, determine the heat of

hydrogenation of Propylene.

6) Based on the calculations of enthanlies of the participating chemical species on

optimized geometry of the molecules, calculate the reaction enthalpy at 298 K for the
following, industrially important reactions:

𝐶𝐶𝐶𝐶4 + 𝐻𝐻2 𝑂𝑂 → 𝐶𝐶𝐶𝐶 + 3𝐻𝐻2 (steam reforming of methane)

≡≡ (Haber-Bosch process)

67
7) Carry out geometry optimisation and determine the energy of the participating chemical
species in the following reactions Using these results calculate the resonance energy of
thiophene.

H2 H2

S S S

8) Carry out geometry optimisation & Energy calculations on the following species and
obtain Frontier Molecular Orbitals. Visualize the Molecular Orbitals of these species
and interpret the results for bonding in these molecules.
Benzene, Naphthalene, and Anthracene.

9) Compare the gas phase basicities of the methylamines by comparing the enthalpies of
the following reactions:

BH+ + NH3 → B + NH4+

Where B = CH3NH2, (CH3)2NH, (CH3)3N

10) On the basis of results of geometry optimization and energy calculations, determine the
enthalpy of isomerization of cis and trans 2-butene.

11) Perform a conformational analysis of butane. Plot the graph between the angle of
rotation and the energy of the conformers using spreadsheet software.

12) Compute the resonance energy of benzene by comparison of its enthalpy of

hydrogenation with that of cyclohexene.

13) Calculate the electronic UV/Visible absorption spectrum of Benzene.

14) Calculate the electronic absorption spectra of formaldehyde.

15) Plot the electrostatic potential mapped on electron density for benzene and use it to
predict the type of stacking in the crystal structure of benzene dimer.

16) On a given set of molecules methylamine (CH3NH2) carry out geometry optimization,
single point energy and NBO calculations and interpret the output results treated at the
ab initio RHF/3-21G level.

17) Study the mechanism of SN2 reaction between Cl- and CH3Br involving a Walden
inversion computationally.

68
 18) Perform a geometry optimization followed by a frequency assessment (opt+freq
keyword) using the B3LYP method and 6-31-G(d) basis set on a given set of small
molecules i.e. BH3, CH4.
Suggestive: A greater number of molecules may be studied as per instructions received
from the concerned teacher.

19) Based on the fundamentals of conceptual DFT calculate the ionization potential (IP),
electron affinity (EA), electronegativity and electron chemical potential of a given set
of molecules.

20) Perform molecular docking of Sulfonamide-type D-Glucose inhibitor into MurrD

active site using Argus Lab.

21) Perform molecular dynamics (MD) simulation of a given alkali metal ion in aqueous
function (RDF)

Essential/recommended readings

Theory:
1. Lewars, E. (2003), Computational Chemistry, Kluwer academic Publisher.
2. Cramer, C.J. (2004), Essentials of Computational Chemistry, John Wiley & Sons.
3. Hinchcliffe, A. (1996), Modelling Molecular Structures, John Wiley & Sons.
4. Leach, A.R. (2001), Molecular Modelling, Prentice-Hall.
5. House, J.E. (2004), Fundamentals of Quantum Chemistry, 2nd Edition, Elsevier.
6. McQuarrie, D.A. (2016), Quantum Chemistry, Viva Books.
7. Levine, I. N.; Physical Chemistry, 5th Edition, McGraw –Hill.

Practical:
1. https://www.afs.enea.it/software/orca/orca_manual_4_2_1.pdf
2. https://dasher.wustl.edu/chem430/software/avogadro/learning-avogadro.pdf
3. http://www.arguslab.com/arguslab.com/ArgusLab.html
4. https://barrett-group.mcgill.ca/tutorials/Gaussian%20tutorial.pdf
5. https://gaussian.com/techsupport/
6. https://gaussian.com/man/
7. https://gaussian.com/wp-content/uploads/dl/gv6.pdf
8. https://dasher.wustl.edu/chem478/software/spartan-manual.pdf
9. http://www.mdtutorials.com/gmx/
10. https://vina.scripps.edu/manual/

Important Instruction Note on working approach:

69
 • A student is required to perform/investigate a minimum of 10 exercises from the
given set of exercises.
• The students may use open source softwares; ArgusLab, Avogadro and ORCA. In
case a licenced version softwares is available, if procured by the college, other
licenced softwares may also be used.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

70
DISCIPLINE SPECIFIC ELECTIVE COURSE – 13 (DSE-13): Research Methodology
for Chemists

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title Credits Credit distribution of the Eligibility Pre-

& Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice (if any)
Research 04 03 -- 01 Class 12th
Methodology with
for Chemists Physics,
(DSE-13) Chemistry

Learning objectives

The objectives of this course are as follows:

• To make the students aware of fundamental but mandatory ethical practices in

chemistry.
• To introduce the concept of data analysis.
• To learn to perform literature survey in different modes.
• To make the students aware of safety handling and safe storage of chemicals.
• To make students aware about plagiarism and how to avoid it.
• To teach the use of different e-resources.

Learning outcomes

By studying this course, students will be able to:

• Follow ethical practices in chemistry
• Do Data analysis
• Literature survey in different modes
• Use e-resources.
• Avoid plagiarism, understand the consequences and how to avoid

71
SYLLABUS OF DSE-13

UNIT – 1: Scope of Research (Hours: 3)

Introduction, overview of research process: define research problem, review literature,

formulate hypothesis, design research/experiment, collect and analyse data, interpret and report,
scope and importance.

UNIT – 2: Literature Survey, Databases and Research metrics (Hours: 15)

Print: Sources of information: Primary, secondary, tertiary sources; Journals: Journal

abbreviations, Digital: Databases and their responsible use: Google Scholar, Web of science,
Scopus, UGC INFONET, SciFinder, PubMed, ResearchGate, E-consortium, e-books; Search
techniques: Phrase, Field, Boolean, Proximity, Concept, Limiting/Refining Search Results.
Research metrics: Impact factor of Journal, h-index, i10 index, Altmetrics, Citation index.
Author identifiers/or profiles: ORCID, Publons, Google Scholar, ResearchGate, VIDWAN

UNIT – 3: Communication in Science (Hours: 12)

Types of technical documents: Full length research paper, book chapters, reviews, short
communication, project proposal, Letters to editor, and thesis.
Thesis writing – different steps and software tools (Word processing, LaTeX, Chemdraw,
Chemsketch etc) in the design and preparation of thesis, layout, structure (chapter plan) and
language of typical reports, Illustrations and tables, bibliography, referencing: Styles (APA,
Oxford etc), annotated bibliography, Citation management tools: Mendeley, Zotero and
Endnote; footnotes. Oral presentation/posters – planning, software tools, creating and making
effective presentation, use of visual aids, importance of effective communication, electronic
manuscript submission, effective oral scientific communication and presentation skills.

UNIT – 4: Research and Publication ethics (Hours: 9)

Scientific Conduct: Ethics with respect to science and research, Scientific Misconducts:
falsification, fabrication and plagiarism, similarity index, software tools for finding plagiarism
(Turnitin, Urkund etc), redundant dublications

Publication Ethics: Introduction, COPE (Committee on Publication Ethics) guidelines; conflicts

of interest, publication misconduct: problems that lead to unethical behaviour and vice versa,
types, violation of publication ethics, authorship and contributorship, predatory publishers and
journals

IPR - Intellectual property rights and patent law, commercialization, copy right, royalty, trade
related aspects of intellectual property rights (TRIPS)

UNIT – 5: Statistical analysis for chemists (Hours: 6)

Types of data, data collection-Methods and tools, data processing, hypothesis testing, Normal
and Binomial distribution, tests of significance: t-test, F-test, chi- square test, ANOVA, multiple
range test, regression and correlation.

Features of data analysis with computers and softwares -Microsoft Excel, Origin, SPSS

72
Practical component Credits: 01
(Laboratory periods:15 classes of 2 hours each)

1. Collection of journal articles on a particular topic using Google Scholar and creating a
database.
2. Collection of journal articles on a particular topic using Science Direct and creating a
database.
3. Collection of journal articles on a particular topic using Scopus and creating a database.
4. Drawing chemical structure, reactions and mechanisms using Chemsketch or ISIS draw
or any other software.
5. Collection of chemical structure using ChemSpider and creating a database.
6. Curve fitting using freely available softwares/apps (any one)
7. Making of power point presentation
8. Experimental learning of safe storage hazardous chemicals
9. Experimental learning of handling of hazardous chemicals
10. Technical writing on topics assigned.
11. Demonstration for checking of plagiarism using recommended software

Essential/recommended readings:

1. Dean, J. R., Jones, A. M., Holmes, D., Reed, R., Weyers, J. & Jones, A. (2011) Practical
skills in chemistry. 2nd Ed. Prentice-Hall, Harlow.
2. Hibbert, D. B. & Gooding, J. J. (2006) Data analysis for chemistry. Oxford University
Press.
3. Topping, J. (1984) Errors of observation and their treatment. Fourth Ed., Chapman Hall,
London.
4. Harris, D. C. Quantitative chemical analysis. 6th Ed., Freeman (2007) Chapters 3-5.
5. Levie, R. de, how to use Excel in analytical chemistry and in general scientific data
analysis. Cambridge Univ. Press (2001) 487 pages.
6. Chemical safety matters – IUPAC – IPCS, Cambridge University Press, 1992.
OSU safety manual 1.01

Note:
• Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

• The students are required to opt one paper each from DSEs 1-3 in Semester 3,
DSEs 4-6 in Semester 4, DSEs 7-9 in Semester 5 and DSEs 10-13 in Semester 6.

• Research Methodology (DSE 13) shall be offered as one of the DSE courses in
semester VI or VII. If a student wishes to pursue four years Honours Degree with
Research, he/she shall compulsorily opt for a Research Methodology course in
either Semester VI or VII.

73
 BSC. (PHYSICAL SCIENCES)- CHEMISTRY COMPONENT
SEMESTER - IV

DISCIPLINE SPECIFIC CORE COURSE CHEM-DSC -10: Chemistry- IV: Chemistry of

Carboxylic Acids & their Derivatives, Amines and Heterocycles

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title Credits Credit distribution of the Eligibility Pre-

& Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Chemistry 04 02 - 02 Class 12th
of with Physics,
Carboxylic Chemistry,
Acids & Mathematics
their
Derivatives,
Amines and
Heterocycles
DSC-10:
Chemistry-
IV

Learning Objectives

The Learning Objectives of this course are as follows:

• To make students learn about the chemistry of carboxylic acids and their derivatives
(aliphatic and aromatic)
• To give basic understanding of amines (aliphatic & aromatic), diazonium salts
• To provide basic understanding of heterocyclic systems.

Learning outcomes

By studying this course, students will be able to:

• Understand reactions of carboxylic acids, esters, amides, amines and diazonium salts
• Understand the concept of protection and deprotection.
• Use the synthetic chemistry learnt in this course to do functional group transformations.
• Gain theoretical understanding of chemistry of heterocyclic compounds.

Syllabus
Unit 1: Carboxylic Acids and their Derivatives (aliphatic and aromatic) ( 1 3 Lectures)
Preparation: Oxidation reactions of alcohols, aldehydes and ketones, Acidic and alkaline

74
 hydrolysis of esters; Reactions: Hell-Volhard Zelinsky reaction,
Carboxylic acid derivatives (aliphatic): Preparation: Acid chlorides, anhydrides, esters and
amides from acids and their interconversion, Claisen condensation. Reactions: Relative
reactivities of acid derivatives towards nucleophiles, Reformatsky reaction, Perkin
condensation.
Active methylene compounds: Keto-enol tautomerism. Preparation and synthetic applications
of ethyl acetoacetate

Unit 2: Amines (aliphatic & aromatic) and Diazonium Salts (Hours:10)

Amines
Preparation: from alkyl halides, Gabriel's Phthalimide synthesis, Hoffmann bromamide
reaction. Reactions: Hoffmann vs Saytzeff elimination, carbylamine test, Hinsberg test, reaction
with HNO2, Schotten-Baumann reaction. Electrophilic substitution (case aniline): nitration,
bromination, sulphonation; basicity of amines.
Diazonium salt
Preparation: from aromatic amines; Reactions: conversion to benzene, phenol and dyes.

Unit 3: Heterocyclic Compounds (Hours: 7)

Introduction, classification, structure, nomenclature and uses. Preparation and properties of the
following heterocyclic compounds with reference to electrophilic and nucleophilic
substitution: furan, pyrrole, thiophene, and pyridine.

Practical Component: Credits: 02

(Laboratory periods: 60)

1. Systematic qualitative analysis and preparation of suitable crystalline derivative

(carboxylic acids, carbonyl, alcohols, phenols, amines (1°, 2°, 3°) and amides).
2. Preparation:
a. Acetylation of Aniline and Phenols.
b. Benzoylation of Aniline and phenols
The above derivatives should be prepared using 0.5-1g of the organic compound. The solid
samples must be collected and may be used for recrystallization and melting point.

References:

Theory:
1. Morrison, R. N.; Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd.
(Pearson Education).
2. Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt. Ltd. (Pearson

75
 Education).
3. Ahluwalia, V.K.; Bhagat, P.; Aggarwal, R.; Chandra, R. (2005), Intermediate for Organic
Synthesis, I.K. International.
4. Solomons, T. W. G.; Fryhle, C. B. ; Snyder, S. A. (2016), Organic Chemistry, 12th Ed.,
Wiley.
Practical:
1. Ahluwalia, V.K.; Dhingra, S.; Gulati, A. (2005), College Practical Chemistry, University
Press (India) Ltd.
2. Ahluwalia, V.K.; Dhingra, S. (2004), Comprehensive Practical Organic Chemistry:
Qualitative Analysis, University Press.
3. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I, I K
International Publishing House Pvt. Ltd., New Delhi.
4. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume II, I K
International Publishing House Pvt. Ltd., New Delhi.
5. Vogel, A.I. (1972), Textbook of Practical Organic Chemistry, Prentice-Hall.

6. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of
Quantitative Chemical Analysis, John Wiley and Sons.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

76
 BSC. (PHYSICAL SCIENCES)- CHEMISTRY COMPONENT
SEMESTER - V

DISCIPLINE SPECIFIC CORE COURSE CHEM-DSC -13: Chemistry- V: Coordination

Chemistry and Organometallics

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Coordination 04 02 - 02 Class 12th
Chemistry and with Physics,
Organometallics Chemistry,
DSC-13: Mathematics
Chemistry- V

Learning Objectives

The Learning Objectives of this course are as follows:

• To develop basic understanding of coordination chemistry and organometallics which are of
immense importance to biological systems, qualitative quantitative analysis, catalysis, medicines,
paints and pigments etc.
• The students learn nomenclature, isomerism and bonding in coordination compounds with special
emphasis on important coordination compounds in the biological system.
• To understand classification of organometallic compounds, the concept of hapticity and the 18-
electron rule governing the stability of a wide variety of organometallic species with special
emphasis on metal carbonyls.

Learning outcomes

By studying this course, students will be able to:

• Understand terms: ligand, denticity of ligands, chelate, coordination number.
• Systematically name coordination compounds.
• Discuss the various types of isomerism possible in Octahedral and Tetrahedral coordination
compounds.
• Use Valence Bond Theory to predict the structure and magnetic behaviour of metal complexes
and understand the terms inner and outer orbital complexes.
• Explain the meaning of the terms ∆o., ∆t, pairing energy, CFSE, high spin and low spin and
how CFSE affects thermodynamic properties like lattice enthalpy and hydration enthalpy.

77
 • Explain magnetic properties and colour of complexes on basis of Crystal Field Theory
• Apply 18-electron rule to rationalize the stability of metal carbonyls and related species.
• Learn how IR data can be used to understand extent of back bonding in metal carbonyls.

Syllabus

Unit 1: Introduction to Coordination compounds (Hours: 6)

Brief discussion with examples of types of ligands, denticity and concept of chelate. IUPAC
system of nomenclature of coordination compounds (mononuclear and binuclear) involving
simple monodentate and bidentate ligands. Structural and stereoisomerism in complexes
with coordination numbers 4 and 6.

Unit 2: Bonding in Coordination Compounds (Hours: 14)

Valence Bond Theory (VBT): Salient features of theory, concept of inner and outer orbital
complexes, Drawbacks of VBT.
Crystal Field Theory: Splitting of d orbitals in octahedral symmetry. Crystal field effects for
weak and strong fields, Crystal field stabilization energy (CFSE), concept of pairing energy,
Factors affecting the magnitude of Δ, Spectrochemical series, Splitting of d orbitals in
tetrahedral symmetry, Comparison of CFSE for octahedral and tetrahedral fields, tetragonal
distortion of octahedral geometry, Jahn-Teller distortion

Unit 3: Organometallic Chemistry (Hours: 10)

Definition and classification with appropriate examples based on nature of metal-carbon bond
(ionic, sigma, pi and multicentre bonds), Structure and bonding of methyl lithium and Zeise’s
salt, Structure and bonding of ferrocene, mononuclear and polynuclear carbonyls of 3d
metals, 18-electron rule as applied to carbonyls, π-acceptor behaviour of carbon monoxide
(MO diagram of CO to be discussed), synergic effect and use of IR data to explain extent of
back bonding.

Practical Component Credits:02

(Laboratory periods:60)
1. Estimation of Mg2+ by direct complexometric titrations using EDTA.
2. Estimation of Zn2+ by direct complexometric titrations using EDTA.
3. Estimation of Ca2+ by direct complexometric titrations using EDTA.
4. Estimation of total hardness of a given sample of water by complexometric titration.
5. Determination of the composition of the Fe3+ - salicylic acid complex / Fe2+-1, 10-
phenanthroline complex in solution by Job’s method.

78
 6. Determination of the composition of the Fe3+ - salicylic acid complex / Fe2+-1,10-
phenanthroline complex in solution by mole ratio method
7. Preparation of the following inorganic compounds:
a). Tetraamminecopper(II) sulphate
b). Potassium trioxalatoferrate(III) trihydrate
c). Chrome alum
d). Cis- and trans-Potassium diaquadioxalatochromate(III)
8. Any suitable experiment (other than the listed ones) based upon complexation reactions.

References:

Theory:
1. Huheey, J.E.; Keiter, E.A., Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry-
Principles of Structure and Reactivity, Pearson Education.
2. Shriver, D.D.; Atkins, P.; Langford, C.H. (1994), Inorganic Chemistry 2nd Ed., Oxford University
Press.
3. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010), Inorganic Chemistry,
5th Edition, W. H. Freeman and Company.
4. Cotton, F.A.; Wilkinson, G.; Gaus, P.L. Basic Inorganic Chemistry, 3rd Edition, Wiley India.
5. Douglas, B.E.; McDaniel, D.H.; Alexander, J.J. (1994), Concepts and Models of Inorganic
Chemistry, John Wiley & Sons.
6. Greenwood, N.N.; Earnshaw, A. (1997), Chemistry of the Elements, 2nd Edition, Elsevier.
7. Lee, J.D.; (2010), Concise Inorganic Chemistry, Wiley India.
8. Sodhi G.S., Principles of Inorganic Chemistry, 3rd Edition, Viva Books India.

Practicals:
1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of Quantitative
Chemical Analysis, John Wiley and Sons.
2. Marr, G.; Rockett, B.W. (1972), Practical Inorganic Chemistry, Van Nostrand Reinhold.
3. Dua A, Manav N, Practical Inorganic Chemistry, (2017), Manakin Press.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

79
 BSC. (PHYSICAL SCIENCES)- CHEMISTRY COMPONENT
SEMESTER -VI

DISCIPLINE SPECIFIC CORE COURSE -16: Chemistry -VI Quantum Chemistry and
Spectroscopy

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Quantum 04 02 -- 02 Class 12th NA
Chemistry with Physics,
and Chemistry,
Spectroscopy Mathematics
DSC-16:
Chemistry-
VI

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce the concepts and methodology of quantum mechanics

• Application of Quantum chemistry to spectroscopy
• To establish the relation between structure determination and spectra.

