, CONTENT
Unit 1 INTRODUCTION TO CHEMISTRY 0003 - 0013
Unit 2 CHEMICAL BONDING 0014 – 0156
Unit 3 SOLUTIONS & COLLIGATIVE PROPERTIES 0157 - 0240
Unit 4 REDUCTION, OXIDATION & HYDROLYSIS REACTIONS 0241 - 0302
Unit 5 CHEMICAL EQUILIBRIUM 0303 – 0376
Unit 6 IONIC EQUILIBRIUM (ELEMENTARY) 0377 - 0416
Unit 7 SURFACE CHEMISTRY 0417 – 0479
Unit 8 EQUIVALENT CONCEPTS & TITRATIONS 0480 – 0521
Unit 9 IONIC EQUILIBRIUM (ADVANCED) 0522 – 0613
Unit 10 METALLURGY 0614 – 0679
Unit 11 MOLE CONCEPTS 0680 - 0753
Unit 12 PERIODIC TABLE & PERIODICITY 0754 – 0805
Unit 13 SOLID STATE 0806 – 0870
Unit 14 ATOMIC STRUCTURE & NUCLEAR CHEMISTRY 0871 - 0974
Unit 15 THERMODYNAMICS & THERMOCHEMISTRY 0975 – 1105
Unit 16 ELECTROCHEMISTRY 1106 – 1203
Unit 17 CHEMICAL KINETICS & RADIOACTIVITY 1204 - 1298
Unit 18 ALL BASIC CONCEPTS OF ORGANIC CHEMISTRY 1299 - 1315
Unit 19 ABC-2 (Phenol & Aniline) 1316 - 1326
Unit 20 ABC-3 (Alkyl halide, Alcohol & Ether) 1327 - 1337
Unit 21 ABC-4 (Carboxylic acid & Carbonyl compounds) 1338 - 1353
,Unit 22 CARBONYL COMPOUNDS(ALDEHYDES & KETONES) 1354 – 1461
AROMATIC COMPOUNDS(PHENOL, ANILINE & DIAZONIUM
Unit 23 1462 – 1532
COMPOUNDS)
AROMATIC COMPOUNDS(PHENOL, ANILINE & DIAZONIUM
Unit 24 1533 – 1581
COMPOUNDS)
Unit 25 GENERAL ORGANIC CHEMISTRY-II 1582 – 1652
Unit 26 IDEAL GASES 1653 – 1723
Unit 27 IONIC EQUILIBRIUM (ADVANCED) 1724 – 1917
Unit 28 ORGANIC REACTION MECHANISMS: I - IV 1816 – 2027
Unit 29 REAL GASES 2028 – 2133
Unit 30 STRUCTURAL IDENTIFICATION & POC 2134 – 2280
Unit 31 CHEMISTRY IN EVERYDAY LIFE & POC 2281 – 2335
Unit 32 BASIC INROGANIC NOMENCLATURE 2336 – 2352
Unit 33 HYDROGEN COMPOUNDS 2353 – 2378
Unit 34 d & f-BLOCK ELEMENTS & THEIR COMPOUNDS 2379 – 2445
Unit 35 p-BLOCK ELEMENTS(B & C FAMILY) 2446 – 2514
Unit 36 p-BLOCK ELEMENTS(HALOGEN & NOBLE GASES) 2513 – 2566
Unit 37 p-BLOCK ELEMENTS(N & O FAMILY) 2567 – 2636
Unit 38 s-BLOCK ELEMENTS 2637 – 2694
Unit 39 QUANTUM NUMBER & ELECTRONIC CONFIGURATION 2695 – 2717
Unit 40 QUALITATIVE ANALYSIS(ANION & CATIONS) 2718 – 2826
Unit 41 ENVIRONMENTAL CHEMISTRY 2827 – 2849
Unit 42 COORDINATION COMPOUNDS 2850 – 2935
, INTRODUCTION TO CHEMISTRY
Atomic hypothesis:
Keeping in view various laws of chemical combination, a theoretical proof for the validity of different
laws was given by John Dalton in the form of hypothesis called Dalton's atomic hypothesis. Postulates
of Dalton's hypothesis are as follows:
(i) Each element is composed of extremely small particles called atoms which can take part in chemical
combination.
