Physical Chemistry For JEE (Main & Advanced) | By Vipul Mehta | 2nd Edition | Wiley Publication ( English Medium )

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Physical Chemistry For JEE (Main & Advanced) | By Vipul Mehta | 2nd Edition | Wiley Publication ( English Medium ).

Wiley Physical Chemistry for JEE (Main and Advanced) is a comprehensive text for understanding Physical Chemistry with focus on development of problem-solving skills. This adaptation of the book aims to enhance the learning experience of the book, deriving advantage from the adapting author's experience with learning pattern of the students and obstacles in their learning curve. The premise is to encourage self-study in students and help them develop understanding of the concept and build an aptitude to apply the same learning to solve a problem.

Contents:- 

Preface

1 Mole Concept–I

1.1 Basic Concepts

Matter and its Nature

Dalton’s Atomic Theory

Concept of Atom, Molecule, Element and Compound

Representation of Physical Quantities

Precision and Accuracy

Significant Figures

The International System of Units (S.I.)

Physical Quantities and Their Measurements

Dimensional Analysis

1.2 Mole – Basic Introduction

Laws of Chemical Combinations

Law of Conservation of Mass

Law of Definite Proportions

Law of Multiple Proportions

Gay–Lussac’s Law of Gaseous Volumes

Avogadro’s Law

Atomic and Molecular Masses

Mole Concept and Molar Masses

Mole Concept and Number of Atoms/Ions/Molecules

Mole Concept and Volume (L) of Ideal Gas at NTP/STP

1.3 Percentage Composition

Empirical and Molecular Formulae

1.4 Mole Concept – Stoichiometry

Balancing of Chemical Equations

Stoichiometry and Stoichiometric Calculations

Limiting Reagent

Theoretical and Actual Yields

1.5 Principle of Atom Conservation (POAC)

1.6 Concentration Terms

Relation between Stoichiometric Quantities

1.7 Miscellaneous Application of Mole Concept: Gravimetric Analysis [JEE (A) only]

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

2 Redox Reactions

2.1 Oxidation Number Concept

Oxidation Number and Oxidation State

Types of Redox Reactions

2.2 Oxidation and Reduction

Oxidation and Reduction as Electron Transfer Reactions

Displacement Reactions and Activity Series

2.3 Calculation of n-Factor in a Reaction

2.4 Balancing of Redox Reactions

Half-Reaction (Ion Electron) Method

Oxidation Number Method

Fastest Method for Balancing an Equation [JEE (A) only]

