Chemistry

There are total 15 Topics in this chapter.

 Matter & its Nature  Chemical Reactions &

Equations
 Structure of an Atom

 Acids, Base & Salts  Chemical Bonding

 Ph Scale  Atmospheric Pollution

 Chemistry in everyday Life

 Organic Chemistry
 Common Elements &
Compounds
 Metals & Non- Metals

 Polymerization
 Important PYQs
 Periodic Table  Recent PYQs

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 Matter and its Nature
Matter is a substance made up of various types of particles that occupies physical space
and has inertia. According to the principles of modern physics, the various types of
particles each have a specific mass and size. The most familiar examples of material
particles are the electron, the proton and the neutron.

 Properties of Matter
 Occupies place
 Having its weight
 Having quality of Inertia
 Change in its state

State of Matter
Physical State Chemical State
1) Physical state
 Solid state: having Definite Shape and Volume.
 Liquid State: having Indefinite shape and definite Volume.
 Gaseous state: having indefinite shape and Volume
 Plasma State: having indefinite shape and Volume (partially Gaseous Form)
2) Chemical State
 Elements
 Compounds
 Mixture

1) Element: An element is a substance which cannot be split up into two or more simpler
substances by usual chemical methods of applying heat, light or electric energy.
e. g. hydrogen, oxygen, sodium, chlorine etc.
 Elements are of two types that is Metals and Non- Metals as explained below:

 Metals:
 All metals are solid except Mercury. Example- Sodium, Gold, Silver, etc
 Release electrons to make Cations.
 Lustre(Shining) in nature.
 Electropositive
 Having solid State.
 Good Conductor of electricity.
 Malleability and Ductility in Nature.

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  Having High Melting Point and Boiling Point.

 Non- Metals
 All Non- Metals are Solid or Gases. Example: Hydrogen, Oxygen
 Receive electrons to make Anions.
 Non- Lustre except Graphite.
 Electropositive.
 Having Solid and Gaseous State.
 Bad Conductor of electricity except Graphite.
 Having Brittle
 Having Low Melting Point and Boiling Point.
 Example: Sulphur(Solid State), Oxygen(Gaseous State), Bromine(Liquid State).

2) Compound: A compound is a substance made up of two or more elements

chemically combined in a fixed ratio by weight e.g. H2O (water), NaCl (sodium chlorid(e)
etc.

3) Mixture: A mixture is a substance which consists of two or more elements or compounds

not chemically combined together. e.g. Air is a mixture of nitrogen, oxygen, inert gases,
water vapour, carbon dioxide etc. Mixtures are impure substances. Types of mixtures: They
are of two types:
a) Homogeneous mixture: It has a uniform composition throughout and its components
cannot be distinguished visually. e.g. A well mixed sample of vinegar.

b) Heterogeneous mixture: It is one that is not uniform throughout. Different samples of

a heterogeneous mixture may have different composition. e.g. a mixture of salt and
pepper.

 Important process
 Freezing: Heat transfer occurs between the warmer tray and the colder air
in the freezer. The warm water loses heat to the cold air in the freezer. This
heat transfer occurs until no energy is available for the particles to slide past
each other. This forces them to remain in fixed positions, locked in place by
the force of attraction between them. This way liquid water is changed into
solid ice. The process of liquid water changing to solid ice is termed as
freezing. The temperature at which it occurs is known as the freezing point.

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 Melting: If you took out the ice cubes from the freezer and placed them in a
warm room, the ice would absorb energy from the warmer air around them. This
absorbed energy would facilitate them to overcome the force of attraction holding
them together, enabling them to slip out of the fixed position that they held as ice.
The process in which a solids change to a liquid is called melting. The melting point
is the temperature at which a solids change to a liquid.

 Vaporization: If the water is hot enough, it starts to boil. Bubbles of water vapor
are formed in the boiling water. This happens as particles of liquid water gain
enough energy to completely overcome the force of attraction between them
and change to the gaseous state. The bubbles rise through the water and escape
from the pot as steam. The process in which a liquid boils and changes to a gas is
called vaporization. The temperature at which a liquid boils is its boiling point.

 Condensation: When you take a hot shower in a closed bathroom, the mirror is
likely to fog up. You may wonder why does this happen? Some hot water from the
shower evaporates and when it comes in contact with cooler surfaces such as the
mirror, it cools and loses energy. The cooler water particles no longer have the
energy to overcome the forces of attraction between them. They come together
and form droplets of liquid water. This process in which a gas changes to liquid is
known as condensation.

 Sublimation: The process in which solids directly change to gases is known as

sublimation. This occurs when solids absorb enough energy to completely
overcome the forces of attraction between them. Dry ice is an example of solids
that undergo sublimation.

 Simple Distillation: Simple distillation involves heating the liquid mixture to the
boiling point and immediately condensing the resulting vapours.This method is only
effective for mixtures wherein the boiling points of the liquids are considerably
different (a minimum difference of 25ºC). The purity of the distillate (the purified
liquid) is governed by Raoult’s law.

 Fractional Distillation: Fractional distillation is often used to separate mixtures

of liquids that have similar boiling points. It involves several vaporization-
condensation steps (which takes place in a fractioning column). This process is also
known as rectification.

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 Steam Distillation: Steam distillation is often used to separate heat-sensitive
components in a mixture. This is done by passing steam through the mixture (which
is slightly heated) to vaporize some of it. The process establishes a high heat-transfer
rate without the need for high temperatures. The resulting vapor is condensed to
afford the required distillate. The process of steam distillation is used to obtain
essential oils and herbal distillates from several aromatic flowers/herbs
 Solution: It is a homogeneous mixture of two or more substances whose composition
can be varied. e.g. Solution of common salt in water, solution of ammonia in water.
Separating the components of a mixture: Various methods are used for separating the
constituents of a mixture.
1. Insoluble solid in solvent - Sedimentation followed by filtration. In case of a
fine solid centrifugation is used instead of filtration
2. Solution of solid in liquid - Evaporation, crystallization, distillation
3. Miscible mixture of liquids - Fractional distillation
4. Immiscible mixture of liquids - Separating funnel
5. Mixture of two solids one of which is sublime – Sublimation
6. Mixture of substances in solution – Chromatography

 Solute: The component of solution that is dissolved and present in smaller quantities in a
solution is known as solute. e.g. common salt in case of solution of common salt in water
and ammonia in case of solution of ammonia in water.

 Solvent: The component of solution in which solute is dissolved is known as solvent. It is

always present in larger amount in a solution. e.g. water in case of the solution of common
salt or ammonia in water.

Types of Solution
 Saturated Solution: A solution in which no more solute can be dissolved at the same
temperature is called Saturated solution.

 Unsaturated Solution: It is a solution in which more solute can be dissolved at the

same temperature.

 Super-saturated Solution: It is a solution which contains more mass of the dissolved

solute than the saturated solution at the same temperature and pressure.

 Alloys: Alloys are homogeneous mixtures of metal and cannot separated into their
components by physical methods. e.g. Brass is a mixture of copper (Cu) and zinc (Zn).

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  Concentration of a solution: Concentration of a solution is the amount of solute
present in a given amount (mass or volume of a solution or the amount of solute dissolved
in a given mass or volume of a solvent.
Amount of solute Concentration = Amount of solvent

 Solubility: It is defined as the amount of solute dissolved in 100g of solvent to form a

saturated solution.
 Suspension: It is a non-homogeneous mixture in which solids are dispersed in liquids. In it
the solute particles do not dissolve but remains suspended through out the bulk of the
medium.

 Colloids or colloidal solution: Colloid is a heterogeneous mixture. The size of

particles of a colloid is intermediate between true solutions and suspensions (i.e,
between 1nm and 100 nm). The particles of a colloid cannot be seen with naked
eye. Types of colloidal solution: Since colloidal solution is heterogeneous mixture it
consists of two phases. These are
(i) dispersed phase (colloidal particles)
(ii) dispersion medium (The medium in which colloidal particles are dispersed.

 Emulsion: Emulsions are liquid-liquid colloids. Types of Emulsion: Emulsions are of two
types:
(i) water in oil
(ii) oil in water
 Emulsifiers are those substances that help in forming stable emulsions of oil and water,
e.g. milk, cod-liver oil, cold creams, vanishing creams, moisturising cream, paints, etc.

STRUCTURE OF ATOM
The atomic theory of matter was first proposed by John Dalton Fundamental particles of an atom
are Electron, Proton and Neutron.

 Proton(p):
 Discovered by E. Goldstein.
 Protons are positively charged.
 The absolute charge on the electron to be + 1.6 x 10-19 C.

 Electron (e):
 Discovered by J.J. Thomson when he was studying the properties of cathode
ray.
 Irish physicist George Johnstone Stoney named this charge 'electron' in 1891.

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  Electrons are negatively charged.
 The absolute charge on the electron to be - 1.6 x 10-19 C.
 e/me as: 1.758820 x 1011 C kg-1
 The charge of an electron was measured by R. Millikan in Oil drop
experiment.

 Neutrons (n)
 Discovered by J. Chadwick
 It has no charge and a mass nearly equal to that of a proton
 The mass of a neutron is taken as one unit each

 Atomic nucleus - Discovered by E Rutherford

 The fast moving alpha (a)-particles (doubly-charged helium ions) were made
to fall on a thin gold foil.
 The mass of an atom is the sum of the masses of protons and neutrons present
in the nucleus.

 Valency
 The number of electrons gained, lost or shared so as to make the octet of
electrons in the outermost shell, is called valency.
 The atoms of elements, having a completely filled outermost shell show little
chemical activity, their valency is zero.
 An outermost-shell, which had eight electrons is said to possess an octet.
Atoms would thus react, so as to achieve an octet in the outermost shell.
 The chemical behaviour of an atom depend upon the number of electrons
orbiting around the nucleus.

 Atomic Number (Z)

 The atomic number is defined as the total number of protons present in the
nucleus of an atom. It is denoted by "Z".
 Mass number
 The mass number is defined as the sum of the total number of nucleons
(protons and neutrons) present in the nucleus of an atom.

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 Isotopes
 Atoms which have the same atomic number but different mass numbers. The
chemical properties of isotopes are similar but their physical properties are
different. But some isotopes have special properties which find them useful in
various fields. Some of them are:
I. An isotope of uranium is used as a fuel in nuclear reactors.
II. An isotope of cobalt is used in the treatment of cancer.
III. An isotope of iodine is used in the treatment of goiter.

Radioactive isotopes
 Arsenic-74-detect tumors
 Sodium-24 Blood clot
 lodine-131 Activity of thyroid gland
 Cobalt-60 Treat of cancer

 Isobars-Atoms of different elements with different atomic numbers, which have

the same mass number, are known as isobars.

 Isotones - Atoms having same number of neutrons.

 Isoelectronics - Isoelectronic refers to two atoms, ions or molecules that have

the same electronic structure and same number of valence electrons.

 Mass defect - The mass defect is the difference between the rest mass of a
nucleus and the sum of the rest masses of its constituent nucleons.

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 PYQs
1. Atomic theory of matter was given by ---- Dalton
2. Atomic size is of the order of ---- 10-8 cm
3. Atom are ---- Proton, electron, neutron
4. The size of the nucleus is measured in ---- Fermi
5. The radius of an atomic nucleus is of the order of ---- 10-13 cm
6. Nucleus of an atom consists of ---- Proton and Neutron
7. When Helium atom loses electron, then it becomes ---- Positive Helium ion
8. Which of the following particle is negatively charged? ---- Electron
9. The absolute value of charge on electron was determined by ---- R.A. Millikan
10. Electrons move around the nucleus in ---- Orbital
11. An atom has 2 electrons in K-shell, 8 electrons in L-shell and 6 electrons in M-shell.
The number of s-electrons present in that element is ------ 6
12. The proton in heavier than an electron by ---- 1837 times
13. CN- ion is isoelectronic with of proton is 1837 times heavier than ----- CO & N2
14. Which of the following is the maximum number of electrons in M- shell ---- 18
15. Which among the following will be a negative ion? ---- If it has more electrons than
protons
16. Electrons in the highest energy level of an atom are called ----- Valence electrons
17. Fe has 26 protons in its nucleus. What are the number of electrons in Fe2+(II) ion? ----
24
18. Number of p-electrons in bromine atom ---- 17
19. Which of the following is not a nucleon? ---- Electron
20. According to Rutherford's atomic model, the electron inside an atom are ---- Non-
stationary
21. Rutherford's a-scattering experiment related to the size of the ---- Nucleus
22. Discovery of the nucleus of an atom was due to the experiment carried out by ----
Rutherford
23. The atomic number of carbon is 6 and its atomic mass in 12. How many are there
protons in the nucleus of carbon? ---- 6
24. Which of the following has maximum Mass? ---- Neutron
25. The mass of proton and mass of __________ is same. ----- Neutron

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26. The nuclear particle having no mass and no charge, but only spin is ---- Neutrino
27. Who is awarded by Noble prize for the discovery of Neutron? ----- Chadwick
28. When cathode rays strike a target of high atomic weight, they give rise to ---- X-rays
29. J.J. Thomson proposed a model which is generally called ________ model. ---- Plum
and pudding
30. Atomic number of an atom gives the number of which of the following? --- Protons
31. Which of the properties of the element is a whole number? ---- Atomic number
32. Element having atomic number 29 is related to ----- d- Block
33. The electronic configuration of a dipositive ion M2+ is 2, 8, 14 and its atomic mass is
56. The number of neutrons in the nucleus would be: ------ 30
34. The unrelated member of the following group is ---- Cyclotron
35. The antiparticle of an electron is ----- Positron
36. Which two basic forces are able to provide an attractive force between two
neutrons? ----- Gravitational and Nuclear forces
37. Cathode rays are ------- Stream of electron
38. Two elements X and Y are isotonic having atomic weight 54 and 56 respectively. If
the atomic number of X is 26, then the atomic number of Y is ---- 28
39. What is the formula of potassium ion in the noble state? ---- K
40. Atomic Number of Hydrogen is ----- 1
41. Atomic number of which of the elements is greater than that of Magnesium
following ---- Aluminium
42. Atomic number of which of the following elements is greater than that of
Aluminium? ---- Phosphorous
43. Atomic number of which of the following elements is greater than that of
Phosphorous? ----- Chlorine
44. Atomic number of which of the following elements is greater than that of Neon? ----
Magnesium
45. Atomic number of which of the following elements is greater than that of silicon ----
Sulphur
46. Atomic number of which of the following elements is greater than that of Zinc ----
Bromine
47. Atomic number of which element is greater than that of Iodine ---- Platinum
48. Atomic number of which element is greater than that of potassium ----- Calcium

