CLASS XII

There will be two papers in the subject:

PAPER I (THEORY) - 70 Marks

S.No. UNIT TOTAL WEIGHTAGE

1. Solid State
2. Solutions
Physical Chemistry
3. Electrochemistry
25 Marks
4. Chemical Kinetics
5. Surface Chemistry
6. General Principles and Processes of Isolation of Elements
7. p -Block Elements
Inorganic Chemistry
8. d -and f -Block Elements
20 Marks
9. Coordination Compounds
10. Haloalkanes and Haloarenes
11. Alcohols, Phenols and Ethers
12. Aldehydes, Ketones and Carboxylic Acids
Organic Chemistry
13. Organic Compounds containing Nitrogen 25 Marks
14. Biomolecules
15. Polymers
16. Chemistry in Everyday Life
TOTAL 70 Marks

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 PAPER I –THEORY – 70 Marks solutes, abnormal molecular mass association and
dissociation, van't Hoff factor.
1. Solid State
Normality, molality, molarity, mole fraction,
Solids: their classification based on different
ppm, as measures of concentration. Definition of
binding forces such as: ionic, covalent
the above with examples. Simple problems based
molecular; amorphous and crystalline solids
on the above.
(difference), metals. Type of unit cell in two
dimensional and three dimensional lattices, (i) Solubility of gases in liquids – Henry’s Law,
number of atoms per unit cell (all types). simple numericals based on the above.
Calculation of density of unit cell, packing in
(ii) Raoult’s Law for volatile solutes and non-
solids, packing efficiency, voids, point defects,
volatile solutes, ideal solution, non-ideal
electrical and magnetic properties.
solution. Azeotropic mixtures – definition,
Band theory of metals. Conductors, types, graphical representation, fractional
semiconductors (n and p type) and insulators. distillation with examples.
(i) Crystalline and amorphous solids. (iii) Colligative properties – definition and
examples, and its use in determination of
(ii) Definition of crystal lattice, unit cell; types of
molecular mass.
unit cell (scc, fcc, bcc); calculation of the
number of atoms per unit cell; relationship (a) Relative lowering of vapour pressure:
between radius, edge length and nearest Definition and mathematical expression
neighbour distance. Calculation of density of of Raoult’s Law. Determination of
unit cell, formula of the compound – relative molecular mass by measurement
numericals based on it; packing in 3 – D, of lowering of vapour pressure.
packing fraction in scc, fcc, bcc with (b) Depression in freezing point: molal
derivation; voids – types, location, formation depression constant (cryoscopic
(derivation of radius of voids). constant) – definition and mathematical
(iii) Characteristics of crystalline solids; ionic expression (derivation included).
(NaCl), metallic (Cu), atomic (diamond and (c) Elevation in boiling point method: molal
graphite). elevation constant (ebullioscopic
constant) definition and mathematical
(iv) Point defects: Stoichiometric, non-
expression (derivation included).
stoichiometric and impurity defects
(F- centres). (d) Osmotic pressure: definition and
explanation. Natural and chemical
(v) Electrical properties: Conductors,
semipermeable membranes, reverse
semiconductors (n & p types) and insulators
osmosis, isotonic, hypotonic and
(Band Theory), piezoelectricity and
hypertonic solutions. Comparison
pyroelectricity.
between diffusion and osmosis.
(vi) Magnetic properties: diamagnetic, Application of osmotic pressure in the
paramagnetic, ferromagnetic, ferrimagnetic determination of relative molecular
and antiferromagnetic. mass.
2. Solutions van’t Hoff- Boyle’s Law, van’t Hoff –
Study of concentration of solutions of solids in Charles’ Law, van’t Hoff - Avogadro’s
liquids, liquid in liquid, solubility of gases in law.
liquids, solid solutions, Colligative properties - (e) Abnormal molecular mass: Dissociation
Raoult's law of relative lowering and Association with suitable examples
of vapour pressure (1st & 2nd), elevation of
boiling point, depression of freezing (f) van’t Hoff factor for the electrolytes
point, osmotic pressure. Use of colligative which dissociate and the molecules
properties in determining molecular masses of which associate in solution.
Modification of the formula of colligative
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 properties based on van’t Hoff factor. (v) Nernst equation and correlation with the free
Simple problems. Calculation of degree energy of the reaction with suitable
of dissociation and association. examples.
Experimental details not required. Prediction of spontaneity of a reaction based
Numerical problems based on all the above on the cell emf.
methods. Experimental details not required. Numericals on standard electrode potential
of half-cells, cell emf, relationship between
3. Electrochemistry free energy and equilibrium constant,
Electrolytic and electrochemical cells. Redox standard electrode potential and free energy.
reactions in electrochemical cells. (vi) Comparison of metallic conductance and
Electromotive Force (emf) of a cell, standard electrolytic conductance. Relationship
electrode potential, Nernst equation and its between conductance and resistance. Specific
resistance and specific conductance.
application to chemical cells. Relation between
Cell constant: Calculation of cell constant.
Gibbs energy change and emf of a cell.
Meaning of equivalent conductance.
Conductance in electrolytic solutions, specific, Meaning of molar conductance. General
equivalent and molar conductivity, variations of relationship between specific conductance,
conductivity with concentration, graphs; molar conductance and equivalent
Kohlrausch's Law of electrolysis and Faraday’s conductance (units and graphs).
Laws of electrolysis. Dry cell and lead Units, numericals.
accumulator, fuel cells, corrosion. Molar conductance of a weak electrolyte at a