2.5 Concept of Equivalent Mass

Normality

2.6 Stoichiometry of Redox Reactions and Concept of Gram Equivalents

2.7 Volumetric Analysis [JEE (A) only]

Some Terms Used in Volumetric Analysis

2.8 Types of Titrations [JEE (A) only]

Redox Titrations

Complexometric Titrations

Precipitation Titrations

Neutralization Titrations

2.9 Applications of Redox Reactions [JEE (A) only]

Volume Strength of H2O2 Solution

Percentage Labeling of Oleum

Other Applications

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

3 Gaseous and Liquid States [JEE (A) only]

3.1 Characteristics of Gases

3.2 Pressure as Measured Property of Gas

Units of Pressure

3.3 Gas Laws

Boyle’s Law

Charles’ Law

Gay–Lussac’s Law

Avogadro’s Law

Combined Gas Laws

3.4 Ideal Gas Law

Dimension and Numerical Values of R

Density and Molar Mass Measurement of a Gas

Illustrations Based on Mercury Column

3.5 Payload

3.6 Variation of Pressure with Change in Density of Fluid

3.7 Faulty Barometer

3.8 Dalton’s Law of Partial Pressures

Relative Humidity

Partial Pressure in Terms of Mole Fraction

3.9 Graham’s Law of Effusion and Diffusion

Variation of Pressure inside a Container during Effusion of a Gas

3.10 Kinetic Theory of Gases

Postulates

Prediction of Gas Laws

Derivation of Kinetic Gas Equation

Kinetic Energy of Gas and Average, Most Probable and Root Mean Square Speeds

Maxwell–Boltzmann Distribution of Molecular Speeds

Derivation of Kinetic Gas Equation

3.11 Molecular Collisions

3.12 Real Gases and Their Deviation from Ideal Gas Behavior

The van der Waals Equation for Deviations from Ideal Behavior

3.13 Compressibility Factor

Virial Equation

3.14 Liquefaction of Gases

Expressions of Critical Constants in Terms of van der Waals Constants

Experimental Methods for Liquefaction of Gases

Joule Thomson Effect

3.15 Law of Corresponding States

3.16 Heat Capacity and Specific Heats of Gases

Heat Capacity at Constant Volume

Heat Capacity at Constant Pressure

3.17 Liquid State

Vapor Pressure

3.18 Intermolecular Forces in Liquids

3.19 Characteristic Properties of Liquids: Surface Tension and Viscosity

Surface Tension

Viscosity

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers 1

4 Solid State [JEE (A) only]

4.1 Classification of Solids

Based on Arrangement of Particles

Based on Nature of Bonds

4.2 Crystal Lattices and Unit Cells

Crystal Systems

Bravais Lattices

4.3 Calculations Involving Unit Cell Dimensions

4.4 Cubic Lattice – Simple, Face Centered and Body Centered

4.5 Close-Packing in Crystals

Close Packing in One Dimension

Close Packing in Two Dimensions

Close Packing in Three Dimensions

4.6 Packing Efficiency and Packing Fraction

Calculation of Height of Unit Cell in Hexagonal Close Packing

4.7 Tetrahedral and Octahedral Voids

Tetrahedral Voids

Octahedral Voids

Formula of a Compound and the Number of Voids Filled

4.8 Radius Ratio Rule and Ionic Radius

Mathematical Calculation for Critical Radius Ratio

Ionic Radius

4.9 Simple Ionic Compounds

Rock Salt (or NaCl) Type of Structure

Sphalerite or Zinc Blende (ZnS) Structure

Fluorite Structure (CaF2 )

Caesium Chloride (CsCl) Type of Structure

Perovskite Structure

Antifluorite Structure (Na2O)

Structure of Diamond

Corundum Structure

Rutile Structure

Spinel Structure

Inverse Spinel Structure

Structure of Oxides of Iron

Effect of Temperature/Pressure on Crystal Structure

4.10 X-Ray Diffraction Used to Study Crystal Structures (Bragg’s Law)

Miller Indices for Crystallographic Planes in Cubic Unit Cells

4.11 Defects in Crystals

Types of Point Defects

4.12 Electrical Properties of Solids

Conduction of Electricity in Metals

Conduction of Electricity in Semiconductors

4.13 Magnetic Properties of Solids

4.14 Dielectric Properties of Solids

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

5 Atomic Structure

5.1 Discovery of Electron

Thomson Experiment – Determination of Mass to Charge Ratio

Millikan Oil Drop Experiment – Charge on an Electron

5.2 Discovery of Protons and Neutrons

Anode Ray Experiment

5.3 Some Prerequisites of Physics

5.4 Atomic Models

Thomson Model of Atom

Rutherford’s Nuclear Model of Atom

Drawbacks of Rutherford Model

5.5 Representation of Atom with Electrons and Neutrons

Isobars and Isotopes

Isotones, Isodiaphers and Nuclear Isomers

5.6 Nature of Waves

5.7 Nature of Electromagnetic Radiation

Wave Nature of Electromagnetic Radiation

5.8 Planck’s Quantum Theory

Blackbody Radiation

5.9 Spectra – Continuous and Discontinuous Spectrum

Atomic Spectra

5.10 Bohr’s Model for Hydrogen Atom

Bohr’s Postulates

Radius of Bohr Orbits in Hydrogen

Velocity of Electron

Energy of Electron in Hydrogen Atom

Ionization Energy (Enthalpy)

Line Spectra of Hydrogen

Limitations of Bohr’s Model

Bohr–Sommerfeld Model [JEE (A) only]

5.11 Photoelectric Effect

Detailed Analysis of Photoelectric Effect

5.12 Dual Nature of Matter

de Broglie Equation

5.13 Heisenberg’s Uncertainty Principle

Significance of Uncertainty Principle

5.14 Number of Waves Made by the Electron [JEE (A) only]

5.15 Quantum Mechanical Model of Atom

Hydrogen Atom and the Schrödinger Equation

Important Features of Quantum Mechanical Model

5.16 Radial and Angular Wave Functions

Radial Distribution Curve

Plot of Angular Wave Function

Plot of Total Wave Function

5.17 Orbitals and Quantum Numbers

Selection Rules Governing Allowed Combinations of Quantum Numbers

Shapes of Atomic Orbitals

Electron Spin and Spin Quantum Number

Energies of Orbitals

Effective Nuclear Charge

5.18 Electronic Configuration of Atoms

Aufbau Principle

Hund’s Rule of Maximum Multiplicity

Pauli’s Exclusion Principle

Writing Electronic Configuration

Explanation for Exceptions in Electronic Configuration in Cu and Cr

5.19 Magnetic Properties

Relation of Colour with Paramagnetic and Diamagnetic Species

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

6 Chemical Bonding

6.1 Chemical Bond Formation – Kössel–Lewis Approach

Concept of Electrovalent Bond (or Ionic Bond)