(ii) All atoms of a given element are identical i.e., atoms of a particular element are all alike but differ
from atoms of other elements.
(iii) Atoms of different elements possess different properties (including different masses).
(iv) Atoms are indestructible i.e., atoms are neither created nor destroyed in chemical reactions.
(v) Atoms of elements combine to form molecules and compounds are formed when atoms of more
than one element combine.
(vi) In a given compound, the relative number and kind of atoms is constant.
Modern atomic hypothesis: The main modifications made in Dalton's hypothesis as a result of new
discoveries about atoms are :
(i) Atom is no longer considered to be indivisible.
(ii) Atoms of the same element may have different atomic weights. E.g. isotopes of oxygen O16, O17 and
O18.
(iii) Atoms of different element may have same atomic weights. E.g. isobars Ca40 and Ar40.
(iv) Atom is no longer indestructible. In many nuclear reactions, a certain mass of the nucleus is
converted into energy along with , and rays.
(v) Atoms may not always combine in simple whole number ratios. E.g. in sucrose (C12H22O11), the
elements carbon, hydrogen and oxygen are present in the ratio of 12 : 22 : 11 and the ratio is not a
simple whole number ratio.
Atomic & Molecular masses:
1
Atomic mass: It is the average relative mass of atom of element as compared with times the mass
12
of an atom of carbon-12 isotope.
Average mass of an atom
Atomic mass =
1/12 Mass of an atom of C12
Average atomic mass: If an element exists in two isotopes having atomic masses 'a' and 'b' in the
(m a) + (n b)
ratio m : n, then average atomic mass = . Atomic mass is expressed in amu. 1 amu =
m+n
1
1.66 × 10–24 g. One atomic mass unit (amu) is equal to th of the mass of an atom of carbon-12
12
isotope.
Gram atomic mass (GAM): Atomic mass of an element expressed in grams is called Gram atomic
mass or gram atom or mole atom.
Mass of an element
(i) Number of gram atoms =
GAM
(ii) Mass of an element in g = No. of gram atoms × GAM
3
Unit 1 INTRODUCTION TO CHEMISTRY 0003 - 0013
Unit 2 CHEMICAL BONDING 0014 – 0156
Unit 3 SOLUTIONS & COLLIGATIVE PROPERTIES 0157 - 0240
Unit 4 REDUCTION, OXIDATION & HYDROLYSIS REACTIONS 0241 - 0302
Unit 5 CHEMICAL EQUILIBRIUM 0303 – 0376
Unit 6 IONIC EQUILIBRIUM (ELEMENTARY) 0377 - 0416
Unit 7 SURFACE CHEMISTRY 0417 – 0479
Unit 8 EQUIVALENT CONCEPTS & TITRATIONS 0480 – 0521
Unit 9 IONIC EQUILIBRIUM (ADVANCED) 0522 – 0613
Unit 10 METALLURGY 0614 – 0679
Unit 11 MOLE CONCEPTS 0680 - 0753
Unit 12 PERIODIC TABLE & PERIODICITY 0754 – 0805
Unit 13 SOLID STATE 0806 – 0870
Unit 14 ATOMIC STRUCTURE & NUCLEAR CHEMISTRY 0871 - 0974
Unit 15 THERMODYNAMICS & THERMOCHEMISTRY 0975 – 1105
Unit 16 ELECTROCHEMISTRY 1106 – 1203
Unit 17 CHEMICAL KINETICS & RADIOACTIVITY 1204 - 1298
Unit 18 ALL BASIC CONCEPTS OF ORGANIC CHEMISTRY 1299 - 1315
Unit 19 ABC-2 (Phenol & Aniline) 1316 - 1326
Unit 20 ABC-3 (Alkyl halide, Alcohol & Ether) 1327 - 1337
Unit 21 ABC-4 (Carboxylic acid & Carbonyl compounds) 1338 - 1353
,Unit 22 CARBONYL COMPOUNDS(ALDEHYDES & KETONES) 1354 – 1461
AROMATIC COMPOUNDS(PHENOL, ANILINE & DIAZONIUM
Unit 23 1462 – 1532
COMPOUNDS)
AROMATIC COMPOUNDS(PHENOL, ANILINE & DIAZONIUM
Unit 24 1533 – 1581
COMPOUNDS)
Unit 25 GENERAL ORGANIC CHEMISTRY-II 1582 – 1652