given concentration and at infinite dilution.
(i) Electrochemical cells: introduction, redox Kohlrausch’s Law – definition, applications
reactions (principle of oxidation and and numericals.
reduction in a cell). (vii) Faraday’s laws of Electrolysis.
(ii) Galvanic cells - introduction; Faraday’s First Law of electrolysis.
representation, principle – oxidation Statement, mathematical form. Simple
reduction. Mechanism of production of problems.
electric current in a galvanic cell. Faraday’s Second Law of electrolysis:
(iii) Measurement of potential. Single electrode Statement, mathematical form. Simple
potentials. problems.
Standard hydrogen electrode (Eo) - Relation between Faraday, Avogadro’s
definition, preparation, application and number and charge on an electron. F = NAe
limitations. should be given (no details of Millikan’s
Standard electrode potential - Measurement experiment are required).
of standard electrode potential of Zn ++ / Zn, (viii) Batteries: Primary and Secondary Cells:
Cu ++ / Cu, half cell (using standard Leclanche cell, mercury cell, Lead storage
hydrogen electrode). battery and fuel cell – structure, reactions
Cell notation – representation. and uses.
Factors affecting electrode potential with (ix) Corrosion: Concept, mechanism of
explanation - main emphasis on the electrochemical reaction, factors affecting it
temperature, concentration and nature of the and its prevention.
electrode.
(iv) Electrochemical series. Its explanation on 4. Chemical Kinetics
the basis of standard reduction potential. Meaning of Chemical Kinetics – slow and fast
Prediction of the feasibility of a reaction. reactions. Rate of a reaction - average and
instantaneous rate (graphical representation).
Factors affecting rate of reaction: surface area,
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nature of reactants, concentration, temperature, (vii) The concept of energy: Exothermic and
catalyst and radiation. Order and molecularity endothermic reactions, concept of energy
barrier, threshold and activation energy,
of a reaction, rate law and specific rate constant.
formation of activated complex, effect of
Integrated rate equations and half-life (only for catalyst on activation energy and reaction
zero and first order reactions), concept of rate.
collision theory (elementary idea, no (viii)Collision Theory: Condition for a chemical
mathematical treatment). Concept of threshold change – close contact, particles should
and activation energy, Arrhenious equation. collide. Collisions to be effective – optimum
energy and proper orientation during
(i) Meaning of chemical kinetics, Scope and collision. Energy barrier built-up when the
importance of Kinetics of the reaction, slow collision is about to take place, Activated
and fast reactions – explanation in terms of complex formation, difference in energy of
bonds. the reactant and the product – exothermic
(ii) Rate of Reaction: definition, representation and endothermic reactions with proper
of rate of reaction in terms of reactants and graphs and labelling.
products, determination of rate of reactions (ix)Mechanism of the reaction: meaning of
graphically, instantaneous and average rate elementary reaction, meaning of complex
of reaction. Factors affecting rate of and overall reaction, explanation of the
reaction. mechanism of the reaction, slowest step of
(iii) Law of mass Action: statement and meaning the reaction. Relationship between the rate
of active mass. Explanation with an example expression, order of reactants and products
– general reactions. at the rate-determining step, units of rate
constant – explanation with suitable
(iv) Effect of concentration of reactants on the examples.
rate of a reaction: Qualitative treatment,
based on the law of mass Action, statement of (x) Effect of temperature on the rate constant of
rate law, General rate equation – a reaction: Arrhenius equation – K=Ae-Ea/RT,
Rate = k(concentration of the reactant)n, Meaning of the symbols of Arrhenius
where k is rate constant and n is the order of equation, related graph, evaluation of Ea and
the reaction, relationship between the rate of A from the graph, meaning of slope of the
the reaction with rate constant with respect graph, conversion from exponential to log
to various reactants. form of the equation, relationship between
the increase in temperature and the number
(v) Order of a reaction: meaning, relation of collisions. Numerical based on Arrhenius
between order and stoichiometric coefficients equation.
in balanced equations, order as an
experimental quantity, rate equation for zero 5. Surface Chemistry
order reaction and its unit, mathematical Absorption and Adsorption - physisorption and
derivation of rate equation for first order chemisorption, factors affecting adsorption of
reaction, characteristics of first order gases on solids and liquids. Catalysis;
reaction – rate constant is independent of the homogenous and heterogenous, activity and
initial concentration, units to be derived, selectivity, enzyme catalysis.
definition of half-life period, derivation of
expression of half-life period from first order Colloidal state distinction between true solutions,
rate equation. colloids and suspension; lyophilic, lyophobic
multi-molecular, macromolecular and associated
Problems based on first order rate equation colloids; properties of colloids; Brownian
and half-life period. movement, Tyndall effect, coagulation and
(vi) Molecularity of the reaction: Meaning – electrophoresis. Emulsion - types of emulsions.
physical picture, Relation between order, (i) Difference between absorption and
molecularity and the rate of a reaction, adsorption: definition of physisorption and
Differences between order and molecularity chemisorption and their differences.
of a reaction.

