Wiley's J. D. Lee Concise Inorganic Chemistry for NEET and other Medical Entrance Examinations, 3ed, 2025

Preface

Note to the Student

1 Structure of an Atom

1.1 Subatomic Particles

Discovery of electron

Discovery of protons

Discovery of neutrons

1.2 Atomic Models

Thomson model

Rutherford model

1.3 Electromagentic Radiation

Properties of waves

1.4 Atomic or Emission Spectra

Continuous spectra

Hydrogen spectra

1.5 Planck’s Quantum Theory

1.6 Bohr’s Atomic Model

Calculation of energy and velocity of an electron according to Bohr’s theory

Merits of Bohr’s atomic model

Limitations of Bohr’s atomic model

1.7 Quantum Mechanical Model of the Atom

1.8 The Schrödinger Wave Equation

1.9 Representation of an Atom

1.10 Electronic Configuration of an Atom

Quantum numbers

Aufbau principle

Pauli exclusion principle

Hund’s rule

Stability of half-filled and fully- filled shells

Electronic configuration of ions

Nodal planes of different orbitals

1.11 Slater’s Rule

Periodic variation of Zeff values

Single Correct Choice Type Questions

Assertion-Reasoning Type Questions

Answers

2 Periodic Table and Periodic Properties

2.1 Periodic Table

Genesis of periodic classification

Moseley’s work

Modern periodic law

2.2 Classification of Elements Based on Electronic Configuration

Prediction of period and group number of an element from its electronic configuration

Neil Bohr’s classification

Naming of super heavy elements

2.3 Periodic Trends in Properties

Atomic radius

Ionic radius

Ionization energy (enthalpy)

Electron affinity

Electronegativity

Lattice energy

Hydration energy

Ionic Mobility

2.4 Born–Haber Cycle

Single Correct Choice Type Questions

Assertion-Reasoning Type Questions

Answers

3 Chemical Bonding

3.1 Attainment of a Stable Configuration

3.2 Types of Bonds

3.3 Transitions Between the Main Types of Bonding

Ionic bonds

Covalent bonds

Oxidation numbers

Coordinate bonds

Double and triple bonds

Metallic bonds and metallic structures

3.4 The Covalent Bond

The Lewis theory

Sidgwick–Powell theory

3.5 Valence Bond Theory

What is the essence of hybridization?