Concept of Covalent Bond

Exceptions to the Octet Rule

6.2 Lewis Structures of Simple Molecules

6.3 Formal Charge

Calculating the Formal Charge on an Atom

6.4 Covalent Bonding

Formation of Covalent Bond

6.5 Coordinate or Dative Bonding

6.6 Valence Bond Theory

Orbital Overlap Concept

Bonding as an Overlap of Atomic Orbitals

6.7 Hybridization

Salient Features of Hybridization

Calculation of Steric Number

Some Examples of Hybridization

Hybridization in Ethane, Ethene and Ethyne

Hybridization of Elements Involving d Orbitals

6.8 The Valence Shell Electron Pair Repulsion (VSEPR) Theory and Shapes of Simple Molecules

Molecular Geometry Based on Number of Electron Pairs

Molecular Geometry in Presence One or More Lone Pairs on Central Atom

Some Examples of Effect of Electronegativity on Molecular Geometry

Drago’s Rule

6.9 Back Bonding [JEE (A) only]

Bridge Bonding

6.10 Ionic Bonding

Formation of Ionic Bond

Lattice Enthalpy

Born–Haber Cycle

Properties of Ionic Compounds

Concept of Electronegativity and Fajans’ Rules

Fajans’ Rules – Covalent Character of Ionic Bonds

Polarity of Bonds and Dipole Moment

6.11 Dipole Moment

Applications of Dipole Moment

6.12 Resonance Structures

6.13 Hydrogen Bonding

Consequences of Hydrogen Bonding

Applications of Hydrogen Bond

6.14 Molecular Orbital Theory

Formation of Molecular Orbitals by Linear Combination of Atomic Orbitals (LCAO)

Conditions for the Combination of Atomic Orbitals

Types of Molecular Orbitals

Energy Level Diagram for Molecular Orbitals

6.15 Concept of Bond Order, Bond Length and Bond Energy

Stability of the Molecules

Magnetic Properties

6.16 Bonding in Some Homonuclear Diatomic Molecules

6.17 Heteronuclear Diatomic Molecules [JEE (A) only]

6.18 Elementary Idea of Metallic Bonding [JEE (A) only]

Electron Sea Model

Band Theory or Molecular Orbital Theory

6.19 Weak Forces [JEE (A) only]

Repulsive Intermolecular Forces

6.20 Interactions between Ions and Covalent Molecules [JEE (A) only]

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

7 Chemical Energetics

7.1 Fundamentals of Thermodynamics

System and its Surroundings

Types of the System

Thermodynamic Properties

Types of Thermodynamic Processes

7.2 The Zeroth Law of Thermodynamics

7.3 Energy of the Thermodynamic System

Internal Energy

Work

Heat

7.4 The First Law of Thermodynamics

Mathematical Derivation of First Law

7.5 Calculation of Work Done in Different Processes

7.6 Enthalpy or Heat Content, H

Mathematical Derivation of ΔH [JEE (A) only]

Relationship between ΔU and ΔH

7.7 Expansion and Compression of an Ideal Gas

Isothermal Expansion or Compression

Adiabatic Expansion or Compression

Isobaric and Isochoric Processes

7.8 Joule–Thomson Effect and Inversion Temperature [JEE (A) only]

7.9 Calorimetry

ΔU Measurement

ΔH Measurement

7.10 Thermochemistry

Enthalpy Changes During Phase Transformations

Enthalpy of Formation

Enthalpy of Reaction

7.11 Thermochemical Equations

7.12 Laws of Thermochemistry

Lavoisier–Laplace Law

Hess’s Law of Constant Heat Summation

7.13 Enthalpies of Different Types of Reactions

Enthalpy of Neutralization

Standard Enthalpy of Combustion (Symbol: ΔcHo)

Enthalpy of Atomization (Symbol: ΔaHo)

Enthalpy of Solution (Symbol: ΔsolHo)

7.14 Bond Enthalpy and Bond Dissociation Enthalpy

Lattice Enthalpy

7.15 Spontaneity

Enthalpy a Criterion for Spontaneity

7.16 Carnot Cycle [JEE (A) only]

7.17 Entropy and Spontaneity

Calculation of ΔS for Different Processes

Factors Affecting Entropy

Entropy of Physical Changes

Entropy of Chemical Changes

7.18 Gibbs Energy and Spontaneity

Mathematical Derivation of ΔG [JEE (A) only]

7.19 Second Law of Thermodynamics

7.20 Gibbs Energy Change and Equilibrium

Calculation of ΔG

Gibb’s Helmholtz Equation [JEE (A) only]

Chemical Potential of Multicomponent System [JEE (A) only]

van ’t Hoff Reaction Isotherm and Equations [JEE (A) only]

7.21 Third Law of Thermodynamics

T–S Curves for Different Processes [JEE (A) only]