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49. Atomic number of which element is greater than that of Calcium? ---- Scandium
50. The mass number of an atom is ---- Sometimes more and sometimes equal to its
atomic number
51. An Element has Atomic number 17 and Mass number 36, then number of neutrons
present in it ----- 19
52. Which of the following element has relative atomic weight that is made up to atom
containing each of 17 protons, 18 Neutrons and 17 Electrons? ---- 35
53. How many neutrons are there in Us atom? ---- 146
54. Atomic number of which element is greater than that of Chlorine ---- Potassium
55. Atomic number of which element is greater than that of Copper? --- Zinc
56. Atomic number of an atom gives the number of which of the following? ---- Protons
57. Atomic number of which element is greater than that of Fluorine? ----- Sodium
58. Atomic number of which element is greater than that of Iron? ----- Cobalt
59. Mass number is the sum of ------- Protons and Neutrons
60. The number of neutrons present in an element having mass number 226 and atomic
number 88 is: ---- 138
61. Atomic mass of Oxygen is 16 and atomic number is 8. What is the mass in grams of 2
moles of oxygen gas? ---- 64
62. The photoelectric effect is described as the ejection of electrons from the surface
of a metal when ----- light of suitable frequency fall on it
63. The photoelectric emission from metal surface starts only when the incident light has
a certain minimum ---- Frequency
64. Propagation of light quanta may be described by ----- Photons
65. The value of planck's constant is ---- 6.62 x 10-34 J.s
66. Who discovered X-Ray? ----- Wilhelm Roentgen
67. By which one of the following, an old written material which cannot be read easily,
can be read? ---- X-rays
68. Which one of the following is the correct sequence of wavelength of radiations? ----
--- IR> Green > UV > Hard X-rays
69. Which of the following is not Electromagnetic in nature? ----- Cathode rays
70. Wavelength of which of the following colours of the visible spectrum of light are
maximum absorbed by green plants ----- Red and blue
71. Which of the following is not true about X rays? ------ Low power

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72. The reverse effect of X-ray emission is ----- Photo-electric effect
73. Which of the following has the lowest frequency? ----- Visible light
74. If an electron and a photon have the same wave length, then they will have the
same ----- Linear momentum
75. Which of the following particle has the dual nature of particle and wave? ----
Electron
76. The concept of dual nature of radiation proposed by ----- De-Broglie
77. "The position and velocity of a small particle like electron cannot be simultaneously
determined. "This statement is ---- Heisenberg uncertainty principle
78. All isotopes of the same element have ----- The same atomic number but different
atomic mass
79. Nuclides have same atomic number are called: ----- Isotopes
80. Atoms of same element having different mass numbers are called ---- Isotopes
81. Chemical properties of isotopes ------ Must be Same
82. Atoms having the same number of protons but different number of neutrons are
called: ---- Isotopes
83. Atoms of different elements have ----- Different atomic number and different number
of valence electrons.
84. Atoms having same no. of neutron but different no. of electrons or protons are
called ---- Isotones
85. Isobars have ----- Same mass numbers but different atomic numbers
86. The total energy of revolving electron in ----- Can never be positive
87. The spectrum of helium is expected to be similar to that of: ----- Li+
88. When an electron drops from a higher energy level to a low energy level then: ----
Energy is emitted
89. In Lyman series an electron jumps from higher energy level to ---- K energy level
90. In which region of electromagnetic spectrum does the Lyman series of hydrogen
atom lie? ----- Ultraviolet Ray
91. The total number of orbitals in a principal shell are ----- n2
92. The mercury and sodium street lamps light up because of ---- Atomic emission
93. The atomic orbital is ------ The region in which there is maximum probability of
finding electron
94. Orientation of atomic orbital is controlled by ---- Magnetic Quantum number

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95. Two electrons in an orbital are differentiated by which of the following? ----- Spin
quantum number
96. "All the four quantum numbers of two electrons in an atom are not the same." It is
the law of ----- Pauli's exclusion principle
97. When there are two electrons in the same orbital, they have: ----- Opposite spin
98. Who was the first to explain hydrogen spectrum? ---- Neil Bohr
99. Bohr's model can explain: ----- Spectrum of any atom or ion having one electron
only
100. When a metal is heated in a flame, the electrons absorb energy and jump to
higher energy state. On coming back to the lower energy state, they emit light,
which we can observe in ----- Emission spectra
101. Bohr's concept of the orbit in an atom was contradicted by ----- Uncertainty
principle
102. Which orbital is dumb- bell shaped? ---- p-orbital
103. In an atom the order of filling up of the orbitals is governed by ----- Aufbau
principle
104. According to Aufbau principle, the correct or der of energy of 3d, 4s and 4p
orbitals is: ------ 4s < 3d < <4p
105. The statement that the electron occupies avail able orbital singly before
pairing occurs is called ----- Hund's rule
106. Nitrogen atom has unpaired electrons. This can be explained as due to: -----
Hund's rule
107. Number of neutrons in an atom of hydrogen is ---- Zero
108. The subatomic particle that does not have any electric charge is a/an (A)
Electron ----- Neutron
109. How is atomic mass number determined? ------ By adding number of protons
and neutrons
110. What are the components of nucleus of an atom? ------ Protons and Neutrons
111. What is the mass of one mole of a substance grams is called? ---- Molecular
Mass
112. Which among the following is a negatively charged ion? ------ Iodine ion
113. Atomic Number is denoted by which alphabet? ----- Z
114. How are 'Cations' formed? ----- Removal of electron

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 115. How are ‘Anions’ are formed? ----- Addition of electron
116. What are Isobars? ---- Elements with different atomic Number But Same Mass
Number.
117. Who discovered Proton? ----- Goldstein.

Acid, Base and Salts

Acid: An acid is a compound, produce hydrogen ions, H+(aq), in solution, which are
responsible for their acidic properties.

Example: HCl H+ + Cl-

According to Bronsted-Lowry theory, an acid is any species that can donate a proton to another
species.

 Characteristics:
 Acids are Sour in Taste.
 Release Hydrogen Gas after react with Metals.
 Blue Litmus change in Red Litmus
 Acid + Base Salt + H2O
 Value of Acids: 0-7 (in Ph Scale)
 Acids are decaying in Nature.
 Acids + Metal Carbonates Salt + H2O + CO2
Example: 2HCl + Na2CO3 2NaCl + H2O + CO2

 Types of Acids:
a) Hydrogenic Acids: which Contains Hydrogen.
Example: hydrochloric acid, HBr, HNO3, etc.

b) Oxy Acids: which contains Oxygen Atoms.

Example: HNO3, H2SO4, etc.

c) Strong Acid: All those acids where hydrogen can be completely ionised takes place.
Examples of strong acids are: hydrochloric acid, sulphuric acid, nitric acid etc.

d) Weak Acid: All those acids where hydrogen can be Partially ionised takes place.
Examples are: acetic acid, formic acid, carbonic acid etc.

Uses of Acids
Substance Acid
Sour Milk Lactic Acid

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 Apple Mallic Acid
Butter/ Curd Butyric Acid
Ant/ Bees Formic Acid
Soda Water Carbonyl Acid
Batteries Sulphuric Acid
To remove Rust in Clothes Use Oxalic Acid
Vinegar Acetic Acid
Guava, Oranges Ascorbic Acid
Proteins Amino Acids
Tea, Tomatoes Oxalic Acid
Grapes/ Tamarind/ Goose Berries Tartaric Acid
Citrus fruits Citric Acid

Base: A Base is a substance that gives OH (Hydroxide ions). when dissolved in water. Bases
-

are usually metal hydroxides (MOH).

Example: NaOH Na+ + OH- (Hydroxide ion)

According to Bronsted-Lowry theory, a base is a proton acceptor.

Example: NH3 + H2O NH4+ (take Proton) + OH- (Hydroxide ion)

 Characteristics:
 Bases are soapy substances with a bitter taste.
 Some Bases soluble in water are called alkalies. All alkalies are bases but all bases
are not alkalies.
 Red Litmus change into Blue Litmus
 Bases turns Phenopthaline into Pink Colour.
 Base + Acid Salt + Water
 Base + Some Metals release Hydrogen Gas
 Base + Oil/ fats Soap/ Glycerol.

 Types of Bases:
a) Strong Base: which are completely soluble in water
Examples: Sodium hydroxide: caustic soda, Potassium hydroxide, etc.

b) Weak Base: which are partially soluble in water.

Examples: Magnesium hydroxide, Ammonium hydroxide, etc.

Uses of Important Base

1. Sodium Hydroxide: Manufacturing of Soap, Purification of petroleum,

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 Paper, Medicines & Textile Industry.

2. Calcium Oxide: Bleaching Powder, White Wash, etc.

3. Calcium Hydroxide: Bleaching Powder, White Wash, in Tanning,
Helps to Hard water into Soft Water.

4. Magnesium Hydroxide: Milk of magnesia, Acid Poisoning, Antidote.

5. Potassium Hydroxide: making of Soft Soap, helps to absorbs SO2 & CO2.

Salt: A salt is an ionic compound that can be formed by the neutralization reaction of an acid
and a base.

Example: HCl + NaOH NaCl + H2O

 Characteristics:
 Solid in Nature.
 Completely dissolved in Water
 Having High Melting Point & Boiling Points.
 Salts are of good Conductors of electricity.

Uses of important Salts

1. Sodium Chloride: helps to melt in Ice, helps to release HCl in Stomach, Nervous
System used in the manufacture of chlorine, caustic soda, washing
soda and baking soda.
2. NaOH: Manufacturing of Soap & Detergent, Paper, Artificial Thread, Petroleum
Purification, Bleach and Colour.
3. Sodium Carbonate/ Washing Soda: to remove Permanent impurity of water,
Soap, Borax, etc.
4. Potassium Nitrate: Gun Powder & Explosive, Fire Cracker, Fertilizers, Glass.
5. Potash Allum: helps to stop Bleeding of Blood, Colour Industry, in Printing.
6. Ammonium Chloride: Ammonia, Fertilizers , Dying of clothes.
7. Hypo/ Sodium Thio Sulphate: Photography, helps to separates Gold & Silver
From Minerals.
8. Ammonium salts are used as fertilizers.
9. Silver bromide is used in photography.
10. Potassium Chlorate is used in the match industry.

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 11. Aluminium sulphate is used in preparing alums.

PH SCALE
The p in pH stands for 'potenz in German, meaning power. The scale that measures the
strength of an acid or a base is called the pH scale. This value lies between 0 and 14.
 Higher the hydronium ion concentration, lower is the pH value.
 The pH of a neutral solution is 7. Values less than 7 on the pH scale represent an
acidic solution. As the pH value increases from 7 to 14, it represents an increase in
OH- ion concentration in the solution, that is, increase in the strength of alkali.
 Most food crops grow best at a PH of 7-7.8.If the soil is too acidic then its pH can be
raised by adding lime or slaked lime which neutralizes the excess acid in the soil.
Similarly, if the soil is too alkaline then its pH can be lowered by adding gypsum or
some other substance which can neutralize the excess alkali present in the soil.
 The medium in our stomach is highly acidic and has pH around 1.2. Our stomach
produces hydrochloric acid which helps in digestion of food. Magnesium hydroxide
(Milk of magnesia), a mild base, is an antacid which neutralises the excess acid.
 Tooth decay starts when the pH of the mouth is lower than 5.5.
 Acid Rain- When pH of rain water is less than 5.6, it is called acid rain.

Substance pH Value
Gastric Juice 1.2
Lemon Juice 2.2

Pure water 7
Milk of magnesia 10

Sodium hydroxide solution 14

Human Blood 7.35 – 7.45

Sea water 7.5 – 8.4
Ammonia 10.6 – 11.6
Milk 6.5 – 6.7
Normal rain 5.6 – 6
Acid rain 2 – 5.6
Human Urine 6
Black coffee 5
Beers 4.5

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 Wines 2.8 – 3.8
Vinegar 2.9
Lemon Juice 2.4

Acid, Base and Salt PYQs

1. ______________ is the strongest acid? --------CF3COOH
2. ______________ is the weakest acid?----------C6H5OH(Phenol)
3. The element common to all acid is?-------------- Hydrogen
4. Concentrated HNO3 is stored in containers made of: -------- Al (Aluminium)
5. Skin becomes yellow in concentrated HNO, because: ------- The proteins are
converted into Xantho proteins.
6. Organic acid containing Hydroxyl group is-----------Carbolic acid
7. Sulphuric acid is---------Dibasic
8. Chemical name of vinegar is---------- Acetic acid
9. Which acid is known as 'King of chemicals'?--------------H₂SO4(Sulphuric Acid)
10. Which is known as Carbolic acid?------------------ C6H5OH(Phenol)
11. Ammonium chloride is acidic salt, because it is a salt of:--- Strong acid and Weak
base
12. Acids turn __________ litmus to________----------- Blue, Red
13. ___________are not bad conductor of electricity in aqueous solution------ Acid
14. The acid used in the Lead storage cell is ------- Sulphuric acid
15. Which one of the following acid is used in the battery?--------- Sulphuric acid
16. Chemical name of 'Oil of Vitriol is----------- Sulphuric acid
17. The compound used in prickly-heat powder to prevent excessive sweating is-------
Boric acid.
18. Name the source from which Aspirin is produced?--------Willow bark
19. Which acid is present in apple? -------------- Malic Acid
20. Which acid is used for making Aspirin? ---------- Salicyclic Acid
21. Which acid is present in tomatoes?----------- Oxalic acid
22. Which acid is used to remove Iron and rust stains from clothes? -------Oxalic Acid
23. Which of the following induces souring of milk?------------Lactic Acid
24. Name the acid present in lemon.--------- Citric acid
25. An Ester used as medicine is:----------Methyl Salicylate

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26. Bee sting contains------------ An acidic liquid
27. If some drops of conc sulphuric acid is added to that substance then turns to black,
which of the following is that substance?------- Sugar
28. The acid used to dissolve gold is ----------- Aquaregia
29. Baking soda is one of the constituents of baking powder. The other constituent is-----
---Tartaric Acid
30. ____________ is the following is battery acid?---------- H₂SO4(Sulphuric Acid)
31. Hydrochloric acid is also known as-----------Muriatic acid
32. The acid which fails to liberate carbon dioxide from Sodium bicarbonate is----
Carbonic acid
33. Sour taste of coca cola is due to ----------- Phosphoric acid
34. __________ is the is used to dissolve noble metals?--------- Aqua regia
35. Which chemical is injected into a person's body when an ant bites?-------Formic
Acid
36. Litmus is obtained from-----------Lichen
37. pH value of Human blood is--------- 7.35-7.45
38. What is the pH of water?----------- 7
39. pH-scale ranges from --------- 0-14
40. The pH of Lemon Juice is expected to be--------- Less than 7
41. Aluminium oxide is a/an?---------- Amphoteric
42. Formic acid is produced by--------Red ants
43. Sodium carbonate is basic salt, because it is a salt of:------Weak acid and strong
base
44. The Base used as an antacid----------Magnesium Hydroxide
45. The natural indicator is-------------Litmus
46. The drying of milk of lime (white washing) is due to the action of-------CO2 in air
47. Soda water was invented by -------- Joseph Priestley
48. Kidney stones are composed of-------- Calcium Oxalate
49. Nitric acid does not react with-------- Gold
50. Iodex, a pain relief balm, has the smell of------- Methyl salicylate
51. What is Brine solution?--------- Excess salt + water
52. Sodium bicarbonate is chemical name of which of the following?-------- Baking
Soda

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53. Which among the following is responsible colour of nitric acid? -------- Nitrogen
dioxide
54. What is the common name of Calcium Hypochlorite? -------- Bleaching powder
55. Spinach contains -------- Oxalic Acid
56. What is the common name of sodium carbonate?-------- Washing soda
57. What is the chemical formula for Sodium Chloride (Salt)?------- NaCl
58. What is nature of pH of Milk?----- Slightly acidic
59. What is the common name of Sodium bicarborate? ----- Baking soda
60. chemical formula of quicklime? -------- CaO
61. Most liquids that conduct electricity are solutions of acids, bases and------- Salts
62. Which base is present in milk of magnesia?--------- Magnesium hydroxide
63. Tartaric Acid is not found in------- Spinach
64. What is the chemical name of quick lime? --------- Calcium oxide
65. What is the common name of CaOCI2?-------- Bleaching powder
66. What is the nature of antacid?------- Basic
67. pH of the human blood is ------- Slightly basic
68. Which base is present in lime water? --------- Calcium hydroxide
69. What is the reaction between an acid and a base called?--------- Neutralisation
70. In an acid base reaction which product is produced along with a salt?------ Water\
71. What is the name of the acid in grapes?----------- Tartaric acid
72. Blue Vitriol is another name of --------- Copper Sulphate
73. The reaction of Copper Sulphate and Iron produces Iron Sulphate and------- Copper
74. Crystallisation is an example of? ------- Physical change
75. Vinegar and Baking Soda together produce ------- Carbon dioxide
76. Chemical formula for sulfurous acid is: ------- H₂SO3

Chemistry in Everyday Life

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Synthetic Materials: The materials created by man using the natural materials, are known
as synthetic materials.