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 Factors affecting adsorption of gases on Occurrence and principles of extraction of
solids, Freundlich adsorption isotherms, aluminium, copper, zinc, iron and silver.
graph, expression and application of (i) Definition of minerals, ores and metallurgy;
adsorption. principle ores of aluminium, iron, copper,
(ii) Catalysis: definition, types of catalysts – zinc and silver.
positive and negative, homogeneous and Methods of concentration of ores: hydraulic
heterogeneous catalyst based on the state of washing, magnetic separation, froth
the reactant and the catalyst, Elementary floatation method, leaching.
treatment of intermediate compound Extraction of metal from concentrated ore –
formation theory with examples; adsorption calcination, roasting and thermal reduction.
Theory, effect of catalyst on the rate of
reaction – the change in the energy of Thermodynamic principle of metallurgy -
activation in the activation energy curve. Gibb’s energy (Ellingham diagram –
significance only).
Characteristics of a catalyst; specificity,
activity, surface area of a catalyst. Promoter Metallurgy of aluminium, iron, copper, zinc
and poison. Enzyme catalysis – basic idea and silver.
and lock and key mechanism. Refining of metals - distillation, liquation,
(iii) Colloidal State: Thomas Graham classified electrolysis, vapour phase refining (nickel),
the substances as crystalloid and colloid, zone refining.
classification of substances on the basis of (ii) Uses of metals and their alloys.
the particle size i.e. true solution, sol and
suspension, colloidal system is 7. p-Block Elements
heterogeneous. lyophilic and lyophobic
Group-15 Elements
colloid; classification of colloidal solutions
as micro, macro and associated colloids. Position in the periodic table, occurrence,
Preparation of lyophilic colloids. electronic configuration, oxidation states, trends
Preparation of lyophobic colloids by colloid in physical and chemical properties. Nitrogen:
preparation properties and its uses; compounds
mill, peptization, Bredig’s arc method,
of nitrogen: oxides of nitrogen. Ammonia and
oxidation, reduction, double decomposition
nitric acid – preparation and properties.
and exchange of solvent method, purification
Phosphorus - allotropic forms, compounds of
of colloids (dialysis, ultra-filtration, and
phosphorus: preparation and properties of
ultracentrifugation). phosphine, halides and oxoacids.
Properties of colloidal solutions: Brownian
(i) General introduction, electronic
movement, Tyndall effect, coagulation,
configuration, occurrence, oxidation states.
electrophoresis (movement of dispersed
Trends in physical properties; chemical
phase), Protection of colloids, Gold number
properties with hydrogen, oxygen and
and Hardy- Schulze rule. Emulsions,
halogens.
surfactants, micelles (only definition and (ii) Nitrogen - Laboratory preparation,
examples). decomposition (ammonium dichromate,
Application of colloids and emulsions in barium azide). Properties and uses.
daily life. (iii) Oxides of nitrogen (N2O, NO, N2O3, N2O4,
N2O5) - preparation, structure and uses.
6. General Principles and Processes of Isolation (iv) Ammonia – Preparation and manufacture.
of Elements Properties: reaction with oxygen, copper
oxide, chlorine, hydrochloric acid, formation
Metals: metallurgy, ores, principles and
of complexes. Uses.
methods of extraction - concentration, (v) Nitric Acid - Preparation and manufacture.
oxidation, reduction, electrolytic refining. Properties: reaction with copper (dilute and