Unit 26 IDEAL GASES 1653 – 1723
Unit 27 IONIC EQUILIBRIUM (ADVANCED) 1724 – 1917
Unit 28 ORGANIC REACTION MECHANISMS: I - IV 1816 – 2027
Unit 29 REAL GASES 2028 – 2133
Unit 30 STRUCTURAL IDENTIFICATION & POC 2134 – 2280
Unit 31 CHEMISTRY IN EVERYDAY LIFE & POC 2281 – 2335
Unit 32 BASIC INROGANIC NOMENCLATURE 2336 – 2352
Unit 33 HYDROGEN COMPOUNDS 2353 – 2378
Unit 34 d & f-BLOCK ELEMENTS & THEIR COMPOUNDS 2379 – 2445
Unit 35 p-BLOCK ELEMENTS(B & C FAMILY) 2446 – 2514
Unit 36 p-BLOCK ELEMENTS(HALOGEN & NOBLE GASES) 2513 – 2566
Unit 37 p-BLOCK ELEMENTS(N & O FAMILY) 2567 – 2636
Unit 38 s-BLOCK ELEMENTS 2637 – 2694
Unit 39 QUANTUM NUMBER & ELECTRONIC CONFIGURATION 2695 – 2717
Unit 40 QUALITATIVE ANALYSIS(ANION & CATIONS) 2718 – 2826
Unit 41 ENVIRONMENTAL CHEMISTRY 2827 – 2849
Unit 42 COORDINATION COMPOUNDS 2850 – 2935
, INTRODUCTION TO CHEMISTRY
Atomic hypothesis:
Keeping in view various laws of chemical combination, a theoretical proof for the validity of different
laws was given by John Dalton in the form of hypothesis called Dalton's atomic hypothesis. Postulates
of Dalton's hypothesis are as follows:
(i) Each element is composed of extremely small particles called atoms which can take part in chemical
combination.
(ii) All atoms of a given element are identical i.e., atoms of a particular element are all alike but differ
from atoms of other elements.
(iii) Atoms of different elements possess different properties (including different masses).
(iv) Atoms are indestructible i.e., atoms are neither created nor destroyed in chemical reactions.
(v) Atoms of elements combine to form molecules and compounds are formed when atoms of more
than one element combine.
(vi) In a given compound, the relative number and kind of atoms is constant.
Modern atomic hypothesis: The main modifications made in Dalton's hypothesis as a result of new
discoveries about atoms are :
(i) Atom is no longer considered to be indivisible.
(ii) Atoms of the same element may have different atomic weights. E.g. isotopes of oxygen O16, O17 and
O18.
(iii) Atoms of different element may have same atomic weights. E.g. isobars Ca40 and Ar40.
(iv) Atom is no longer indestructible. In many nuclear reactions, a certain mass of the nucleus is
converted into energy along with , and rays.
(v) Atoms may not always combine in simple whole number ratios. E.g. in sucrose (C12H22O11), the
elements carbon, hydrogen and oxygen are present in the ratio of 12 : 22 : 11 and the ratio is not a
simple whole number ratio.
Atomic & Molecular masses:
1
Atomic mass: It is the average relative mass of atom of element as compared with times the mass
12
of an atom of carbon-12 isotope.
Average mass of an atom
Atomic mass =
1/12 Mass of an atom of C12
Average atomic mass: If an element exists in two isotopes having atomic masses 'a' and 'b' in the
(m a) + (n b)
ratio m : n, then average atomic mass = . Atomic mass is expressed in amu. 1 amu =
m+n
1
1.66 × 10–24 g. One atomic mass unit (amu) is equal to th of the mass of an atom of carbon-12
12
isotope.
Gram atomic mass (GAM): Atomic mass of an element expressed in grams is called Gram atomic
mass or gram atom or mole atom.
Mass of an element
(i) Number of gram atoms =
GAM
(ii) Mass of an element in g = No. of gram atoms × GAM
3