Cement
 It was discovered by an English Mason, Joseph Aspdin in 1824. He called it Portland
cement because he thought that it resembled the limestone found in Portland.
 It is a complex mixture of Calcium silicates & Aluminium silicates.
 Raw materials are limestone provides (lime), clay (provides alumina and silica),
gypsum (reduces the setting time of cement).
 When water is mixed with cement and left as such for sometime, it becomes a hard
mass. This is know as setting of cement. It is an exothermic process, therefore
cement structures have to be cooled upto 7 days by sprinkling water.
 Mortar is a mixture of cement, sand and water. It is used for plastering walls and
binding bricks and stones.
 Concrete is a mixtures of cement, sand, gravel or small pieces of stone and water.
It is used for the construction of floors.
 The structure having iron rods embedded in wet concrete, is known as reinforced
concrete.

Approximate Composition of Portland cement

 Calcium oxide (CaO) : 60-70%
 Silica (SiO2): 20-25%
 Alumina (Al2O3): 5-10%
 Magnesium Oxide(MgO): 2- 5 %
 Ferric oxide(Fe2O3): 1- 2 %
 Gypsum(CaSO4.2H2O): 2-5%
 Sulphur trioxide(SO3): 0-1%

Glass (Na O.CaO.6SiO2)

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 It is a supercooled liquid of silicates.
 Raw material used for the formation of glass are sodium carbonate, calcium
carbonate and sand.
 Finely powdered mixture known as batch, is mixed with cullet (broken glass pieces)
and then fused in a tank furnace at 1673 K. After few hours, molten glass is
obtained.
 Molten glass is cooled slowly and uniformly. The process of slow and uniform cooling
is known as Annealing.
 Different addition may produce different coloured glasses.

Substance used Colour of glass

Cuprous oxide Red
Cupric oxide Peacock blue
Potassium dichromate Green or Greenish yellow
Ferrous oxide Green
Ferric oxide Brown
Manganese dioxide Light pink, in excess black
Cobalt oxide Blue
Gold chloride Ruby
Cadmium Yellow
Carbon Amber colour
Millennium Oxide Orange Red
Cupric Oxide/ Ferric Oxide Black

Variety of glass and Uses

1. Soft glass: It is a mixture of sodium or calcium silicates. It is used in making
window glass, Tube light, Apparatus of chemistry Labs, mirrors and common glass
wares etc.

2. Hard glass - It is a mixture of potassium and calcium silicates. It is more resistant

to the action of acids for making hard glass apparatus.

3. Flint glass: It is mainly a mixture of sodium, potassium and lead silicates. It is used
in making bulbs, Lens, Prisms, Bulbs and Optical Instruments.

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4. Pyrex glass (Borosilicate glass) - It is used in making pharmaceutical
containers, lab apparatus, over ware and Luxury Utensils of Glass.

5. Quartz glass (Silica glass) - It is used in the preparation of chemical

apparatus, optical instrument and Lamps of UV Bulbs.

6. Crookes glass: It is used for making lenses for spectacles. It absorbs UV rays.

7. Photochromatic glass: On exposure to bright light, photochromatic glass

darkens temporarily. So, it is very useful as a Sun shield. In these glasses Black colour
obtained because of Silver Bromide.

8. Safety glass: The three layers are joined together by the action of heat and
pressure. It does not break easily under impact and is used in auto vehicle wind
shield.

9. Xena Glass: It helps to store Chemicals in Xena Glass.

10. Optical glass - It is used for making lenses for microscope, telescope and
spectacles.

11. Glass fibres: It used as insulating material in oven, refrigerator etc.

12. Optical fibres: They are extensively used in telecommunication surgical

operations etc. Optical fibres can transmit images round corners.

13. Lead crystal glass: Lead glass has a high refractive index. So, it is used for
making expensive glass ware.

14. Etching of glass - Glass is attacked by hydrofluoric Sadd acid (H(F), therefore it
is used in the etching of glass.

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 CHEMICALS IN AGRICULTURE
Fertilizers
 Urea is the best fertilizer as it leaves only carbon dioxide after ammonia, has been
assimilated by plants.
 It has 46.6% Nitrogen and it does not alter the pH of the soil.
 Mixture of Ca(CN)2 and C is known as nitrolin. Commercially, calcium nitrate is
known as Norwegian saltpetre.
 The mixture of nitrogenous, phosphatic and potash fertilizers in suitable amounts, is
called NPK fertilizers.

Pesticides
 Pesticides are the chemicals which are applied to crops, e.g: DDT and malathion.

Difethialone
 Vitamin K has been suggested and successfully used, as antidote for pets or
humans accidentally or intentionally exposed to anticoagulant poisons.

Chemicals in medicines
Analgesics (Pain relievers)
 These reduce pain. Aspirin and paracetamol are non-narcotic analgesics. Aspirin
reduces fever, prevents platelet coagulation.

Narcotic analgesics are chiefly used for the relief of post operative pain, cardiac
pain and pains of terminal cancer and in child birth.

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 PYQs
1. Gun Powder is a Mixture of ------- Nitrate, Sulphur and Charcoal
2. Which of the following mixture cause the explosion of TNT (Trinitrotoluene) ----
Ammonium Nitrate
3. Ammonal is a mixture of ---- Aluminium powder and Ammonium nitrate
4. Limestone is a raw material used by which industry? ----- Cement
5. The process of setting of cement under water is essentially---- A hydration process
6. Setting of cement is ------ An exothermic reaction
7. ____________ decreases the rate of setting of cement.----- Gypsum
8. The addition of Gypsum to Portland cement helps in ---- Preventing rapid setting of
cement.
9. Trinitrotoluene is ---- used as an explosive
10. Who discovered cement? ------ Joseph Aspdin
11. Chemical composition of cement is ------ Limestone, Clay and Gypsum
12. Cement is formed by strongly heating mixture of ----- Lime Stone and clay
13. Cement is a mixture of ------ Calcium Silicate and calcium aluminates
14. Concrete is a mixture of ----- Cement, sand, gravel and water
15. Glass is a ------- Super Cooled Liquid
16. Which one of the following is used for sun glasses?---- Crookes glass
17. Which type of Glass is used for making glass reinforced plastic? ----- Fibre glass
18. The calorie requirement of the body increases in winter as compared to summer
because more calories are necessary to ----- Sustain body temperature
19. Pasteurization is a process in which milk is heated at ---- 63°C for 30 min
20. Combustion is a ----- Chemical Process
21. Which one of the following fuel causes Least environmental Pollution?---- Hydrogen
22. Wheat harvesting is an ------- Gravity separation
23. Water is not effective in extinguishing a fire caused by petrol because ------- Water
and petrol are immiscible with each other and petrol forms upper Layer continue to
burn.
24. Which of the following is responsible for extra strength of Pyrex glass? ---- Borax
25. Adding which substance gives green colour to glass? ---- Chromium Oxide
26. Adding which substance gives blue colour to glass? --- Cobalt Oxide

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27. Which glass is used to make spectacles? ---- Crookes glass
28. __________ is used for making chemical apparatus like beakers, flasks etc. ----------
Hard glass
29. Diesel oil is preferred for heavy motor vehicles because it--- It has more capacity
and saves fuel.
30. Quality of Petrol is expressed in terms of ---- Cetane number
31. Which one of the following is main constituent of LPG? ------ Butane

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 SOME COMMON ELEMENTS & COMPOUNDS
1. Carbon:
 Carbon exhibits allotropy and shows maximum catenation.
 Carbon occurs both in free state as diamond, coal etc. and also in the combined
form as CO2.
 Diamond is one of the allotropic forms of carbon and is the purest form of natural
carbon. It is the hardest natural substance.
 Graphite is also an allotropic form of carbon, which is very soft and slippery.
Graphite are prepared artificially by Acheson process.
 Fullerene (C60) looks like a soccer ball. It contains 20 six membered and 12-five
membered rings of carbon atoms.
 Graphene is an allotrope of carbon. It is a strong substance and used as a
conducting material for touch screen, LCD and LED.

Compounds of Carbon
 Carbon monoxide (CO)
 Carbon monoxide (CO) combines with haemoglobin to form carboxyhaemoglobin
which is not able to absorb oxygen and as a result of this, suffocation takes place
(Asphyxi(a).
 The death of persons in closed rooms with wood, coal or coke fires and in closed
bathrooms with gas geyser is due to the formation of carbon monoxide.

 Carbon dioxide (CO2)

 0.03-0.05 percent in atmosphere.
 Solid CO2 is known as dry ice. It is used in refrigerators under the name drikold. It is
used in transport of perishable food materials as it provides cold as well as the inert
atmosphere.

 Carbides
 They are the compounds of carbon with metals or electronegative elements.
 Destructive distillation of coal gives products like coal gas, gas carbon, coal tar and
ammonical liquor.
 Lamp Black is also known as Soot.

2. Nitrogen:
 Nitrogen is a neutral gas and is neither combustible nor a supporter of
combustion.

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  In air - 79% of Nitrogen is present (by volume). In combined state, nitrogen is
found as nitrates (Chile) saltpetre-sodium nitrate (NaNO3), Indian saltpetre --
potassium nitrate (KNO3)

Compounds of Nitrogen
 Ammonia
 It is prepared from nitrogen and hydrogen by Haber's process. It has pungent odour.
 Ammonia is used in manufacturing fertilizers and explosives etc.
 Nitrogen fixation involves the fixation of atmospheric nitrogen into nitrate by lightning
and by nitrogen fixing bacteria called Rhizobia.

3. Oxygen:
 Oxygen is an important constituent of atmosphere (21% by volume). Supporter of
combustion.
 Liquid oxygen mixed with freshly divided carbon, is used in place of dynamite in
coal mining.
 Ozone(O3) It protects the life on the earth by not allowing UV rays to reach the
Earth. The common refrigerants, chlorofluorocarbons deplete this ozone layer.
 Its bleaching action is due to its oxidizing action.
 Ozone is also used as a germicide and disinfectant, for sterilizing water.

4. Phosphorus (P):
 It is highly reactive non-metal, so it occurs only in combined state.
 Phosphorus is an essential constituent of bones, teeth, blood and nerve tissues.
Bone ash contains about 80% of phosphorus.

5. Sulphur (S):
 It occurs in free state in volcanic region.
 Rhombic sulphur is the most stable form at ordinary temperature and all other
forms gradually change into this form.

Compounds of Sulphur
 Sulphuric acid is also known as oil of vitriol or king of chemicals. It has a great affinity for
water and thus it acts as a powerful dehydrating agent. Corrosive action of sulphuric is due
to its dehydrating action.
 Hypo (Sodium thiosulphate) It is mainly used in photography as a fixing agent. It is used to
remove undecomposed silver halide on photographic paper or film.

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 6. Halogens:
Halogens are highly reactive elements and therefore, they do not exist in free state but
exist only in combined form. Halogens have highest electron affinity so they act as
strong oxidizing agent. Their oxidizing power decreases from fluorine to iodine.
 Chlorine:
 Chlorine was first discovered by Scheele (1774)
 Chlorine is used as a germicide, disinfectant, oxidizing agent, bleaching agent in
paper and textile industry.
 Chlorine being an acidic gas turns moist blue litmus paper to red and then bleaches
it.

 Iodine (I2)
 Chile saltpeter or caliche contains iodine as sodium iodate (5-20%).
 It turns starch solution blue. Solution of KI/ I2, is used in the treatment of goiter. It is
used as an antiseptic as tincture of iodine.

7. Noble Gases
 Helium (H(e), Neon (N(e), Argon (Ar), Krypton (Kr), Xenon (X(e) and Radon (Rn)
are known as inert gases or noble gases or rare gases.
 These elements have completely filled valence shell.
 It atmosphere, argon is most abundant noble gas but in universe, helium is most
abundant gas.
 Natural gas in the most important source of helium.
 The mixture of helium and oxygen is used for artificial breathing of asthama
patients.
 85% helium + 15% hydrogen is used for filling in balloons and airships.
 Mixture of helium and oxygen is used for respiration by sea divers.
 Helium is used as pressuring agent in rockets to expel liquid oxygen and liquid
hydrogen.
 Xe is also known as stranger gas and Xe-Kr is used in high intensity photographic
flash tubes.
 Radon is used in the preparation of ointment for the treatment of cancer.

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 Polymerization
 Polymers are defined as high molecular mass macromolecules, which consist of repeating
structural units derived from the corresponding monomers.
 Polymers occur in nature also. Cotton, for example, is a polymer called cellulose. Cellulose
is made up of a large number of glucose units.
 On the basis of intermolecular forces Polymers are classified as:
1) Elastomers- rubber, buna-S, buna-N, neoprene etc
2) Fibres - polyamides (nylon 6, 6), polyesters (Terylene),etc.
3) Thermoplastic polymers - Such plastic which gets deformed easily on heating and
can be bent easily are known as thermoplastics. Polythene and PVC, Polythene,
Polystyrene, Polyvinyls, etc.
4) Thermosetting Polymers - some plastics which when moulded once, can not be
softened by heating. These are called thermosetting plastics.eg: bakelite, melamine
etc.

 Few important polymers are:

A. Polythene:
 Low density polythene - polymerisation of ethene under high pressure in the
presence of traces of dioxygen or a peroxide initiator (catalyst).
 High density Polythene - polymerisation of ethene in the presence of a
catalyst such as triethylaluminium and titanium tetrachloride (Ziegler-Natta
catalyst).
B. Polytetrafluoroethene (Teflon)- Teflon is manufactured by heating
tetrafluoroethene with a free radical or persulphate catalyst at high pressures.

C. Polyacrylonitrile - polymer of acrylonitrile in presence of a peroxide catalyst.

Condensation Polymerisation
 Polyamides - possess amide linkages
 Nylon 6, 6 - prepared by the condensation polymerization of
hexamethylenediamine with adipic acid under high pressure and at high
temperature
 Nylon 6- obtained by heating caprolactum with water at a high temperature.

 Polyesters- polycondensation products of dicarboxylic acids and diols. Polyester is

another synthetic fibre. Fabric made from this fibre does not get wrinkled easily. It remains
crisp and is easy to wash. So, it is quite suitable for making dress material.

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 Eg: Terylene is the best known example of polyesters. It is prepared by ethylene glycol and
terephthalic acid. It can be drawn into very fine fibres that can be woven like any other
yarn.