Learning outcomes
By studying this course, students will be able to:

• Understand basic principles of quantum mechanics: operators, eigen values, averages,

probability distributions.
• Understand and use basic concepts of microwave, IR and UV-VIS spectroscopy for
interpretation of spectra.

Syllabus

Unit 1: Quantum Chemistry (Hours: 16)

80
Postulates of quantum mechanics, quantum mechanical operators.

Schrodinger equation and its application to free particle and particle in a 1-D box (complete
solution), quantization, normalization of wave functions, concept of zero-point energy.

Qualitative treatment of H and H like atoms. Setting up of Schrodinger equation for many
electron atoms.

Rotational Motion: Schrödinger equation of a rigid rotator and brief discussion of its results
(solution not required). Quantization of rotational energy levels.

Vibrational Motion: Schrödinger equation of a linear harmonic oscillator and brief discussion
of its results (solution not required). Quantization of vibrational energy levels.
Unit 2: Spectroscopy (Hours: 14)

Electromagnetic radiation and its interaction with matter. Lambert-Beer’s law, Jablonski’s
diagram. Florescence and Phosphorescence.
Difference between atomic and molecular spectra. Born- Oppenheimer approximation:
Separation of molecular energies into translational, rotational, vibrational and electronic
components.

Microwave Spectroscopy: Microwave (pure rotational) spectra of diatomic molecules. Selection

rules.
Structural information derived from rotational spectroscopy.

IR Spectroscopy: Selection rules, IR spectra of diatomic molecules. Structural information

derived from vibrational spectra. Effect of hydrogen bonding (inter- and intramolecular) and
substitution on vibrational frequencies.

Electronic Spectroscopy: Electronic excited states. Free electron model and its application to
electronic spectra of polyenes. chromophores, auxochromes, bathochromic and hypsochromic
shifts.

Practical component Credits:02

(Laboratory periods: 60 )

UV/Visible spectroscopy

1. Study the 200-500 nm absorbance spectra of KMnO4 and K2Cr2O7 (in 0.1 M H2SO4) and
determine the λmax values. Calculate the energies of the two transitions in different units
-1 -1 -1
(J molecule , kJ mol , cm , eV).
2. Study the pH-dependence of the UV-Vis spectrum (200-500 nm) of K2Cr2O7
3. Record the 200-350 nm UV spectra of the given compounds (acetone, acetaldehyde, 2-
propanol, acetic acid) in water. Comment on the effect of structure on the UV spectra of

81
 organic compounds.

Colorimetry

4. Verify Lambert-Beer’s law and determine the concentration of CuSO4/ KMnO4/ K2Cr2O7/
CoCl2 in a solution of unknown concentration
5. Determine the concentrations of KMnO4 and K2Cr2O7 in a mixture.
6. Study the kinetics of iodination of propanone in acidic medium.
7. Determine the amount of iron present in a sample using 1, 10-phenanthroline.
8. Determine the dissociation constant of an indicator (phenolphthalein).
9. Study the kinetics of interaction of crystal violet/ phenolphthalein with sodium hydroxide.

References:

Theory:

1. Banwell, C.N.; McCash, E.M.(2006), Fundamentals of Molecular Spectroscopy,

Tata McGraw- Hill.
2. Kapoor, K.L.(2015),A Textbook of Physical Chemistry, McGraw Hill Education,
,Vol 4, 5th Edition, McGraw Hill Education.
3. McQuarrie, D.A.(2016),Quantum Chemistry, Viva Books.
4. Chandra, A. K.(2001),Introductory Quantum Chemistry, Tata McGraw-Hill.
5. Dua A and Tyagi P, Molecular Spectroscopy: Quantum to Spectrum, (2022)
Atlantic Publishers & Distributors Pvt Ltd.
6. Dua A, Singh C, Quantum Chemistry: Classical to Computational (2015)
ManakinPress.

Practical:

1. Khosla, B.D.; Garg, V.C.; Gulati, A. (2015),Senior Practical Physical Chemistry,

R. Chand & Co, New Delhi.
2. Kapoor, K.L. (2019),A Textbook of Physical Chemistry, Vol.7, 1st Edition,
McGraw Hill Education.
3. Garland, C. W.; Nibler, J. W.; Shoemaker, D. P.( 2003),Experiments in Physical
Chemistry, 8th Edition, McGraw-Hill, New York.

Additional Resources:

1. Castellan, G. W .(2004),Physical Chemistry, Narosa.

2. Petrucci, R. H.(1989),General Chemistry: Principles and Applications, Macmillan
Publishing

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

82
 POOL OF DISCIPLINE SPECIFIC ELECTIVES FOR SEMESTER -III/IV/V/VI

SEMESTER III

DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -1: Main Group Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lect Tutorial Practical of the
ure / course (if
Practice any)
Chem-DSE 1: 04 02 - 02 Class XII
Main Group with
Chemistry Science

Learning Objectives

The Learning Objectives of this course are as follows:

• To provide basic understanding of the fundamental principles of metallurgy through study of the
different methods of extraction and refining of metals.
• To illustrate the diversity and fascinating aspects of inorganic chemistry through the study of
structure, properties and utilities of s- and p-block elements and their compounds.

Learning outcomes

By studying this course, students will be able to:

• Understand the basis of occurrence of metals in nature and the methods that can be applied on
minerals to extract the metals from them.
• Explain the importance of free energy of formation of oxides with the choice of reducing
agents for extracting the metals.
• Understand and explain the importance of refining of metals and the choice of a refining
procedure.
• Explain the group trends observed for different properties of s and p block elements.
• Explain the structures and the bonding of compounds of s- and p- block elements
• Explain the unique properties of alkali metals and some other main group elements
• Understand and explain the polymerization mechanism of inorganic ions to generate inorganic
polymers and the difference between organic and inorganic polymers.

Syllabus

83
 Unit 1: General Principles of Metallurgy (Hours: 6)

Chief modes of occurrence of metals based on standard electrode potentials. Ellingham diagrams for
reduction of metal oxides using carbon and carbon monoxide as reducing agent. Electrolytic
Reduction, Hydrometallurgy with reference to cyanide process for silver and gold. Methods of
purification of metals: Electrolytic process, Van Arkel-De Boer process, Zone refining.

Unit 2: General Properties (4 Hours)

General group trends of s- and p-block elements with special reference to melting and boiling points,
flame colour, metallic character and complex formation tendency, diagonal relationship and
anomalous behaviour of first member of each group, Alkali metal solutions in liquid ammonia

Unit 3: Structure, Bonding, Properties and Applications (Hours: 16)

Structure, bonding, properties (Acidic/Basic nature, stability, ionic/covalent nature,

oxidation/reduction, hydrolysis, thermal stability) and applications of the following:
Crown Ethers and cryptates of Alkali metals
Hydrides: hydrides of Group 13 (only diborane), Group 14, Group 15 (EH3 where E = N, P, As,
Sb, Bi), Group 16 and Group 17.
Oxides: Oxides of nitrogen, phosphorus and sulphur.
Oxoacids: oxoacids of phosphorus, sulphur and chlorine
Halides of phosphorus

Unit 4: Inorganic Polymers (4 Hours)

Preparation, properties, structure and uses of the following:

Borazine, Silicates and Silicones.

Practicals Credits:02
(Laboratory periods:60)
Qualitative semi-micro analysis of mixtures containing 2 anions and 2 cations (preferably 7-8
mixtures). Emphasis should be given to the understanding of the chemistry of different reactions.
The following radicals are suggested:

CO32-, NO2- , S2-, SO32-, SO42- , S2O32-, CH3COO-, F-, Cl-, Br-, I- , NO3- , BO33-, C2O42-, PO43-,
NH4+, K+, Pb2+ , Cu2+, Cd2+, Bi3+, Sn2+, Sb3+, Fe3+, Al3+, Cr3+, Zn2+, Mn2+, Co2+, Ni2+, Ba2+, Sr2+,
Ca2+, Mg2+.
The mixtures may contain combination of anions/one interfering anion.
Spot tests should be preferred wherever applicable.

References:
Theory:

84
1. Lee, J.D.; (2010), Concise Inorganic Chemistry, Wiley India.
2. Huheey, J.E.; Keiter, E.A.; Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry- Principles of
Structure and Reactivity, Pearson Education.
3. Douglas, B.E.; McDaniel, D.H.; Alexander, J.J. (1994), Concepts and Models of Inorganic
Chemistry, John Wiley & Sons.
4. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010), Shriver and Atkins
Inorganic Chemistry, 5th Edition, Oxford University Press.
5. Housecraft, E. H.; Sharpe, A.G. (2018), Inorganic Chemistry, 5th Edition, Pearson.
6. F.A. Cotton & G. Wilkinson (1999), Advanced Inorganic Chemistry, 6th Edition, John Wiley &
Sons.

Practicals:
1. Vogel, A.I. (1972), Qualitative Inorganic Analysis, Longman.
2. Svehla, G. (1996), Vogel’s Qualitative Inorganic Analysis, Prentice Hall.
3. Dua A, Manav N, Practical Inorganic Chemistry, (2017), Manakin Press.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

85
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -2: Green Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lectur Tutorial Practical/ of the
e Practice course (if
any)
Chem-DSE-2: 04 02 - 02 Class XII
Green with
Chemistry Science

Learning Objectives

The Learning Objectives of this course are as follows:

• To learn about the environmental status, public awareness in evolution, principles involved in
green chemistry, bio-catalytic reactions, global warming and its control measures, availability of
green analytical methods.

• To practice chemistry in the safest way possible

• To imbibe safeworking conditions in the laboratories as well as the chemical industry

extending to society in a sustainable future for the planet.

Learning outcomes

By studying this course, students will be able to:

● Understand the twelve principles of green chemistry and also build the basic
understanding of toxicity, hazard and risk related to chemical substances.
● Calculate atom economy, E-factor and relate them in all organic synthesis
● Appreciate the use of catalyst over stoichiometric reagents
● Learn to use green solvents, renewable feedstock and renewable energy sources
for carrying out safer chemistry
● Appreciate the use of green chemistry in problem solving skills and critical
thinking to innovate and find solutions to environmental problems.
● Learn to design safer processes, chemicals and products through understanding
of inherently safer design (ISD)
● Appreciate the success stories and real-world cases as motivation for them
topractice green chemistry

Syllabus

86
Unit 1: Introduction (Hours: 8)

Definition of green chemistry and how it is different from conventional chemistry and environmental
chemistry.

Need of green chemistry.

Importance of green chemistry in- daily life, Industries and solving human health problems (four
examples each).

A brief study of Green Chemistry Challenge Awards (Introduction, award categories and study about
five last recent awards).

.
Unit 2: Twelve Principles of Green Chemistry (Hours: 12)

The twelve principles of the Green Chemistry with their explanations Special emphasis on
the following:
• Prevention of waste / by products, pollution prevention hierarchy.
• Green metrics to assess greenness of a reaction: environmental impact factor, atom
economy and calculation of atom economy.
• Green solvents-supercritical fluids, water as a solvent for organic reactions, ionic liquids,
solvent less reactions, solvents obtained from renewable sources.
•Catalysis and green chemistry- comparison of heterogeneous and homogeneous catalysis,
biocatalysis, asymmetric catalysis and photocatalysis.
• Green energy and sustainability.
• Real-time analysis for pollution prevention.

Prevention of chemical accidents, designing greener processes, principles of inherent safer design
(ISD). Bhopal Gas Tragedy (safer route to carbaryl) and Flixborough accident (safer route to
cyclohexanol), subdivision of ISD, minimization, simplification, substitution, moderation and
limitation.

Unit 3: Real-world Cases in Green Chemistry (Hours: 10)

Discussion of the following Real-world Cases in green chemistry: Surfactants for carbon dioxide –
replacing smog producing and ozone depleting solvents with CO2 for precision cleaning and dry
cleaning of garments. Designing of environmentally safe marine antifoulant. Right fit pigment:
Synthetic azo pigments to replace toxic organic and inorganic pigments. An efficient, green synthesis
of a compostable and widely applicable plastic (polylactic acid) made from corn.

Practical Component Credits:02

87
 (Laboratory periods:60)
Characterization by melting point, UV-Visible spectroscopy, IR spectroscopy and any other
specific method should be done (wherever applicable).
1. Preparation and characterization of nanoparticles of gold using tea leaves/silver
nanoparticles using plant extracts.
2. Preparation of biodiesel from waste cooking oil and characterization (TLC, pH,
solubility, combustion test, density, viscosity, gel formation at low temperature and IR
can be provided).
3. Benzoin condensation using thiamine hydrochloride as a catalyst instead of cyanide.
4. Extraction of D-limonene from orange peel using liquid CO2 prepared from dry ice.
5. Mechanochemical solvent free, solid-solid synthesis of azomethine using p-toluidine and
o-vanillin/p-vanillin.
6 Microwave-assisted Knoevenagel reaction using anisaldehyde, ethyl cyanoacetate and
ammonium formate.
7. Photoreduction of benzophenone to benzopinacol in the presence of sunlight.
8. Photochemical conversion of dimethyl maleate to dimethyl fumarate (cis-trans
isomerisation)
9. Benzil- Benzilic acid rearrangement: Preparation of benzilic acid in solid state under
solvent-free condition.

References:

Theory:
1. Anastas, P.T., Warner, J.C. (2014), Green Chemistry, Theory and Practice, Oxford
University Press.
2. Lancaster, M. (2016), Green Chemistry: An Introductory Text, 3rd Edition, RSC
Publishing.
3. Cann, M. C., Connely, M.E. (2000), Real-World cases in Green Chemistry, American
Chemical Society, Washington.
4. Matlack, A.S. (2010), Introduction to Green Chemistry, 2nd Edition, Boca Raton:
CRC Press/Taylor & Francis Group publisher.
5. Alhuwalia, V.K., Kidwai, M.R. (2005), New Trends in Green chemistry, Anamalaya
Publishers.
6. Sidhwani, I.T, Sharma, R.K. (2020), An Introductory Text on Green Chemistry,
Wiley India Pvt Ltd.

Practicals:
7. Kirchoff, M.; Ryan, M.A. (2002), Greener approaches to undergraduate chemistry
experiment, American Chemical Society, Washington DC.

88
 8. Sharma, R.K.; Sidhwani, I.T.; Chaudhari, M.K. (2013), Green Chemistry
Experiments: A monograph, I.K. International Publishing House Pvt Ltd. New Delhi.
9. Pavia, D.L.; Lamponam, G.H.; Kriz, G.S.W. B. (2012), Introduction to organic
Laboratory Technique- A Microscale approach, 4th Edition, Brooks-Cole
Laboratory Series -for Organic chemistry.
10. Sindhwani I.T. (2015), Wealth from Waste: A green method to produce biodiesel
from waste cooking oil and generation of useful products from waste further
generated. DU Journal of Undergraduate Research and Innovation, 1(1),131-151. ISSN:
2395- 2334.
11. Sidhwani, I.T; Sharma, R.K. (2020), An Introductory Text on Green Chemistry,
Wiley India Pvt Ltd.
12. Monograph on Green Chemistry Laboratory Experiments, Green Chemistry Task
Force Committee, Department of Science and Technology, Government of India.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University
of Delhi, from time to time.

89
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 3: Chemistry of Colloids and
Adsorption

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice (if any)
Chem-DSE 3: 04 02 - 02 Class XII
Chemistry of with
Colloids and Science
Adsorption

Learning Objectives

The Learning Objectives of this course are as follows:

• To develop basic concepts of colloids and colloidal phenomenon.
• Preparation and characterization of sols, understanding about applications of colloid in
food, petroleum and cosmetic industry.
• Basic understanding of adsorption, types of adsorption, chemistry of adsorption and its
applications.

Learning outcomes

By studying this course, students will be able to:

• Understand colloid solutions, preparation of sols.
• Understand the concept of Electrical double layer, charge on colloidal particles.
• Characterize the colloids sols, learn colloid phenomenon like Tyndall effect, Brownian
movement, electrophoresis, dialysis, coagulation and flocculation.
• Understand adsorption, types of adsorption. Characteristics, factors affecting adsorption and
its applications

Syllabus

Unit 1: Colloidal State (Hours: 8)

Distinction among true solutions, colloids and suspensions, components of Colloids, classification
of colloids - lyophilic, lyophobic; Preparation methods and properties of lyophobic solutions,
Hydrophile-lyophile balance (HLB), multi molecular, macromolecular and associated colloids
(micelles formation), Schulze -Hardy law.

Unit 2: Preparation and Properties of Colloids (Hours: 14)

90
Methods of preparation of colloids, Tyndall effect, Brownian movement, coagulation and flocculation;
electrophoresis, dialysis.

Emulsification by surfactants, selection of surfactants as emulsifying agent, colloidal phenomenonin

food chemistry, Protein based functional colloids.

Unit 3: Surface Chemistry (Hours: 8)

Adsorption, Distinction between adsorption and absorption, Types of Adsorption, Physisorption
and chemisorption and their characteristics, factors affecting adsorption of gases on solids -
Freundlich and Langmuir adsorption isotherms, Adsorption from solutions. Applications of
Adsorption phenomenon in living systems.

Practical component Credits: 02

(Laboratory periods: 60)
1. Preparation of Colloidal Sols of following
a. Egg Albumin
b. Starch /Gum
c. Ferric chloride
d. Aluminum hydroxide
e. Antimony Sulphide

2. To find out the precipitation values of Antimony Sulphide sol by using monovalent,
bivalentand trivalent cations.
3. To verify the Schulze -Hardy law.
4. To verify the Freundlich’s Adsorption isotherms.
5. Study of adsorption of HAc on charcoal and prove the validity of Langmuir’s adsorption
isotherms
6. Study of adsorption of Oxalic acid on charcoal and prove the validity of Langmuir’s adsorption
isotherms.

References:
Theory:
1. Puri B. R., Sharma L. R. and Pathania M.S., (2020) Principles of Physical Chemistry, Vishal
Publishing Co.Jalandhar, Punjab, India.
2. Kapoor K L, Text Book of Physical Chemistry, Vol. 4, McGraw Hill Education
(India) Private Limited, Chennai, India.
3. Evans D F and Wennerström’s, The Colloidal Domain, Second Edition, John Wiley & Sons
Inc.
4. Adamson A. W. and Gast A., Physical Chemistry of Surfaces (Main text) Sixth Edition, John
Wiley & Sons Inc.
5. Berg J. C., An Introduction to Interfaces and Colloids, World Scientific Publishing Co., Inc.
New Jersey.
6. Israelachvili J. N., Intermolecular and Surface Forces, Elsevier Inc.

91
Practical:
1. Giri, S; Bajpai, D.N.; Pandey, O.P. Practical Chemistry, S. Chand Limited.
2. Khosla, B.D.; Garg, V.C.; Gulati, A.(2015), Senior Practical Physical Chemistry, R.
Chand & Co.
Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

92
 SEMESTER IV

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -4: Nanoscale Materials and their
Applications
Course title & Credits Credit distribution of the Eligibility Pre-
Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE-4: 04 02 - 02 Class XII
Nanoscale with
Materials and Science
their
Applications

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce nanoscale materials and their applications.
• To provide an insight into bottom-up and top-down-approach, the methods of synthesis of
nanoparticles, simple characterization techniques and applications of nanomaterials.

Learning outcomes

By studying this course, students will be able to:

● Understand the concept of nano dimensions.
● Know the various methods of preparation of nanomaterials.
● Understand the principles of optical and electron microscopy techniques of characterizing
nanomaterials.
● Understand and appreciate the real life applications of nanomaterials.