195
 concentrated HNO3), carbon and sulphur. Sulphuric Acid: manufacture by Contact
Uses. Process (equations, conditions and
(vi) Allotropes of phosphorus and their diagram), properties - acidic nature,
structures. mode of dilution, oxidising action,
Phosphine – preparation from phosphorus dehydrating nature and uses of sulphuric
and properties: reaction with halo acids). acid in industry.
Phosphorus trichloride - Preparation from
phosphorous. Uses. Group-17 Elements
Phosphorus pentachloride - preparation Position in the periodic table, occurrence,
from PCl3. Thermal dissociation and electronic configuration, oxidation states,
hydrolysis. Uses, properties. trends in physical and chemical properties;
Oxoacids of phosphorus (structures and Preparation, properties and uses of chlorine
preparation only). and hydrochloric acid. Compound of
Group-16 Elements halogen, oxoacids of halogens (structures
Position in the periodic table, occurrence, only), Interhalogen compounds.
electronic configuration, oxidation states, (i) General introduction, electronic
trends in physical and chemical properties. configuration, oxidation states. Trends in
Oxygen: methods of preparation, properties physical properties and chemical
and uses, classification of oxides. Ozone – properties (hydrogen, oxygen, halogens
methods of preparation. Sulphur -allotropic and metals).
forms. Compounds of sulphur: (ii) Chlorine – preparation from MnO2 and
preparation, properties and uses of sulphur- HCl, from NaCl, MnO2 and conc. H2SO4
dioxide, sulphuric acid (industrial process (only equations), reactions of chlorine
of manufacture). Oxoacids of sulphur with H2S, NH3, cold, dilute NaOH and
(structures only). hot, concentrated NaOH.
(i) Electronic configuration, oxidation (iii)Hydrochloric acid: Lab preparation, its
states, occurrence. Trends in physical acidic nature, reaction with ammonia,
properties; chemical properties with carbonates and sulphites, formation of
hydrogen, oxygen and halogens. aqua regia and its uses.
(ii) Oxygen – lab method of preparation, (iv) Oxoacids of halogens: structures and
formation of oxides with metals and non- acidic property.
metals and their common nature.
(v)Interhalogen compounds – structure,
(iii) Ozone: manufacture by Siemen’s hybridisation and shapes: XX′, XX′3,
ozoniser, thermal decomposition of XX′5, XX′7.
ozone, its oxidising nature – reaction
with lead sulphide, potassium iodide and Group-18 Elements
mercury, its uses. Position in the periodic table, occurrence,
(iv) Sulphur: allotropes of sulphur - electronic configuration, trends in physical and
rhombic, monoclinic, structure of chemical properties, inert nature, uses.
sulphur and action of heat; extraction (i) General introduction, electronic
by Frasch process. configuration, occurrence, trends in
(v) Sulphur dioxide: laboratory and physical; chemical properties, state and low
industrial preparation from sulphites and reactivity.
sulphide ores, reaction of sulphur (ii) Formation of xenon compounds with fluorine
dioxide with NaOH, Cl2, KMnO4 and and oxygen (equations only), hybridisation,
structure of SO2. shape and structure of compounds.
(vi) Oxoacids of sulphur: structures only. (iii) Uses of noble gases.
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8. d and f Block Elements Colour, magnetic properties and shapes.
Position in the periodic table, occurrence, Importance of coordination compounds (in
electronic configuration and characteristics of qualitative analysis, extraction of metals and
biological system).
transition metals, general trends in properties of
the 3d-series of transition metals - metallic (i) Definition of coordination compounds /
character, ionisation enthalpy, oxidation states, complex compounds, differences with a
ionic radii, colour of ions, catalytic property, double salt, study of ligands – mono-, bi-, tri-
magnetic properties, interstitial compounds, , tetra-, penta-, hexa- and polydentate,
chelating ligands, definition of coordination
alloy formation, preparation and properties of
number, its calculation for a complex
K2Cr2O7 and KMnO4. coordination sphere, study of oxidation state
Lanthanoids and actinoids. of an element in a complex, its calculation,
(i) d-Block: 3d, 4d and 5d series IUPAC rules of nomenclature of
coordination compounds.
Study in terms of metallic character, atomic
(ii) Isomerism – structural, stereo types and
and ionic radii, ionisation enthalpy,
examples.
oxidisation states, variable valency,
formation of coloured compounds, formation (iii) Valence bond theory of coordination
of complexes, alloy formation. compounds – examples of formation of inner
orbital and outer orbital complexes (high
(ii) f-Block: 4f and 5f series and low spin, octahedral, tetrahedral and
Electronic configuration, atomic and ionic square planar), prediction of magnetic
radii, oxidisation states, formation of character.
coloured compounds, formation of (iv) Crystal field theory – crystal field splitting in
complexes, alloy formation. Lanthanoid tetra and octahedral systems. Explanation of
contraction and its consequences. Chemical colour and magnetic character.
reactivity – with oxygen, hydrogen, halogen, (v) Stability of coordination compounds (explain
sulphur, nitrogen, carbon and water. stability on the basis of magnitude of K) as
Actinoids - oxidation states and comparison mentioned above).
with lanthanoids. (vi) Importance and uses.
(iii) Potassium permanganate: structure, shape,
10. Haloalkanes and Haloarenes.
equation of extraction from pyrolusite ore, its
oxidising nature in acidic, basic and neutral Haloalkanes: General formula, nomenclature
medium, use in redox titration. and classification. Nature of C–X bond,
physical and chemical properties, mechanism
Oxidising nature in acidic [FeSO4,
of substitution reactions, optical rotation.
(COOH)2.2H2O, KI], basic (KI) and neutral
(H2S) mediums to be done. Haloarenes: Basic idea, nature of C–X bond,
substitution reactions (directive influence of
(iv) Potassium dichromate: structure, shape, halogen in monosubstituted compounds only).
equation of extraction from chromite ore and
its use in titration. Oxidising nature in acidic, Uses and environmental effects of -
dichloromethane, trichloromethane, tetra-
basic and neutral medium, use in redox
chloromethane, iodoform, freons and DDT.
titration. Interconversion of chromate and
dichromate ion (effect of pH). Nature of C-X bond
Naming the halogen derivatives of alkanes by
9. Coordination Compounds using common system and IUPAC system for
Concept of complexes, definition of ligands, mono, di and tri-halo derivatives.
coordination number, oxidation number. IUPAC Preparation of haloalkanes from:
nomenclature of mononuclear coordination
compounds. Isomerism (structural and stereo). - Alkane and halogen.
Bonding, Werner's theory, VBT and CFT. - Alkene and hydrogen halide.