 Phenol - formaldehyde polymer (Bakelite and related polymers)

Prepared by the condensation reaction of phenol with formaldehyde in the presence of
either an acid or a base catalyst.
The initial product could be a linear product - Novolac used in paints. Novolac on heating
with formaldehyde undergoes cross linking to form an infusible solid mass called bakelite. It
is used for making combs, phonograph records, electrical switches and handles of various
utensils. Eg. Melamine - Melamine formaldehyde polymer is formed by the condensation
polymerisation of melamine and formaldehyde. Melamine is a versatile material. It resists
fire and can tolerate heat better than other plastics. It is used for making floor tiles,
kitchenware and fabrics which resist fire. It is used in the manufacture of unbreakable
crockery.

Copolymerisation
 Natural rubber - Natural rubber may be considered as a linear polymer of isoprene
(2-methyl-1, 3-butadien(e) and is also called as cis-1, 4-polyisoprene.

 Vulcanisation of rubber-This process consists of heating a mixture of raw rubber

with sulphur and an appropriate additive at a temperature range between 373 K to 415 K
so that rubber gets stiffened.

Synthetic Rubbers
1) Neoprene - by the free radical polymerisation of chloroprene.

2) Rayon - rayon or artificial silk. Although rayon is obtained from a natural source, wood
pulp, yet it is a man-made fibre.

3) Nylon - Nylon is also used for making parachutes and ropes for rock climbing. A nylon
thread is actually stronger than a steel wire.

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 PYQs
1. ________ fibre is used in making bulletproof vests. ------- Kevlar
2. What is the full form of PVC? ----- Polyvinyl Chloride
3. Which fibre is used for making bristles of brushes. ----- Nylon-66
4. ________ is a Synthetic rubber? ------ Neoprene
5. Milbemycin is used in the eradication of _________ ------ agricultural pests
6. Barbituric acid and its derivatives are well known as ------ Tranquilizers
7. The helical structure of protein is stabilized by------ Hydrogen bonds
8. The sugar which is not a disaccharide ----- Galactose
9. Which one of the following is non-reducing sugar? ------ Sucrose
10. Which of the following is a biodegradable polymer? ----- Cellulose
11. Plastic bottles are made of a polymer called PET. The expanded form of PET is-------
Polyethylene terephthalate
12. In chemistry, soap is a salt of a _______ ------- Fatty acid
13. The brand name Teflon represents which polymer? ------- Polytetrafluoroethylene
14. Which is widely used in the plastic industry for manufacturing Bakelite?----- Phenol
15. Which is used as raw material for the manufacture of rayon?---- Cellulose
16. Which of the following is related to the discovery of Nylon?------ Dr. Wallace H.
Carothers
17. PVC is obtained by the polymerization of ------- Vinyl chloride
18. Polyethene is formed by - ------- Ethylene
19. Which one of the following is a Natural Polymer? -------- Cellulose
20. Natural rubber is a polymer of ------ Isoprene
21. Bakelite is a polymer of Phenol and ------ Formaldehyde
22. Which one of the following is a synthetic polymer? ------ Polystyrene
23. Which among the following is a petroleum wax? ----- Paraffin Wax
24. Wax used for making candles is chemically a mixture of ------ Aliphatic
Hydrocarbons
25. Glycogen, Cellulose and starch are the polymers of ------ Glucose
26. Which of the following element is used for vulcanisation of rubber? ------ Sulphur
27. The process of heating of Rubber with sulphur to increase its quality is known as ------
Vulcanisation.

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28. Petroleum is a Mixture of ----- Hydrocarbons
29. Which of the following could be used as fuel in propellant of Rockets? ----------
Liquid Hydrogen + Liquid oxygen
30. Glycol is added to aviation gasoline because ------ it Prevents freezing of petrol
31. Aqueous Hydrolysis of sucrose formed ----- Glucose and Fructose
32. Which of the following gas is used to destroy the microbes? ---- Chlorine
33. Substance which are used as a food preservative --- Sodium salts of benzoic acids
34. Which gas is used as a disinfectant in drinking water? ----- Chlorine
35. 'Saponification' is a process by which ---- Soap is prepared
36. What is the by Product obtained in soap industry? ---- Glycerol
37. The process involved in the making of soap is ------ Saponification
38. Glycol is used to manufacture which of the following? ----- Terylene
39. Which of the following is used as non-stick coating for cooking utensils? --- Teflon
40. The antiseptic compound present in Dettol is ---- Enloroxylenol
41. KMnO4 can be used as -------- Disinfectant
42. Tincture of iodine is a solution of Iodine in ----- Potassium iodide
43. Glucose is a type of ----- Hexose Sugar
44. The class of drugs used for the treatment of stress is ------- Tranquilizer
45. The drug which lowers anxiety and provide peace ------- Tranquilizer
46. The branch of medicine involving synthetic chemical compounds is ----- Allopathic
47. Zinc Phosphide is commonly used as -------- Rodenticide
48. Terylene is a condensation polymer of glycol and which acid?---- Terephthalic acid
49. Which of the following fibres is considered the strongest natural fibre? ----- Silk
50. Which of the following is a natural polymer? ----- Starch
51. Synthetic detergents are prepared from ------ Hydrocarbons of petroleum
52. Which of the following gas is used in bulb? ----- Argon
53. Chlorine gas a major component of which of is the following? ----- Tear gas
54. In which of the following silicon is not used? ----- Ink pen
55. Bleaching action of Chlorine is due to which reaction? ----- Oxidation
56. Which of the following is used for ripening of fruits? ----- Ethylene
57. What is the major component of Gobar Gas? ------ Methane
58. Rock Salt contains which mineral? ---- Sodium

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59. Which of the following elements are commonly found in most fertilizers? --------
Nitrogen, Potassium, Phosphorous
60. Which of the following metal shown by its symbol is generally used for making
filaments of bulb? ---- W
61. In which industry Potassium nitrate is used commercially?---- Fire cracker
manufacturing.
62. Which among the following is used to treat Indigestion? ---- Antacid
63. Which base is present in soap? ----- Sodium hydroxide
64. Which fibre is also called as artificial silk? ---- Rayon
65. Fire extinguishers emit which gas? ----- Carbon dioxide
66. _________ is obtained by evaporation of sea. ---- Salt
67. What is a Vermicompost? ----- Organic fertilizer
68. What is dry ice? ----- Solid Carbon dioxide
69. PET is a very familiar form of ________ is used for making bottles.---- Polyester
70. Which acid is released when an ant bites? ----- Formic acid
71. The rubbing surface of a matchbox has powdered glass and a little red ______ ------
Phosphorous
72. A _________ thread is actually stronger than a steel wire. ------ Nylon
73. Fabric made from _______ does not get wrinkled easily. ----- Polyester

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 Periodic Table
 Newlands’ law of octaves
 Law of octaves, in chemistry, the generalization made by the English chemist
J.A.R. Newlands in 1865 that, if the chemical elements are arranged according
to increasing atomic weight, those with similar physical and chemical properties
occur after each interval of seven elements. In 1864, Newlands made an
attempt to classify elements. There are seven musical notes in music. Every
eighth note is similar to the first one and it is the first note of the nest scale.
Similarly, Newland stated that the eighth element starting from a given one is a
kind of repetition of the first like the eighth notes of an octave of music. So he
called this relationship as the Law of octaves.
 In Newland’s table of elements lithium, sodium and potassium occupied places
near each other.

 Fluorine and chlorine or oxygen and sulphur were placed near each other.

 Note: This classification worked well with the elements with small atomic weights
but failed in the case of elements with large atomic weights.

 Mendeleev’s table
 Mendeleev published in 1869, using atomic weight to organize the elements, information
determinable to fair precision in his time. Atomic weight worked well enough to allow
Mendeleev to accurately predict the properties of missing elements.
 The atomic number is the absolute definition of an element and gives a factual basis for the
ordering of the periodic table.
 Mendeleev realized that the physical and chemical properties of elements were related to
their atomic mass in a ‘periodic’ way, and arranged them so that groups of elements with
similar properties fell into vertical columns in his table. Modern-day periodic tables are
expanded beyond Mendeleev’s initial 63 elements.

 Modern Periodic Table

1) VALENCY: Valency may be defined as “the combining capacity of the atom of

an element with atoms of other elements in order to acquire the stable
configuration (i.e. 8 electrons in the valence shell. In some special cases it is 2
electrons).”

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2) ATOMIC SIZE:

 It refers to the distance between the centre of the nucleus of an isolated atom to its
outermost shell containing electrons.
 The atomic radius decreases on moving from left to right along a period. This is due
to an increase in nuclear charge which tends to pull the electrons closer to the
nucleus and reduces the size of the atom.
 In a group, atomic size increases from top to bottom due to the increase in a
number of shells.

3) METALLIC AND NON-METALLIC PROPERTIES

 In a period from left to right metallic nature decreases while non-metallic character
increases.
 In a group metallic character increases from top to bottom while non-metallic
character decrease.

4) ELECTRONEGATIVITY: The relative tendency of an atom to attract the shared

pair of electrons towards itself is called electronegativity. In a period from left to
right, the value of electronegativity increases while in a group from top to bottom
the value of electronegativity decreases.

5) IONIZATION ENERGY
 The ionization energy (IE) is the amount of energy required to remove the most
loosely bound electron, the valence electron, of an isolated gaseous atom to form
a cation.
 In a period from left to right, the value of ionization energy increases while in a
group from top to bottom the value of ionization energy decreases.

6) ELECTRON AFFINITY: The electron affinity of an atom or molecule is defined as

the amount of energy released or spent when an electron is added to a neutral
atom or molecule in the gaseous state to form a negative ion. In a period from left
to right, the value of electron affinity increases while in a group from top to bottom
the value of electron affinity decreases.

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 Modern Periodic Table

List periodic table elements

 Group 1 (Alkali Metals)
The alkali metals are the series of elements in Group 1 of the periodic table. The
series consists of the elements lithium (Li), sodium (Na), potassium (K), rubidium (Rb),
caesium (Cs), and francium (Fr).

TRICK: LiNa ki Rubi Se Friendship ho gyi.

Lithium(Li) + Sodium(Na) Pottasium(k) Rubidium(Rb) caesium (Cs) francium (Fr).

Properties:

 The alkali metals are silver-coloured (caesium has a golden tinge), soft, low-density
metals.

 These elements all have one valence electron which is easily lost to form an ion with
a single positive charge.

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  They have the lowest ionization energies in their respective periods. This makes
them very reactive and they are the most active metals.

 Due to their activity, they occur naturally in ionic compounds, not in their elemental
state.

 The alkali metals react readily with halogens to form ionic salts, such as table salt,
sodium chloride (NaCl).

 They react with water to liberate hydrogen gas.

Alkali metal + water → Alkali metal hydroxide + hydrogen

 Group 2 (Alkaline Earth Metals)

Group 2 of Periodic Table the series consists of the elements beryllium (Be),
magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra).

TRICK:
Ber Mehnge kr ke Sarkar Bahut Roi

beryllium(Be) magnesium(Mg) calcium(Ca) strontium(Sr) barium(Ba) radium(Ra)

Properties for Group 2 of Periodic Table elements:

 The alkaline earth metals are silvery coloured, soft, low-density metals, though are
a bit harder than the alkali metals.
 These elements all have two valence electrons and tend to lose both to form ions
with a two-plus charge.
 Beryllium is the least metallic element in the group and tends to form covalent
bonds in its compounds.
 They react readily with halogens to form ionic salts and can react slowly with water.

 Group 13 (Boron Group)

Group 13 of the Periodic Table consists of the elements boron (B), aluminium (Al),
gallium (Ga), indium (In), thallium (Tl).
TRICK:
Baba Ali Gya India Thaila Lekar

Boron(B) Aluminium(Al) Gallium(Ga) Indium(In) Thallium(Tl)

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 Properties for Group 13 of Periodic Table elements

 In this group, we begin to see the changeover toward the non-metallic character.
First appearing at the top of the group. Boron is a metalloid, it has characteristics
intermediate between metals and non-metals, and the rest of the group are
metals.

 These elements are characterized by having three valence electrons. The metals
can lose all three electrons to form ions with a three-plus charge in ionic
compounds.

 Aluminium is the third most abundant element in the earth’s crust (7.4 percent), and
is widely used in packaging materials. Aluminium is an active metal, but the stable
oxide forms a protective coating over the metal making it resistant to corrosion.

 Group 14 (Carbon Group)

Group 14 of the Periodic Table consists of the elements carbon (C), silicon (Si),
germanium (Ge), tin (Sn), & lead (Pb)
TRICK:
Kl Sita Gita Sangita Punjab Gyi

Carbon(C) Silicon(Si) Germanium(Ge) Tin(Sn) Lead(Pb)

Properties of Group 14 of Periodic Table elements

 This group has a mixed type of element with the non-metal carbon, two metalloids,
and two metals. The common characteristic is four valence electrons.

 The two metals, tin and lead, are unreactive metals and both can form ions with a
two-plus or a four-plus charge in ionic compounds.

 Carbon forms four covalent bonds in compounds rather than form monatomic ions.
In the elemental state, it has several forms, the most known of which are graphite
and diamond.

 Silicon in some respects is similar to carbon in that it forms four covalent bonds, but
it does not form a wide range of compounds. Silicon is the second most abundant
element in the earth’s crust (25.7 percent) and we are surrounded by silicon-
containing materials: bricks, pottery, porcelain, lubricants, sealants, computer chips,
and solar cells.

 The simplest oxide, silicon dioxide (SiO2) or silica, is a component of many rocks
and minerals.

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  Group 15 (Nitrogen Group)
The Nitrogen group is the series of elements in group 15 (formerly Group V) of the
periodic table. It consists of the elements Nitrogen (N), Phosphorus (P), Arsenic (As),
Antimony (Sb), and Bismuth (Bi) The collective name pnictogens is also sometimes
used for elements of this group.
TRICK:
Newspaper Aaj Sb Bikega

Nitrogen(N) Phosphorus(P) Arsenic(As) Antimony(Sb) Bismuth (Bi)

Properties for Group 15 of Periodic Table elements

 These elements all have five valence electrons. Nitrogen and Phosphorous are non-
metals. They can gain three electrons to form fairly unstable ions with a three minus
charge, the nitride and phosphide ions.

 Nitrogen, as a diatomic molecule is the major constituent of air and both elements
are essential for life. Nitrogen comprises about 3 percent of the weight of the
human body and phosphorous about 1.2 percent. Commercially, these elements
are important for fertilizers. Arsenic and Antimony are metalloids, and bismuth is the
only metal in the group. Bismuth can lose three electrons to form an ion with a
three-plus charge.

 Bismuth is also the heaviest completely stable element that does not decay
radioactively to other simpler elements.
 Group 16 (Chalcogens)
They are oxygen (O), Sulfur (S), selenium (Se), tellurium (Te), the radioactive
polonium (Po), and the synthetic ununhexium (Uuh).
TRICK:
Oo Sanam Se Tere Pore Hai Hum

Oxygen(O) Sulphur(S) Selenium(Se) Tellurium(Te) polonium(Po) ununhexium (Uuh)

Properties for Group 16 of Periodic Table elements

 This group has six valence electrons. Oxygen and sulphur are non-metals; their
elemental form is molecular, and they can gain two electrons to form ions with a
two minus charge.