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

8 Solutions

8.1 Type of Solutions

8.2 Solubility

Factors Affecting Solubility

8.3 Effect of Nature of Solute and Solvent

8.4 Effect of Temperature on Solubility

8.5 Effect of Pressure on Solubility of Gases

Henry’s Law Relates Gas Solubility to Pressure

8.6 Different Methods for Expressing Concentration of Solution

Conversions Among Concentration Units

8.7 Vapor Pressure of Solutions

Raoult’s Law

Vapor Pressure of Liquid–Liquid Solutions

Vapor Pressure of Solutions of Solids in Liquids

8.8 Enthalpy of Solution

8.9 Ideal Solutions

Vapor Pressure of Ideal Binary Liquid Solution

8.10 Non-Ideal Solutions

Azeotropic (Constant Boiling) Mixtures

8.11 Colligative Properties and Determination of Molar Mass

Relative Lowering of Vapor Pressure

Elevation of Boiling Point

Depression in Freezing Point

Osmotic Pressure

8.12 Abnormal Molar Masses and van ’t Hoff Factor

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

9 Chemical Equilibrium

9.1 Physical Equilibria

Solid–Liquid Equilibrium

Liquid–Vapor Equilibrium

Solid–Vapor Equilibrium

Equilibrium in Dissolution of Solids and Gases in Liquids and Henry’s Law

Characteristics of Physical Equilibria

9.2 Chemical Equilibria – Dynamic Equilibrium

9.3 Law of Chemical Equilibrium and Equilibrium Constant

Law of Mass Action

Equilibrium Constants Kp and KC

Units of Kp and KC

Characteristics of Equilibrium Constant

9.4 Homogeneous and Heterogeneous Equilibria

9.5 Applications of Equilibrium Constants

Predicting the Extent of Reaction

Predicting the Direction of Reaction

Calculating Equilibrium Concentrations

Degree of Dissociation

9.6 Gibbs Energy Change and Chemical Equilibrium

9.7 Simultaneous Equilibrium

9.8 Le Chatelier’s Principle and Factors Affecting Equilibria

Effect of Change in Concentration

Effect of Change in Pressure

Effect of Change of Volume

Effect of Change in Temperature

Effect of Addition of Inert Gas

Some Special Cases [JEE (A) only]

Effect of Adding Catalyst

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

10 Ionic Equilibrium 669

10.1 Weak and Strong Electrolytes

10.2 Ionization of Electrolytes

Ostwald’s Dilution Law

Common Ion Effect

10.3 Concepts of Acids and Bases

Arrhenius Concept

Brönsted–Lowry Concept

Lewis Concept of Acids and Bases

10.4 Acid–Base Equilibria and Ionization Constants

Ionization Constants of Weak Acids

Ionization Constants of Weak Bases

Ionic Product of Water

pH Concept

Deriving Relation between Ka and Kb

10.5 Relative Strength of Acids and Bases

10.6 Ionization of Polyprotic Acids

10.7 Factors Affecting Acid Strength

10.8 Acid–Base Neutralization – Formation of Salts

10.9 pH Calculation of Single Monobasic Acid or Monoacidic Base

Charge and Mass Balance [JEE (A) only]

10.10 pH Calculation of a Mixture of Two Acids or Bases [JEE (A) only]

pH of Mixture of Strong Acids in Water

10.11 pH Calculation for Polyprotic Acids [JEE (A) only]

10.12 Hydrolysis of Salts and pH of Their Solutions

Salt of Strong Acid and Strong Base

Salt of Weak Acid and Strong Base

Salt of Strong Acid and Weak Base

Salt of Weak Acid and Weak Base

Salts of Weak Polyprotic Acids [JEE (A) only]

pH Calculation of Amphoteric and Amphiprotic Ions [JEE (A) only]

10.13 Buffer Solutions

Identification of Buffer

pH of Buffer Solutions: Henderson–Hasselbalch Equation

Salt Buffer [JEE (A) only]

Buffer Capacity [JEE (A) only]

Buffer Range [JEE (A) only]

10.14 Acid–Base Titrations [JEE (A) only]

Strong Acid vs. Strong Base

Weak Acid vs. Strong Base

Weak Base vs. Strong Acid

Titration Curves for Diprotic Acids

10.15 Theory of Indicators [JEE (A) only]

Working of Indicators

Ostwald and Quinoid Selection of Indicators

10.16 Solubility Equilibria of Sparingly Soluble Salts

Solubility Product Constant

Calculation of Solubility of Salts

Effect of Common Ion on Solubility

Effect of Hydrolysis on Solubility

Effect of pH on Solubility [JEE (A) only]

10.17 Preferential Precipitation of Salts [JEE (A) only]

10.18 Applications of Solubility Product

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

11 Electrochemistry

11.1 Electrochemical Cells

Galvanic Cell

11.2 Electrode Potential

Oxidation and Reduction Potential

Potential of a Cell or EMF

Reversible and Irreversible Cells

Electrochemical Conventions

11.3 Measurement of Electrode Potential

Some Reference Electrodes [JEE (A) only]