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 - Alcohols with PX3, PCl5 and SOCl2. mechanism of dehydration, uses with special
- Halide exchange method (Finkelstein and reference to methanol and ethanol.
Swarts) (i) Classification into monohydric, dihydric and
- Silver salt of fatty acids (Hunsdiecker). polyhydric alcohols, general formulae,
structure and nomenclature of alcohols.
Physical properties: State, melting point, boiling
Difference between primary, secondary and
point and solubility.
tertiary alcohols in terms of structure,
Chemical properties: nucleophilic substitution physical properties and chemical properties.
reactions (SN1, SN2 mechanism in terms of
(ii) Methods of preparation:
primary, secondary and tertiary halides)
Reaction with: sodium hydroxide, water, sodium - Hydration of Alkenes – direct hydration,
iodide, ammonia, primary amine, secondary indirect hydration, hydroboration
amine, potassium cyanide, silver cyanide, oxidation.
potassium nitrite, silver nitrite, silver salt of fatty - From Grignard’s reagent.
acid and lithium-aluminium hydride. - Hydrolysis of alkyl halides.
Elimination reaction (Saytzeff’s rule) / β - Reduction of carbonyl compounds.
elimination.
- From primary amines.
Reaction with metals: sodium and magnesium
Manufacture of methanol by Bosch process
(Wurtz’s reaction, Grignard’s reagent
and ethanol by fermentation of
preparation).
carbohydrates, chemical equations required
Chloroform and iodoform: preparation and (only outline of the method of manufacture,
properties. detail not required).
Structure of freons. Properties:
Preparation of haloarenes by Sandmeyer’s and - Acidic nature of alcohols:
Gattermann’s reaction, by electrophilic - Reaction with sodium.
substitution.
- Esterification with mechanism.
Physical properties: State, melting point, boiling
point and solubility. - Reaction with hydrogen halides.
Chemical properties: - Reaction with PCl3, PCl5, and SOCl2.
- Electrophilic substitution (chlorination - Reaction with acid chlorides and acid
nitration and sulphonation) with mechanism. anhydrides
- Nucleophilic substitution (replacement of - Oxidation.
chlorine with -OH, -NH2) with mechanism. - Dehydration with mechanism.
- Reduction to benzene. Uses of alcohols.
- Wurtz-Fittig reaction. (iii) Conversion of one alcohol into another.
- Fittig reaction. (iv) Distinction between primary, secondary and
- Addition reaction with magnesium tertiary alcohols by Lucas’ Test.
(formation of Grignard reagent). Phenols: Classification and nomenclature.
- Structure of DDT. Methods of preparation, physical and chemical
properties, acidic nature of phenol, electrophilic
11. Alcohols, Phenols and Ethers substitution reactions, uses of phenols.
Alcohols: Classification, general formula, Preparation of phenol from diazonium salt,
structure and nomenclature. Methods of chlorobenzene (Dow’s process) and from
benzene sulphonic acid.
preparation, physical and chemical properties
(of primary alcohols only), identification of Manufacture from Cumene.
primary, secondary and tertiary alcohols, Physical properties: state and solubility.