 Sulphur has probably the most allotropes of any element, though the most common
and stable form is the yellow crystals of S8 molecules.

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 Group 17 (Halogens)
The halogens are the elements in Group 17 (formerly Group VII or VIIa) of the
periodic table. They are fluorine (F), chlorine (Cl), bromine (Br), iodine (I), astatine
(At).
TRICK:
Fakire kol Barfi aayi Aate vali

Fluorine(F) Chlorine(Cl) Bromine(Br) Iodine(I) Astatine (At)

Properties for Group 17 of Periodic Table elements

 These elements all have seven valence electrons.

 This group is the first one to consist of entirely non-metals.
 They exist as diatomic molecules in their natural state
 Fluorine and chlorine exist as gases at room temperature, bromine as a liquid, and
iodine as a solid.

 They requires one more electron to fill their outer electron shells, and so have a
tendency to gain one electron to form singly-charged negative ions. These
negative ions are referred to as halide ions, and salts containing these ions are
known as halides.

 Halogens are highly reactive, and as such can be harmful or lethal to biological
organisms in sufficient quantities.

 Fluorine is the most reactive and the reactivity declines as we go down the group.
 Chlorine and iodine are both used as disinfectants.
 In their elemental state, the halogens are oxidizing agents and are used in
bleaches.

 Chlorine is the active ingredient of most fabric bleaches and is used in the
production of most paper products

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 Group 18 (Noble Gases)
The noble gases are the chemical elements in group 18 (formerly group VIII) of the
periodic table. They are helium, neon, argon, krypton, xenon, and radon. They are
sometimes called inert gases or rare gases. The name ‘noble gases’ is an allusion to
the similarly unreactive Noble metals, so-called due to their preciousness, resistance
to corrosion and long association with the aristocracy.
TRICK:
Harbhajan Ne Ar Kr Zero Run Banaye

Helium(He) Neon(Ne) Argon(Ar) Krypton(Kr) Xenon(Xe) Radon(Rn)

Properties for Group 18 of Periodic Table elements

 The noble gasses are all non-metals and are characterized by having completely
filled shells of electrons.

 Physically they exist as monatomic gases at room temperature, even those with
larger atomic masses. This is because they have very weak inter-atomic forces of
attraction, and consequently very low melting points and boiling points.

 Krypton and Xenon are the only noble gasses that form any compounds at all.
These elements can do this because they have the potential to form an expanded
octet by accepting electrons in an empty d subshell.

Applications of Noble gases

1. Helium
 Swimmers can carry Helium + Oxygen in their oxygen tank while going into the sea.
 Helium and Oxygen can use to treat Asthma’s Patients.
 Helium can be filled in the Balloons.
 Helium Gas is used to preserve Food.

2. Neon
 It is used for Signals on Railway Tracks, Roads, etc.
 Use Neon Bulbs in Decorative Items and Tube Lights.

3. Argon
 It is used in Arc Welding.
 It is used in Fluorescent Tubes.

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4. Kripton
 It is used in Electric Discharge Tubes.

5. Xenon
 It is used in Electric Discharge Tubes.
 it helps to formation of large no. of Compounds.
 It is used in Bubble Chamber for the identification of Gamma & Neutrons.

6. Redon
 It is used in Cancer Treatments.

Applications of Halogens
1. Fluorine
 Fluorine is the most Electronegative Element in the Periodic Table.
 It is the Strong Oxidising in Nature.
 Its reaction is very Furious and Exothermic in Nature.
 It helps in writing at glass.
 It is used in the manufacturing of Chloro Fluoro Carbons(CFCs) & Teflon.
 Dichloro, Difluoro Methane used in the manufacturing of Freon that are used
in the Refrigrators.

2. Chlorine
 It is used in the Oxidation.
 It is used in the manufacturing of Bleaching Powder.
 It is used as a Bleaching Agent.
 It is used to kill Bacteria in Water.
 It is used in the manufacturing of DDT, Chloroform & Phosphine Gas.

3. Bromine
 It is bad smell gas in nature.
 It is used in Dying Clothes.
 It is used as a Bleaching Agent.
 It is used in the manufacturing of Tear Gas & Chloropicrin Gas.
 It is used in the manufacturing of Medicines.

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  AgBr is used in the negatives of PhotoGraphy.

4. Iodine
 It is used in Tincture Iodine
 It is used in the manufacturing of Iodex & Iodoform.
 It is used in the manufacturing of Explosives.
 It is also used as Germicides & Antipirates.

5. Astatine
 It is Radioactive in Nature.

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 Periodic table PYQs
1. Who proposed the Modern Periodic Table? ----- Mendeleev
2. Total number of Inner Transition Elements. Are ----- 28
3. The Modern Periodic table consists of 18 groups and 7 periods. What is the atomic
number of the element placed in the 2nd group and the 4th period? ----- 20
4. In the Modern Periodic table one of the following does not have appropriate
position.----- Inner-transition elements
5. The Modern Periodic Table consists of 18 groups and 7 periods. What is the atomic
number of the element placed in the 1st group and the 4th period?------ 19
6. The electronegativity of the following elements increases in the order: ---- Si, P, C, N
7. The correct order of electronegativity of F, N, O and P is------- F>O>N >P
8. In the periodic table, the element with atomic number 38 belongs to: ---- Period V
and group II
9. Which of the following is not a representative element? ----- Fe
10. The Modern Periodic Table consists of 18 groups and 7 periods. What is the atomic
number of the element placed in the 4th group and the 4th period? ----- 22
11. The modern periodic table consists of 18 groups and 7 periods. What is the atomic
number of the element placed in the 3rd group and the 4th period? ---- 21
12. Electronegativity values of Fe, Fe2+ and Fe3+ are in the order: ----- Fe3+ > Fe2+ > Fe
13. Which among the following elements has low highest electronegativity?---- Arsenic
14. Element with Highest Ionization energy is ---- Helium
15. Nitrogen has higher ionization energy than oxygen because in Nitrogen there is ----
Half Filled Stable configuration in 2p orbital
16. Ionization Potential for inert gas is ---- High
17. Which of the following atoms has the lowest ionisation potential? ----- Cs
18. What is the common characteristic of the elements of the same group in the
periodic table? ----- Electrons in outer most shell
19. Who amongst the following gave the 'Periodic Law'? ---- Dmitri Mendeleev
20. Rn' is chemical symbol of which element? ---- Radon
21. What is the chemical symbol of 'Iron'? ----- Fe
22. In a periodic table, while moving from left to right in a period, number of remains
same.--- Shells

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 CHEMICAL REACTIONS AND EQUATION
 Physical Change: The change that only affect physical properties, but the
chemical compositions remains unchanged, are called physical change.
 These can be reversed by changing the conditions of temperature and
pressure, boiling, cutting of trees, dissolving common salt in water burning of
wax.

 Chemical Change: The change which affect the composition as well as

chemical properties of matter and result in the formation of a new substance is
called a chemical change.
 Chemical changes are generally irreversible. Some examples of chemical
changes are burning of candle (gases), photosynthesis, ripening of fruits,
electrolysis of water.
 A chemical reaction involves bond breaking or bond formation between any
two atoms to produce new substances.

Laws of Chemical Combination - There are three laws of Chemical combination.

1. Law of conservation of mass: This law was stated by Lavoisier in 1744. It states
that "In all physical and chemical changes, the total mass of reactants is equal to
total mass of products."

2. Law of constant proportions (or constant composition): This law was first
stated by Proust in 1797. According to the law "a chemical compound is always
found to be made up of the same elements combined together in the same
proportions by weight" e.g. the ratio of hydrogen and oxygen in pure water is
always 1 : 8 by weight. This law is also called law of definite proportions.

3. Law of multiple proportions: This law was given by John Dalton (1803) and
states that "when two elements combine to form two or more compounds, the
different mass of one of the elements and the fixed mass of the one with which it
combines always form a whole number ratio". This law explains the concept of
formation of more than one compound by two elements.

Types of Chemical Reactions.

 Exothermic Reactions: Reactions in which heat is released along with the
formation of products, are called exothermic reactions.

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 Endothermic Reactions: Burning of fuel is an example of exothermic
reaction. Reactions in which heat is absorbed, are known as endothermic
reactions.

Oxidation
 Oxidation is removal of electrons.
 Oxidation means: addition of oxygen and removal of hydrogen.

Reduction
 Reduction is the addition of electrons.
 Reductions means: Removal of oxygen and Addition of hydrogen.

Oxidizing agent
 The substance that causes oxidation is called the oxidizing agent.
 Acceptors of electrons.
 It is a substance which removes the electron from an atom.
 It brings about oxidation.

Reducing agent
 The substance that causes reduction is called the reducing agent.
 Donors of electrons.
 It is a substance which adds electrons to an atom.
 It brings about reduction.

 REDOX REACTION: A reaction which involves oxidation and reduction

occurring simultaneously together are called redox reaction. Photosynthesis in
plants digestion of food in animals; dry and wet batteries and corrosion of metals
are diverse examples of oxidation and reduction reactions.

Electrolysis
 Electrolysis is carried out in an electrolytic cell.
 A simple electrolytic cell consists of two copper strips dipping in an aqueous solution
of copper sulphate.
 On applying DC voltage to the two electrodes, copper metal is deposited on
cathode and copper is dissolved at anode.

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  Used In the purification of impure metals.
 In the extraction of metals The blocks used in typing industries are prepared by
electrolysis.
 Steel is coated with zinc metal during the process of galvanization.

Batteries
These convert chemical energy into electrical energy. Mainly two types of batteries are
used, i.e. primary and secondary.

Primary Batteries
In the primary batteries, reaction occurs only once and after a period of time
battery becomes dead.

 Dry Cell or Leclanche Cell: It consists of a zinc container that acts as

anode and the cathode is a carbon (graphite) rod surrounded by powdered
manganese dioxide and carbon.
A moist paste of ammonium chloride (NH,CI) and zinc chloride (ZnCl2) is used as an
electrolyte. Dry cell is commonly used in our transistors and clocks.

 Mercury Cell: It is commonly used in low current devices such as hearing aids,
watches etc.
The electrolyte is a past of potassium hydroxide (KOH) and zinc oxide (ZnO).

Secondary Batteries
 Lead Storage Battery
It consists of a lead as anode and a grid of lead packed with lead dioxide (PbO2)
as cathode.
A 38% solution of sulphuric acid is used as an electrolyte. On charging the battery,
the reaction is reversed and lead sulphate gives lead on anode and cathode is
converted into lead dioxide respectively.

 Nickel Cadmium Cell

It has longer life that the lead storage cell. It consists of a cadmium as anode and
nickel dioxide as cathode. The electrolyte is a potassium hydroxide (KOH) solution.

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 Fuel Cells
Fuel cells convert energy from the combustion of fuels such as hydrogen, carbon
monoxide, methane directly into electrical energy
A fuel cell with hydrogen and oxygen has been used for electric power in Apollo
Space Programme.

Corrosion
 When iron is exposed to moist air for a long period of time, its surface acquires a
coating of brown flaky substance called rust.
 Rust is mainly hydrated iron (III) oxide (Fe2O3.xH2O).
 In corrosion, a metal is oxidized by the loss of electrons to oxygen and form oxide.
 The rusting of iron can be prevented by painting, oiling and greasing, galvanizing
(by coating iron objects with zin(c), chrome plating etc.

Catalysis
 A catalyst is a substance which alter the rate of reaction.
 The catalyst itself does not alter during the reaction.
 The phenomena in which the rate of reaction is altered by the presence of a
substance (catalyst) is known as catalysis.
 Catalysts are specific in their action.
 A catalyst does not change the equilibrium state of a reversible reaction, only
brings it quickly.
 The main function of a catalyst in a reaction is to decrease the activation energy.

Applications of Catalysts in Industrial Processes

 Haber process for ammonia-- Iron is used as a catalyst and molybdenum is used as
a promoter of catalyst iron.
 Contact process for Sulphuric acid--- Vanadium pentoxide is used as a catalyst.
 Ostwald process for Nitric acid---- Platinum gauze is used as a catalyst.
 Deacon process for Chlorine ----- Cupric chloride is used as a catalyst.
 Synthesis of petrol ------ Nickel, iron, cobalt and alumina is used as a catalyst.

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 PYQs
1. What happens in an Oxidation reaction? ---- Electrons are lost
2. Which among the following is not a characteristic of Oxidation reaction? ----- It
involves addition of hydrogen
3. Cooking oil is converted into vegetable ghee by the process of ------ Hydrogenation
4. Which of the following causes Rusting of iron? ----- Oxidation & Chemical reaction
with oxygen
5. Rusting of Iron is ----- Due to oxidation
6. The rusting of iron metal in air needs both ----- Oxygen and Moisture
7. What is Rusting of Iron? ----- Chemical Change
8. Iron rusts quickly in ------- Sea water
9. The liberation of oxygen during photosynthesis is due to ----- Photolysis of water
10. When Hydrogen combusts in air, then formed ----- Water
11. Browning of paper in old books is caused by ------ Oxidation of cellulose
12. Nitrogen forms a variety of compounds in all oxidation states ranging from ---- -3 to
+5
13. The rusting of iron ----- Increases its weight
14. The coating of thin layer of zinc on steel or iron object is known as ---- Galvanising
15. The metal, used to galvanise iron to protect it from rusting is ---- Zinc
16. Which metal does not undergo corrosion due to the formation of Oxide layer? ---
Aluminium
17. Carbon dioxide is ----- An Oxidising agent
18. The reactions in which oxidation and reduction occur simultaneously are called
_______ ------ Redox reactions
19. Rusting is ___________ ------- Oxidation
20. Process of gaining electrons is known as ----- Reduction
21. Process of loosing electrons is known as ----- Oxidation
22. What is the process of rust forming on iron called? ------ Rusting
23. The process of deposition of a layer of zinc on iron is called-------- Galvanisation
24. The process of deposition of a layer of any desired metal on another material by
means of electricity is called ___________ ----- Electroplating
25. Brownish film formed on iron when left in open is called? __________ Rust

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26. The metal chiefly used for galvanising iron is------ Zinc
27. The process of deposition of a layer of Zinc over water pipes for being protected
from rusting is known as ---- Galvanization
28. Which metal is used to Galvanize iron? ------ Zinc
29. Which of the following is not favourable prevent iron from rusting? ----- Annealing
30. Potassium Permanganate is used for purifying drinking water, because _______ -----
It is an oxidising agent

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 Chemical Bonding
 Chemical Bonding
Constituents (atoms, molecules or ions) of different elements except noble gases, do not
have complete octet so they combine with other constituent atoms by chemical bonds to
achieve complete (stable) octet. The process of their combination is called chemical
bonding. Chemical bonding depends upon the valency of atoms.

Types of Chemical Bond

They are divided in the following types depending upon the mode electron transferred or shared
electrons or forces of attraction

 Electrovalent or ionic bond

 Covalent bond
 Coordinate or dative covalent bond
 Van der Waal's forces
 Hydrogen bond

 Electrovalent Bond
 The bond formed by the transfer of electrons from one atom to another is called
electrovalent bond and the compound is called electrovalent compound or ionic
compound.
 These bonds are formed between metals and non-metals.
 These conduct electricity when dissolved in water and also soluble in water. These
are insoluble in organic solvents like alcohol etc.