Electrochemical Series

11.4 Thermodynamics of a Cell

Cell Potential and Gibbs Energy Change

Calculation of Cell Potential and Other Thermodynamic Parameters

11.5 Nernst Equation

Equilibrium Constant from Nernst Equation

Applications of Nernst Equation

11.6 Calculation of E.

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Product Details

SKU / BOOK Code:	Wiley-Vipul-Jee-phy-chemtry(E)
Publisher:	Wiley Publication
Author:	By Vipul Mehta
Binding Type:	Paperback
No. of Pages:	1074
ISBN-10:	9357468919
ISBN-13:	978-9357468916
Edition:	2nd Edition
Language:	English Medium
Publish Year:	2024-07
Weight (g):	500
Product Condition:	New
Reading Age:	Above 10 Years
Country of Origin:	India
Genre:	Book
Manufacturer:	As Per Publisher
Importer:	Not Applicable
Packer:	Fulfilled by The Supplier

Product Description

Physical Chemistry For JEE (Main & Advanced) | By Vipul Mehta | 2nd Edition | Wiley Publication ( English Medium ).

Wiley Physical Chemistry for JEE (Main and Advanced) is a comprehensive text for understanding Physical Chemistry with focus on development of problem-solving skills. This adaptation of the book aims to enhance the learning experience of the book, deriving advantage from the adapting author's experience with learning pattern of the students and obstacles in their learning curve. The premise is to encourage self-study in students and help them develop understanding of the concept and build an aptitude to apply the same learning to solve a problem.

Contents:- 

Preface

1 Mole Concept–I

1.1 Basic Concepts

Matter and its Nature

Dalton’s Atomic Theory

Concept of Atom, Molecule, Element and Compound

Representation of Physical Quantities

Precision and Accuracy

Significant Figures

The International System of Units (S.I.)

Physical Quantities and Their Measurements

Dimensional Analysis

1.2 Mole – Basic Introduction

Laws of Chemical Combinations

Law of Conservation of Mass

Law of Definite Proportions

Law of Multiple Proportions

Gay–Lussac’s Law of Gaseous Volumes

Avogadro’s Law

Atomic and Molecular Masses

Mole Concept and Molar Masses

Mole Concept and Number of Atoms/Ions/Molecules

Mole Concept and Volume (L) of Ideal Gas at NTP/STP

1.3 Percentage Composition

Empirical and Molecular Formulae

1.4 Mole Concept – Stoichiometry

Balancing of Chemical Equations

Stoichiometry and Stoichiometric Calculations

Limiting Reagent

Theoretical and Actual Yields

1.5 Principle of Atom Conservation (POAC)

1.6 Concentration Terms

Relation between Stoichiometric Quantities

1.7 Miscellaneous Application of Mole Concept: Gravimetric Analysis [JEE (A) only]

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

2 Redox Reactions

2.1 Oxidation Number Concept

Oxidation Number and Oxidation State

Types of Redox Reactions

2.2 Oxidation and Reduction

Oxidation and Reduction as Electron Transfer Reactions

Displacement Reactions and Activity Series

2.3 Calculation of n-Factor in a Reaction

2.4 Balancing of Redox Reactions

Half-Reaction (Ion Electron) Method

Oxidation Number Method

Fastest Method for Balancing an Equation [JEE (A) only]