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 Chemical properties: • From alkynes (hydration).
- Acidic character of phenol. • From acid chlorides (Rosenmund’s
- Reaction with sodium hydroxide. reduction, reaction with dialkyl cadmium).
- Reaction with sodium. • From calcium salt of carboxylic acids.
- Reaction with zinc. • From nitriles (Stephen reaction, Grignard’s
- Reaction with acetyl chloride and acetic reagent).
anhydride. • From esters.
- Reaction with phosphorus penta chloride. Physical properties – state and boiling point.
- Bromination, nitration and sulphonation Chemical properties:
(Electrophilic substitution reactions). • Nucleophilic addition reactions with
- Kolbe’s reaction (formation of salicylic mechanism (ammonia and its derivatives,
acid). HCN, NaHSO3 and Grignard’s reagent).
- Reimer – Tiemann reaction • Oxidation reactions, iodoform reaction.
- Test for phenol – FeCl3 test, azo dye test. • Reduction: reduction to alcohol and alkanes
Aliphatic Ethers: General formula, structure and (Clemmensen’s reduction, Wolff-Kishner
nomenclature. Methods of preparation, physical reduction, Red phosphorus and HI).
and chemical properties, uses.
• Base catalysed reactions (with mechanism):
Ethers: structure of ethereal group. Aldol condensation, cross Aldol
Preparation from alcohol (Williamson’s condensation, Cannizzaro’s reaction.
synthesis). Tests: difference between formaldehyde and
Physical properties: state, miscibility. acetaldehyde; aldehydes and ketones.
Chemical properties: Uses of aldehydes and ketones.
- Reaction with chlorine.
- Oxidation (peroxide formation). Aromatic aldehyde (Benzaldehyde)
Lab preparation from toluene by oxidation with
- Reaction with HI.
chromyl chloride.
- Reaction with PCl5.
Physical properties: state and stability.
Aryl ethers
Chemical properties:
Physical properties – state and solubility.
• Oxidation and reduction.
Chemical properties – preparation of anisole
• Nucleophilic addition reaction (hydrogen
(Williamson’s synthesis), electrophilic
cyanide and sodium bisulphite).
substitution (halogenation, nitration and
Friedel-Crafts reaction.) • Reactions with ammonia and its derivatives
(hydroxyl amine, hydrazine and phenyl
Uses of ether.
hydrazine).
12. Aldehydes, Ketones and Carboxylic Acids • Reaction with phosphorus pentachloride.
Aldehydes and Ketones: Nomenclature, • Cannizzaro reaction.
structure of methods of preparation of • Benzoin condensation.
aldehydes and ketones, physical and chemical
• Perkin’s reaction.
properties, mechanism of nucleophilic addition,
reactivity of alpha hydrogen in aldehydes and • Electrophilic substitution - halogenation,
uses. nitration and sulphonation.
Preparation: Test: distinction between aromatic and aliphatic
• From alcohol. aldehydes.
• From alkenes (ozonolysis). Uses of benzaldehyde.

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 Carboxylic Acids: Classification, general - From alcohol.
formula and structure of carboxylic group.
Nomenclature, acidic nature, methods of - From alkyl halide.
preparation, physical and chemical properties - From cyanide.
and uses.
- From amide (Hofmann’s degradation).
Classification of mono and di carboxylic acids
with examples. - From nitro compounds.
Preparation of aliphatic and aromatic carboxylic - Gabriel phthalimide Synthesis.
acid: Physical properties: comparison between
- From alcohols, aldehydes. primary, secondary and tertiary amines in
- From nitriles. terms of – state, solubility, boiling point
- From Grignard’s reagent. (hydrogen bonding), comparison with
Physical properties: state, boiling point and alcohols.
solubility. Chemical properties:
Chemical properties: - Basic character of amines – comparison
between primary, secondary and tertiary
- Acidic character: (aliphatic, aromatic
alkyl amines/ ammonia/ aniline. Effect of
carboxylic acids with the effect of substituents on the basic strength of
substituents on the acidic character – to be aniline
dealt with in detail)
- Alkylation and acylation with
- Reaction with active metals, alkalies, mechanism.
carbonates and bicarbonates, - Reaction with nitrous acid.
- Formation of acid derivatives. - Carbylamine reaction.
- Decarboxylation (chemical and Kolbe’s Distinction between primary, secondary
electrolytic reaction). and tertiary amines (Hinsberg’s Test).
- HVZ reactions. Aniline
- Substitution of benzene ring (meta directive Preparation reduction of nitrobenzene.
effect of carboxylic acid group) nitration and Physical properties – state, solubility and boiling
sulphonation. point.
Tests for acids: formic acid, acetic acid and Chemical properties:
benzoic acid. - Reaction with HCl and H2 SO4 .
Uses of formic acid, acetic acid and benzoic acid. - Acetylation, alkylation.
- Benzoylation.
13. Organic compounds containing Nitrogen - Carbylamine reaction.
Aliphatic Amines: General formula and, - Diazotisation.
classification of amines. Structure of the amino - Electrophilic substitution (bromination,
group, nomenclature. Methods of preparation, nitration and sulphonation).
physical and chemical properties, uses, Tests for aniline.
identification of primary, secondary and tertiary
Uses of aniline.
amines.
• Amines Cyanides and Isocyanides
Nomenclature, classification with examples, Methods of preparation:
structure, general formula. Cyanides:
Methods of preparation: - From alkyl halide.