Some Electrovalent Compounds (Ionic Compounds)

Name Formula Ions Present

Aluminium Oxide Al2O3 Al3+ & O2-
Ammonium Chloride NH4Cl NH4+ & Cl-
Calcium Chloride CaCl2 Ca2+ & Cl-

 Covalent Bond
 The bond is formed by the sharing of electrons between two atoms of same (or
different) elements, is called covalent bond.
 Covalent bond may be single, double or triple depends upon the number of sharing
pairs of electrons.

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  Covalent compounds are usually liquids or gases having low melting point and
boiling point. These do not conduct electricity and are insoluble in water but dissolve
in organic solvent.

Some Covalent Compounds

Name Formula Element's part

Alcohol (Ethanol) C₂H₂OH C, H and O

Ammonia NH3 N and H

Acetylene (Ethyne) C₂H₂ Cand H

 Coordinate or Dative Bond

 The bond is formed by one sided sharing of one pair of electrons between two
atoms. The necessary condition for the formation of coordinate bond is that octet of
one atom should be complete, having at least one lone pair of electrons and other
atom should have a deficiency of at least one pair of electrons.
 The atom having complete octet which provides the electron pair for sharing, is
known as donor.
 The other atom which accept the electron pair, is called the acceptor.

Bonding between A and B is predominantly

 lonic if there is large difference in electronegativity.
 Covalent if both A and B have approximately same value of
electronegativity.
 Coordinate if lone pair on A (or (B) is donated to electron deficient B or A.

Compounds Containing Ionic and Covalent Bonds

Name Formula
Potassium cyanide KCN
Sodium hydroxide NaOH

Calcium carbonate CaCO3

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 Compounds Containing Covalent and Coordinate Bonds
Name Formula
Carbon monoxide CO
Ozone O3
Dinitrogen oxide N₂O
Dinitrogen trioxide N₂O3
Nitric acid HNO3

Compounds Containing Electrovalent, Covalent and Coordinate Bonds

Name Formula
Ammonium chloride NH4Cl
Ammonium bromide NH4Br

 Hydrogen Bond
 The electrostatic force of attraction between hydrogen atom (which is covalently
bonded to a highly electronegative atom) and any other electronegative atom
which is present in the same or different molecules, is known as hydrogen bond.
 It is maximum in the solid state and minimum in the gaseous state.
 Intermolecular H-bonding (e.g. HF, water (H2O) molecule) It occurs between
different molecules of a compound and results in increasing solubility in water and
high boiling point.

 Intramolecular H-bonding
It occurs within different parts of a same molecule and results in decreasing solubility in
water and low boiling point. (e.g. o-nitrophenol)

 Van der Waals' Forces

The ability of geckos (lizard) which can hang on a glass surface using only one toe to climb
on sheer surfaces had been attributed to the Van der Waals forces between these surfaces
and their foot-pads.

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 ATMOSPHERIC POLLUTION
 Atmospheric pollution
 The substance which causes pollution is known as pollutant.
 Pollutants are of two types

 Primary pollutants: persist in the environment in the form, they are produced, e.g.
sulphur dioxide (SO2), nitrogen dioxide (NO₂) etc.

 Secondary pollutants are the products of reaction of primary pollutants, e.g.

peroxyacetye nitrate (PAN), ozone(O3) aldehyde etc.

Major Gaseous Air Pollutants

Major gaseous air pollutants are oxides of sulphur, nitrogen, carbon and hydrocarbons.

 Sulphur dioxide (SO2)

 It is highly toxic for both animals and plants, bronchitis, asthma, emphysema.
 It also causes eye and throat irritation and breathlessness.
 Sulphur dioxide reduces the rate of formation of chloroplast and thus, causes
chlorosis. SO2 is highly corrosive and damage buildings, marbles (Taj Mahal) and
textiles.
 SO2 is oxidized to SO3 which reacts with water to give H₂SO4 . H₂SO4 remains
suspended in the air as droplets or come down in the form of acid rain.

 Oxides of nitrogen
 Among the oxides of nitrogen, nitric oxide (NO), a colourless, odourless gas and
nitrogen dioxide (NO2), a brown gas with pungent odour act as tropospheric
pollutants.
 NO2 is highly toxic for living tissues causes leaf fall. It is a corrosive oxide and helps in
the formation of smog.
 In the presence of oxygen, NO2 reacts with water or moisture and produces nitric
acid (HNO3) which is an important factor for making acid rain.

 Carbon monoxide (CO)

 From more stable carboxyhaemoglobin complex with haemoglobin due to which
the delivery of oxygen to the organs and tissues is blocked.

 Hydrocarbons
Out of the hydrocarbons, methane (CH4)is the most abundant hydrocarbon pollutant.
Higher concentrations of hydrocarbons given carcinogenic effect, i.e. are cancer

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 producing. They cause ageing of plants, breakdown of plant tissues and shedding of
leaves.

Consequences of Atmospheric Pollution

 Green House Effect: Green house gases such as carbon dioxide, methane and water
vapours trap the heat radiated from Earth. This leads to an increase in Earth's temperature.
This heating up of Earth and its objects due to the trapping of infrared radiation by green
house gases in the atmosphere, is called green house effect.

 Global Warming: Green house effect is very essential for the existence of life because
in its absence, Earth would be converted into extremely cold planet. When concentration
of green house gases increases, green house effect also increases. This is known as global
warming.

 Acid rain: It is caused by the presence of oxides of nitrogen and sulphur in the air. These
oxides dissolve in rain water and from nitric acid and sulphuric acid respectively. The rain
carrying acids, is called acid rain.

 Smog: It is two types: Classical smog & Photochemical smog

 Classical smog : These occur in cool, humid climate. Sulphur dioxide (SO2) and
particulate matter from fuel combustion are the main components of classical
smog.

 Photochemical smog: These occur in warm, dry and sunny climate. It consists of a
mixture of primary pollutants (nitrogen oxides and carbon monoxides) and
secondary pollutants (ozone, formaldehyde).

Peroxyacetyl nitrate (PAN) and aldehydes present in smog causes irritation in eyes.
PAN has the highest toxicity to plants. It attacks younger leaves and causes bronzing
and glazing of their surfaces.

 Stratospheric Pollution: In stratosphere, ozone layer absorbs the ultraviolet

radiation of the Sun which are harmful to living organisms.

 Depletion of ozone layer: causes skin cancer and cataract in human and
reduction of planktons in ocean and depletion of plants. Depletion of ozone layer is
caused by chlorofluoro carbons which are used in refrigeration, fire extinguishers and
aerosol sprayers.

In stratosphere, the depletion of ozone layer leading to ozone hole has been mainly
observed in the stratosphere of Antarctica. The formation of this hole occur due to the
accumulation of special clouds in the region called Polar Stratospheric Clouds (PSCs) and
inflow of chlorofluoro carbons (CFCs).

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 Water pollution
 In some part of India, drinking water is contaminated by the impurities of arsenic, fluoride,
uranium, etc. In water, some dissolved Oxygen (DO) is also present. For a healthy aquatic
life, the optimum value of DO is 5-6 ppm.
 If DO is below 5 ppm, the growth of fishes is inhibited.
 Biochemical Oxygen Demand (BOD) is the total amount of oxygen (in mg) required by
microbes to decompose the organic matter present in 11 of water sample while Chemical
Oxygen Demand (COD) refers to the total amount of oxygen (in ppm) consumed by the
pollutants in a water sample.

 BOD = (
(
)
)

 For clean water, BOD is less than 5 ppm while for highly polluted water, it is 17 ppm or more.

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 PROPERTIES OF GASES
 Properties of Gases
 Gas has no definite volume or shape.
 The other outstanding characteristic of gases is their low densities, compared with
those of liquids and solids.
 All gases expand equally due to equal temperature difference.
 Diffusion of gases: The phenomenon in which a substance mixes with another
because of molecular motion, even against gravity- is called diffusion.
 The pressure of a gas: The molecules of a gas, being in continuous motion,
frequently strike the inner walls of their container
 Temperature and Temperature Scales: Temperature is defined as the measure of
average heat. Temperature is independent of the number of particles or size and
shape of the object.

 Compressibility: Particles of a gas have large intermolecular spaces among them.

By the application of pressure much of this space can be reduced and the particles be
brought closer. Hence, the volume of a gas can be greatly reduced. This is called
compressing the gas.

 Gas Laws: All gases, irrespective of their chemical composition, obey certain laws that
govern the relationship between the volume, temperature and pressure of the gases. A
given mass of a gas, under definite conditions of temperature and pressure, occupies a
definite volume.
When any of the three variables is altered, then the other variables get altered. Thus these
Gas laws establish relationships between the three variables of volume, pressure and
temperature of a gas.

 Boyle's Law: "The product of the volume and pressure of a given mass of dry gas is
constant, at constant temperature".

 Charles Law: "At constant pressure, the volume of a given mass of gas increases or
decreases by 1/273 of its original volume at 32°F, for each degree centigrade rise or
lowering in temperature."

 Pressure Law: Volume remaining constant, the pressure of a given mass of gas
increases or decreases by a constant fraction (=1/273) of its pressure at 0°C for each
degree Celsius rise or fall of temperature.

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 Avogadro's Law: This is quite intuitive: the volume of a gas confined by a fixed
pressure varies directly with the quantity of gas. Equal volumes of gases, measured at the
same temperature and pressure, contain equal numbers of molecules. Avogadro's law thus
predicts a directly proportional relation between the number of moles of a gas and its
volume.

 Gay-Lussac's Law: When different gases react with each other chemically to
produce gaseous substances, then under the same condition of temperature and pressure,
the volume of the reacting gases and product gases bear a simple ration among one
another.

 Avogadro Number: From Avogadro's hypothesis, we know equal volume of all

gases contain equal number of molecules at normal temperature and pressure. The
number is known as Avogadro Number and is equal to 6.06 x 1023.

 The ideal gas equation of state: If the variables P. V. T and n (the number of
moles) have known values, then a gas is said to be in a definite state, meaning that all
other physical properties of the gas are also defined. The relation between these state
variables is known as an equation of state.

An ideal gas is an imaginary gas that follows the gas laws and has 0 volume at 0 K i.e., the
ideal gas does not exist.

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 ORGANIC CHEMISTRY
 Organic chemistry is defined as the study of hydrocarbons and their derivatives. Most
atoms are only capable of forming small molecules. However one or two can form larger
molecules.
 Urea was the first organic compound prepared in laboratory. It was prepared by Wohler
(1828) from inorganic compound i.e. ammonium cyanate.
 Acetic acid was the first organic compound synthesized from the elements by Kolbe.

 Functional group is responsible for the chemical properties of the molecules ex. OH is
alcoholic group.

 Isomers Compounds having the same molecular formula but different structures, e.g.
C₂H6O can have the structure, i.e. CH3OCH3 (dimethyl ether) and C2H5OH (ethanol).

Hydrocarbons
These are the compounds of only carbon and hydrogen.

 Saturated hydrocarbons: They contain only single bonds. These are also called
alkanes or paraffins and have general formula CnH2n+2 . Methane is the first member of this
group.

 Unsaturated hydrocarbons: They have general formula CnH2n for alkene and CnH2n-2
for alkynes. These have at least one double (=) or triple (Ξ) bond and are called alkenes
and alkynes respectively.

 Aromatic hydrocarbons: They have ring structure with alternate double bonds and
(4n+2)πe- (Huckel's rule). e.g. benzene.

Important Hydrocarbons and their Uses

1. Methane (CH4):
 It is also known as marsh gas or damp fire.
 Natural gas contains mainly 90% methane along with ethane, propane, butane etc.
Rice agriculture is a big source of atmospheric methane.
 It is the cause of occurrence of the explosions in mines.
 It is used as a fuel gas in making carbon black

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2. Biogas:
 Produced during decay of biomass in the absence of oxygen.
 Methane (75%) is the main constituent of biogas).

3. Ethane (C2H6):
 Natural gas contains approx. 10% ethane.

 Its hexachloro derivative C2CI6 is used as an artificial camphor.

4. Butane (C4H10): It is the main constituent of LPG (liquefied petroleum gas).

5. Ethylene (CH2 = CH2):

 In World war | (1914-18), it was used for the manufacturing of mustard gas
(poisonous gas).
 It is used as an anesthetic for the preservation and artificial ripening of green fruits.

6. Benzene (C6H6)
 It is the simplest aromatic hydrocarbon. It was discovered by Faraday in 1825.
 It is also used as a motor fuel under the name benzol.

7. Toluene (C6H5CH3)
 It is used as a commercial solvent in the manufacturing of explosive (TNT), drugs
(chloramines-T) and dyestuffs.
 Used in the manufacturing of saccharin and printing inks. toluene is used as
antifreeze.

8. Naphthalene (C10H8): It is used for preventing moths in clothes, as an insecticide.

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 Halogen Derivatives of Hydrocarbons
1. Chloroform (CHCI3):
 It was discovered by Sir James Young Simpson.
 It is stored in closed dark coloured bottles completely filled because it is oxidized by
air in the presence of sunlight to an extremely poisonous gas phosgene (COCI₂).
 It reacts with conc. HNO3 and form chloropicrin (CI3C – NO2). Chloropicrin is an
insecticide and also used as poisonous gas at the time of war.
 The major use of chloroform today is in the production of the Freon refrigerant, R-22.

2. Iodoform (CHI3): It is used as an antiseptic due to liberation free Iodine.

3. Carbon tetrachloride (CCI4): used as a fire extinguishers under the name

pyrene.

4. Dichloro diphenyl trichloro ethane (DDT): It was the first chlorinated

organic insecticides and originally prepared in 1873.

5. Alcohols
 Methyl alcohol (CH3OH):
 It is also known as wood spirit or wood naphtha.
 Methyl alcohol is poisonous in nature and when taken internally it can cause
blindness and even death.

 It is used for denaturing alcohol (methylated spirit is denatured ethyl alcohol).

 Ethyl alcohol (C₂H5OH): It is simply known as alcohol, spirit of wine or grain alcohol.

 Glycerol (CH₂OH.CHOH.CH₂OH):
 It is an important trihydric alcohol known as glycerine.
 It is sweet in taste and very hygroscopic in nature.
 It is used in the manufacturing of cosmetics and transparent soaps.

 Phenol (C6H5OH): It is a monohydric benzene derivative. It is commonly known as

carbolic acid or benzenol.

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6. Methyl isocyanate (CH3NCO): Leakage of this gas is responsible for Bhopal
gas tragedy.

Coal
 It is believed that is was formed by (carbonization).
 Different varieties of coal are anthracite (90% carbon), bituminous (70% carbon), lignite
(40% carbon) and peat (10-15% carbon).
 On heating at 1270-1675 K in the absence of air, coal decomposes and gives the following
products.
 Coke is the solid residue left after the distillation.
 Coal tar It is a mixture of about 700 substances.
 Now-a-days bitumen, a petroleum product, is used in place of coal tar for metalling the
roads.
 The most significant characteristics of Indian coal are its high ash content, entrained
gasifires and low sulphur content.
 The process of separation of various constituents/ fractions of petroleum is known as
refining.
 Knocking - In a petrol engine, vapours of petrol and air are first compressed to a small
volume and then ignited by a spark. If the quality of petrol is not good, it leads to the pre-
ignition of fuel in the cylinder. This gives rise to a metallic sound known as knocking.
Tetraethyl lead (TEL) and Benzene - Toluene - Xylene (BTX) are common antiknock
compounds.
 Octane number - The antiknocking property of petrol is measured in terms of octane
number. Higher the octane number, better is the quality of fuel. Gasoline used in
automobiles has an octane number 80 or higher while in aeroplane, it has an octane
number 100 or over higher.