Features of hybrid orbitals

Calculation of steric number

3.6 Valence Shell Electron Pair Repulsion (VSEPR) Theory

Effect of lone pair

Effect of double bond

Effect of electronegativity

Back bonding

3.7 The Extent of d Orbital Participation in Molecular Bonding

3.8 Types of Covalent Bonds (Sigma (s) and Pi (π) Bonds)

Bridge bonding

3.9 Molecular Orbital Method

3.10 LCAO Method

s–s combinations of orbitals

s–p combinations of orbitals

p–p combinations of orbitals

p–d combinations of orbitals

d–d combinations of orbitals

Non-bonding combinations of orbitals

3.11 Rules for Linear Combination of Atomic Orbitals

3.12 Examples of Molecular Orbital Treatment for Homonuclear Diatomic Molecules

H2

+ molecule ion

H2 molecule

He2

+ molecule ion

He2 molecule

Li2 molecule

Be2 molecule

B2 molecule

C2 molecule

N2 molecule

O2 molecule

O-

2 molecule ion

F2 molecule

3.13 Examples of Molecular Orbital Treatment for Heteronuclear

Diatomic Molecules

NO molecule

CO molecule

3.14 Dipole Moment

Applications of dipole moment

Some special cases

3.15 The Ionic Bond

3.16 Polarizing Power and Polarizability – Fajans’ Rules

Properties of ionic compounds affected by polarization

3.17 Melting Point of Ionic Compounds

3.18 Solubility of Ionic Compounds

Prediction of solubility order in ionic compounds

3.19 Electrical Conductivity and Colour

3.20 Acidic Nature of Oxides

3.21 Thermal Stability of Ionic Compounds

3.22 Weak Forces

Attractive intermolecular forces

Repulsive intermolecuar forces

Lennard–Jones potential

3.23 Interactions between Ions and Covalent Molecules

3.24 The Metallic Bond

Conductivity

Lustre

Malleability and cohesive force

Crystal structure of metals

Bond lengths

3.25 Theories of Bonding in Metals

Free electron theory

Single Correct Choice Type Questions

Assertion-Reasoning Type Questions

Answers

4 Coordination Compounds

4.1 Double Salts and Coordination

Compounds

4.2 Werner’s Work

4.3 More Recent Methods of Studying Complexes

4.4 Classification of Ligands

4.5 Effective Atomic Number (EAN)

Sidgwick EAN rule

4.6 Shapes of d Orbitals

4.7 Bonding in Transition Metal Complexes

Valence bond theory

Crystal field theory

Molecular orbital theory

4.8 Valence Bond Theory

4.9 Crystal Field Theory

Octahedral complexes

4.10 Effects of Crystal Field Splitting

4.11 Tetragonal Distortion of Octahedral Complexes (Jahn-Teller Distortion)

4.12 Square Planar Arrangements

4.13 Tetrahedral Complexes

4.14 Magnetism

4.15 Extension of The Crystal Field Theory to Allow for Some Covalency

4.16 Nomenclature of Coordination Compounds

4.17 Isomerism

Polymerization isomerism

Ionization isomerism

Hydrate isomerism

Linkage isomerism

Coordination isomerism

Coordination position isomerism

Geometrical isomerism and optical isomerism

Single Correct Choice Type Questions

Assertion-Reasoning Type Questions

Answers

5 The p-Block Elements and their Compounds

The Group 13 Elements

5.1 Oxidation States and Types of Bonds

The (+III) oxidation state

The (+I) oxidation state – the ‘inert pair effect’

5.2 General Properties

Melting points, boiling points and structures

Size of atoms and ions

Electropositive character

Ionization energy

The Group 14 Elements

5.3 Structure and Allotropy of the Elements

5.4 Differences Between Carbon, Silicon and the Remaining Elements

5.5 Physical Properties

Covalent radii

Ionization energy

Melting points

Metallic and non-metallic character

Four-covalent compounds

5.6 Chemical Reactivity

Inert pair effect

The Group 15 Elements

5.7 General Properties and Structures of the Elements

Nitrogen

Phosphorus

Bond type

Metallic and non-metallic character

Reactivity

5.8 Hydrides

Ammonia NH3

The Group 16 Elements – Chalcogens

5.9 General Properties

Electronic structure and oxidation states

Acid rain and SO2

Uses of sulphur

5.10 Structure and Allotropy of the Elements

Oxygen

Ozone

Sulphur

5.11 Physical Properties

5.12 Chemical Reactivity

Oxidation states (+II), (+IV) and (+VI)

Bond lengths and pπ – dπ bonding

Differences between oxygen and the other elements

5.13 General Properties of Oxides

Classification based on structure

Classification based on chemical properties

5.14 Oxides of Sulphur

Dioxide SO2

Trioxide SO3

5.15 Oxoacids of Sulphur

The Group 17 Elements – The Halogens

5.16 Extraction and Uses of the Elements

Fluorine

Chlorine

Bromine

Iodine

5.17 General Properties

Size of atoms and ions

Ionization energy

Type of bonds formed and oxidation states

Melting and boiling points

Bond energy in X2 molecules

Oxidizing power

The Group 18 Elements – Noble Gases

5.18 Occurrence and Recovery of the Elements

5.19 Uses of the Elements

5.20 Physical Properties

5.21 Special Properties of Helium

5.22 Chemical Properties of the Noble Gases

Molecular ions formed under excited conditions

Clathrate compounds

Single Correct Choice Type Questions

Assertion-Reasoning Type Questions

Answers

6 The d-Block Elements and their Properties

6.1 Variable Oxidation State

Stability of the various oxidation states

6.2 Complexes

6.3 Size of Atoms and Ions

6.4 Density

6.5 Melting and Boiling Points

6.6 Reactivity of Metals

6.7 Ionization Energy

6.8 Colour

Polarization

Incompletely filled d or f shell

6.9 Magnetic Properties

6.10 Catalytic Properties

6.11 Nonstoichiometry

6.12 Abundance

6.13 Chromate and Dichromate

Preparation

Properties

Tests for chromate (CrO2

4

-

) and dichromate (Cr2O2

7

-) radicals

6.14 Manganate and Permanganate

Preparation

Properties

Tests for permanganate (MnO4

- ) and manganate (MnO2

4

-) radicals

Single Correct Choice Type Questions

Assertion-Reasoning Type Questions

Answers

7 The f-Block Elements and their Properties

7.1 Lanthanoids

Properties of lanthanoids and their ions

Uses of lanthanoids

7.2 Actinoids

Properties of actinoids and their ions

Uses of actinoids

7.3 Comparison between Lanthanoids and Actinoids

Similarities

Differences

Single Correct Choice Type Questions

Assertion-Reasoning Type Questions

Answers

8 Qualitative Salt Analysis

8.1 Test of Carbonate (CO3

2−)

8.2 Tests for Sulphide (S2−) Radical

8.3 Tests for Nitrite (NO2

−) Radical

8.4 Tests for Nitrite (NO3

−) Radical

8.5 Tests for Halide (Cl−, Br−