Syllabus

Unit 1: Introduction to Nanodimensions (Hours: 12)

0D, 1D, 2D nanomaterials, Quantum Dots, Nanoparticles, Nanostructures (nanowires, thin films,
nanorods), carbon nanostructures (carbon nanotubes, carbon nanofibers, fullerenes), Size Effects in
nano systems, Quantum confinement and its consequences, Semiconductors. Band structure and band
gap. Optical Properties Surface plasmon resonance

.
Unit 2: Preparation of Nanomaterials (Hours: 10)

93
 Top down and Bottom up approach, Photolithography. Ball milling. Vacuum deposition. Physical
vapor deposition (PVD), Chemical vapor deposition (CVD), Thermal decomposition, Chemical
reduction, Sol-Gel synthesis, Hydrothermal synthesis, Spray pyrolysis, Electrochemical deposition,
Pulsed Laser deposition. Characterization of nanomaterials: Basic principle of optical methods and
electron microscopy.

Unit 3: Applications of Nanomaterials (Hours: 8)

Nanomaterials as Catalysts, semiconductor nanomaterials as photocatalysts, Nanocomposites as

catalysts. Carbon nanostructures as catalytic nanoreactors, metal and metal oxides confined inside
carbon nanostructures, Nanowires and thin films for photonic devices (LEDs, solar cells, transistors).

Practical Component Credits:02

(Laboratory periods:60)
1. Synthesis of silver nanoparticles by chemical methods and characterization using UV-visible
spectrophotometer.
a. Turkevich Method
b. Burst Method
2. Synthesis of silver nanoparticles by green approach methods (using soluble starch, glucose or
cinnamon bark) and characterization using UV-visible spectrophotometer.
3. Synthesis of metal sulphide nanoparticles and characterization using UV-visible
spectrophotometer.
a. MnS
b. ZnS
c. CuS
4. Intercalation of hydrogen in tungsten trioxide and its conductivity measurement using
conductometer.
5. Synthesis of pure ZnO and Cu doped ZnO nanoparticles.
6. Phytochemicals mediated synthesis of gold nanoparticles (AuNPs) using tea leaves and to study
the effect of size on color of gold/silver nanoparticles.
7. Preparation of magnetic nanoparticles (MNPs) of Fe3O4 using green tea leaf extract.
8. Any suitable experiment (other than the listed ones) based upon complexation reactions.

References:

Theory:
1. West, A. R. (2014), Solid State Chemistry and Its Application, John Wiley and Sons Inc.
2. Smart, L. E.; Moore, E. A., (2012), Solid State Chemistry: An Introduction, CRC Press
Taylor & Francis.
3. Rao, C. N. R.; Gopalakrishnan, J. (1997), New Direction in Solid State Chemistry,
Cambridge University Press.

94
 4. Poole Jr.; Charles P.; Owens, Frank J. (2003), Introduction to Nanotechnology, John Wiley
and Sons. Inc. Harris, D. C. (2007), Quantitative Chemical Analysis, 6th Edition, Freeman.
5. Chattopadhyay, K.K.; Banerjee, A. N. (2009), Introduction to Nanoscience and
Technology, Prentice Hall India.

Practicals:
1. Orbaek, W.; McHale, M.M.; Barron, A. R.; Synthesis and Characterization of Silver
Nanoparticles for An Undergraduate Laboratory, J. Chem. Educ. 2015, 92, 339−344.
2. MacDiarmid, G.; Chiang, J.C.; Richter, A.F.; Somasiri, N.L.D.(1987), Polyaniline: Synthesis and
Characterization of the Emeraldine Oxidation State by Elemental Analysis, L. Alcaeer (ed.),
Conducting Polymers, 105-120, D. Reidel Publishing.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

95
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -5: Molecules of Life

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE-5: 04 02 - 02 Class XII
Molecules of with
Life Science

Learning Objectives

The Learning Objectives of this course are as follows:

• To deliver information about the chemistry of carbohydrates, proteins & enzymes and its
relevance in the biological system using suitable examples.
• To provide an insight into the structural principles that govern reactivity/physical /biological
properties of biomolecules as opposed to learning structural details.

Learning outcomes

By studying this course, students will be able to:

● Learn and demonstrate how the structure of biomolecules determines their chemical properties,
reactivity and biological uses.
● Gain an insight into the mechanism of enzyme action and inhibition.
● Understand the basic principles of drug-receptor interaction and SAR.

Syllabus

Unit 1: Carbohydrates (Hours: 12)

Classification of carbohydrates, reducing and non-reducing sugars, biological functions, general
properties and reactions of glucose and fructose, their open chain structure, epimers, mutarotation and
anomers, reactions of monosaccharides, determination of configuration of glucose (Fischer proof),
cyclic structure of glucose. Haworth projections. Cyclic structure of fructose. Linkage between
monosaccharides: structure of disaccharides (sucrose, maltose, lactose) and polysaccharides (starch
and cellulose) excluding their structure elucidation.

.
Unit 2: Amino acids, Peptides and Proteins (Hours: 10)

Classification of amino acids and biological uses of amino Acids, peptides and proteins. Zwitterion
structure, isoelectric point and correlation to acidity and basicity of amino acids. Determination of
primary structure of peptides, determination of N-terminal amino acid (by Edman method) and C–

96
 terminal amino acid (with carboxypeptidase enzyme). Synthesis of simple peptides (up to dipeptides)
by N-protection (t-butyloxycarbonyl) & C-activating groups (only DCC) and Merrifield solid phase
synthesis, Overview of primary, secondary, tertiary and quaternary structure of proteins, denaturation
of proteins.

Unit 3: Enzymes (Hours: 4)

Classification of enzymes and their uses (mention Ribozymes). Mechanism of enzyme action, factors
affecting enzyme action, Coenzymes and cofactors and their role in enzyme action, specificity of
enzyme action (including stereospecificity).
-
Unit 4: Nucleosides, Nucleotides and Nucleic Acids (Hours: 4)

Components of Nucleic acids: Adenine, guanine, thymine, cytosine and uracil (structure only), other
components of nucleic acids, nucleosides and nucleotides (nomenclature), structure of
polynucleotides; structure of DNA (Watson-Crick model) and RNA (types of RNA), difference
between DNA and RNA.
Practical Component Credits:02
(Laboratory periods:60)

1. Estimation of glucose by Fehling’s solution.

2. Determination of total sugar content by ferricyanide method
(volumetric/colorimetric method).
3. Study of the titration curve of glycine and determine the isoelectic point of glycine.
4. Estimation of proteins by Lowry’s method.
5. Qualitative tests for amino acids, proteins and carbohydrates.
6. Separation and identification of mixture of sugars by paper chromatography.
7. Separation and identification of mixture of Amino acids by paper chromatography.
8. Study of the action of salivary amylase on starch under optimum conditions and find
the enzyme activity.
9. Study the effect of temperature on activity of salivary amylase.
10. Extraction of DNA from onion/cauliflower.

References:

Theory:
1. Finar, I. L. Organic Chemistry (Volume 1 & 2), Dorling Kindersley (India) Pvt. Ltd.
(Pearson Education).
2. Morrison, R. N.; Boyd, R. N., Bhattacharjee, S.K. (2010), Organic
Chemistry, 7th Edition, Dorling Kindersley (India) Pvt. Ltd. (Pearson
Education India).
3. Berg, J. M.; Tymoczko, J. L.; Stryer, L. (2019), Biochemistry, 9th Ed., W. H.
Freeman Co Ltd.

97
 Practicals:
1. Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. (2012), Vogel's
Textbook of Practical Organic Chemistry, Pearson Education India.
2. Manual of Biochemistry Workshop, 2012, Department of Chemistry, University
of Delhi.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

98
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -6: Conductance, Electrochemistry
and Chemical Kinetics
CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Chem-DSE 6: 04 02 - 02 Class XII
Conductance, with
Electrochemistry Science
and Chemical
Kinetics

Learning Objectives

The Learning Objectives of this course are as follows:

• To develop basic understanding of electrolytic and galvanic cells.
• Measurementof conductance and its applications, measurement of emf and its applications.
• To understand reaction rate, order, activation energy and theories of reaction rates.

Learning outcomes

By studying this course, students will be able to:

• Explain the factors that affect conductance, migration of ions and application of
conductance measurement.
• Understand the importance of Nernst equation, measurement of emf, calculations of
thermodynamic properties and other parameters from the emf measurements.
• Understand rate law and rate of reaction, theories of reaction rates and catalysts; both
chemical and enzymatic.

Syllabus

Unit 1: Conductance (Hours: 8)

Conductivity, equivalent and molar conductivity and their variation with dilution for weak and
strong electrolytes, Kohlrausch Law of independent migration of ions, Ionic velocity, mobility and
their determination, transference number and its relation to ionic mobility, Conductometric
titrations (only acid-base).

99
Unit 2: Electrochemistry (Hours: 12)

Concept of reversible and irreversible electrochemical cells, Standard hydrogen electrode, standard
electrode potential, concept of EMF of a cell, measurement of EMF of a cell, Nernst equation and
its importance, types of electrodes (Reference and inert electrodes), electrochemical series.

Thermodynamics of a reversible cell, calculation of thermodynamic properties: G, H and S from EMF

data. Calculation of equilibrium constant from EMF data. pH determination using glass electrode,
Potentiometric titrations-qualitative treatment (acid-base and oxidation-reduction only).

Unit 3: Chemical Kinetics and Catalysis (Hours: 10)

The concept of reaction rates, effect of temperature, pressure, catalyst and other factors on reaction
rates. Order and molecularity of a reaction, integrated rate equations for zero, first and second order
reactions (derivation not required), half–life of a reaction, Concept of activation energy and its
calculation from Arrhenius equation.
Catalysis: Types of catalyst, specificity and selectivity, generalized treatment of catalyzed reactions
at solid surfaces. Enzyme catalysis, Michaelis-Menten mechanism, acid-base catalysis.

Practical component Credits:02

Laboratory periods: 60
1. Determination of molar conductance, degree of dissociation and dissociation constant of
aweak acid.
2. Perform the following conductometric titrations: Strong acid vs strong base.
3. Perform the following conductometric titrations: Weak acid vs strong base.
4. Determination of TDS of water from different sources.
5. Determination of Soil pH of soil collected from various locations.
6. Perform the potentiometric titrations of strong acid vs strong base
7. Perform the potentiometric titrations of Weak acid vs strong base.
8. Perform the potentiometric titrations of Potassium dichromate vs. Mohr's salt.
9. Perform the potentiometric titrations of KMnO4 vs. Mohr's salt.
10. Study the kinetics of acid hydrolysis of methyl acetate with hydrochloric acid.

References:
Theory:

100
 1. Castellan, G. W .(2004), Physical Chemistry, Narosa Publications.
2. Kapoor, K.L. (2015),A Textbook of Physical Chemistry, Vol.1, 6th Edition, McGraw Hill
Education.
3. Kapoor, K.L. (2015),A Textbook of Physical Chemistry, Vol.5, 3rd Edition, McGraw Hill
Education.
4. Puri, B.R., Sharma, L.R. and Pathania M.S. (2020),Principles of Physical Chemistry,
Vishal Publishing Co.
*
Practicals:
1. Khosla, B.D.; Garg, V.C.; Gulati, A.(2015), Senior Practical Physical Chemistry, R.
Chand & Co.Kapoor, K.L. (2019), A Textbook of Physical Chemistry, Vol 7, 1st
Edition, McGrawHill Education.
2. Batra, S.K., Kapoor, V and Gulati, S. (2017) 1st Edition, Experiments in Physical
Chemistry, Book Age series.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

101
 SEMESTER V

DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -7: Inorganic Materials of

Industrial Importance
CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE-7: 04 02 - 02 Class XII
Inorganic with
Materials of Science
Industrial
Importance

Learning Objectives

The Learning Objectives of this course are as follows:

• The course introduces learners to the importance of Inorganic compounds in Industries.
• To provide an insight into how the inorganic materials form a basis of the products used in day-
to-day life like silicates, fertilizers, surface coatings.

Learning outcomes

By studying this course, students will be able to:

• Learn the composition and applications of the different kinds of glass.
• Understand glazing of ceramics and the factors affecting their porosity.
• Give the composition of cement and discuss the mechanism of setting of cement.
• Explain the suitability of fertilizers for different kinds of crops and soil.
• Understand and explain the polymerization of inorganic ions to generate inorganic polymers
and the difference between organic and inorganic polymers.

Syllabus

Unit 1: Silicate Industries (Hours: 10)

Glass: Glassy state and its properties, classification (silicate and non-silicate glasses). Manufacture
and processing of glass. Composition and properties of the following types of glasses: Soda lime

102
glass, lead glass, armoured glass, different types of safety glass, borosilicate glass, fluorosilicate glass,
coloured glass, photosensitive glass, photochromic glass, glass wool and optical fibre.
Ceramics: Brief introduction to types of ceramics. glazing of ceramics.
Cement: Manufacture of Portland cement and the setting process, Different types of cements: quick
setting cements, eco-friendly cement (slag cement), pozzolana cement.

Unit 2: Fertilizers (Hours: 8)

Different types of fertilizers (N, P and K). Importance of fertilizers, chemistry involved in the
manufacture of the following fertilizers: urea, ammonium nitrate, calcium ammonium nitrate,
ammonium phosphates, superphosphate of lime, potassium chloride and potassium nitrate.
Environmental impact of fertilizers.

Unit 3: Surface Coatings (Hours: 12)

Brief introduction to and classification of surface coatings, paints and pigments: formulation,
composition and related properties, pigment volume concentration (PVC) and critical pigment volume
concentration (CPVC), fillers, thinners, enamels and emulsifying agents. Special paints: heat
retardant, fire retardant, eco-friendly paints, plastic paints, water and oil paints. Preliminary methods
for surface preparation, metallic coatings (electrolytic and electroless with reference to chrome plating
and nickel plating), metal spraying and anodizing. Contemporary surface coating methods like
physical vapor deposition, chemical vapor deposition, galvanising, carburizing, sherardising,
boriding, nitriding and cementation.

Practical Component
Credits:02
(Laboratory periods:60)
1. Detection of constituents of CAN fertilizer (Calcium, Ammonium and Nitrate ions) fertilizer and
estimation of Calcium content.
2. Detection of constituents of Superphosphate fertilizer (Calcium and Phosphate ions) and
estimation of phosphoric acid content.
3. Detection of constituents of Dolomite (Calcium, Magnesium and carbonate ions) and determination
of composition of Dolomite (Complexometric titration).
4. Analysis of (Cu, Ni) in alloy or synthetic samples (Multiple methods involving Complexometry,
Gravimetry and Spectrophotometry).
5. Analysis of (Cu, Zn) in alloy or synthetic samples (Multiple methods involving Iodometry,
Complexometry and Potentiometry).
6. Preparation of following Inorganic Pigments:
a). Barium white
b). Chrome Yellow

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 c). Malachite
d).Chromium oxide
e). Prussian Blue
7. Any suitable experiment other than the listed ones.
References:
Theory:
1. West, A. R. (2014), Solid State Chemistry and Its Application, Wiley & sons.
2. Smart, L. E.; Moore, E. A. (2012), Solid State Chemistry An Introduction, CRC Press Taylor
& Francis.
3. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A.(2010), Inorganic
Chemistry, W. H. Freeman and Company.
4. Kent, J. A. (ed) (1997), Riegel’s Handbook of Industrial Chemistry, CBS Publishers, New
Delhi.
5. Jain P.C., Jain M., Engineering Chemistry, Dhanpat Rai & Sons, Delhi.
6. Gopalan R., Venkappaya D.,Nagarajan S., Engineering Chemistry, Vikas Publications, New
Delhi.
7. Sharma, B.K., Engineering Chemistry, Goel Publishing House, Meerut.
8. Kingery W.D., Bowen H. K., Uhlmann, D.R., (1976), Introduction to Ceramics, Wiley & sons,
Delhi.

Practicals:
1. Vogel A. I., Vogel’s Quantitative Inorganic Analysis, Pearson Education.
2. Banewicz, J. J.; Kenner, C.T. Determination of Calcium and Magnesium in Limestones and
Dolomites, Anal. Chem., 1952, 24 (7), 1186–1187.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

104
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 8: Polynuclear Hydrocarbons,
Pharmaceutical Compounds, UV- Visible & IR Spectroscopy

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Code Credits Credit distribution of the Eligibility Pre-
course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Chem-DSE 8: 04 02 - 02 Class XII
Polynuclear with
Hydrocarbons, Science
Pharmaceutical
Compounds, UV-
Visible & IR
Spectroscopy

Learning Objectives

The Learning Objectives of this course are as follows:

• To provide an insight to the fundamentals of polynuclear hydrocarbons and heterocyclic compounds
• The course introduces learners to IR and UV-Vis spectroscopic techniques and their importance in
functional group identification.

Learning outcomes

By studying this course, students will be able to:

• Understand the fundamentals of polynuclear hydrocarbons and heterocyclic compounds
through the study of methods of preparation, properties and chemical reactions with
underlying mechanism.
• Gain insight into the basic fundamental principles of IR and UV-Vis spectroscopic
techniques.
• Use basic theoretical principles underlying UV-visible and IR spectroscopy as a tool for
functional group identification in organic molecules.

Syllabus

UNIT-1: Polynuclear Hydrocarbons (Hours: 6)

Introduction, classification, uses, aromaticity of polynuclear compounds, Structure elucidation

of naphthalene, preparation and properties of naphthalene and anthracene.

105
UNIT-2: Pharmaceutical Compounds (Hours: 12)
Introduction, classification, general mode of action of antipyretics and analgesics, aspirin;
Synthesis, uses and side effects of the following drugs:
Antipyretics - Paracetamol (with synthesis and mode of action); Analgesics- Ibuprofen (with
synthesis and overview of the mode of action); Antimalarials - Chloroquine (synthesis and
mode of action).
An elementary treatment of Antibiotics and detailed study of chloramphenicol including mode
of action. Medicinal values of curcumin (haldi), azadirachtin (neem), vitamin C and antacid
(ranitidine).

UNIT-3: UV-Vis and IR Spectroscopy (Hours: 12)

UV-Vis and IR Spectroscopy and their application to simple organic molecules.

Electromagnetic radiations and their properties; double bond equivalence and hydrogen
deficiency. UV-Vis spectroscopy (electronic spectroscopy): General electronic transitions,
λmax & εmax, chromophores & auxochromes, bathochromic & hypsochromic shifts.
Application of Woodward rules for the calculation of λmax for the following systems:
conjugated dienes - alicyclic, homoannular and heteroannular; α, β-unsaturated aldehydes and
ketones, charge transfer complex.

Infrared (IR) Spectroscopy: Infrared radiation and types of molecular vibrations, the
significance of functional group & fingerprint region. IR spectra of alkanes, alkenes, aromatic
hydrocarbons (effect of conjugation and resonance on IR absorptions), simple alcohols (inter
and intramolecular hydrogen bonding and IR absorptions), phenol, carbonyl compounds,
carboxylic acids and their derivatives (effect of substitution on >C=O stretching absorptions).

Practical component Credit:02

(Laboratory periods: 15 classes of 4 hours each)
1. Isolation and estimation of the amount of aspirin in a commercial tablet.
2. Synthesis of ibuprofen.
3. Systematic qualitative identification and derivative preparation of organic compounds (Aromatic
hydrocarbons, Aryl halides)
4. Detection of simple functional groups through examination of IR spectra (spectra to be provided). IR
spectra of simple compounds like phenols, aldehydes, ketones, carboxylic acids may be given.
5. Differentiation between of o-/p-hydroxybenzaldehyde by IR spectroscopy (Spectra to be provided).
6. Differentiation between benzoic acid and cinnamic acid by UV spectroscopy.
7. Laboratory preparation of paracetamol.
8. Diel’s Alder reaction using Anthracene and Maleic anhydride.