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 - From amide. and quaternary, structures of proteins,
Isocyanides: denaturation of proteins. (Definitions only.
Details and diagrams are not required).
- From alkyl halide.
From primary amines Vitamins - Classification and functions.
Vitamins A, B, C, D, E and K: classification
Diazonium salts: Preparation, chemical (fat soluble and water soluble), deficiency
reactions and importance in synthetic organic diseases. (Chemical names and structures are not
chemistry. required).
Preparation from aniline;
Properties: Sandmeyer’s reaction, Gattermann Nucleic Acids - DNA and RNA.
reaction and Balz – Scheimann reaction, Nucleic acids: basic unit – purine and
replacement of diazo group by – H, -OH, -NO2, pyrimidine, DNA – structure (double helical),
coupling reaction with phenol and aniline. RNA (No chemical structure required).
Differences between DNA and RNA.
14. Biomolecules
Carbohydrates – Definition, Classification 15. Polymers
(aldoses and ketoses), monosaccahrides (glucose Definition and classification on different
and fructose), D-L configuration parameters. Methods of polymerisation
oligosaccharides (sucrose, lactose, maltose), (addition and condensation), copolymerisation,
polysaccharides (starch, cellulose, glycogen); and some important polymers: natural and
Importance of carbohydrates. synthetic like polythene, nylon polyesters,
Carbohydrates: definition, classification - mono bakelite, rubber. Biodegradable and non-
(aldose, ketose), oligo (di, tri, tetra saccharides) biodegradable polymers.
and polysaccharides with examples: reducing Classification based on source, on structure, on
sugars and non-reducing sugars – examples and mode of polymerisation, on molecular forces, on
uses. growth (with free radical mechanism).
Establishment of structures for glucose and Preparation of important addition polymers -
fructose (open and cyclic) heating with HI, Polythene, polypropene, PVC, PTFE,
reaction with hydroxylamine, bromine water, polystyrene.
acetic anhydride, nitric acid and phenyl Rubber – natural and synthetic (Buna-N and
hydrazine. Buna-S), vulcanisation of rubber.
Test for glucose and fructose (bromine water test Preparation of important condensation polymers
with equation).
- polyester, Nylon 66, Nylon 6, Bakelite,
Disaccharides – structures of sucrose, maltose
melamine (to be learnt in terms of monomers and
and lactose (glycosidic linkage).
Polysaccharides – starch, cellulose, glycogen. equations).
Biodegradable polymers – PHBV, Nylon 2 -
Proteins – structural units of proteins. Basic Nylon 6.
idea of - amino acids, peptide bond, Uses.
polypeptides, proteins, structure of proteins -
primary, secondary, tertiary structure and 16. Chemistry in Everyday life
quaternary structures (qualitative idea only),
Chemicals in medicines - analgesics,
denaturation of proteins. Enzymes, hormones -
tranquilizers antiseptics, disinfectants,
elementary idea only.
antimicrobials, antifertility drugs, antibiotics,
Proteins: Amino acids – general structure, antacids, antihistamines.
classification and zwitter ion formation.
In medicine: antipyretics, analgesics,
Isoelectric point.
tranquillisers, antiseptics, disinfectants,
Classification of proteins on the basis of
molecular shape; primary, secondary, tertiary
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 anti-microbials, anti-fertility drugs, OBSERVATION TABLE
antihistamines, antibiotics, antacids.
S. (A) (B) (B – A)
Definition, common examples, uses. No.
Differences between antiseptics and
Initial Final Difference
disinfectants. burette burette (ml)
Structure not required. reading reading
Chemicals in food - preservatives, artificial (ml) (ml)
sweetening agents, elementary idea of 1
antioxidants. 2
Preservatives: role, example (Sodium benzoate). 3
Artificial sweetening agents: role, examples
(aspartame, saccharine, sucralose and alitame). • Concordant reading is to be used for titre value.
Soaps and detergents - Classification and their Concordant reading is two consecutive values
cleansing action. which are exactly the same. Average will not be
Soaps and detergents: classification, structure accepted as titre value.
and some important examples. • The table is to be completed in ink only. Pencil is
Advantage of detergents over soaps; not to be used.
classification of detergents into • Overwriting will not be accepted in the tabular
anionic/biodegradable, cationic/non- column.
biodegradable and non-ionic. Observations:
• Pipette size (should be same for all the
PAPER II candidates at the centre).
PRACTICAL WORK – 15 Marks
• Titre value (concordant value).
Candidates are required to complete the following 2. Study of the rate of reaction
experiments: The candidates will be required, having been
1. Titrations given full instructions, to carry out an experiment
Oxidation-reduction titrations: potassium on the rate of reaction, e.g. reaction between
manganate (VII) / ammonium iron (II) sulphate; sodium thiosulphate and hydrochloric acid
(using different concentrations for either),
potassium manganate (VII) / oxalic acid.
magnesium and dil. sulphuric acid/ dil.
The candidate may be required to determine the
hydrochloric acid (using different
percentage purity of a compound and the number
concentrations).
of molecules of water of crystallization in • Graph of volume vs. time and its
hydrated salts. In such experiments sufficient interpretation.
working details including recognition of the end • Relationship between concentration and rate,
point will be given. volume and rate and time and rate.
Candidates will be required to calculate:
3. Identification of the following compounds and
• Molarity
functional groups based on observations
• Concentration in grams L-1 / molecular mass
• Alcoholic group - glycerol
• Number of molecules of water of
crystallisation/ percentage purity. • Aldehyde group- formaldehyde
• Ketonic group – acetone
NOTE: Molarity must be calculated upto 4
decimal places at least, in order to avoid error. • Carboxylic group – benzoic acid
• Amino group - aniline