Fuels
 Producer gas: It is a mixture of carbon monoxide and nitrogen. Water gas in mixture of
carbon monoxide and hydrogen.

 Coal gas: It is a mixture of hydrogen, methane, carbon monoxide, ethane, acetylene,

carbon dioxide, nitrogen and oxygen.

 Oil gas and petrol gas: It is a mixture of methane, ethylene and acetylene etc., and is
obtained by cracking of kerosene.

 LPG (Liquefied Petroleum Gas): the mixtures of hydrocarbons such as propane,

propene, n-butane, isobutene and various butane with small amount of ethane.The major
sources of LPG are natural gas.

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 CNG (Compressed Natural Gas): It is highly compressed from of natural gas,
octane rating of CNG is 130.

 Gasohol: It is a mixture of ethyl alcohol (10%) and petrol (90%).

Flame
It is the hot part of fire and has three parts.

 Innermost region of flame: It is black because of the presence of unburned carbon

particles.

 Middle region: It is yellow luminous due to partial combustion of fuel.

 Outermost region: It is blue (non-luminous) due to complete combustion of fuel. It is

the hottest part of flame and is used by the Goldsmith to heat the gold.

Rocket Fuel
 The fuel used in rockets is called rocket propellant.
 Liquid propellants are alcohol, liquid hydrogen, liquid ammonia (NH3), kerosene oil
etc.
 Solid propellants are polybutadiene and acrylic acid used along with oxidizers such
as aluminium per chlorate, nitrate or chlorate.

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 PYQs
1. Which among the following is used in making liquors, medicines and as a fuel in
aircrafts? ------ Ethyl alcohol
2. Ethane gas has a slightly _____________ taste. ---- Sweet
3. Pentane has structural isomers. ------ 3
4. What is used to prevent freezing of fuel in space crafts? ------ Glycol
5. Which among the following is used to generate light, to weld metals? ------
Acetylene
6. _________ gets converted to phosgene, when exposed to sunlight. ---- Chloroform
7. Who discovered benzene? ----- Michael Faraday
8. What is wood spirit? ------ Methyl Alcohol
9. The compound that has least value for octane number is ---- n-Heptane
10. The Chemical formula of Urea is _________ ----- (NH2)2CO & (NH2)2CO NH2
11. Alkenes were earlier known as ___________ ----- Olefins
12. Decane has how many hydrogen atoms? ------- 22
13. Carcinogenic chemicals cause------- Cancer
14. Aromatic hydrocarbons contain at least _______ benzene like ring in their molecules.
------ One
15. Chloroform can be used as ----- Anaesthetic
16. The of conversion of sugar into Alcohol is known as ------ Fermentation
17. Denatured spirit or denatured alcohol is mixed with ------ Pyridine
18. The chief source of naphthalene is ------- Coal tar
19. Formalin is an aqueous solution of------- Methanal
20. Isomer of ethyl alcohol is ------ Dimethyl ether
21. Fermentation of starch gives ------ Ethanol
22. Which one of the following is a Heterocyclic compound? ------ Furan
23. The temperature of oxy-acetylene flame is around ------- 3200°C
24. Production of alcohol from organic compounds by micro-organism is known as ------
Fermentation
25. The pair of compounds used as anaesthetic in medicine is ------ Nitrous oxide,
Chloroform
26. Which one of the following is the constituent of teargas? ------- Chloropicrin

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27. Chemical name of Gamma hexane is ------ Benzene Hexa Chloride
28. Which of the following known as 'Marsh gas'? ------- CH4
29. What is Baeyer's reagent? ----- Alkaline Potassium Permanganate
30. Bagasse is used in the manufacturing of ----- Paper
31. Which of the following gas is used for the artificial ripening of Fruits? ----- Ethylene
32. Ethanol containing 5% water is known as ------- Rectified spirit
33. What are Aldehydes? ------ Strong reducing agents
34. Alcohol obtained Saponification is by the process of ----- Ethyl alcohol
35. Which of the following is also known as Carbolic Acid? ----- Phenol
36. Which of the following is used as a test for aliphatic primary amines? ------
Isocyanide test
37. The gas that usually cause explosion in coal mines is ------ Methane
38. Which one of the following reacts with Fehling's solution? ------ HCHO
39. The most extensive use of molasses after fermentation is to produce ----- Ethanol
40. Which organism is responsible fermentation? ------- Yeast
41. During fermentation of sugar, the compound which is always formed is ----- Ethyl
Alcohol

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 Metals
 Sodium:
 Basic Metal
 Highly Reactive
 Atomic No. – 11
 White & Soft in Nature
 Na + Air Explosive(Exothermic Reaction)
 Na + Cl NaCl
 Sodium must be kept in Kerosine Oil.
Uses:
 It is strong Reducing Agent.
 Liquid Sodium is used in the Atomic Reactions
 It is used in Sodium Lamps & Antilocking Agent.
 It is also used in Synthetic Reactions

 Magnesium:
 It is Found in Magnesium Sulphate & Magnesium Chloride.
 It is the main Component of Chlorophyll.
 It is Reducing Agent.
 It is white, Soft and Ductile Metal.
 It does not react with Bases.
 After Reacting with Acids it makes Salt and Hydrogen Gas.
Uses:
 It is used in Flash Light Ribbon & Bulbs.
 It is also used in Fire Crackers and Photography.

 Calcium:
 It is basic Metal & Highly Reactive.
 It is white, Lustrous and Soft in Nature.
 Calcium (Ca) + Acids H2 (Hydrogen) Gas
 Calcium (Ca) + H2O Ca(OH)2 + H2 (Hydrogen) Gas
 Calcium (Ca) + Air CaO
USES:
 It is used in the manufacturing of Glass, Cement & Potteries.
 It is used in White Wash and to Kill Bacteria

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 Aluminium:
 It does not find in the Free State.
 Atomic No. -- 13
 It is white Coloured Substance.
 It is Good Conductor of Heat & Electricity.
 It is Strong Reducing Agent
 Al + Air makes layer of Aluminium Oxide
 Al + Halogens Halides
Eg: 2Al + 3Cl2 2AlCl3
Uses:
 It is used in Wires, Utensils & Aluminium Foil.
 It is used in Welding.
 It is also used in the manufacturing of Paint.

 Copper:
 It is in free state & Red in Colour.
 It is Ductile and Malleable
 It is good conductor of heat & Electricity
 It has slow corrosion in Air.
 Conc. HCl + Cu CuCl3(Cupric Chloride)
 It does not react with dil. HCl
 Cu + H2SO4 SO2(Sulphur Dioxide Gas)
Uses:
 It is used in electric products & Wires, Electric Painting.
 It is used in calorie meter, coins & Utensils.
 It is also used in the manufacturing of Alloys & Medicines.

 Zinc
 It is bluish white & hard in nature.
 Atomic No. -- 30
 Zn + dil. Hcl Salt + H2(Hydrogen gas)
 Zn + dil. H2SO4 Salt + SO2
 Zn + CuSO4 ZnSO4 + Cu
USES:
 It is used in the manufacturing of Alloys
 It helps in the Galvanise of Iron
 It is used in the extraction of Gold & Silver

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  Zinc Phosphite used in Rat Killers.
 Zinc Oxide is used in the making of Artificial Teeths & Creams.

 Silver:
 It is very less reactive, free in state & Compound.
 Atomic No. – 47
 It is good conductor of heat & Electricity.
 Silver(Ag) + Air(Sulphur) Ag2S(black coat in silver)
 Silver(Ag) + Conc. HNO3 NO2
 Silver(Ag) + Conc. H2SO4 SO2
 It does not react with Base.
USES:
 It used in Ornaments, Silver Coins & Silver Work.
 It is used in electroplating, Alloys & feeling of teeths.
 It is also used in Artificial Rain, Photography, Election Ink & Photo
chromatic Glass.

 Gold(Au):
 It is free & in Compound State.
 Atomic No. -- 79
 It is soft, highly malleable, yellow & Lustrous.
 It is Good conductor of Heat & Electricity
 It is corrosion free & Soluble in Aquarazia
 It does not react with Bases.
USES:
 It is used in the making of Ornaments & Coins.
 It is used in Photography, Electroplating, Gold Work & Medicines.

 Lead(Pb):
 it is Bluish Brown and most stable metal
 Atomic No. – 82
 It is heavy metal & Poisonous metal.
 Pb + Moist Air PbO + PbCO3
USES:
 It is used in metal formations, Bullets, Atomic Research.
 It is used in Artificial Body Organs.
 It is used in Soliders, Fuse Wires, Inks & Paints

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 Uranium(U):
 It is radioactive & Rare element.
 It is not in free state.
 Atomic No. – 92
 It is white(Lustrous), Ductile & Malleable in Nature.
USES:
 It is used in Nuclear Reactors.
 It is used in Atomic Bombs, Alloys & Medicines.

Non- Metals
 Nitrogen(N):
 Atomic No. – 7
 It is in composite form
 It is colourless, odourless, Tasteless & Transparent in Nature.
 Its presence is 78% in the environment.
 It is soluble in water & Neutral in nature.
USES:
 It helps in the manufacturing of Ammonia, Nitrites & Nitric Acids.
 It is used in medicines, fertilizers & Explosives
 It is filled in the tyres of Aeroplanes
 It is used electric Bulbs.

 Sulphur(S):
 Atomic No. – 16
 It is in free & Composite state
 It is yellow in colour.
 It is non- conductor of electricity & weak Conductor of heat.
 It is Non- Soluble in water but Soluble in Tarbin oil
 It has poisonous effect on the lower form of life.
USES:
 It helps in the production of SO2
 It helps to kill Bacteria & germs, even in Fungicide
 It is used in the Vulcanization of Rubber.
 It is also used as a Bleaching Agent.

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 Phosphorous(P):
 It is very reactive & not found in free state.
 Atomic No. – 15
 Its main Ore is --- Ca3(PO4)
a) White Phosphorous/ Yellow Phosphorous(P4)
 It has Garlic like smell.
 It is insoluble in water but soluble in Carbon disulphide
 It is poisonous & Lustrous in dark room.
 P4 + Human Being Phossy Jaw(Disease)
 White Phosphorous(P4) + Air Slightly Flame
USES:
 It is used in fire crackers, rat Killers .
 It is also used in Agni Bomb.

b) Red Phosphorous(P2):
 It is red colour Solid & Odourless in nature.
 It is Non-Poisonous in nature.
 It does not react with NaOH.
USES:
 it is used in the manufacturing of Matchsticks.

c) Black Phosphorous:
 It is very less reactive
 Non-reactive Atmosphere + High Pressure + 473K Black Phosphorous
 It is more stable
USES:
 It is used in Photosynthesis, Fertilizers
 It is also used in Medicines & Alloys.

 Hydrogen(H):
 It is gaseous non-Metal.
 It is future fuel.
 Atomic No. -- 1
 It is mostly present element in the atmosphere.
 Founded by – Kavindex(1766)
 It is colourless, odourless & Transparent Gas.
 It is very light Gas in all elements & Neutral in nature.
 H2 + Air Fire/ Explosive + Water
 H2 + S H2S(Hydrogen Sulphide gas)
 H2 + 2Na 2NaH(makes Hydride)

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  Proton=1, Electron=1, Neutron =0

Isotopes of Hydrogen:
a) Protium(1H1)
 Mass No. -1
 Proton + Neutron = 1 + 0
 Light weight Hydrogen
b) Deuterium(1H2)
 Mass No. – 2
 Proton + Neutron = 1 + 1
 Deiterium + Air D2O
c) Tritium(1H3)
 Mass No. – 3
 Proton + Neutron = 1+ 2
 It is rare, Unstable & Radiothermi

USES:
 It is used in welding, Methyl Alcohol, Artificial petrol
 It is also used in Atomic Fuel & Future Fuel

 Oxygen(O):
 It is colourless, odourless and tasteless in nature
 It is minute soluble in water
 It is neutral in Nature(pH-7)
 It is combustible in nature.
 Metal + Oxygen Metal Oxides
USES:
 It is used in respiration, welding & Dynamites.
 It is used in the manufacturing of KNO3, H2SO4 & Cl2.
 Liquid Oxygen is also used as Fuels

 Ozone(O3):
 It is allotrope of Oxygen
 It is very less available and Explosive in nature.
 It is in gaseous form(Heavy than Air)
 Its smell like rotten Fish
 In Liquid form its colour is dark Blue.
 In Solid Form its Colour is Violet
 Dry Oxygen + Silent electric discharge O3

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 USES:
 It is used in cleaning of water & Air.
 It is used as a food preservation, Silk
 It is used as a bleaching agent and an insectisides
 It helps to protect from the ultra violet Rays of the Sun.

 Carbon (C)
 It is free and composite in state.
 Atomic No. -- 6
 It is found in Diamond & Graphite(Pure & Crystalline form)
 It is non-conductor of Heat & Electricity.
 Carbon(C) + Metal Carbides
 Carbon + Air CO2
 Carbon + Air CO
USES:
 Diamond is used in the cutting of Glass
 Graphite is used in the formation of Electrodes, Colours & Lead of
Pencils.
 Graphite is used in Artificial Diamonds.

 Silicon(Si):
 Atomic No. – 14
 It is crystalline and non-crystalline in nature.
 It is non- metal and semiconductor.
 It is the 2nd mostly Found non-metal on the Earth
USES:
 It is used in IC Chips, Glass & Cement
 It is also used ad Drying Agent
 It is used in Carbo random Diamond & Ornaments.