106
References:
Theory:
1. Finar, I. L. Organic Chemistry (Volume 1 & 2), Dorling Kindersley (India) Pvt.
Ltd. (Pearson Education).
2. Morrison, R. N.; Boyd, R. N. Organic Chemistry, Dorling Kindersley (India)
Pvt. Ltd. (Pearson Education).
3. Bahl, A; Bahl, B. S. (2012), Advanced Organic Chemistry, S. Chand.
4. Pavia, D.L. Introduction to Spectroscopy, Cengage learning (India) Pvt. Ltd.
5. Kemp, W. (1991), Organic Spectroscopy, Palgrave Macmillan.

Practicals

1. Ahluwalia, V.K.; Dhingra, S.; Gulati, A. (2005), College Practical Chemistry,

University Press (India) Ltd.
2. Ahluwalia, V.K.; Dhingra, S. (2004), Comprehensive Practical Organic
Chemistry: Qualitative Analysis, University Press.
3. Vogel, A.I. (1972), Textbook of Practical Organic Chemistry, Prentice-Hall.
4. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I, I K
International Publishing House Pvt. Ltd., New Delhi.
5. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I, I K
International Publishing House Pvt. Ltd., New Delhi.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

107
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 9: Computer Applications in
Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 9: 04 02 - 02 Class XII
Computer with
Applications Science
in Chemistry

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce the students to basic computer skills that will help them in solving chemistry problems
using spreadsheets and BASIC language.
• To acquaint the students with different software for data tabulation, calculation, graph plotting, data
analysis and document preparation.
• To expose the students to the concept of molecular modelling, its applications to various molecular
systems, energy minimization techniques, analysis of Mulliken Charge and ESP Plots.

Learning outcomes

By studying this course, students will be able to:

● Have knowledge of most commonly used commands and library functions used in programming in
BASIC language.
● Develop algorithm to solve problems and write corresponding programs in BASIC language for
performing calculations involved in laboratory experiments.
● Use various spreadsheet software to perform theoretical calculations and plot graphs

Syllabus

Unit 1: Programming using BASIC (Hours: 20)

Programming Language – Elements of BASIC language, Numeric and string Constants and Variables,
arithmetic expressions, hierarchy of operations, inbuilt functions. Syntax and use of the various QBASIC
commands: REM, CLS, INPUT, PRINT, GOTO, IF, IF…THEN, IF...THEN..ELSE, IF and END IF, FOR

108
and NEXT etc., DIM, READ, DATA, GOSUB, RETURN, RESTORE, DEF FNR and Library Functions,
Simple programs based on usage of the commands mentioned above.
Statistical analysis using BASIC: Mean, Least square fit - Linear regression, variance, standard deviation.
Unit 2 : Handling of Numerical Data (Hours: 4)

Spreadsheet software: MS Excel. Creating a spreadsheet, entering and formatting information, applying
basic functions and formulae to the data, drawing charts, tables and graphs, displaying the equation of graph
along with the R2 value, incorporating tables and graphs in Word files, graphical solution of equations,
plotting pressure-volume curves of van der Waals gases, Maxwell-Boltzmann distribution, concentration
versus time graphs, spectral data, titration curves, etc.
Unit 3: Molecular Modelling (Hours: 6)

Introduction to molecular modelling, overview of classical and quantum mechanical methods (molecular
mechanics, semi empirical, ab initio and DFT), general considerations and comparison of these methods.

Practical component Credit:02

(Laboratory periods: 15 classes of 4 hours each)
Exercises of Programing
1. Calculate pressure of a real gas using Van der Waal’s Equation.
2. Calculate the most probable speed, average speed and root men square velocity of an ideal gas.
3. Roots of quadratic equations
4. Binomial coefficient using GOSUB statement.
5. Mean, standard deviation
6. Least square curve fitting method for linear equation.
Plotting graphs using a spreadsheet
1. Van der Waals isotherms
2. Maxwell-Boltzmann distribution curves as function of temperature and molecular weight
3. Plot the conductometric titration curve for
a) strong acid vs strong base and b) weak acid vs strong base
4. Plot the pH metric titration curve for
a) strong acid vs strong base and b) weak acid vs strong base and determine the pKa of the weak acid
5. Plot the graphs for the kinetics of first order reaction and determine the rate constant
6. Plot the UV-vis absorbance spectra and determine the molar absorption coefficient.
Molecular Modelling
1. Optimize and compare the geometry parameters of H2O and H2S using ArgusLab.
2. Compare the basicities of N atom in ammonia, methylamine, dimethylamine and trimethylamine
using ArgusLab by comparing Mulliken charges and ESP map in ArgusLab.

109
 3. Compare C-C bond lengths and bond order in ethane, ethene and ethyne using ArgusLab.
4. Determine enthalpy of isomerization of cis and trans-2-butene using ArgusLab.
5. Compare the HAH bond angles for the second row hydrides (BeH2, CH4, NH3, H2O) and compare
with the results from qualitative MO theory.

References:
Theory:
1. Levie, R. de. (2001), How to use Excel in analytical chemistry and in general scientific data
analysis, Cambridge Univ. Press.
2. Venit, S.M. (1996), Programming in BASIC: Problem solving with structure and style. Jaico
Publishing House.
3. Lewars, E. (2003), Computational Chemistry, Kluwer academic Publisher.
4. Cramer, C.J.(2004), Essentials of Computational Chemistry, John Wiley & Sons.
5. Hinchcliffe, A. (1996), Modelling Molecular Structures, John Wiley & Sons.
6. Leach, A.R.(2001), Molecular Modelling, Prentice-Hall.

Practicals
1. Lewars, E. (2003), Computational Chemistry, Kluwer academic Publisher.
2. Cramer, C.J. (2004), Essentials of Computational Chemistry, John Wiley & Sons.
3. Hinchcliffe, A. (1996), Modelling Molecular Structures, John Wiley & Sons.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

110
 SEMESTER VI

DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -10: Analytical Methods in

Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE- 04 02 - 02 Class XII
10: with
Analytical Science
Methods in
Chemistry

Learning Objectives

The Learning Objectives of this course are as follows:

• To familiarize students with the concepts of sampling, errors in analysis, accuracy, precision and
introduce basics of statistical analysis.
• To introduces students to important instrumentation and separation techniques routinely used in
the laboratory analysis of samples. The experiments expose students to instrumentation and they
learn to detect and separate analytes in a mixture.

Learning outcomes

By studying this course, students will be able to:

● Understand various sources of errors in chemical analysis.
● Learn about methods to minimize error.
● Understand basic principle of instrumentation (Flame Photometer, UV-vis spectrophotometer,
Atomic Absorption spectrophotometer).
● Apply the principles of analysis and instrumentation to analyse soil samples, soft drinks and
synthetic mixtures provided in the laboratory.
● Learn basic principles of separation techniques (chromatography and solvent extraction) and
apply them to separate mixtures.
● Understand principles of Gravimetric analysis and apply them in determination of Ni2+ and Al3+
● Analyse samples independently in the laboratory.
Syllabus

Unit 1: Errors in Chemical Analysis (Hours: 8)

111
 Types of errors, Accuracy and Precision, Absolute and relative uncertainty, propagation of
uncertainty. The Gaussian distribution, mean and standard deviation, confidence intervals.

Unit 2: Optical Methods of Analysis (Hours: 10)

Origin of spectra, interaction of radiation with matter, fundamental laws of spectroscopy and selection
rules, Beer’s-Lambert Law.
UV-Vis Spectrophotometry
Basic principles of instrumentation for single and double beam instruments. Determination of
concentration of unknown compounds, composition of metal complexes using Job’s method of
continuous variation and mole ratio method.
Flame Atomic Absorption and Emission Spectroscopy
Basic principles of instrumentation. Techniques of atomization and sample introduction; Method of
background correction, sources of chemical interferences and their method of removal.
Application of these techniques in analysis of samples.

Unit 3: Separation Techniques (Hours: 12)

Solvent extraction
Classification, principle and efficiency of the technique. Mechanism of extraction: extraction by
solvation and chelation. Technique of extraction: batch, continuous and counter current extractions.
Chromatography
Principles of Chromatographic separations, Classification of Chromatographic techniques, Thin Layer
Chromatography, Column Chromatography, efficiency of separation (Resolution, Efficiency of
Resolution, Plate Height) Application of these techniques in analysis of samples.

Practical Component Credits:02

(Laboratory periods:60)
1. Analysis of soil.
a. Determination of pH of soil, Total soluble salts, carbonate and bicarbonate, calcium and
magnesium by titration.
b. Estimation of Potassium, calcium and magnesium by flame photometry.
2. Separation of constituents of leaf pigments by thin layer chromatography.
3. Determination of the ion exchange capacity of an anion exchange resin.
4. Determination of the ion exchange capacity of a cation exchange resin.
5. Separation of amino acids by ion exchange chromatography.

112
 6. Spectrophotometric analysis of Co2+ and Ni2+ ions in a mixture.
7. Spectrophotometric analysis of Caffeine and Benzoic acid in a soft drink.
8. Gravimetric estimation of Ni2+ using Dimethylglyoxime or Al3+ using oxine.
References:

Theory:
1. Willard, H.H. (1988), Instrumental Methods of Analysis, 7th Edition, Wardsworth Publishing
Company.
2. Christian, G.D. (2004), Analytical Chemistry, 6th Edition, John Wiley & Sons, New York.
3. Harris, D. C. (2007), Quantitative Chemical Analysis,6th Edition, Freeman.
4. Skoog, D.A.; Holler F.J.; Nieman, T.A. (2005), Principles of Instrumental Analysis, Thomson
Asia Pvt. Ltd.
5. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of Quantitative
Chemical Analysis, John Wiley and Sons.

Practicals:
1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of Quantitative
Chemical Analysis, John Wiley and Sons.
2. Christian, G.D. (2004), Analytical Chemistry, 6th Edition, John Wiley & Sons, New York.
3. Harris, D. C. (2007), Quantitative Chemical Analysis, 6th Edition, Freeman.
4. Skoog, D.A.; Holler F.J.; Nieman, T.A. (2005), Principles of Instrumental Analysis, Thomson
Asia Pvt. Ltd.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

113
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 11: Chemistry of Polymers,
Dyes and Natural Products

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 04 02 - 02 Class XII
11: with
Chemistry of Science
Polymers,
Dyes and
Natural
Products

Learning Objectives

The Learning Objectives of this course are as follows:

• To understand the process of converting knowledge of chemistry into marketable
products for commercial gain.
• To familiarize the basic nomenclature of polymers, dyes and natural products,
classification and important terms.

Learning outcomes
By studying this course, students will be able to:

• Learn about the chemistry of natural and synthetic polymers including fabrics and rubbers.
• Understand the chemistry of biodegradable and conducting polymers and appreciate the need of
biodegradable polymers with emphasis on basic principles.
• Comprehend the theory of colour and constitution as well as the chemistry of dyeing.
• Know applications of various types of dyes including those in foods and textiles.
• Understand the chemistry and applications of natural products like terpenoids and alkaloids.

Syllabus

Unit 1: Polymers (Hours: 12)

Introduction and classification based on origin, monomer units, thermal response, mode of
formation, structure, application and tacticity; di-block, tri-block and amphiphilic polymers;

114
Weight average molecular weight, number average molecular weight, glass transition
temperature (Tg) of polymers; Polymerisation Reactions-Addition and condensation.
Mechanism of cationic, anionic and free radical addition polymerization; Ziegler-Natta
polymerisation of alkenes.
Preparation and applications of: Plastics -thermosetting (phenol-formaldehyde,
polyurethanes) and thermosoftening(PVC, polythene); Fabrics -natural (cellulose and
synthetic derivatives of cellulose like rayon and viscose); synthetic (acrylic, polyamide,
polyester); Rubbers-natural
and synthetic: Buna-N, Buna-S, Neoprene, silicon rubber; Vulcanization; Polymer additives;
Introduction to Specialty Polymers: electroluminescent (Organic light emitting diodes),
conducting, biodegradable polymers and liquid crystals.

Unit 2: Dyes (Hours: 8)

Classification, Colour and constitution; Mordant and Vat Dyes; Chemistry of dyeing. Synthesis
and applications of Azo dyes – Methyl orange, Congo red; Triphenyl methane dyes- Crystal
violet; Phthalein Dyes – Phenolphthalein; Natural dyes –Structure elucidation and synthesis of
Alizarin and Indigotin; Edible Dyes with examples.
Unit 3: Natural Product Chemistry- An Introduction to Terpenoids and Alkaloids
(Hours: 10)
Terpenes: Introduction, occurrence, classification, uses, isoprene and special isoprene rule;
structure elucidation, synthesis and industrial application of citral.
Alkaloids: Introduction, occurrence, classification, uses, general structural features, general
methods for structure elucidation including Hoffmann’s exhaustive methylation and Emde’s
method. Structure elucidation, synthesis and physiological action of Nicotine.

Practical component Credits: 02

(Laboratory periods: 60)

1. Preparation of Methyl Orange.

2. Preparation of Malachite Green.
3. Recycling of Plastic: Moulding of plastic or Cracking of plastic.
4. Preparation of Urea-formaldehyde resin.
5. Preparation of Methyl Orange.
6. (a) Dyeing of different fabrics (cotton, wool, silk) using Alizarin or any other dye.
7. (b) Preparation of azo dye on the surface of the fabric.
8. Qualitative test for identification of alkaloids (Dragendorff’s reagent and Mayer’s reagent test)
and terpenoids (Salkowski test).
9. Preparation of perichromic dye using p-amino phenol and p-nitro benzaldehyde.

References:
Theory:
1. Finar, I.L. (2008), Organic Chemistry, Vol 2, 5th Edition, Pearson Education

115
 2. Saunders, K. J. (1988), Organic Polymer Chemistry, 2nd Edition Chapman &
Hall, London
3. Campbell, Ian M., (2000), Introduction to Synthetic Polymers, 2nd Edition
Oxford University Press, USA.
4. Bahadur, P. and Sastry, N.V. (2002) Principles of Polymer Science, Narosa,
New Delhi
5. Patrick, G. An Introduction to Medicinal Chemistry (2013), 4th Edition,
Oxford University Press.
6. Priscilla Abarca, Patricia Silva, Iriux Almodovar and Marcos Caroli
ezende*Quim. Nova, Vol. 37, No. 4, 745-747, 2014.
http://dx.doi.org/10.5935/0100- 4042.20140120

Practical:
1. Furniss B S., Hannaford A. J., Smith Peter W. G. & Tatchell Austin R., Vogel’s
Textbook of Practical Organic Chemistry Fifth Edition, Longman Scientific
& Technical.

2. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I, I

K International Publishing House Pvt. Ltd., New Delhi.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

116
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -12: Phase Equilibria and
Photochemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Chem-DSE 12: 04 02 - 02 Class XII
Phase with
Equilibria and Science
Photochemistry

Learning Objectives

The Learning Objectives of this course are as follows:

• To develop basic understanding of Phase, Component, Degree of freedom, basic
principles of phase equilibria,
• To understand phase diagram of one and two component systems.
• The students will also gain an understanding of Binary solution, distillation of binary
solution, CST and distribution law & its applications.

Learning outcomes

By studying this course, students will be able to:

• Understand phase equilibrium, criteria, CST, Gibbs-Duhem-Margules equation.

• Apply the concepts of phase, conductance and distribution law while studying
otherchemistry courses and every-day life.
• Explain low and high quantum yield, photosensitized reactions

Syllabus

Unit 1: Phase Equilibria (Hours: 22)

Concept of phases, components and degrees of freedom, derivation of Gibbs Phase Rule for
nonreactive and reactive systems; Clausius-Clapeyron equation and its applications to solid-
liquid, liquid-vapour and solid-vapour equilibria, Phase diagram for one component systems
(H2O and S). Phase diagrams for systemsof solid-liquid equilibria involving eutectic, congruent
and incongruent melting points.

117
Binary solutions: Gibbs-Duhem-Margules equation, its derivation and applications to
fractional distillation of binary miscible liquids (ideal and non-ideal), azeotropes, lever rule,
partial miscibility of liquids, CST, miscible pairs, steam distillation. Nernstdistribution law:
its derivation and applications.
Unit 2: Photochemistry (Hours: 8)
Characteristics of electromagnetic radiation. Lambert-Beer’s law and its limitations,
physical significance of absorption coefficients. Laws of photochemistry, quantum yield,
examples of low and high quantum yields
Photosensitized reactions, Jablonski’s diagram. Role of photochemical reactions in
biochemical processes, chemiluminescence.

Practical component Credits: 02

(Laboratory periods: 60)

Phase Equilibrium
1. Determination of critical solution temperature and composition at CST of the phenol water
system.
2. Effect of impurity on CST of phenol-water system (NaCl and succinic acid).
3. Construction of the phase diagram using cooling curves :
a. Simple eutectic.
b. Congruent melting system(s).
4. Distribution of acetic/ benzoic acid between water and chloroform or cyclohexane.
5. Study of equilibrium of any one of the following reactions by distribution method:
(i) I2 (aq) + I- (aq) ⇌ I3-(aq)
(ii) Cu2+ (aq) + nNH3⇌ [Cu(NH3)n]2+

References:
Theory:
1. Atkins, P.W.; Paula, J.de. (2014), Atkin’s Physical Chemistry Ed., 10th
Edition, OxfordUniversity Press.
2. Ball, D. W. (2017), Physical Chemistry, 2nd Edition, Cengage Learning, India.
3. Castellan, G. W. (2004), Physical Chemistry, 4th Edition, Narosa.
4. Kapoor, K.L. (2015), A Textbook of Physical Chemistry, Vol 1, 6th Edition,
McGraw Hill Education.
5. Kapoor, K.L., A Textbook of Physical Chemistry, Vol 3, 5th Edition,
McGraw Hill Education.
Practical:

1. Khosla, B.D.; Garg, V.C.; Gulati, A. (2015), Senior Practical Physical

Chemistry, R. Chand & Co, New Delhi.
2. Kapoor, K.L. (2019), A Textbook of Physical Chemistry, Vol.7, 1st Edition,
McGraw Hill Education.
3. Garland, C. W.; Nibler, J. W.; Shoemaker, D. P. (2003), Experiments in
Physical Chemistry, 8th Edition, McGraw-Hill, New York

118
 Additional Resources:

1. Moore, W.J. (1972), Physical Chemistry, 5th Edition, Longmans Green & Co. Ltd.
2. Glasstone, S. (1948), Textbook of Physical Chemistry, D. Van Nostrand
company, NewYork.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

119
DISCIPLINE SPECIFIC ELECTIVE COURSE – 13 (DSE-13): Research Methodology
for Chemists

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE

COURSE
Course title Credits Credit distribution of the Eligibility Pre-
& Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice (if any)
Research 04 03 -- 01 Class 12th
Methodology with
for Chemists Physics,
(DSE-13) Chemistry

Learning objectives

The objectives of this course are as follows:

• To make the students aware of fundamental but mandatory ethical practices in

chemistry.
• To introduce the concept of data analysis.
• To learn to perform literature survey in different modes.
• To make the students aware of safety handling and safe storage of chemicals.
• To make students aware about plagiarism and how to avoid it.
• To teach the use of different e-resources.

Learning outcomes

By studying this course, students will be able to:

• Follow ethical practices in chemistry
• Do Data analysis
• Literature survey in different modes
• Use e-resources.
• Avoid plagiarism, understand the consequences and how to avoid

SYLLABUS OF DSE-13

UNIT – 1: Scope of Research (Hours: 3)

Introduction, overview of research process: define research problem, review literature,

formulate hypothesis, design research/experiment, collect and analyse data, interpret and report,
scope and importance.