2.5 Concept of Equivalent Mass

Normality

2.6 Stoichiometry of Redox Reactions and Concept of Gram Equivalents

2.7 Volumetric Analysis [JEE (A) only]

Some Terms Used in Volumetric Analysis

2.8 Types of Titrations [JEE (A) only]

Redox Titrations

Complexometric Titrations

Precipitation Titrations

Neutralization Titrations

2.9 Applications of Redox Reactions [JEE (A) only]

Volume Strength of H2O2 Solution

Percentage Labeling of Oleum

Other Applications

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

3 Gaseous and Liquid States [JEE (A) only]

3.1 Characteristics of Gases

3.2 Pressure as Measured Property of Gas

Units of Pressure

3.3 Gas Laws

Boyle’s Law

Charles’ Law

Gay–Lussac’s Law

Avogadro’s Law

Combined Gas Laws

3.4 Ideal Gas Law

Dimension and Numerical Values of R

Density and Molar Mass Measurement of a Gas

Illustrations Based on Mercury Column

3.5 Payload

3.6 Variation of Pressure with Change in Density of Fluid

3.7 Faulty Barometer

3.8 Dalton’s Law of Partial Pressures

Relative Humidity

Partial Pressure in Terms of Mole Fraction

3.9 Graham’s Law of Effusion and Diffusion

Variation of Pressure inside a Container during Effusion of a Gas

3.10 Kinetic Theory of Gases

Postulates

Prediction of Gas Laws

Derivation of Kinetic Gas Equation

Kinetic Energy of Gas and Average, Most Probable and Root Mean Square Speeds

Maxwell–Boltzmann Distribution of Molecular Speeds

Derivation of Kinetic Gas Equation

3.11 Molecular Collisions

3.12 Real Gases and Their Deviation from Ideal Gas Behavior

The van der Waals Equation for Deviations from Ideal Behavior

3.13 Compressibility Factor

Virial Equation

3.14 Liquefaction of Gases

Expressions of Critical Constants in Terms of van der Waals Constants

Experimental Methods for Liquefaction of Gases

Joule Thomson Effect

3.15 Law of Corresponding States

3.16 Heat Capacity and Specific Heats of Gases

Heat Capacity at Constant Volume

Heat Capacity at Constant Pressure

3.17 Liquid State

Vapor Pressure

3.18 Intermolecular Forces in Liquids

3.19 Characteristic Properties of Liquids: Surface Tension and Viscosity

Surface Tension

Viscosity

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers 1

4 Solid State [JEE (A) only]

4.1 Classification of Solids

Based on Arrangement of Particles

Based on Nature of Bonds

4.2 Crystal Lattices and Unit Cells

Crystal Systems

Bravais Lattices

4.3 Calculations Involving Unit Cell Dimensions

4.4 Cubic Lattice – Simple, Face Centered and Body Centered

4.5 Close-Packing in Crystals

Close Packing in One Dimension

Close Packing in Two Dimensions

Close Packing in Three Dimensions

4.6 Packing Efficiency and Packing Fraction

Calculation of Height of Unit Cell in Hexagonal Close Packing

4.7 Tetrahedral and Octahedral Voids

Tetrahedral Voids

Octahedral Voids

Formula of a Compound and the Number of Voids Filled

4.8 Radius Ratio Rule and Ionic Radius

Mathematical Calculation for Critical Radius Ratio

Ionic Radius

4.9 Simple Ionic Compounds

Rock Salt (or NaCl) Type of Structure

Sphalerite or Zinc Blende (ZnS) Structure

Fluorite Structure (CaF2 )

Caesium Chloride (CsCl) Type of Structure

Perovskite Structure

Antifluorite Structure (Na2O)

Structure of Diamond

Corundum Structure

Rutile Structure

Spinel Structure

Inverse Spinel Structure

Structure of Oxides of Iron

Effect of Temperature/Pressure on Crystal Structure

4.10 X-Ray Diffraction Used to Study Crystal Structures (Bragg’s Law)

Miller Indices for Crystallographic Planes in Cubic Unit Cells

4.11 Defects in Crystals

Types of Point Defects

4.12 Electrical Properties of Solids

Conduction of Electricity in Metals

Conduction of Electricity in Semiconductors

4.13 Magnetic Properties of Solids

4.14 Dielectric Properties of Solids

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

5 Atomic Structure

5.1 Discovery of Electron

Thomson Experiment – Determination of Mass to Charge Ratio

Millikan Oil Drop Experiment – Charge on an Electron

5.2 Discovery of Protons and Neutrons

Anode Ray Experiment

5.3 Some Prerequisites of Physics

5.4 Atomic Models

Thomson Model of Atom

Rutherford’s Nuclear Model of Atom

Drawbacks of Rutherford Model

5.5 Representation of Atom with Electrons and Neutrons

Isobars and Isotopes

Isotones, Isodiaphers and Nuclear Isomers

5.6 Nature of Waves

5.7 Nature of Electromagnetic Radiation

Wave Nature of Electromagnetic Radiation

5.8 Planck’s Quantum Theory

Blackbody Radiation

5.9 Spectra – Continuous and Discontinuous Spectrum

Atomic Spectra

5.10 Bohr’s Model for Hydrogen Atom

Bohr’s Postulates

Radius of Bohr Orbits in Hydrogen

Velocity of Electron

Energy of Electron in Hydrogen Atom

Ionization Energy (Enthalpy)

Line Spectra of Hydrogen

Limitations of Bohr’s Model

Bohr–Sommerfeld Model [JEE (A) only]