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 *Please Note: Carbylamine and acrolein tests Anions: Dilute acid group – CO32-, NO2-, S2-,
should not be performed. SO32-
The student should learn to differentiate between Concentrated Acid Group – NO3-, Cl-,
colours, solution, ring and precipitate. Br-, I-, CH3COO-.
4. Characteristic tests of carbohydrates and Special Group - SO42-, PO43-, C2O42-.
proteins Cations: Group Zero: NH4+
• Carbohydrates – glucose Group I: Pb2+
• Proteins – powdered milk Group II : Cu2+, Pb2+
Identification should be of ‘Carbohydrate’ and Group III: Al3+, Fe3+
‘Protein’ not of individual substances. Group IV: Zn2+, Mn2+, Ni2+, Co2+
Group V: Ba2+, Sr2+, Ca2+
5. Experiments related to pH change using pH
Group VI: Mg2+
paper or universal indicator. NOTE:
• Determination of pH of some solutions • Formal analytical procedure is required for
obtained from fruit juice, solutions of known Qualitative Analysis.
and varied concentrations of acids, bases and • Specific solvent for O.S. to be used;
salts. • Before adding Group III reagents to the
• Comparison of pH of the solutions of strong filtrate of Group II, H2S must be removed
and weak acids of the same concentration. followed by boiling with conc. Nitric acid.
Use of universal indicator/pH paper must be • The right order for buffer (NH4Cl and
taught to the students. NH4OH) must be used.
• The flame test with the precipitate obtained
6. Electrochemistry in Group V for Ba2+, Sr2+, Ca2+ will also be
Setting up a simple voltaic cell. accepted as a confirmatory test.
Variation of cell potential in Zn/Zn2+//Cu2+/Cu For wet test of anions, sodium carbonate
with change in concentration of electrolyte extract must be used (except for carbonate).
(CuSO4, ZnSO4) at room temperature.
PATTERN OF CHEMISTRY
7. Qualitative analysis PRACTICAL PAPER
Qualitative analysis: identification of single salt
Questions in the practical paper will be set as
containing one anion and one cation:
follows:
Anions: CO32-, NO2-, S2-, SO32-, SO42-, NO3-,
Question 1 Volumetric Analysis
CH3COO-, Cl-, Br-, I-, C2O42-, PO43-.
Question 2 Any one or a combination of the
Cations: NH4+, Pb2+, Cu2+, Al3+, Fe3+, Zn2+, Mn2+ following experiments:
, Ni2+, Co2+, Ba2+, Sr2+, Ca2+, Mg2+. • Study of the rate of reaction.
• Identification of the organic
NOTE: compounds and functional groups
Chromyl chloride test not to be performed. based on observations.
For wet test of anions, sodium carbonate • Characteristic tests of carbohydrates
extract must be used (except for carbonate). and proteins.
(Insoluble salts such as lead sulphate, barium • Experiments related to pH
sulphate, calcium sulphate, strontium sulphate determination using pH paper or
universal indicator.
will not be given).
• Electrochemistry.
Question 3 Qualitative Analysis (single salt).

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 PROJECT WORK AND PRACTICAL FILE - 5. Simple idea of chemical evolution.
15 Marks 6. Natural polymers (any five) - structure,
Project Work – 10 Marks characteristics, uses. Synthetic polymers (any
five) - method of preparation, structure,
The project work is to be assessed by a Visiting
characteristics and uses.
Examiner appointed locally and approved by the
Council. 7. Types of Dyes - methods of preparation,
characteristics and uses.
The candidate is to creatively execute one
8. Chemicals in medicines: antiseptics, antibiotics,
project/assignment on an aspect of Chemistry. antacids, etc. and their uses.
Teachers may assign or students may select a topic of
their choice. Following is only a suggestive list of 9. Preparation of soap, nail polish, boot polish,
projects. varnish, nail polish remover, shampoo and
perfumes.
Suggested Evaluation criteria for Project Work:
10. Chemicals and chemical processes in forensic
• Introduction / purpose
studies.
• Contents
11. Insecticides, pesticides and chemical fertilisers.
• Analysis/ material aid (graph, data, structure, pie
12. Ancient Indian medicines and medicinal plants.
charts, histograms, diagrams, etc.)
13. Organic Chemistry in Nutrition, Food Science
• Presentation
and Biotechnology.
• Bibliography
14. Effect of Green House Gases.
Suggested Assignments: 15. How Plastics have changed the world, both
1. Amino acids: Peptides, structure and socially and economically.
classification, proteins structure and their role in
the growth of living beings.
2. Nucleic Acid: DNA and RNA – their structure. Practical File – 5 Marks
Unique nature. Importance in evolution and their
The Visiting Examiner is required to assess students
characteristic features. on the basis of the Chemistry Practical file
3. Carbohydrates and their metabolism, Blood - maintained by them during the academic year.
haemoglobin and respiration.
4. Vitamins and hormones

NOTE: According to the recommendation of International Union of Pure and Applied Chemistry (IUPAC), the
groups are numbered from 1 to 18 replacing the older notation of groups IA ….. VIIA, VIII, IB …… VIIB and
0. However, for the examination both notations will be accepted.

Old IA IIA IIIB IVB VB VIB VIIB VIII IB IIB IIIA IVA VA VIA VIIA 0
notation
New 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
notation

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