UNIT – 2: Literature Survey, Databases and Research metrics (Hours: 15)

120
Print: Sources of information: Primary, secondary, tertiary sources; Journals: Journal
abbreviations, Digital: Databases and their responsible use: Google Scholar, Web of science,
Scopus, UGC INFONET, SciFinder, PubMed, ResearchGate, E-consortium, e-books; Search
techniques: Phrase, Field, Boolean, Proximity, Concept, Limiting/Refining Search Results.
Research metrics: Impact factor of Journal, h-index, i10 index, Altmetrics, Citation index.
Author identifiers/or profiles: ORCID, Publons, Google Scholar, ResearchGate, VIDWAN

UNIT – 3: Communication in Science (Hours: 12)

Types of technical documents: Full length research paper, book chapters, reviews, short
communication, project proposal, Letters to editor, and thesis.
Thesis writing – different steps and software tools (Word processing, LaTeX, Chemdraw,
Chemsketch etc) in the design and preparation of thesis, layout, structure (chapter plan) and
language of typical reports, Illustrations and tables, bibliography, referencing: Styles (APA,
Oxford etc), annotated bibliography, Citation management tools: Mendeley, Zotero and
Endnote; footnotes. Oral presentation/posters – planning, software tools, creating and making
effective presentation, use of visual aids, importance of effective communication, electronic
manuscript submission, effective oral scientific communication and presentation skills.

UNIT – 4: Research and Publication ethics (Hours: 9)

Scientific Conduct: Ethics with respect to science and research, Scientific Misconducts:
falsification, fabrication and plagiarism, similarity index, software tools for finding plagiarism
(Turnitin, Urkund etc), redundant dublications

Publication Ethics: Introduction, COPE (Committee on Publication Ethics) guidelines; conflicts

of interest, publication misconduct: problems that lead to unethical behaviour and vice versa,
types, violation of publication ethics, authorship and contributorship, predatory publishers and
journals

IPR - Intellectual property rights and patent law, commercialization, copy right, royalty, trade
related aspects of intellectual property rights (TRIPS)

UNIT – 5: Statistical analysis for chemists (Hours:

6)

Types of data, data collection-Methods and tools, data processing, hypothesis testing, Normal
and Binomial distribution, tests of significance: t-test, F-test, chi- square test, ANOVA,
multiple range test, regression and correlation.

Features of data analysis with computers and softwares -Microsoft Excel, Origin, SPSS

Practical component Credits: 01

(Laboratory periods:15 classes of 2 hours each)

1. Collection of journal articles on a particular topic using Google Scholar and creating a
database.
2. Collection of journal articles on a particular topic using Science Direct and creating a
database.
3. Collection of journal articles on a particular topic using Scopus and creating a database.
4. Drawing chemical structure, reactions and mechanisms using Chemsketch or ISIS draw
or any other software.

121
 5. Collection of chemical structure using ChemSpider and creating a database.
6. Curve fitting using freely available softwares/apps (any one)
7. Making of power point presentation
8. Experimental learning of safe storage hazardous chemicals
9. Experimental learning of handling of hazardous chemicals
10. Technical writing on topics assigned.
11. Demonstration for checking of plagiarism using recommended software

Essential/recommended readings:

1. Dean, J. R., Jones, A. M., Holmes, D., Reed, R., Weyers, J. & Jones, A. (2011) Practical
skills in chemistry. 2nd Ed. Prentice-Hall, Harlow.
2. Hibbert, D. B. & Gooding, J. J. (2006) Data analysis for chemistry. Oxford University
Press.
3. Topping, J. (1984) Errors of observation and their treatment. Fourth Ed., Chapman Hall,
London.
4. Harris, D. C. Quantitative chemical analysis. 6th Ed., Freeman (2007) Chapters 3-5.
5. Levie, R. de, how to use Excel in analytical chemistry and in general scientific data
analysis. Cambridge Univ. Press (2001) 487 pages.
6. Chemical safety matters – IUPAC – IPCS, Cambridge University Press, 1992.
OSU safety manual 1.01

122
 BSC. (LIFE SCIENCE)- CHEMISTRY COMPONENT
SEMESTER-IV

DISCIPLINE SPECIFIC CORE COURSE CHEM-DSC -10: Chemistry- IV: Chemistry of

Carboxylic Acids & their Derivatives, Amines and Heterocycles
CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Code Credits Credit distribution of the Eligibility Pre-
course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Chemistry of 04 02 - 02 Class 12th
Carboxylic Acids & with Physics,
their Derivatives, Chemistry,
Amines and Mathematics
Heterocycles DSC-
10: Chemistry- 04

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce the basics of coordination chemistry and which are of immense importance to
biological systems, qualitative and quantitative analysis, catalysis, medicines, paints and pigments
etc.
• Nomenclature, isomerism, bonding in coordination compounds has been dealt with in sufficient
detail along with special emphasis on important coordination compounds in the biological system.

Learning outcomes

By studying this course, students will be able to:

• Understand terms: ligand, denticity of ligands, chelate, coordination number.
• Systematically name coordination compounds.
• Discuss the various types of isomerism possible in Octahedral and Tetrahedral coordination
compounds.
• Use Valence Bond Theory to predict the structure and magnetic behaviour of metal complexes and
understand the terms inner and outer orbital complexes.
• Explain the meaning of the terms ∆o., ∆t, pairing energy, CFSE, high spin and low spin and how
CFSE affects thermodynamic properties like lattice enthalpy and hydration enthalpy.
• Explain magnetic properties and colour of complexes on basis of Crystal Field Theory
• Understand reaction mechanisms of coordination compounds and differentiate between kinetic
and thermodynamic stability.
• Discuss the application of coordination compounds in the biological systems such as
Heamoglobin, myoglobin and some enzymes

123
Syllabus

Unit 1: Carboxylic acids and their Derivatives (aliphatic and aromatic) ( Hours:13)
Preparation: Oxidation reactions of alcohols, aldehydes and ketones, Acidic and alkaline hydrolysis of
esters; Reactions: Hell-Volhard Zelinsky reaction,
Carboxylic acid derivatives (aliphatic): Preparation: Acid chlorides, anhydrides, esters and amides from
acids and their interconversion, Claisen condensation. Reactions: Relative reactivities of acid derivatives
towards nucleophiles, Reformatsky reaction, Perkin condensation.
Active methylene compounds: Keto-enol tautomerism. Preparation and synthetic applications of ethyl
acetoacetate

Unit 2: Amines (aliphatic & aromatic) and Diazonium Salts (Hours:10)

Amines
Preparation: from alkyl halides, Gabriel's Phthalimide synthesis, Hofmann Bromamide reaction. Reactions:
Hofmann vs Saytzeff elimination, carbylamine test, Hinsberg test, reaction with HNO2, Schotten-Baumann
reaction. Electrophilic substitution (case aniline): nitration, bromination, sulphonation; basicity of amines.
Diazonium salt
Preparation: from aromatic amines; Reactions: conversion to benzene, phenol and dyes.

Unit 3: Heterocyclic Compounds (Hours:07)

Introduction, classification, structure, nomenclature and uses. Preparation and properties of the following
heterocyclic compounds with reference to electrophilic and nucleophilic substitution: furan, pyrrole,
thiophene, and pyridine.

PRACTICALS: Credits: 02
(Laboratory periods: 60)

1. Systematic qualitative analysis and preparation of suitable crystalline derivative (carboxylic

acids, carbonyl, alcohols, phenols, amines (1°, 2°,3°) and amides).
2. Preparation:

a. Acetylation of Aniline and Phenols.

b. Benzoylation of Aniline and phenols.

The above derivatives should be prepared using 0.5-1g of the organic compound. The solid samples must be
collected and may be used for recrystallization and melting point.

References:

124
Theory:
1. Morrison, R. N.; Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson
Education).
2. Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt. Ltd. (Pearson
Education).
3. Ahluwalia, V.K.; Bhagat, P.; Aggarwal, R.; Chandra, R. (2005), Intermediate for Organic
Synthesis, I.K. International.
4. Solomons, T. W. G.; Fryhle, C. B.; Snyder, S. A. (2016), Organic Chemistry, 12th Ed., Wiley.
5. Parashar, R.K., Negi, B. (2016) Chemistry of Heterocyclic Compounds, Ane Books Pvt Ltd.

Practical:
1. Ahluwalia, V.K.; Dhingra, S.; Gulati, A. (2005), College Practical Chemistry, University Press
(India) Ltd.
2. Ahluwalia, V.K.; Dhingra, S. (2004), Comprehensive Practical Organic Chemistry:
Qualitative Analysis, University Press.
3. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I, I K International
Publishing House Pvt. Ltd., New Delhi.
4. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume II, I K International
Publishing House Pvt. Ltd., New Delhi.

5. Vogel, A.I. (1972), Textbook of Practical Organic Chemistry, Prentice-Hall.

6. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of Quantitative
Chemical Analysis, John Wiley and Sons.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

125
 BSC. (LIFE SCIENCE)- CHEMISTRY COMPONENT
SEMESTER-V

DISCIPLINE SPECIFIC CORE COURSE CHEM-DSC -13: Chemistry- V: Coordination

Chemistry and its Application in Biological Systems

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Coordination 04 02 - 02 Class 12th
Chemistry with Physics,
and its Chemistry,
Application Mathematics
in Biological
Systems
DSC-13
Chemistry- 5

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce the basics of coordination chemistry and which are of immense importance to
biological systems, qualitative and quantitative analysis, catalysis, medicines, paints and pigments
etc.
• Nomenclature, isomerism, bonding in coordination compounds has been dealt with in sufficient
detail along with special emphasis on important coordination compounds in the biological system.

Learning outcomes
By studying this course, students will be able to:
• Understand terms: ligand, denticity of ligands, chelate, coordination number.
• Systematically name coordination compounds.
• Discuss the various types of isomerism possible in Octahedral and Tetrahedral coordination
compounds.
• Use Valence Bond Theory to predict the structure and magnetic behaviour of metal complexes and
understand the terms inner and outer orbital complexes.
• Explain the meaning of the terms ∆o., ∆t, pairing energy, CFSE, high spin and low spin and how
CFSE affects thermodynamic properties like lattice enthalpy and hydration enthalpy.
• Explain magnetic properties and colour of complexes on basis of Crystal Field Theory

126
 • Understand reaction mechanisms of coordination compounds and differentiate between kinetic
and thermodynamic stability.
• Discuss the application of coordination compounds in the biological systems such as
Heamoglobin, myoglobin and some enzymes

Syllabus

Unit 1: Introduction to Coordination Compounds (Hours: 6)

Brief discussion with examples of types of ligands, denticity and concept of chelate. IUPAC system of
nomenclature of coordination compounds (mononuclear and binuclear) involving simple monodentate
and bidentate ligands. Structural and stereoisomerism in complexes with coordination numbers 4 and 6.

Unit 2: Bonding in Coordination Compounds (Hours: 14)

Valence Bond Theory (VBT): Salient features of theory, concept of inner and outer orbital complexes,
Drawbacks of VBT.

Crystal Field Theory: Splitting of d orbitals in octahedral symmetry. Crystal field effects for weak and
strong fields, Crystal field stabilization energy (CFSE), concept of pairing energy, Factors affecting the
magnitude of Δ, Spectrochemical series, Splitting of d orbitals in tetrahedral symmetry, Comparison of
CFSE for octahedral and tetrahedral fields, tetragonal distortion of octahedral geometry, Jahn-Teller
distortion.

Unit 3: Thermodynamic and Kinetic aspects of Metal Complexes (Hours: 6)

A brief outline of thermodynamic and kinetic stabilities of metal complexes and factors affecting the
stability. Substitution reactions of square-planar complexes – Trans effect: cisplatin and transplatin.
Unit 4: Application of coordination compounds in biological systems (Hours: 4)

Haemoglobin, Myoglobin, carboxypeptidase, carbonic anhydrase

Practicals Component Credits: 02

(Laboratory periods: 60)
1. Estimation of Mg2+ by direct complexometric titrations using EDTA.
2. Estimation of Zn2+ by direct complexometric titrations using EDTA.
3. Estimation of Ca2+ by direct complexometric titrations using EDTA.
4. Estimation of Zn2+ in zinc tablet.
5. Estimation of Ca2+ in milk sample.
6. Estimation of total hardness of a given sample of water by complexometric titration.
7. Determination of the composition of the Fe3+ - salicylic acid complex / Fe2+ -1,10-
phenanthroline complex in solution by Job’s method
8. Determination of the composition of the Fe3+ - salicylic acid complex / Fe2+-1,10-
phenanthroline complex in solution by mole ratio method

127
 9. Preparation of the following inorganic compounds:
a). Tetraamminecopper(II) sulphate
b). Potassium trioxalatoferrate(III) trihydrate
c). Chrome alum
10. Any suitable experiment (other than the listed ones) based upon complexation reactions.

References:
Theory:

9. Huheey, J.E.; Keiter, E.A., Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry-
Principles of Structure and Reactivity, Pearson Education.
10. Shriver, D.D.; Atkins, P.; Langford, C.H. (1994), Inorganic Chemistry 2nd Ed., Oxford University
Press.
11. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010), Inorganic
Chemistry, 5th Edition, W. H. Freeman and Company.
12. Cotton, F.A.; Wilkinson, G.; Gaus, P.L. Basic Inorganic Chemistry, 3rd Edition, Wiley India.
13. Douglas, B.E.; McDaniel, D.H.; Alexander, J.J. (1994), Concepts and Models of Inorganic
Chemistry, John Wiley & Sons.
14. Greenwood, N.N.; Earnshaw, A. (1997), Chemistry of the Elements, 2nd Edition, Elsevier.
15. Lee, J.D.; (2010), Concise Inorganic Chemistry, Wiley India.
16. Sodhi G.S., Principles of Inorganic Chemistry, Third Edition, Viva Books, India.

Practicals:

1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of Quantitative
Chemical Analysis, John Wiley and Sons.
2. Marr, G.; Rockett, B.W. (1972), Practical Inorganic Chemistry, Van Nostrand Reinhold.
3. Dua A, Manav N, Practical Inorganic Chemistry, (2017), Manakin Press.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

128
 BSC. (LIFE SCIENCE)- CHEMISTRY COMPONENT
SEMESTER-VI

DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSC 16: Chemistry- VI: Conductance,

Electrochemistry and Chemical Kinetics

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Conductance, 04 02 - 02 Class XII
Electrochemistry with
and Chemical Science
Kinetics
DSC-16:
Chemistry- 6

Learning Objectives

The Learning Objectives of this course are as follows:

• To develop basic understanding of electrolytic and galvanic cells.
• Measurementof conductance and its applications, measurement of emf and its applications.
• To understand reaction rate, order, activation energy and theories of reaction rates.

Learning outcomes

By studying this course, students will be able to:

• Explain the factors that affect conductance, migration of ions and application of
conductance measurement.
• Understand the importance of Nernst equation, measurement of emf, calculations of
thermodynamic properties and other parameters from the emf measurements.
• Understand rate law and rate of reaction, theories of reaction rates and catalysts; both
chemical and enzymatic.

Syllabus

Unit 1: Conductance (Hours: 8)

Conductivity, equivalent and molar conductivity and their variation with dilution for weak and

129
 strong electrolytes, Kohlrausch Law of independent migration of ions, Ionic velocity, mobility and
their determination, transference number and its relation to ionic mobility, Conductometric
titrations (only acid-base).

Unit 2: Electrochemistry (Hours: 12)

Concept of reversible and irreversible electrochemical cells, Standard hydrogen electrode, standard
electrode potential, concept of EMF of a cell, measurement of EMF of a cell, Nernst equation and
its importance, types of electrodes (Reference and inert electrodes), electrochemical series.

Thermodynamics of a reversible cell, calculation of thermodynamic properties: G, H and S from

EMF data. Calculation of equilibrium constant from EMF data. pH determination using glass
electrode, Potentiometric titrations-qualitative treatment (acid-base and oxidation-reduction only).

Unit 3: Chemical Kinetics and Catalysis (Hours: 10)

The concept of reaction rates, effect of temperature, pressure, catalyst and other factors on reaction
rates. Order and molecularity of a reaction, integrated rate equations for zero, first and second order
reactions (derivation not required), half–life of a reaction, Concept of activation energy and its
calculation from Arrhenius equation.
Catalysis: Types of catalyst, specificity and selectivity, generalized treatment of catalyzed reactions
at solid surfaces. Enzyme catalysis, Michaelis-Menten mechanism, acid-base catalysis.

Practical Component: Credits:02

Laboratory periods: 60
1. Determination of molar conductance, degree of dissociation and dissociation constant of a
weak acid.
2. Perform the following conductometric titrations: Strong acid vs strong base.
3. Perform the following conductometric titrations: Weak acid vs strong base.
4. Determination of TDS of water from different sources.
5. Determination of Soil pH of soil collected from various locations.
6. Perform the potentiometric titrations of strong acid vs strong base
7. Perform the potentiometric titrations of Weak acid vs strong base.
8. Perform the potentiometric titrations of Potassium dichromate vs. Mohr's salt.
9. Perform the potentiometric titrations of KMnO4 vs. Mohr's salt.
10. Study the kinetics of acid hydrolysis of methyl acetate with hydrochloric acid.
References:
Theory:

130
 1. Castellan, G. W .(2004), Physical Chemistry, Narosa Publications.
2. Kapoor, K.L. (2015),A Textbook of Physical Chemistry, Vol.1, 6th Edition, McGraw Hill
Education.
3. Kapoor, K.L. (2015),A Textbook of Physical Chemistry, Vol.5, 3rd Edition, McGraw Hill
Education.
4. Puri, B.R., Sharma, L.R. and Pathania M.S. (2020), Principles of Physical Chemistry,
Vishal Publishing Co.

Practical:
1. Khosla, B.D.; Garg, V.C.; Gulati, A.(2015), Senior Practical Physical Chemistry, R.
Chand & Co.
2. Kapoor, K.L. (2019), A Textbook of Physical Chemistry, Vol 7, 1st Edition, McGraw
Hill Education.
3. Batra, S.K., Kapoor, V and Gulati, S. (2017) 1st Edition, Experiments in Physical
Chemistry, Book Age series.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

131
 POOL OF DISCIPLINE SPECIFIC ELECTIVES (DSEs)
SEMESTER III

DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -1: Chemistry of Major and Minor
Biogenic Elements

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE-1: 04 02 - 02 Class XII
Chemistry of with
Major and Science
Minor
Biogenic
Elements

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce learners to review periodic properties of main group elements and their
role in the biological systems. It further discusses the patterns and trends exhibited by
main group elements and their compounds with emphasis on synthesis, structure,
bonding and their diverse applications in the environment, industry and in the
biological system.
• To develop the interest of students in the frontier areas of inorganic and material
chemistry, it gives an insight into how these compounds such as oxides of N and S affect
our day-to-day life. Students learn about inorganic polymeric compounds borazine,
silicates, silicones, phosphonitrilic compounds and their applications.

Learning outcomes

By studying this course, students will be able to:

• Understand the periodicity in atomic and ionic radii, electronegativity, ionization enthalpy,
electron gain enthalpy of elements of the periodic table.
• Understand oxidation states with reference to the existence of elements in unusual and rare
oxidation states in alkalides, carbides and nitrides.