5.11 Photoelectric Effect

Detailed Analysis of Photoelectric Effect

5.12 Dual Nature of Matter

de Broglie Equation

5.13 Heisenberg’s Uncertainty Principle

Significance of Uncertainty Principle

5.14 Number of Waves Made by the Electron [JEE (A) only]

5.15 Quantum Mechanical Model of Atom

Hydrogen Atom and the Schrödinger Equation

Important Features of Quantum Mechanical Model

5.16 Radial and Angular Wave Functions

Radial Distribution Curve

Plot of Angular Wave Function

Plot of Total Wave Function

5.17 Orbitals and Quantum Numbers

Selection Rules Governing Allowed Combinations of Quantum Numbers

Shapes of Atomic Orbitals

Electron Spin and Spin Quantum Number

Energies of Orbitals

Effective Nuclear Charge

5.18 Electronic Configuration of Atoms

Aufbau Principle

Hund’s Rule of Maximum Multiplicity

Pauli’s Exclusion Principle

Writing Electronic Configuration

Explanation for Exceptions in Electronic Configuration in Cu and Cr

5.19 Magnetic Properties

Relation of Colour with Paramagnetic and Diamagnetic Species

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

6 Chemical Bonding

6.1 Chemical Bond Formation – Kössel–Lewis Approach

Concept of Electrovalent Bond (or Ionic Bond)

Concept of Covalent Bond

Exceptions to the Octet Rule

6.2 Lewis Structures of Simple Molecules

6.3 Formal Charge

Calculating the Formal Charge on an Atom

6.4 Covalent Bonding

Formation of Covalent Bond

6.5 Coordinate or Dative Bonding

6.6 Valence Bond Theory

Orbital Overlap Concept

Bonding as an Overlap of Atomic Orbitals

6.7 Hybridization

Salient Features of Hybridization

Calculation of Steric Number

Some Examples of Hybridization

Hybridization in Ethane, Ethene and Ethyne

Hybridization of Elements Involving d Orbitals

6.8 The Valence Shell Electron Pair Repulsion (VSEPR) Theory and Shapes of Simple Molecules

Molecular Geometry Based on Number of Electron Pairs

Molecular Geometry in Presence One or More Lone Pairs on Central Atom

Some Examples of Effect of Electronegativity on Molecular Geometry

Drago’s Rule

6.9 Back Bonding [JEE (A) only]

Bridge Bonding

6.10 Ionic Bonding

Formation of Ionic Bond

Lattice Enthalpy

Born–Haber Cycle

Properties of Ionic Compounds

Concept of Electronegativity and Fajans’ Rules

Fajans’ Rules – Covalent Character of Ionic Bonds

Polarity of Bonds and Dipole Moment

6.11 Dipole Moment

Applications of Dipole Moment

6.12 Resonance Structures

6.13 Hydrogen Bonding

Consequences of Hydrogen Bonding

Applications of Hydrogen Bond

6.14 Molecular Orbital Theory

Formation of Molecular Orbitals by Linear Combination of Atomic Orbitals (LCAO)

Conditions for the Combination of Atomic Orbitals

Types of Molecular Orbitals

Energy Level Diagram for Molecular Orbitals

6.15 Concept of Bond Order, Bond Length and Bond Energy

Stability of the Molecules

Magnetic Properties

6.16 Bonding in Some Homonuclear Diatomic Molecules

6.17 Heteronuclear Diatomic Molecules [JEE (A) only]

6.18 Elementary Idea of Metallic Bonding [JEE (A) only]

Electron Sea Model

Band Theory or Molecular Orbital Theory

6.19 Weak Forces [JEE (A) only]

Repulsive Intermolecular Forces

6.20 Interactions between Ions and Covalent Molecules [JEE (A) only]

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

7 Chemical Energetics

7.1 Fundamentals of Thermodynamics

System and its Surroundings

Types of the System

Thermodynamic Properties

Types of Thermodynamic Processes

7.2 The Zeroth Law of Thermodynamics

7.3 Energy of the Thermodynamic System

Internal Energy

Work

Heat

7.4 The First Law of Thermodynamics

Mathematical Derivation of First Law

7.5 Calculation of Work Done in Different Processes

7.6 Enthalpy or Heat Content, H

Mathematical Derivation of ΔH [JEE (A) only]

Relationship between ΔU and ΔH

7.7 Expansion and Compression of an Ideal Gas

Isothermal Expansion or Compression

Adiabatic Expansion or Compression

Isobaric and Isochoric Processes

7.8 Joule–Thomson Effect and Inversion Temperature [JEE (A) only]

7.9 Calorimetry

ΔU Measurement

ΔH Measurement

7.10 Thermochemistry

Enthalpy Changes During Phase Transformations

Enthalpy of Formation

Enthalpy of Reaction

7.11 Thermochemical Equations

7.12 Laws of Thermochemistry

Lavoisier–Laplace Law

Hess’s Law of Constant Heat Summation

7.13 Enthalpies of Different Types of Reactions

Enthalpy of Neutralization

Standard Enthalpy of Combustion (Symbol: ΔcHo)

Enthalpy of Atomization (Symbol: ΔaHo)

Enthalpy of Solution (Symbol: ΔsolHo)