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 PYQ
1. Identify the metal which is Non-toxic in nature ----- Gold
2. Main constituent of liquid bleach is ----- Sodium hypochlorite
3. Caustic Soda is ------ Deliquescent
4. Match Stick uses the allotrope of Phosphorous ------ Red phosphorous
5. Most abundant inert gas in the atmosphere is ------ Ar
6. Green colour seen in firework display, is due to the chloride salt of ------ Barium
7. Which of the following will displace Hydrogen from acids to form salts? ------- Na
8. Liquid Chemical used for artificial rain or cloud seeding----- Silver iodide, Sodium
chloride, Dry ice
9. The inert gas used as beacon Light is ------- Neon
10. Hydrogen was discovered by ------ Cavendish
11. Which of the following is used in welding broken pieces of iron rails and parts of
machine ------ Aluminium powder
12. Hydrogen sulphide is a ------ Colourless gas with rotten egg smell
13. Tip of match stick contains ------- Red phosphorous
14. Gas used in the production of vegetable ghee ------ Hydrogen Gas
15. Ozone Contains ----- Only oxygen
16. Ozone is represented as ------ O3
17. Chemical name of bleaching powder is ------ Calcium hypochlorite
18. Which one among the following is used commonly in the dehydration of water? ----
Bleaching powder
19. Lime water becomes milky when exposed to air due to the presence of -------
Carbon dioxide
20. Charcoal is used in water treatment as a/an ------ Adsorbent
21. The gas which turns into Liquid at the Lowest E temperature among the following is -
---- Hydrogen
22. Heavy water means ------- Water containing Maximum density
23. Soda water contains ------
24. Which of the following is used for making smoke bombs? -------- Phosphorous
25. ___________ of the following gas is coloured? ------- Chlorine
26. Chemically Lime water is ------- Calcium Hydroxide

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27. Which gas is used as a fire extinguisher? ------- Carbon monoxide
28. Mercury is a -------- Liquid metal
29. What is dry ice? ------ Solid carbon
30. Diamond does not conduct electricity, because ------ No free electrons are present
in it
31. Hydrogen Peroxide is an effective Sterilizing agent. Which one of the following
product is
formed when it readily loses active oxygen? ----- Water
32. In deep see diving, divers use a mixture of gases consisting of oxygen and --------
Helium (He)
33. The Gas dissolved in water that makes it basic is ----- Ammonia
34. Which metal is extracted from Sea water? ------ Magnesium
35. Which of the following oxide is amphoteric in character? ------- SnO2
36. Which one of the following is a biochemical sediment rock? ------- Coal
37. Which one of the following element is an example of noble gas? ------- Helium
38. Silicon is a Polymer of ----- Dialkyl dichloro silane
39. Which one of the following gases mixed oxygen in aqualungs used by divers for the
breathing? ------- Helium
40. Which of the oxide is neutral? ----- CO
41. Which one of the following is not a form of carbon? ------ Haematite
42. Percentage of Lead in Lead Pencils is ------ 0%
43. Silver halides are used in photographic plate because they are ---- Reduced by
Light
44. Chemically 'Philosopher Wool' is a ------- Zinc oxide
45. Oxygen is a -------- Combustion nourishing
46. Carbon monoxide is an inflammable gas which one of the following is also
inflammable? ------ Hydrogen
47. Select the incorrect statement regarding the carbon compounds ------ These are
not easily combustible
48. Chemical Name of common salt is ------- Sodium chloride
49. Sodium chloride or Table salt occurs in nature as the mineral------- Halite
50. The material used in the manufacture of Lead pencil is ------ Graphite
51. Plaster of Paris is made by the Partial dehydration of ------ Gypsum salt

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52. Which among the following halogens is the most reactive? ------ Fluorine
53. Non-metal found in Liquid State ------ Bromine
54. Which silver salt is used for making film of photography? ----- Silver bromide
55. The chemical name of Hypo commonly used in Photography is ------ Sodium
thiosulphate
56. Sodium carbonate commonly known as ------ Washing soda
57. The common name of sodium bicarbonate is ------- Baking soda
58. Commercial name of sodium bicarbonate is ------- Baking Soda
59. Chemical name of baking soda is ------ Sodium bicarbonate
60. White Phosphorous is placed under the ------- Cold Water
61. Commonly sodium is kept under the -------- Kerosene oil
62. Which of the following can be used as an anesthetic? ------- N2O.
63. Dry powder fire extinguisher contains ------- Sand and sodium bicarbonate
64. No. of unpaired electron in inert gas is ------ zero
65. Noble gas used in the treatment of cancer is ------ Radon
66. Mortar is a mixture of water, sand -------- Slaked lime
67. What is baking soda? ------- Sodium bicarbonate
68. Most commonly bleaching agent is --------- Chlorine
69. Which gas is filled in balloons ------ Hydrogen
70. Which of the following noble gas can forms Compounds ----- Helium
71. The maximum density of water is at ------ 4°C
72. Old oil painting becomes black due to the formation of ------- PbS
73. Which is the 2nd abundant element on the surface of earth except Hydrogen? ----
Helium
74. What is Asbestos? ----- Calcium magnesium Silicate
75. At room temperature, the metal that liquid is ------ Mercury
76. If the bullets could not be removed from gunshot injury of a man, it May causes
poisoning by ------ Lead
77. Which one of the following is known as the brown coal? ------ Lignite
78. Which one of the following is not a coal variety? ----- Dolomite
79. Which of the following elements behave chemically both as Metal and a Non-
metal? ----- Silver
80. Which of the following metal has maximum electrical conductivity? ----- Silver

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81. Illumination of Metal is caused by the ------ Reflection of Light due to presence of
free
82. Heavy metals got their names because compared to others atoms they ----- Higher
densities
83. Which of the following is the most bad conductor? ------- Lead
84. Which metal is protected by the layer of its own oxide? ------- Aluminium
85. The ore of only two metals that are Non-Silver in colour, they are ----- Copper & Gold
86. T The ratio of pure gold in 18 carat gold is ------ 75%
87. Purity of gold is expressed in terms of carat Purest form of gold is ------ 24 Carat
88. The King of metal is ------ Gold
89. Standard 18 carat Gold sold in the Market is ------ 18 parts gold and 6 parts other
metal
90. he Soft Silvery Metallic element which ionizes easily when heated or exposed to
Light and it present in atomic clocks is ------ Cesium
91. Which one of the following metals cannot be used as an electromagnet? ------
Copper
92. Quartz is a type of ------- Silicon dioxide
93. Which one of the following is used in Pencils? ----- Graphite
94. Which of the following property is generally found in non metals? ------ Brittleness
95. Fire-Fighting clothes are made from ------ Asbestos
96. Fullerene is a newly discovered crystalline carbon allotrope, contains ----- 60 C
atoms
97. Chile saltpeter is the common name of ------ Sodium Nitrate
98. In Graphite layers are held together by ------- Vander waal forces
99. Which one among the following is Lubricant? ------- Graphite
100. Diamond is harder than Graphite because of ----- Difference of crystalline
structure
101. One carat of Diamond is equal to ----- 200 mg
102. Which among the following elements is a liquid at room temperature? -----
Mercury
103. Which among following is white the phosphorus? ----- P4
104. Alkali metals can ------ Easily lose electrons
105. Which among the following has the maximum density? ---- Water

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106. Who discovered Nitrogen? ----- Rutherford
107. Which of the following gases is present in the atmosphere can be detected
by its odour? ----- Sulphur dioxide
108. If water smells bad, then that odour can be removed by adding -----
Activated carbon
109. Which of the following elements has the lowest melting point? ----- Bromine
110. Heavy water is ------ Deuterium oxide
111. Solid carbon dioxide is known as ------ Dry ice
112. Who discovered Oxygen? ------ Carl Scheele
113. Which of these is not a macronutrient for Plants? ------ Chlorine
114. Which of the following elements has the lowest melting point? ----- Krypton
115. Why metals conduct electricity? ----- Because of free electrons
116. Density of water is maximum ------ 4 degree Celsius
117. Which of the following gases is known as "Laughing Gas"? ----- Nitrous oxide
118. The Chemical formula of Cadmium nitrate is ------ Cd(NO3)2
119. The common name of hydrogen peroxide is ----- Bleach (liquid)
120. Which is the elements has the lowest melting point? ----- Radon
121. Barium loses electrons to achieve noble gas electron configuration.----- 2
122. The Chemical formula of Ammonium Oxalate is ------- (NH4)2C2O4
123. Chemical Formula of Water is ----- H2O
124. The Chemical formula of Ammonium sulphate is ------ (NH4)2SO4
125. Which is the element has the lowest melting point? ------- Krypton
126. The common name of Magnesium Sulphate heptahydrate is ------ Epsom salt
127. Which is the elements has the lowest melting point?------ Helium
128. The chemical formula of Ammonia is ----- NH3
129. Who discovered Fullerene (an allotrope of carbon)? ---- Richard Smalley
130. The common name of sodium tetraborate decahydrate is ---- Borax
131. Which gas among the following used as an anaesthetic? ---- Nitrous oxide
132. Which is the element has the lowest melting point? ------- Argon
133. The common name of sulphur is ------ Brimstone
134. Which of the following is not a Halon gas? ------ Methane
135. Which is the element has the lowest melting point? ----- Hydrogen
136. The Chemical formula of Ammonium chloride is ______ ------ NH4CI

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137. Which is the element has the lowest melting point? ------ Nitrogen
138. What is washing soda? ------- Sodium carbonate
139. Zeolite is ------ Hydrated sodium aluminium silicate
140. Helium is added to the oxygen supply of deep sea divers because it is ------
Less soluble in blood than nitrogen at high pressure
141. Water is used in a hot water bag because ----- It has high specific heat
142. What is contained in Chlorophyll ? ------ Magnesium
143. Filament of electric bulb is made of ------ Tungsten
144. Which is the element has the lowest melting point? ----- Oxygen
145. Which is the element has the lowest melting point? ------ Hydrogen
146. Which is the element has the lowest melting point? ------- Neon
147. Which is the element has the lowest melting point? ------ Xenon
148. What is the product formed when sodium bicarbonate is heated strongly? ----
-- Sodium carbonate
149. The most pure form of carbon among the options is ----- Graphite
150. Activated Charcoal is used to remove colouring matter from pure substances
by ----- Adsorption
151. Silica gel is a ----- Drying agent
152. Phosphorous is kept in water because ----- Its ignition temperature is very low
153. In arc welding Argon is used because of its ------ Ability to lower the melting
point of the metal
154. Inert gases are ------ Chemically unreactive
155. Which of the following fuels causes minima environmental pollution? ------
Hydrogen
156. Which of the following is the most important raw material for generation of
power in India? ----- Coal
157. The purest form of water in nature is ----- Rain water
158. Silver gets corroded due to _________ in air. ------ Hydrogen sulphide
159. Which of the metals has the maximum thermal conductivity? ----- Silver
160. Which one of the following forms phosphorous is most reactive? -------- White
Phosphorous
161. Magnesium is a constituent metal of ------ Chlorophyll molecule
162. Name the gas used in preparation of bleaching ------ Chlorine

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163. Highest percentage of carbon is found in which form of coal? ----- Anthracite
164. Which one of the following is a good electrical conductor? ---- Graphite
165. Which of the following acts as best adsorbent? ------ Activated Coconut
Charcoal
166. Which is the metal has the least melting point? ----- Mercury
167. The property of metals by which they can be beaten into thin sheets is called
----- Malleability
168. The property of metal by which it can be drawn into wires is called -----
Ductility.
169. Which of the following metal is the heaviest? ----- Osmium
170. Which of the following metal has the lowest density? ----- Lithium
171. Which of the following is the most reactive in nature? ------ Potassium
172. Which of the following is not a property of a metal? ----- Poor conductivity of
heat

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 Physical Chemistry PYQs
1. Which among the following is an endothermic reaction? ------ Sweating
2. Name the catalyst used in the conversion of milk into curd. ---- Lactase
3. In a rechargeable cell what kind of energy stored within the cell? ---- Chemical
energy
4. Which acid is stored in batteries? ----- Sulphuric acid
5. Which of the following pairs of Material is commonly used in rechargeable batteries
used in Torch Lights, Electric Shaver etc. ------ Nickel and Cadmium
6. What happens during the charging of Lead operated battery? ---- Consumption of
Lead Sulphate
7. Catalyst are those substances ---- Which increase rate of reaction
8. What does a catalyst do in a reaction? ---- Changes activation energy
9. The unit of ionic Product of water (Kw) is ----- Mol2 ltr-2
10. Which one of the following has highest value of specific heat? ---- Water
11. Which one of the following is known as solution? ----- Homogeneous mixture
12. Electrolysis of copper sulphate solution with copper electrodes gives ----- Copper at
cathode and oxygen at anode
13. When H2 gas is allowed to expand from a region of High pressure to a region of Low
pressure, the temperature of gas ---- Increases
14. Example of Aerosol is ----- Smoke
15. Blood may be purified by ----- Dialysis
16. Isotonic solutions have equal. ------ osmotic pressure
17. Strong electrolytes are those which ----- dissociate into ions even at high
concentration
18. Water and ice crystal are in equilibrium at 0°C. when pressure is applied to this
system -------- No effective change occur
19. Light Scattering take place in ---- Colloidal solution
20. Muddy water is treated with alum in Purification process ----- Coagulation
21. Alum is used for the water treatment in process named the ----- Coagulation
22. Which of the following is used to Purify the muddy water? ----- Potash alum
23. Which of the following is not a crystalline solid? --- Rubber
24. Enzyme which coagulate the milk into curd ---- Rennin

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25. Which one of the following is an example of gel? ---- Cheese
26. What changes will happen to a bowl of ice and water kept at exactly zero degree
Celsius? ---- No change will happen
27. Suspended colloidal particles in water can be removed by the process of ---
Coagulation
28. Alum stops bleeding in a minor cut because of ------ Coagulation
29. A colloidal system in which a Liquid is dispersed in a Liquid is called ----- Emulsion
30. Which of the following is strongest coagulant ----- Aluminium Chloride
31. Cloud is a colloidal of --- Water drop in a dispersion medium of air
32. An Emulsion is a colloid of a ---- Liquid in a Liquid
33. Milk is a ---- Emulsion

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 Recent CGL PYQs
1. At least __________ of the carbon dioxide fixation on earth is carried out by algae
through photosynthesis. ---- a half
2. _________ is reducing the degree or intensity of, or eliminating, pollution.---
Abatement
3. What is the name of the compound having the formula CH3CH2OH?--> Ethanol
4. Which of the following compounds in petroleum can cause corrosion to parts of
internal combustion engines and refineries?--> Sulphur
5. The chemical symbol of arsenic is:-> As
6. Which of the following is an example of monosaccharides? --- Fructose & Glucose
7. Ozone is an allotrope of _________ ---- oxygen
8. Urea, a commonly used nitrogen-based fertiliser, is prepared by the reaction
between ammonia and __________ ---- carbon dioxide
9. __________ refers to an environment in which oxygen is readily available.--- Aerobic
10. Acidic nature of soil is shown by high concentration of _________ ----- hydrogen
11. _____________ is defined as the temperature to which the air would have to cool (at
constant pressure and constant water vapour content) in order to reach
saturation.------ Dew point temperature
12. Which of the following is correctly paired?--> Cyanide ion-CN-
13. _____________ is the measure of relative clarity of a liquid.--> Turbidity
14. Ferrum is the Latin name for ________________ ---- iron
15. Nitrogen is a _____________ element. ---- diatomic
16. Ozone is a molecule made up of ___________ Oxygen atoms.---- three
17. How many electrons are there in the outermost shell of a group 16 element?-> 6
18. What is the atomic mass of oxygen (expressed in 'u')?-- > 16
19. Who among the following science fiction/ popular science writers wrote '2001: A
Space Odyssey' and held the position of a Professor at the Physical Research
Laboratory, Ahmedabad?-- > Arthur C. Clarke
20. How many sodium atoms are there in one molecule of sodium peroxide?--> Two
21. Which of the following is NOT a chemical coagulant used in water treatment?----->
Nitrogen dioxide

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22. Which of the following is a characteristic of amorphous solids?------ > Gradual
softening over a range of temperatures
23. Capsaicinoids, carotenoids, phenolics, and vitamins are dominant chemicals in
which of the following foods?--> Chilli
24. What is the atomic number of nitrogen?----- > 7
25. One mole of an ideal gas occupies a volume of at 273 K and 1 atm pressure.-->
22.4 litre
26. Carbon monoxide contains approximately ___________ of oxygen for each 1.00 g
of carbon.--> 1.33 g
27. Irrespective of the source, pure water contains _________ of oxygen by mass---
88.89%
28. Acidic drain cleaners made of _____________ or ______________ acid are powerful
enough to clear heavy-duty hair, food, grease, soap scum or paper-based clogs in
15 minutes or less.--> sulphuric, hydrochloric
29. Which of the following is a property of Beryllium?--> Forms covalent compounds
30. Hot water can be a pollutant if it comes from:--- A power plant & An industry

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