132
 • Understand vital role of sodium, potassium, calcium and magnesium ions etc. in biological
systems and the role of oxides of N and S in our environment.
• Distribution of major and minor biogenic elements in human beings

Syllabus
Unit 1: Periodic Properties (Hours: 6)

Electronic configurations of the atoms. Stability of half-filled and completely filled orbitals, the concept
of exchange energy, inert pair effect.
General group trends of main group elements with special reference to size (atomic and ionic), Ionization
Enthalpy, Electron Gain Enthalpy, Electronegativity, oxidation states (including rare oxidation states of
alkali metals, carbides and nitrides), melting and boiling points, flame colour, metallic character and
complex formation tendency (crown ethers and cryptates), Alkali metal solutions in liquid ammonia
Distribution of major and minor biogenic elements in human beings

Unit 2: Structure, Bonding and Properties (Hours: 16)

Structure, bonding and properties: Acidic/Basic nature, stability, ionic/covalent nature,

oxidation/reduction, hydrolysis, thermal stability of the following:
Hydrides: hydrides of Group 13 (only diborane), Group 14, Group 15 (EH3 where E = N, P, As, Sb, Bi),
Group 16 and Group 17.
Oxides: Oxides of nitrogen, phosphorus and sulphur
Oxoacids: oxoacids of phosphorus, sulphur and chlorine
Halides of phosphorus
Relevance of above compounds in industrial/environmental/biological systems wherever applicable

Unit 3: Preparation, Properties, Structure and Uses (Hours: 8)

Preparation, properties, structure and uses of the following compounds: Borazine, Silicates, silicones,
Phosphonitrilic halides {(PNCl2)n where n = 3 and 4}

Practicals Credits:02
(Laboratory periods: 60)

Qualitative semi-micro analysis of mixtures containing 2 anions and 2 cations (preferably 7-8 mixtures).
Emphasis should be given to the understanding of the chemistry of different reactions. The following
radicals are suggested:
CO32-, NO2- , S2-, SO32-, SO42- , S2O32-, CH3COO-, F-, Cl-, Br-, I-, NO3- , BO33-, C2O42-,
PO43-,
NH4+, K+, Pb2+, Cu2+, Cd2+, Bi3+, Sn2+, Sb3+, Fe3+, Al3+, Cr3+, Zn2+, Mn2+, Co2+, Ni2+, Ba2+, Sr2+, Ca2+,
Mg2+
The mixtures may contain combination of anions/one interfering anion.
Spot tests should be preferred wherever applicable.

133
 References:
Theory:
1. Lee, J.D.; (2010), Concise Inorganic Chemistry, Wiley India.
2. Huheey, J.E.; Keiter, E.A.; Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry- Principles of
Structure and Reactivity, Pearson Education.
3. Douglas, B.E.; McDaniel, D.H.; Alexander, J.J. (1994), Concepts and Models of Inorganic
Chemistry, John Wiley & Sons.
4. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010), Shriver and Atkins
Inorganic Chemistry, 5th Edition, Oxford University Press.
5. Housecraft, E. H.; Sharpe, A.G. (2018), Inorganic Chemistry, 5th Edition, Pearson.

Practicals:
4. Vogel, A.I. (1972), Qualitative Inorganic Analysis, Longman.
5. Svehla, G. (1996), Vogel’s Qualitative Inorganic Analysis, Prentice Hall.
6. Dua A, Manav N, Practical Inorganic Chemistry, (2017), Manakin Press.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

134
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -2: Polynuclear Hydrocarbons,
Pharmaceutical Compounds,

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course
(if any)
Chem-DSE-2: 04 02 - 02 Class XII
Polynuclear with
Science
Hydrocarbons,
Pharmaceutical
Compounds,
UV- Visible &
IR
Spectroscopy

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce the chemistry and applications of polynuclear hydrocarbons and heterocyclic

compounds.
• Introduction to spectroscopy, an important analytical tool which allows identification of organic
compounds by correlating their spectra to structure.

Learning outcomes
By studying this course, students will be able to:
• Understand the fundamentals of polynuclear hydrocarbons and heterocyclic compounds through the
study of methods of preparation, properties and chemical reactions with underlying mechanism.
• Gain insight into the basic fundamental principles of IR and UV-Vis spectroscopic techniques.
• Use basic theoretical principles underlying UV-visible and IR spectroscopy as a tool for functional
group identification in organic molecules.

Syllabus
UNIT-1: Polynuclear Hydrocarbons (Hours: 6)
Introduction, classification, uses, aromaticity of polynuclear compounds, Structure elucidation of
naphthalene, preparation and properties of naphthalene and anthracene.

135
UNIT-2: Pharmaceutical Compounds (Hours: 12)
Introduction, classification, general mode of action of antipyretics and analgesics, aspirin; Synthesis, uses
and side effects of the following drugs:
Antipyretics - Paracetamol (with synthesis and mode of action); Analgesics- Ibuprofen (with synthesis and
overview of the mode of action); Antimalarials - Chloroquine (synthesis and mode of action).
An elementary treatment of Antibiotics and detailed study of chloramphenicol including mode of action.
Medicinal values of curcumin (haldi), azadirachtin (neem), vitamin C and antacid (ranitidine).

UNIT-3: UV-Vis and IR Spectroscopy (Hours: 12)

UV-Vis and IR Spectroscopy and their application to simple organic molecules. Electromagnetic radiations
and their properties; double bond equivalence and hydrogen deficiency. UV-Vis spectroscopy (electronic
spectroscopy): General electronic transitions, λ & ε , chromophores &auxochromes, bathochromic &
max max

hypsochromic shifts. Application of Woodward rules for the calculation of λ for the following systems:
max

conjugated dienes - alicyclic, homoannular and heteroannular; α, β-unsaturated aldehydes and ketones,
charge transfer complex.

Infrared (IR) Spectroscopy: Infrared radiation and types of molecular vibrations, the significance of
functional group & fingerprint region. IR spectra of alkanes, alkenes, aromatic hydrocarbons (effect of
conjugation and resonance on IR absorptions), simple alcohols (inter and intramolecular hydrogen bonding
and IR absorptions), phenol, carbonyl compounds, carboxylic acids and their derivatives (effect of
substitution on >C=O stretching absorptions).

Practical component Credit:02

(Laboratory periods: 15 classes of 4 hours each)

1. Isolation and estimation of the amount of aspirin in a commercial tablet.

2. Preparation of Aspirin.
3. Synthesis of ibuprofen.
4. Systematic qualitative identification and derivative preparation of organic compounds (Aromatic
hydrocarbons, Aryl halides)
5. Detection of simple functional groups through examination of IR spectra (spectra to be provided). IR
spectra of simple compounds like phenols, aldehydes, ketones, carboxylic acids may be given.
6. Differentiation between of o-/p-hydroxybenzaldehyde by IR spectroscopy (Spectra to be provided).
7. Differentiation between benzoic acid and cinnamic acid by UV spectroscopy.
8. Diel’s Alder reaction using Anthracene and Maleic anhydride.
9. Partial Reduction of m-dinitrobenzene to m-nitroaniline and then analysing the IR spectra of reactant
and Product.
10. Laboratory preparation of Paraacetamol.

References:
Theory:
1. Finar, I. L. Organic Chemistry (Volume 1 & 2), Dorling Kindersley (India) Pvt. Ltd. (Pearson
Education).
2. Morrison, R. N.; Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson
Education).
3. Bahl, A; Bahl, B. S. (2012), Advanced Organic Chemistry, S. Chand.

136
 4. Pavia, D.L. Introduction to Spectroscopy, Cengage learning (India) Pvt. Ltd.
2. Kemp, W. (1991), Organic Spectroscopy, Palgrave Macmillan.

Practicals:

1. Ahluwalia, V.K.; Dhingra, S.; Gulati, A. (2005), College Practical Chemistry, University Press
(India) Ltd.
2. Ahluwalia, V.K.; Dhingra, S. (2004), Comprehensive Practical Organic Chemistry: Qualitative
Analysis, University Press.
3. Vogel, A.I. (1972), Textbook of Practical Organic Chemistry, Prentice-Hall.
4. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I, I K International
Publishing House Pvt. Ltd., New Delhi.
5. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I, I K International
Publishing House Pvt. Ltd., New Delhi.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

137
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 3: Chemistry of Colloids and Adsorption

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Code Credits Credit distribution of the Eligibility Pre-
course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 3: 04 02 - 02 Class XII
Chemistry of Colloids with
and Adsorption Science
Learning Objectives
The Learning Objectives of this course are as follows:
• To develop basic concepts of colloids and colloidal phenomenon.
• Preparation and characterization of sols, understanding about applications of colloid in food,
petroleum and cosmetic industry.
• Basic understanding of adsorption, types of adsorption, chemistry of adsorption and its
applications.

Learning outcomes

By studying this course, students will be able to:

• Understand colloid solutions, preparation of sols.
• Understand the concept of Electrical double layer, charge on colloidal particles.
• Characterize the colloids sols, learn colloid phenomenon like Tyndall effect, Brownian
movement, electrophoresis, dialysis, coagulation and flocculation.
• Understand adsorption, types of adsorption. Characteristics, factors affecting adsorption and
its applications
Syllabus
Unit 1: Colloidal State (Hours: 8)
Distinction among true solutions, colloids and suspensions, components of Colloids, classificationof
colloids - lyophilic, lyophobic; Preparation methods and properties of lyophobic solutions,
Hydrophile-lyophile balance (HLB), multi molecular, macromolecular and associated colloids
(micelles formation), Schulze -Hardy law.

Unit 2: Preparation and properties of colloids (Hours: 14) Methods

of preparation of colloids, Tyndall effect, Brownian movement, coagulation and flocculation;
electrophoresis, dialysis.
Emulsification by surfactants, selection of surfactants as emulsifying agent, colloidal phenomenonin
food chemistry, Protein based functional colloids.
UNIT 3: Surface Chemistry (Hours: 8)

138
Adsorption, Distinction between adsorption and absorption, Types of Adsorption, Physisorption and
chemisorption and their characteristics, factors affecting adsorption of gases on solids - Freundlich
and Langmuir adsorption isotherms, Adsorption from solutions. Applications of Adsorption
phenomenon in living systems.

Practical component Credits: 02

(Laboratory periods: 60)
7. Preparation of Colloidal Sols of following
a. Egg Albumin
b. Starch /Gum
c. Ferric chloride
d. Aluminum hydroxide
e. Antimony Sulphide
8. To find out the precipitation values of Antomony Sulphide sol by using monovalent, bivalent
and trivalent cations.
9. To verify the Schulze -Hardy law.
10. To verify the Freundlich’s Adsorption isotherms.
11. Study of adsorption of HAc on charcoal and prove the validity of Langmuir’s adsorption
isotherms
12. Study of adsorption of Oxalic acid on charcoal and prove the validity of Langmuir’s adsorption
isotherms.
References:
Theory:
7. Puri B. R., Sharma L. R. and Pathania M.S., (2020) Principles of Physical Chemistry, Vishal
Publishing Co.Jalandhar, Punjab, India.
8. Kapoor K L, Text Book of Physical Chemistry, Vol. 4, McGraw Hill Education (India)
Private Limited, Chennai, India.
9. Evans D F and Wennerström’s, The Colloidal Domain, Second Edition, John Wiley & Sons
Inc.
10. Adamson A. W. and Gast A., Physical Chemistry of Surfaces (Main text) Sixth Edition,
John Wiley & Sons Inc.
11. Berg J. C., An Introduction to Interfaces and Colloids, World Scientific Publishing Co.,
Inc.
New Jersey.
12. Israelachvili J. N., Intermolecular and Surface Forces, Elsevier Inc.

Practical:
3. Giri, S; Bajpai, D.N.; Pandey, O.P. Practical Chemistry, S. Chand Limited.
4. Khosla, B.D.; Garg, V.C.; Gulati, A.(2015), Senior Practical Physical Chemistry, R.
Chand & Co.
Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

139
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -4: Acids & Bases and Aqueous
Chemistry of Metal Ions
CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE-4: 04 02 - 02 Class XII
Acids & Bases with
and Aqueous Science
Chemistry of
Metal Ions

Learning Objectives

The Learning Objectives of this course are as follows:

• To provide basic understanding of the various concepts of acids and bases and Buffers
to students and the factors responsible for variable acid and bases strength. This will
help the learner to understand the importance of pH maintenance for a large number of
biological processes especially enzyme systems.
• The unit of Aqueous Chemistry of metal ions provides an insight into the types of
reactions a metal ion undergoes in aqueous medium- hydration, hydrolysis, redox,
complexation, precipitation. The knowledge of these let a learner ascertain the
feasibility of a proposed reaction and also to predict the possible outcomes of a new
reaction. This additionally equips a biology student to understand different biological
processes involving metal ions in a better way.

Learning outcomes

By studying this course, students will be able to:

• Define the Arrhenius, Bronsted Lowry, Lewis and Hard & soft acids and bases.
• Distinguish one class of acids and bases from the other and will be able to classify different
types of available acids (synthetic and natural) under these classes.
• Understand the parameters affecting the relative strength of acids and bases and the effect
of solvent on them.
• Explain the effect of mixing a strong/weak acid with a weak/strong base and will be able to
calculate the pH of buffers.
• Correlate the concepts of acids and bases to the biological processes, the importance of pH
and the buffers in sustaining specific metabolic activities.
• Explain the behavior of metal ions in aqueous solutions in presence of other reagents

140
 • Differentiate between solvation and solvolysis and explain the formation of oxo ions as a
result of hydrolysis.
• Write the redox reactions involving metal ions, use the Nernst equation to calculate redox
potentials and correlate them with the relative oxidizing/reducing strength of metal ions
• Explain the successive reduction or oxidation of a metal ion capable of displaying more than
two oxidation states and hence predict the spontaneity of a redox reaction
• Explain the disproportionation of an oxidation state and the stability of an oxidation state in
aqueous medium by comparing the redox potentials with that of water at different pH.
• Explain the chemistry involved in the quantitative chemical analysis involving redox
• reactions like redox titrations.
• Explain the formation of metal complexes based on two different modes of ligand metal
interaction.
• Understand the importance of complexation process in stabilizing some oxidation states
more than the other.
• Write the reactions involving the precipitation of metal ions, and predict the relative
precipitations based on solubility products.
• Explain the identification and separation of metal ions in a mixture based on difference in
precipitation behavior of metal ions.
• Correlate the redox, complexation and precipitation behavior of metal ions in aqueous
medium to the role of metal ions and metalloproteins in biological systems.
Syllabus

Unit 1: Acids & Bases (Hours: 10)

Concepts: Arhenius, Bronsted-Lowry (aqua, hydroxo, oxo), Lewis acids and bases, Hard and Soft acids
and bases.
Strength of Acids and Bases: factors affecting relative strength of acids and bases, solvent levelling,
superacids and superbases.
Buffers (NH4OH/NH4Cl, NaOAc/HOAc, boric acid and borate, Phosphate buffers, Universal
Buffer), buffer capacity, calculation of pH of buffer solutions, pH calculation using Handerson-
Hasselbalch equation, Applications of Acids & Bases and buffers in biological processes

Unit 2: Aqueous Chemistry of Metal ions (Hours: 20)

Solvation effects on metal ions, oxocations and oxoanions

Redox reactions: Half reactions, balancing of redox reactions, Nernst equation, standard potentials and
spontaneity, trends in standard potentials, electrochemical series
Redox stability of species in aqueous solutions (influence of pH, effect of solvation, redox reaction with
water, disproportionation)
Diagrammatic presentation of potential data: Latimer diagrams, Frost diagrams and Pourbaix diagrams
their significance
Applications of redox reactions in quantitative analysis: permanganate, dichromate & iodine titrations
Examples of Redox reactions in biological processes
Complexation behaviour of metal ions: Lewis acid – base type (d block), electrostatic interactions based
(s block elements with crown ethers and cryptates), stabilisation of oxidation states by complexation
(Cu(I), Mn(III)),
Applications of complexes in biological systems with special mention of metalloenzymes.

141
Precipitation: Insoluble salts with anions like S2-, SO42-, PO43-, halides, OH-, C2O42-, CO32- and their
application in metal ions analysis.
Practical Component: Credits:02
(Laboratory periods: 60)
1. Preparation of Potassium trioxalatochromate(III).
2. Preparation of Potassium trisoxalatomanganate(III).
3. Preparation of acetylacetonato complexes of
a). Cu(II)
b). Fe(III)
4. Determination of strength of oxalate ions and oxalic acid in a mixture titrimetrically.
5. Determination of available chlorine in bleaching powder iodometrically.
6. Preparation of a phosphate buffer solution and measurement of its pH using pHmeter.
7. Determination of buffer capacity of phosphate buffer.
8. Determination of strength of chloride ions argentometrically
a). Volhard’s Method
b). Fajan’s Method
c). Mohr’s Method
9. pHmetric titration of a strong acid with a strong base.

10. Any suitable experiment other than the listed ones.

References:
Theory:

1. Shriver, D.D.; Atkins, P.; Langford, C.H. (1994), Inorganic Chemistry 2nd Ed., Oxford
University Press.
2. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010),
Inorganic Chemistry, 5th Edition, W. H. Freeman and Company.
3. Lee, J.D.; (2010), Concise Inorganic Chemistry, Wiley India.
4. Miessler, G. L. (2008). Inorganic chemistry. Pearson Education India.
5. Sharpe, A. G. (1992). Inorganic chemistry. Longman Publishing Group.
6. Lehninger, A. L., Nelson, D. L., Cox, M. M., & Cox, M. M. (2005). Lehninger principles
of biochemistry. Macmillan India.
7. Svehla, G. (2008). Vogel's qualitative inorganic analysis, 7/e. Pearson Education India.
Practicals:
1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook of
Quantitative Chemical Analysis, John Wiley and Sons.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch, University of
Delhi, from time to time.

142
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 5 Biomolecule-I

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 5: 04 02 - 02 Class XII
Biomolecules-I with
Science
Learning Objectives

The Learning Objectives of this course are as follows:

• To understand the process of converting knowledge of chemistry into marketable
products for commercial gain.
• To teach students about important biomolecules essential to life
processes.
• 2. To discuss aspects of the principles of organic chemistry in the
structure and function of important biomolecules.

Learning outcomes

By studying this course, students will be able to:

• Learn about the chemistry of natural and synthetic polymers including fabrics and
rubbers.
• Understand the chemistry of biodegradable and conducting polymers and appreciate
the need of biodegradable polymers with emphasis on basic principles.
• Comprehend the theory of colour and constitution as well as the chemistry of dyeing.
• Know applications of various types of dyes including those in foods and textiles.
• Understand the chemistry and applications of natural products like terpenoids and
alkaloids.

Syllabus

Unit 1: Chemistry of Carbohydrates (Hours:10)

Classification of carbohydrates, reducing and non-reducing sugars, biological functions, general properties

143
and reactions of glucose and fructose, their open chain structure, epimers, mutarotation and anomers,
reactions of monosaccharides, determination of the configuration of glucose (Fischer proof), the cyclic
structure of glucose. Haworth projections. The cyclic structure of fructose. The linkage between
monosaccharides: structure of disaccharides (sucrose, maltose, lactose) and polysaccharides (starch and
cellulose) excluding their structure elucidation.

Unit 2: Nucleosides, Nucleotides and Nucleic Acids ( Hours:10)

Components of Nucleic acids: Adenine, guanine, thymine, cytosine and uracil (structure only), other
components of nucleic acids, nucleosides and nucleotides (nomenclature), structure of polynucleotides;
structure of DNA (Watson-Crick model) and RNA (types of RNA), difference between DNA and RNA,
genetic code, biological roles of DNA and RNA: replication, transcription and translation.

Unit-3: Lipids (Hours:10)

Introduction to oils and fats; common fatty acids present in oils and fats, Hydrogenation of fats and oils,
Saponification value, acid value, iodine number. Reversion and rancidity.
Lipids: Classification. Biological importance of triglycerides and phosphoglycerides and cholesterol; Lipid
membrane, Liposomes and their biological functions and underlying applications. Lipoproteins.
Properties, functions and biochemical functions of steroid hormones.

