CONTENTS
Foreword iii
Unit 1 Some Basic Concepts of Chemistry 1
1.1 Importance of Chemistry 4
1.2 Nature of Matter 4
1.3 Properties of Matter and their Measurement 6
1.4 Uncertainty in Measurement 10
1.5 Laws of Chemical Combinations 14
1.6 Dalton’s Atomic Theory 16
1.7 Atomic and Molecular Masses 16
1.8 Mole Concept and Molar Masses 18
1.9 Percentage Composition 18
1.10 Stoichiometry and Stoichiometric Calculations 20
Unit 2 Structure of Atom 29
2.1 Discovery of Sub-atomic Particles 30
2.2 Atomic Models 32
2.3 Developments Leading to the Bohr’s Model of Atom 37
2.4 Bohr’s Model for Hydrogen Atom 46
2.5 Towards Quantum Mechanical Model of the Atom 49
2.6 Quantum Mechanical Model of Atom 53
Unit 3 Classification of Elements and Periodicity in Properties 74
3.1 Why do we Need to Classify Elements ? 74
3.2 Genesis of Periodic Classification 75
3.3 Modern Periodic Law and the present form of the Periodic Table 79
3.4 Nomenclature of Elements with Atomic Numbers > 100 79
3.5 Electronic Configurations of Elements and the Periodic Table 82
3.6 Electronic Configurations and Types of Elements: 83
s-, p-, d-, f- Blocks
3.7 Periodic Trends in Properties of Elements 86
Unit 4 Chemical Bonding and Molecular Structure 100
4.1 Kössel-Lewis Approach to Chemical Bonding 101
4.2 Ionic or Electrovalent Bond 106
4.3 Bond Parameters 107
4.4 The Valence Shell Electron Pair Repulsion (VSEPR) Theory 112
4.5 Valence Bond Theory 117
4.6 Hybridisation 120
4.7 Molecular Orbital Theory 125
4.8 Bonding in Some Homonuclear Diatomic Molecules 129
4.9 Hydrogen Bonding 131
Unit 5 States of Matter 136
5.1 Intermolecular Forces 137
5.2 Thermal Energy 139
5.3 Intermolecular Forces vs Thermal Interactions 139
5.4 The Gaseous State 139
5.5 The Gas Laws 140
5.6 Ideal Gas Equation 145
5.7 Kinetic Energy and Molecular Speeds 147
5.8 Kinetic Molecular Theory of Gases 149
5.9 Behaviour of Real Gases: Deviation from Ideal Gas Behaviour 150
5.10 Liquefaction of Gases 152
5.11 Liquid State 154
Unit 6 Thermodynamics 160
6.1 Thermodynamic Terms 161
6.2 Applications 164
6.3 Measurement of ∆U and ∆H: Calorimetry 169
6.4 Enthalpy Change, ∆rH of a Reaction – Reaction Enthalpy 171
6.5 Enthalpies for Different Types of Reactions 176
6.6 Spontaneity 181
6.7 Gibbs Energy Change and Equilibrium 186
Unit 7 Equilibrium 192
7.1 Equilibrium in Physical Processes 193
7.2 Equilibrium in Chemical Processes – Dynamic Equilibrium 196
7.3 Law of Chemical Equilibrium and Equilibrium Constant 198
7.4 Homogeneous Equilibria 201
7.5 Heterogeneous Equilibria 203
7.6 Applications of Equilibrium Constants 205
7.7 Relationship between Equilibrium Constant K, 208
Reaction Quotient Q and Gibbs Energy G
7.8 Factors Affecting Equilibria 208
7.9 Ionic Equilibrium in Solution 212
7.10 Acids, Bases and Salts 213
7.11 Ionization of Acids and Bases 216
7.12 Buffer Solutions 226
7.13 Solubility Equilibria of Sparingly Soluble Salts 228
Appendices 239
Answer to some Selected Questions 253
Index 259