PRACTICALS: Credits: 02
(Laboratory periods: 60)
1. Preparation of osazone of glucose, fructose and Maltose (Comparing the time of formation of the
two and the shape of crystals using microscope).
2. Identification of given carbohydrates as
a. Reducing and Non-reducing
b. Monosaccharide and Disaccharide
c. Aldose and Ketose
3. Estimation of glucose by Fehling’s solution.
4. Determination of the iodine number of oil.
5. Determination of the saponification number of oil.
6. Identification and separation of mixture of sugars by paper chromatography.
7. Isolation of DNA from cauliflower/ onion.
8. Determination of total sugar content by ferricyanide method (volumetric/colorimetric method).

144
References:
Theory
1. Finar, I. L. Organic Chemistry (Volume 1 & 2), Dorling Kindersley (India) Pvt. Ltd. (Pearson
Education).
2. Morrison, R. N.; Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson
Education).
3. Berg, J. M.; Tymoczko, J. L.; Stryer, L. (2002), Biochemistry, W. H. Freeman.
4.Devlin, T.M. (2010), Textbook of Biochemistry with Clinical Correlation, Wiley.
5. Satyanarayana, U.; Chakrapani, U. (2017), Fundamentals of Biochemistry, Books and Allied (P)
Ltd.

6. Lehninger, A.L; Nelson, D.L; Cox, M.M. (2009), Principles of Biochemistry, W. H. Freeman.

Practical:
1. Dean, J.R.; Jones, A.M.; Holmes, D;, Reed, R.; Jones, A.Weyers, J. (2011), Practical skills in
chemistry, Prentice-Hall.
2. Wilson, K.; Walker, J. (2000), Principles and techniques of practical biochemistry, Cambridge
University Press.
3. Gowenlock. A.H. (1988), Varley’s Practical Clinical Biochemistry, CRC Press.
4. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume II, I K International
Publishing House Pvt. Ltd., New Delhi.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

145
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -6 Quantum Chemistry and
Spectroscopy

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 04 02 -- 02 Class 12th NA
6: with Physics,
Quantum Chemistry,
Chemistry Mathematics
and
Spectroscopy

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce the concepts and methodology of quantum mechanics

• Application of Quantum chemistry to spectroscopy
• To establish the relation between structure determination and spectra.

Learning outcomes
By studying this course, students will be able to:

• Understand basic principles of quantum mechanics: operators, eigen values, averages,

probability distributions.
• Understand and use basic concepts of microwave, IR and UV-VIS spectroscopy for
interpretation of spectra.

Syllabus

Unit 1: Quantum Chemistry (Hours: 16)

Postulates of quantum mechanics, quantum mechanical operators.

Schrodinger equation and its application to free particle and particle in a 1-D box (complete
solution),quantization, normalization of wave functions, concept of zero-point energy.

146
Qualitative treatment of H and H like atoms. Setting up of Schrodinger equation for many
electron atoms.

Rotational Motion: Schrödinger equation of a rigid rotator and brief discussion of its results
(solution not required). Quantization of rotational energy levels.

Vibrational Motion: Schrödinger equation of a linear harmonic oscillator and brief discussion
of its results (solution not required). Quantization of vibrational energy levels.
Unit 2: Spectroscopy (Hours: 14)

Electromagnetic radiation and its interaction with matter. Lambert-Beer’s law, Jablonski’s
diagram. Florescence and Phosphorescence.
Difference between atomic and molecular spectra. Born- Oppenheimer approximation:
Separation of molecular energies into translational, rotational, vibrational and electronic
components.

Microwave Spectroscopy: Microwave (pure rotational) spectra of diatomic molecules. Selection

rules.
Structural information derived from rotational spectroscopy.

IR Spectroscopy: Selection rules, IR spectra of diatomic molecules. Structural information

derived from vibrational spectra. Effect of hydrogen bonding (inter- and intramolecular) and
substitution on vibrational frequencies.

Electronic Spectroscopy: Electronic excited states. Free electron model and its application to
electronic spectra of polyenes. chromophores, auxochromes, bathochromic and hypsochromic
shifts.

Practical component Credits:02

(Laboratory periods: 60 )

UV/Visible spectroscopy

10. Study the 200-500 nm absorbance spectra of KMnO4 and K2Cr2O7 (in 0.1 M H2SO4) and
determine the λmax values. Calculate the energies of the two transitions in different units
-1 -1 -1
(J molecule , kJ mol , cm , eV).
11. Study the pH-dependence of the UV-Vis spectrum (200-500 nm) of K2Cr2O7
12. Record the 200-350 nm UV spectra of the given compounds (acetone, acetaldehyde, 2-
propanol, acetic acid) in water. Comment on the effect of structure on the UV spectra of
organic compounds.

Colorimetry

147
13. Verify Lambert-Beer’s law and determine the concentration of CuSO4/ KMnO4/ K2Cr2O7/
CoCl2 in a solution of unknown concentration
14. Determine the concentrations of KMnO4 and K2Cr2O7 in a mixture.
15. Study the kinetics of iodination of propanone in acidic medium.
16. Determine the amount of iron present in a sample using 1, 10-phenanthroline.
17. Determine the dissociation constant of an indicator (phenolphthalein).
18. Study the kinetics of interaction of crystal violet/ phenolphthalein with sodium hydroxide.

References:

Theory:

1. Banwell, C.N.; McCash, E.M.(2006), Fundamentals of Molecular Spectroscopy,

Tata McGraw- Hill.
2. Kapoor, K.L.(2015),A Textbook of Physical Chemistry, McGraw Hill Education,
,Vol 4, 5th Edition, McGraw Hill Education.
3. McQuarrie, D.A.(2016),Quantum Chemistry, Viva Books.
4. Chandra, A. K.(2001),Introductory Quantum Chemistry, Tata McGraw-Hill.
5. Dua A and Tyagi P, Molecular Spectroscopy: Quantum to Spectrum, (2022)
Atlantic Publishers & Distributors Pvt Ltd.
6. Dua A, Singh C, Quantum Chemistry: Classical to Computational (2015)
ManakinPress.

Practical:

4. Khosla, B.D.; Garg, V.C.; Gulati, A. (2015),Senior Practical Physical Chemistry,

R. Chand & Co, New Delhi.
5. Kapoor, K.L. (2019),A Textbook of Physical Chemistry, Vol.7, 1st Edition,
McGraw Hill Education.
6. Garland, C. W.; Nibler, J. W.; Shoemaker, D. P.( 2003),Experiments in Physical
Chemistry, 8th Edition, McGraw-Hill, New York.

Additional Resources:

3. Castellan, G. W .(2004),Physical Chemistry, Narosa.

4. Petrucci, R. H.(1989),General Chemistry: Principles and Applications, Macmillan
Publishing

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

148
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -7: Analytical Methods in
Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE-7: 04 02 - 02 Class XII
Analytical with
Methods in Science
Chemistry

Learning Objectives

The Learning Objectives of this course are as follows:

• To familiarize students with the concepts of sampling, errors in analysis, accuracy,
precision and introduce basics of statistical analysis. The course introduces students
to important instrumentation and separation techniques routinely used in the
laboratory analysis of biological samples.
• To expose students to instrumentation in the practical and they learn to detect and
separate analytes in a mixture.

Learning outcomes

By studying this course, students will be able to:

• Understand various sources of errors in chemical analysis.
• Learn about methods to minimize error.
• Understand basic principle of instrumentation (Flame Photometer, UV-vis
spectrophotometer, Atomic Absorption spectrophotometer).
• Apply the principles of analysis and instrumentation to analyse soil samples, soft
drinks and synthetic mixtures provided in the laboratory.
• Learn basic principles of separation techniques (chromatography and solvent
extraction) and apply them to separate mixtures.
• Understand principles of Gravimetric analysis and apply them in determination of Ni2+
and Al3+
• Analyse samples independently in the laboratory.

Syllabus
Unit I: Errors in Chemical Analysis (Hours: 8)

149
Types of errors, Accuracy and Precision, Absolute and relative uncertainty, propagation of
uncertainty. The Gaussian distribution, mean and standard deviation, confidence intervals.

Unit 2: Optical Methods of Analysis (Hours: 10)

Origin of spectra, interaction of radiation with matter, fundamental laws of spectroscopy and
selection rules, Beer’s-Lambert Law.
UV-Visible Spectrophotometry: Basic principles of instrumentation for single and double
beam instruments. Determination of concentration of unknown compounds, composition of
metal complexes using Job’s method of continuous variation and mole ratio method.
Flame Atomic Absorption and Emission Spectroscopy: Basic principles of instrumentation.
Techniques of atomization and sample introduction; Method of background correction,
sources of chemical interferences and their method of removal.
Application of these techniques in analysis of biological samples.
Unit 3: Separation Techniques (12 Hours)
Solvent extraction: Classification, principle and efficiency of the technique. Mechanism of
extraction: extraction by solvation and chelation. Technique of extraction: batch, continuous
and counter current extractions.
Chromatography: Principles of Chromatographic separations, Classification of
Chromatographic techniques, Thin Layer Chromatography, Column Chromatography,
efficiency of separation (Resolution, Efficiency of Resolution, Plate Height)
Application of these techniques in analysis of biological samples.

Practical Component Credits: 02

(Laboratory periods: 60)
1. Analysis of soil.
(a) Determination of pH of soil, Total soluble salts, carbonate and bicarbonate,
calcium and magnesium by titration.
(b) Estimation of Potassium, calcium and magnesium by flame photometry.
2. Separation of constituents of leaf pigments by thin layer chromatography.
3. Determination of the ion exchange capacity of an anion exchange resin.
4. Determination of the ion exchange capacity of a cation exchange resin.
5. Separation of amino acids by ion exchange chromatography.
6. Spectrophotometric analysis of Co2+ and Ni2+ ions in a mixture.
7. Spectrophotometric analysis of Caffeine and Benzoic acid in a soft drink
8. Gravimetric estimation of Ni2+ using Dimethylglyoxime.
9. Gravimetric estimation of Al3+ using oxine.
10. Any suitable experiment (other than the listed ones) based upon analytical
techniques discussed in theory section.

150
References:
Theory:
1. Willard, H.H. (1988), Instrumental Methods of Analysis, 7th Edition,
Wardsworth Publishing Company.
2. Christian, G.D. (2004), Analytical Chemistry, 6th Edition, John Wiley & Sons,
New York.
3. Harris, D. C. (2007), Quantitative Chemical Analysis, 6th Edition, Freeman.
4. Skoog, D.A.; Holler F.J.; Nieman, T.A. (2005), Principles of Instrumental
Analysis, Thomson Asia Pvt. Ltd.
5. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook
of Quantitative Chemical Analysis, John Wiley and Sons.

Practical:
1. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denney, R.C. (1989), Vogel’s Textbook
of Quantitative Chemical Analysis, John Wiley and Sons.
2. Marr, G.; Rockett, B. W. (1972), Practical Inorganic Chemistry, Van Nostrand
Reinhold.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

151
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 8: Biomolecule-II

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 8: 04 02 - 02 Class XII
Biomolecules-II with
Science
Learning Objectives

The Learning Objectives of this course are as follows:

• To understand the process of converting knowledge of chemistry into
marketable products for commercial gain.
• To teach students about important biomolecules essential to life
processes.
• 2. To discuss aspects of the principles of organic chemistry in the
structure and function of important biomolecules.

Learning outcomes

By studying this course, students will be able to:

• Learn about the chemistry of natural and synthetic polymers including fabrics
and rubbers.
• Understand the chemistry of biodegradable and conducting polymers and
appreciate the need of biodegradable polymers with emphasis on basic
principles.
• Comprehend the theory of colour and constitution as well as the chemistry of
dyeing.
• Know applications of various types of dyes including those in foods and
textiles.
• Understand the chemistry and applications of natural products like terpenoids
and alkaloids.

Syllabus

Unit 1: Amino acids, Peptides & Proteins (Lecture : 12)

Amino Acids and Peptides -Zwitterion, isoelectric point and electrophoresis. Preparation of
amino acids: Strecker synthesis and using Gabriel’s phthalimide synthesis. Reactions of amino
acids: ester of –COOH group, acetylation of –NH2 group, complexation with Cu2+ ions,
ninhydrin test.

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Determination of the primary structure of peptides by degradation Edman degradation (N-
terminal) and C– terminal (thiohydantoin and with carboxypeptidase enzyme).
Synthesis of simple peptides (up to dipeptides) by N-protection (t-butyloxycarbonyl and
phthaloyl) & C-activating groups and Merrifield solid-phase synthesis. An Overview of
primary, secondary, tertiary and quaternary structure of proteins.

UNIT 2 : Enzymes (Hours: 08)

Classification of enzymes and their uses (mention ribozymes). Mechanism of enzyme action,
factors affecting enzyme action, coenzymes and cofactors and their role in biological reactions,
specificity of enzyme action (including stereo-specificity), enzyme inhibitors and their
importance, and the phenomenon of inhibition (competitive and non-competitive inhibition
including allosteric inhibition). Drug action-receptor theory. Structure – activity relationships
of drug molecules, binding role of –OH group, -NH2 group, double bond and aromatic ring.

Unit 3: Concept of Energy in Biosystems (Hours: 10)

Cells obtain energy by the oxidation of foodstuff (organic molecules). Introduction to
metabolism (catabolism, anabolism). ATP: The universal currency of cellular energy, ATP
hydrolysis and free energy change. Agents for transfer of electrons in biological redox systems:
NAD+, FAD. Conversion of food to energy: Outline of catabolic pathways of carbohydrate-
glycolysis, fermentation, Krebs cycle. The caloric value of food, the standard caloric content
of food types.

PRACTICALS:
Credits: 02
(Laboratory periods: 60)
1. Qualitative tests for amino acids and proteins.
2. Separation and identification of mixture of amino acids by paper chromatography.
3. Study of the action of salivary amylase on starch under optimum conditions and determine
the enzyme activity.
4. Study the effect of temperature on activity of salivary amylase.
5. Isolation of casein from milk.
6. Estimation of proteins by Lowry’s method.
7. Estimation of glucose by Fehling’s solution.
8. Determination of total sugar content by ferricyanide method (volumetric/colorimetric
method).
9. Study of the titration curve of glycine and determine the isoelectric point of glycine.
10. Estimation of proteins by Lowry’s method.
11. Estimation of Glycine by Sorensen’s method.

153
References:
Theory:
1. Devlin, T.M. (2010), Textbook of Biochemistry with Clinical Correlation, Wiley.
2. Berg, J. M.; Tymoczko, J. L.; Stryer, L. (2019), Biochemistry, 9th Ed., W. H. Freeman
Co Ltd.
3. Lehninger, A.L; Nelson, D.L; Cox, M.M. (2009), Principles of Biochemistry, W. H.
Freeman.
5. Finar, I.L. Organic Chemistry (Volume 1 & 2), Dorling Kindersley (India) Pvt. Ltd.
(Pearson Education).

Practical:

1. Dean, J.R.; Jones, A.M.; Holmes, D., Reed, R.; Jones, A. Weyers, J. (2011), Practical
skills in chemistry, Prentice-Hall.
2. Wilson, K.; Walker, J. (2000), Principles and techniques of practical biochemistry,
Cambridge University Press.
3. Gowenlock. A.H. (1988), Varley’s Practical Clinical Biochemistry, CRC Press.
4. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume II, I K
International Publishing House Pvt. Ltd., New Delhi.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

154
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 9: Computer Applications in
Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 9: 04 02 - 02 Class XII
Computer with
Applications Science
in Chemistry

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce the students to basic computer skills that will help them in solving
chemistry problems using spreadsheets and BASIC language.
• To acquaint the students with different software for data tabulation, calculation, graph
plotting, data analysis and document preparation.
• To expose the students to the concept of molecular modelling, its applications to various
molecular systems, energy minimization techniques, analysis of Mulliken Charge and
ESP Plots.

Learning outcomes

By studying this course, students will be able to:

• Become familiar with the simple use of BASIC Language.
• Use software for tabulating data, plotting graphs and charts, carry out statistical
analysis of the data.
• Solve chemistry problems and simulate graphs.
• Prepare documents that will incorporate chemical structure, chemical equations,
mathematical expressions from chemistry.
• Understand theoretical background of computational techniques and selective
application to various molecular systems.
• Learn Energy minimization methods through use of different force fields.
• Learn ESP Plots by suitable soft wares, electron rich and electron deficient sites.
• Compare computational and experimental results and explain deviations.
• Perform Optimization of geometry parameters of a molecule (such as shape, bond
length and bond angle) through use of software like Chem Sketch and Argus Lab
in interesting hands-on exercises.

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Syllabus

Unit 1: Programming using BASIC (Hours: 20)

Programming Language – Elements of BASIC language, Numeric and string Constants and
Variables, arithmetic expressions, hierarchy of operations, inbuilt functions. Syntax and use of
the various QBASIC commands: REM, CLS, INPUT, PRINT, GOTO, IF, IF…THEN,
IF...THEN..ELSE, IF and END IF, FOR and NEXT etc., DIM, READ, DATA, GOSUB,
RETURN, RESTORE, DEF FNR and Library Functions, Simple programs based on usage of
the commands mentioned above.
Statistical analysis using BASIC: Mean, Least square fit - Linear regression, variance, standard
deviation.
Unit 2 : Handling of Numerical Data (Hours: 4)

Spreadsheet software: MS Excel. Creating a spreadsheet, entering and formatting information,

applying basic functions and formulae to the data, drawing charts, tables and graphs, displaying
the equation of graph along with the R2 value, incorporating tables and graphs in Word files,
graphical solution of equations, plotting pressure-volume curves of van der Waals gases,
Maxwell-Boltzmann distribution, concentration versus time graphs, spectral data, titration
curves, etc.
Unit 3: Molecular Modelling (Hours: 6)

Introduction to molecular modelling, overview of classical and quantum mechanical methods

(molecular mechanics, semi empirical, ab initio and DFT), general considerations and
comparison of these methods.

Practical component Credit:02

(Laboratory periods: 15 classes of 4 hours each)
Exercises of Programing
7. Calculate pressure of a real gas using Van der Waal’s Equation.
8. Calculate the most probable speed, average speed and root men square velocity of an
ideal gas.
9. Roots of quadratic equations
10. Binomial coefficient using GOSUB statement.
11. Mean, standard deviation
12. Least square curve fitting method for linear equation.
Plotting graphs using a spreadsheet
4. Van der Waals isotherms
5. Maxwell-Boltzmann distribution curves as function of temperature and molecular
weight

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 6. Plot the conductometric titration curve for
a) strong acid vs strong base and b) weak acid vs strong base
5. Plot the pH metric titration curve for
a) strong acid vs strong base and b) weak acid vs strong base and determine the pKa of
the weak acid
7. Plot the graphs for the kinetics of first order reaction and determine the rate constant
8. Plot the UV-vis absorbance spectra and determine the molar absorption coefficient.
Molecular Modelling
6. Optimize and compare the geometry parameters of H2O and H2S using ArgusLab.
7. Compare the basicities of N atom in ammonia, methylamine, dimethylamine and
trimethylamine using ArgusLab by comparing Mulliken charges and ESP map in
ArgusLab.
8. Compare C-C bond lengths and bond order in ethane, ethene and ethyne using ArgusLab.
9. Determine enthalpy of isomerization of cis and trans-2-butene using ArgusLab.
10. Compare the HAH bond angles for the second row hydrides (BeH2, CH4, NH3, H2O)
and compare with the results from qualitative MO theory.

References:
Theory:
7. Levie, R. de. (2001), How to use Excel in analytical chemistry and in general
scientific data analysis, Cambridge Univ. Press.
8. Venit, S.M. (1996), Programming in BASIC: Problem solving with structure and
style. Jaico Publishing House.
9. Lewars, E. (2003), Computational Chemistry, Kluwer academic Publisher.
10. Cramer, C.J.(2004), Essentials of Computational Chemistry, John Wiley & Sons.
11. Hinchcliffe, A. (1996), Modelling Molecular Structures, John Wiley & Sons.
12. Leach, A.R.(2001), Molecular Modelling, Prentice-Hall.

Practicals
4. Lewars, E. (2003), Computational Chemistry, Kluwer academic Publisher.
5. Cramer, C.J. (2004), Essentials of Computational Chemistry, John Wiley & Sons.
6. Hinchcliffe, A. (1996), Modelling Molecular Structures, John Wiley & Sons.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

157
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE -10: Applied Inorganic Chemistry
CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 10: 04 02 - 02 Class XII
Applied with
Inorganic Science
Chemistry

Learning Objectives

The Learning Objectives of this course are as follows:

• To introduce the principles of catalysis. It further discusses the types of catalysts and
their industrial applications. It gives an insight into different types of fertilizers and
chemistry involved in their manufacturing.
• To learn about applications of metals and inorganic compounds as diagnostic agents
and medicines. The course helps develop the interest of students in the frontier areas
of applied inorganic and medicinal chemistry.

Learning outcomes

By studying this course, students will be able to:

• Get a general idea of catalysis and describe in detail the mechanism of
Wilkinson’s catalyst, Zeigler- Natta catalyst and synthetic gasoline
manufacture by Fischer-Tropsch process and applications of zeolites and
biocatalysis.
• Explain the suitability of fertilizers for different kinds of crops and soil.
• Explain the inorganic compounds and metals in medicine and, specifically,
the role of cisplatin in cancer therapy

Syllabus

Unit 1: Catalysis (Hours: 10)

General principles of catalysis, properties of catalysts, homogeneous and
heterogeneous catalysis (catalytic steps, examples) and their industrial applications,
deactivation and regeneration of catalysts, catalytic poison, promoter. Study of the
following processes and their mechanism:
1. Alkene hydrogenation (Wilkinson’s Catalyst)
2. Synthetic gasoline (Fischer-Tropsch reaction)

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3. Polymerisation of ethene and propene using Ziegler-Natta catalyst
4. Application of zeolites as catalysts.
Introduction and importance of biocatalysis

Unit 2: Fertilizers (Hours: 8)

Different types of fertilizers (N, P and K). Importance of fertilizers, chemistry involved in
the manufacture of the following fertilizers: Urea, ammonium nitrate, calcium ammonium
nitrate, ammonium phosphates, superphosphate of lime and potassium chloride,
Environmental aspects of fertilizers.

Unit 3: Medical Applications of Inorganic Compounds (Hours: 12)

Introduction, Use of Chelating agents, metal complexes as diagnostic agents, Lithium in

mental health, Gold containing drugs, role of metals in Neurodegenerative Diseases,
Inorganic compounds in Chemotherapy: Cisplatin; mode of action, basic idea of second and
third generation drugs.

Practical Component Credits:02

(Laboratory Periods: 60)
1.Preparation of magnesium pyrosilicate (Antacid).
2.Determination of ascorbic acid in vitamin C tablets by iodometric titrations.
3. Preparation of borax.
4. Preparation of boric acid.
5. Catalytic oxidation of potassium sodium tartrate by cobalt(II) chloride.
6. Estimation of boric acid and borax in a mixture by titrimetric analysis
7. Detection of constituents of CAN fertilizer (Calcium, Ammonium and Nitrate ions)
fertilizer and estimation of Calcium content.
8. Detection of constituents of Superphosphate fertilizer (Calcium and Phosphate ions) and
estimation of phosphoric acid content.
9. Detection of constituents of Dolomite (Calcium, Magnesium and carbonate ions) and
determination of composition of Dolomite (Complexometric titration)
References:
Theory:

1. Huheey, J.E.; Keiter, E.A.; Keiter; R. L.; Medhi, O.K. (2009), Inorganic Chemistry-
Principles of Structure and Reactivity, Pearson Education.
2. Atkins, P.W.; Overton, T.L.; Rourke, J.P.; Weller, M.T.; Armstrong, F.A. (2010),
Shriver and Atkins Inorganic Chemistry, 5th Edition, Oxford University Press.
3. Housecraft, E. H.; Sharpe, A.G. (2018), Inorganic Chemistry, 5th Edition, Pearson.
4. Greenwood, N.N.; Earnshaw, A. (1997), Chemistry of the Elements, 2nd Edition,
Elsevier (Ziegler Natta Catalyst and Equilibria in Grignard Solution).
5. Lippard, S.J.; Berg, J.M. (1994), Principles of Bioinorganic Chemistry, Panima
Publishing Company.
6. Spessard, Gary O.; Miessler, Gary L. (1996), Organometallic Chemistry, Prentice-
Hall.

159
 7. Fertilizers and Their Composition, Characteristics, Quality, Transformations and
Applications, Tandon, H.L.S., 2008., Riegel’s Handbook of Industrial Chemistry,
CBS Publishers, New Delhi.
8. Patrick, G. (2017), Introduction to Medicinal Chemistry, Oxford University Press.
9. Wolfgang Kaim, Brigite Schwederski, Axel Klein, Bioinorganic chemistry:
Inorganic elements in the chemistry of life, Jojn Wiley & Sons Inc.

Practicals:

1. Vogel, A.I. (1972), Qualitative Inorganic Analysis, Longman.

2. Svehla, G. (1996), Vogel’s Qualitative Inorganic Analysis, Prentice Hall.
3. Marsh, D.G.; Jacobs, D.L.; Veening, H., J. Chem. Educ., Analysis of commercial
vitamin C tablets by iodometric and coulometric titrimetry. 1973, 50 (9), p 626. DOI:
10.1021/ed050p626
4. https://edu.rsc.org/experiments/catalytic-oxidation-of-potassium-
sodiumtartrate/1736.article

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

160
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 11: Chemistry of Polymers, Dyes
and Natural Products
CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 11: 04 02 - 02 Class XII
Chemistry of with
Polymers, Dyes Science
and Natural
Products
Learning Objectives

The Learning Objectives of this course are as follows:

• To understand the process of converting knowledge of chemistry into
marketable products for commercial gain.
• To familiarize the basic nomenclature of polymers, dyes and natural
products, classification and important terms.

Learning outcomes

By studying this course, students will be able to:

• Learn about the chemistry of natural and synthetic polymers including
fabrics and rubbers.
• Understand the chemistry of biodegradable and conducting polymers and
appreciate the need of biodegradable polymers with emphasis on basic
principles.
• Comprehend the theory of colour and constitution as well as the chemistry
of dyeing.
• Know applications of various types of dyes including those in foods and
textiles.
• Understand the chemistry and applications of natural products like
terpenoids and alkaloids.

Syllabus

UNIT-1: Polymers ( Hours: 12)

Introduction and classification based on origin, monomer units, thermal response, mode of
formation, structure, application and tacticity; di-block, tri-block and amphiphilic polymers;
Weight average molecular weight, number average molecular weight, glass transition

161
 temperature (Tg) of polymers; Polymerisation Reactions-Addition and condensation.
Mechanism of cationic, anionic and free radical addition polymerization; Ziegler-Natta
polymerisation of alkenes.
Preparation and applications of: Plastics -thermosetting (phenol-formaldehyde,
polyurethanes) and thermosoftening(PVC, polythene); Fabrics -natural (cellulose and
synthetic derivatives of cellulose like rayon and viscose); synthetic (acrylic, polyamide,
polyester); Rubbers-natural and synthetic: Buna-N, Buna-S, Neoprene, silicon rubber;
Vulcanization; Polymer additives; Introduction to Specialty Polymers: electroluminescent
(Organic light emitting diodes), conducting, biodegradable polymers and liquid crystals.

UNIT 2: Dyes (Hours: 08)

Classification, Colour and constitution; Mordant and Vat Dyes; Chemistry of dyeing. Synthesis
and applications of Azo dyes – Methyl orange, Congo red; Triphenyl methane dyes- Crystal
violet; Phthalein Dyes – Phenolphthalein; Natural dyes –Structure elucidation and synthesis of
Alizarin and Indigotin; Edible Dyes with examples.

Unit 3: Natural Product Chemistry- An Introduction to Terpenoids and Alkaloids

(Hours: 10)
Terpenes: Introduction, occurrence, classification, uses, isoprene and special isoprene
rule; structure elucidation, synthesis and industrial application of citral.
Alkaloids: Introduction, occurrence, classification, uses, general structural features, general
methods for structure elucidation including Hoffmann’s exhaustive methylation and Emde’s
method. Structure elucidation, synthesis and physiological action of Nicotine.

Practicals: - Credits: 02
(Laboratory periods: 60)

1. Preparation of Starch-PVA Film.

2. Recycling of Plastic: Moulding of plastic or Cracking of plastic.
3. Preparation of Urea-formaldehyde resin.
4. Preparation of Methyl Orange.
(a) Dyeing of different fabrics (cotton, wool, silk) using Alizarin or any other dye.
(b) Preparation of azo dye on the surface of the fabric.
5. Qualitative test for identification of alkaloids (Dragendorff Reagent and Mayer’s
reagent test) and terpenoids (Salkowski test).
6. Preparation of Malachite Green.
7. Preparation of perichromic dye using p-amino Phenol and p-nitro benzaldehyde.

References:

Theory

1. Finar, I.L. (2008), Organic Chemistry, Volume 2, 5th Edition, Pearson Education
2. Saunders, K. J. (1988), Organic Polymer Chemistry,2nd Edition Chapman & Hall,
London
3. Campbell, Ian M., (2000), Introduction to Synthetic Polymers, 2nd Edition Oxford
University Press, USA.
4. Bahadur, P. and Sastry, N.V. (2002) Principles of Polymer Science Narosa
Publications, New Delhi
5. Patrick, G. An Introduction to Medicinal Chemistry (2013), 4th Edition, Oxford
University Press.

162
 6. Priscilla Abarca, Patricia Silva, Iriux Almodovar and Marcos Caroli Rezende* Quim.
Nova, Vol. 37, No. 4, 745-747, 2014. http://dx.doi.org/10.5935/0100-4042.20140120

Practical:

1. Ashraf S.M., Ahmad S., Riaz U., A Laboratory Manual of Polymers, I. K.

International Publishing House Pvt. Ltd., New Delh.
2. Hannaford FA J., Smith P. W. G. & Tatchell A. R.; Vogel’s Textbook of
Practical Organic Chemistry Fifth Edition, Longman Scientific and Technical.
3. Pasricha, S., Chaudhary, A. (2021), Practical Organic Chemistry: Volume I,
I K International Publishing House Pvt. Ltd., New Delhi.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

163
 DISCIPLINE SPECIFIC ELECTIVE COURSE CHEM-DSE 12: Biophysical Chemistry

CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE COURSE

Course title & Credits Credit distribution of the Eligibility Pre-

Code course criteria requisite
Lecture Tutorial Practical/ of the
Practice course (if
any)
Chem-DSE 04 02 - 02 Class XII
12: with
Biophysical Science
Chemistry

Learning Objectives

The Learning Objectives of this course are as follows:

• To provide students with a sound background of latest techniques used in biophysical
research
• To provide them with an understanding of the principles underlying these techniques.

Learning outcomes
By studying this course, students will be able to:
• The students will acquire knowledge of structure and biological functions of
proteins and enzyme.
• Students will acquire knowledge about the principles and applications of latest
methods used to analyse amino acid and proteins.
• The course will also provide students an opportunity for hands-on-experience to
develop their laboratory skills expected for working in a biophysical research lab.

Syllabus

Unit I: Fundamentals of Biological Macromolecules (Hours: 10)

Structure and physical properties of amino acids, structure, function, and folding of
proteins, internal rotational angle, conformations of proteins (Ramachandran plot,
secondary, tertiary and quaternary structure). Structures of nucleic acids, Properties of
nucleosides and nucleotides;composition of nucleic acids, Stabilizing interactions in
biomolecules.

Unit II: Biophysical techniques for the Structural and Conformational Analysis
(Hours: 20)

Overview : General principle and qualitative treatment of the techniques to understand the
structure and characteristics of enzymes, protein and nucleic acid: X-ray crystallography –
protein crystals, myoglobin, nitrogenase, pepsinogen; NMR spectroscopy-NMR spectra of

164
 amino acids, UV-vis absorption spectroscopy, Fluorescence spectroscopy and Vibrational
spectroscopy. Determination of protein structures by spectroscopic methods (FTIR, NMR),
thermodynamics of protein folding by spectroscopic methods, protein conformational study
by NMR and fluorescence spectroscopy. Methods for the separation of biomolecules:
General principles, including Chromatography; Sedimentation, Moving Boundary
Sedimentation, Electrophoresis, Isoelectric focusing.
Practical Component Credits: 02
(Laboratory periods: 60)

1. Separate and identify amino acids by paper chromatography.

2. Determine the isoelectric point of the given proteins.
3. Estimation of Proteins by Biuret, Lowry and Bradford.
4. Estimation of Urea.
5. Separation and identification of Sugars/lipids by TLC.
6. To check the purity of the proteins by calculating A260/ A280 ratio
spectrophotometrically.
7. Agarose gel electrophoresis to check the size of DNA (For example- Calf
ThymusDNA).
8. Characterization of the DNA (genomic/ designed oligonucleotide) as a
function of pH, salt-concentration spectrophotometrically.
9. Determination of the isobestic point by titrating DNA sample with any
ligand using UV- Visiblespectrophotometer.
10. SDS-PAGE analysis of proteins.

References:
Theory:

1. Lesk, A.M., Introduction to Protein Science: Architecture, Function, and

Genomics, 2nd edition, 2010, Oxford University Press.
2. Cantor, C.R. and Schimmel, P.R., Biophysical Chemistry, 1980, Freeman.
3. Van Holde, K.E., Johnson, W.C. and Ho, P.S., Principles of Physical
Biochemistry, 2nded, 2006, Pearson Education.
4. Harding, S.E. and Chowdhry, B. Z. Protein-Ligand Interactions, Oxford
UniversityPress.

Practical:
1. Hofmann, A ., Clokie,S., Wilson and Walker’s Principles &amp; Techniques of
Practical Biochemistry, 2018, Cambridge University Press.
2. Friefelder D. Physical Biochemistry- Application to Biochemistry and Molecular
Biology, 1983, WH Freeman and Company.
3. R. N. Roy, Viva and Practical Physiology, Biochemistry and Biophysics, 1998,
Books and allied Pvt. Ltd.
4. Sawhney, S.K. and Singh , R.,Introductory Practical Biochemistry , 2nd Edition,
2005, Alpha Science International.
5. Keith Wilson , John Walker, John M. Walker Principles and Techniques of
Practical Biochemistry, 5th Edition, 2000, Cambridge University Press.

Note: Examination scheme and mode shall be as prescribed by the Examination Branch,
University of Delhi, from time to time.

165
 CREDIT DISTRIBUTION, ELIGIBILITY AND PRE-REQUISITES OF THE
COURSE
Course title Credits Credit distribution of the Eligibility Pre-
& Code course criteria requisite of
Lecture Tutorial Practical/ the course
Practice (if any)
Research 04 03 -- 01 Class 12th
Methodology with
for Chemists Physics,
(DSE-13) Chemistry

Learning objectives

The objectives of this course are as follows:

• To make the students aware of fundamental but mandatory ethical practices in

chemistry.
• To introduce the concept of data analysis.
• To learn to perform literature survey in different modes.
• To make the students aware of safety handling and safe storage of chemicals.
• To make students aware about plagiarism and how to avoid it.
• To teach the use of different e-resources.

Learning outcomes

By studying this course, students will be able to:

• Follow ethical practices in chemistry
• Do Data analysis
• Literature survey in different modes
• Use e-resources.
• Avoid plagiarism, understand the consequences and how to avoid

SYLLABUS OF DSE-13

UNIT – 1: Scope of Research (Hours: 3)

Introduction, overview of research process: define research problem, review literature,

formulate hypothesis, design research/experiment, collect and analyse data, interpret and report,
scope and importance.

UNIT – 2: Literature Survey, Databases and Research metrics (Hours: 15)

Print: Sources of information: Primary, secondary, tertiary sources; Journals: Journal

abbreviations, Digital: Databases and their responsible use: Google Scholar, Web of science,

166
Scopus, UGC INFONET, SciFinder, PubMed, ResearchGate, E-consortium, e-books; Search
techniques: Phrase, Field, Boolean, Proximity, Concept, Limiting/Refining Search Results.
Research metrics: Impact factor of Journal, h-index, i10 index, Altmetrics, Citation index.
Author identifiers/or profiles: ORCID, Publons, Google Scholar, ResearchGate, VIDWAN

UNIT – 3: Communication in Science (Hours: 12)

Types of technical documents: Full length research paper, book chapters, reviews, short
communication, project proposal, Letters to editor, and thesis.
Thesis writing – different steps and software tools (Word processing, LaTeX, Chemdraw,
Chemsketch etc) in the design and preparation of thesis, layout, structure (chapter plan) and
language of typical reports, Illustrations and tables, bibliography, referencing: Styles (APA,
Oxford etc), annotated bibliography, Citation management tools: Mendeley, Zotero and
Endnote; footnotes. Oral presentation/posters – planning, software tools, creating and making
effective presentation, use of visual aids, importance of effective communication, electronic
manuscript submission, effective oral scientific communication and presentation skills.

UNIT – 4: Research and Publication ethics (Hours: 9)

Scientific Conduct: Ethics with respect to science and research, Scientific Misconducts:
falsification, fabrication and plagiarism, similarity index, software tools for finding plagiarism
(Turnitin, Urkund etc), redundant dublications

Publication Ethics: Introduction, COPE (Committee on Publication Ethics) guidelines; conflicts

of interest, publication misconduct: problems that lead to unethical behaviour and vice versa,
types, violation of publication ethics, authorship and contributorship, predatory publishers and
journals

IPR - Intellectual property rights and patent law, commercialization, copy right, royalty, trade
related aspects of intellectual property rights (TRIPS)

UNIT – 5: Statistical analysis for chemists (Hours:

6)

Types of data, data collection-Methods and tools, data processing, hypothesis testing, Normal
and Binomial distribution, tests of significance: t-test, F-test, chi- square test, ANOVA,
multiple range test, regression and correlation.

Features of data analysis with computers and softwares -Microsoft Excel, Origin, SPSS

Practical component Credits: 01

(Laboratory periods:15 classes of 2 hours each)

12. Collection of journal articles on a particular topic using Google Scholar and creating a
database.
13. Collection of journal articles on a particular topic using Science Direct and creating a
database.
14. Collection of journal articles on a particular topic using Scopus and creating a database.
15. Drawing chemical structure, reactions and mechanisms using Chemsketch or ISIS draw
or any other software.
16. Collection of chemical structure using ChemSpider and creating a database.
17. Curve fitting using freely available softwares/apps (any one)

167
 18. Making of power point presentation
19. Experimental learning of safe storage hazardous chemicals
20. Experimental learning of handling of hazardous chemicals
21. Technical writing on topics assigned.
22. Demonstration for checking of plagiarism using recommended software

Essential/recommended readings:

7. Dean, J. R., Jones, A. M., Holmes, D., Reed, R., Weyers, J. & Jones, A. (2011) Practical
skills in chemistry. 2nd Ed. Prentice-Hall, Harlow.
8. Hibbert, D. B. & Gooding, J. J. (2006) Data analysis for chemistry. Oxford University
Press.
9. Topping, J. (1984) Errors of observation and their treatment. Fourth Ed., Chapman Hall,
London.
10. Harris, D. C. Quantitative chemical analysis. 6th Ed., Freeman (2007) Chapters 3-5.
11. Levie, R. de, how to use Excel in analytical chemistry and in general scientific data
analysis. Cambridge Univ. Press (2001) 487 pages.
12. Chemical safety matters – IUPAC – IPCS, Cambridge University Press, 1992.
OSU safety manual 1.01

168