7.14 Bond Enthalpy and Bond Dissociation Enthalpy

Lattice Enthalpy

7.15 Spontaneity

Enthalpy a Criterion for Spontaneity

7.16 Carnot Cycle [JEE (A) only]

7.17 Entropy and Spontaneity

Calculation of ΔS for Different Processes

Factors Affecting Entropy

Entropy of Physical Changes

Entropy of Chemical Changes

7.18 Gibbs Energy and Spontaneity

Mathematical Derivation of ΔG [JEE (A) only]

7.19 Second Law of Thermodynamics

7.20 Gibbs Energy Change and Equilibrium

Calculation of ΔG

Gibb’s Helmholtz Equation [JEE (A) only]

Chemical Potential of Multicomponent System [JEE (A) only]

van ’t Hoff Reaction Isotherm and Equations [JEE (A) only]

7.21 Third Law of Thermodynamics

T–S Curves for Different Processes [JEE (A) only]

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

8 Solutions

8.1 Type of Solutions

8.2 Solubility

Factors Affecting Solubility

8.3 Effect of Nature of Solute and Solvent

8.4 Effect of Temperature on Solubility

8.5 Effect of Pressure on Solubility of Gases

Henry’s Law Relates Gas Solubility to Pressure

8.6 Different Methods for Expressing Concentration of Solution

Conversions Among Concentration Units

8.7 Vapor Pressure of Solutions

Raoult’s Law

Vapor Pressure of Liquid–Liquid Solutions

Vapor Pressure of Solutions of Solids in Liquids

8.8 Enthalpy of Solution

8.9 Ideal Solutions

Vapor Pressure of Ideal Binary Liquid Solution

8.10 Non-Ideal Solutions

Azeotropic (Constant Boiling) Mixtures

8.11 Colligative Properties and Determination of Molar Mass

Relative Lowering of Vapor Pressure

Elevation of Boiling Point

Depression in Freezing Point

Osmotic Pressure

8.12 Abnormal Molar Masses and van ’t Hoff Factor

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

9 Chemical Equilibrium

9.1 Physical Equilibria

Solid–Liquid Equilibrium

Liquid–Vapor Equilibrium

Solid–Vapor Equilibrium

Equilibrium in Dissolution of Solids and Gases in Liquids and Henry’s Law

Characteristics of Physical Equilibria

9.2 Chemical Equilibria – Dynamic Equilibrium

9.3 Law of Chemical Equilibrium and Equilibrium Constant

Law of Mass Action

Equilibrium Constants Kp and KC

Units of Kp and KC

Characteristics of Equilibrium Constant

9.4 Homogeneous and Heterogeneous Equilibria

9.5 Applications of Equilibrium Constants

Predicting the Extent of Reaction

Predicting the Direction of Reaction

Calculating Equilibrium Concentrations

Degree of Dissociation

9.6 Gibbs Energy Change and Chemical Equilibrium

9.7 Simultaneous Equilibrium

9.8 Le Chatelier’s Principle and Factors Affecting Equilibria

Effect of Change in Concentration

Effect of Change in Pressure

Effect of Change of Volume

Effect of Change in Temperature

Effect of Addition of Inert Gas

Some Special Cases [JEE (A) only]

Effect of Adding Catalyst

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

10 Ionic Equilibrium 669

10.1 Weak and Strong Electrolytes

10.2 Ionization of Electrolytes

Ostwald’s Dilution Law

Common Ion Effect

10.3 Concepts of Acids and Bases

Arrhenius Concept

Brönsted–Lowry Concept

Lewis Concept of Acids and Bases

10.4 Acid–Base Equilibria and Ionization Constants

Ionization Constants of Weak Acids

Ionization Constants of Weak Bases

Ionic Product of Water

pH Concept

Deriving Relation between Ka and Kb

10.5 Relative Strength of Acids and Bases

10.6 Ionization of Polyprotic Acids

10.7 Factors Affecting Acid Strength

10.8 Acid–Base Neutralization – Formation of Salts

10.9 pH Calculation of Single Monobasic Acid or Monoacidic Base

Charge and Mass Balance [JEE (A) only]

10.10 pH Calculation of a Mixture of Two Acids or Bases [JEE (A) only]

pH of Mixture of Strong Acids in Water

10.11 pH Calculation for Polyprotic Acids [JEE (A) only]

10.12 Hydrolysis of Salts and pH of Their Solutions

Salt of Strong Acid and Strong Base

Salt of Weak Acid and Strong Base

Salt of Strong Acid and Weak Base

Salt of Weak Acid and Weak Base

Salts of Weak Polyprotic Acids [JEE (A) only]

pH Calculation of Amphoteric and Amphiprotic Ions [JEE (A) only]

10.13 Buffer Solutions

Identification of Buffer

pH of Buffer Solutions: Henderson–Hasselbalch Equation

Salt Buffer [JEE (A) only]

Buffer Capacity [JEE (A) only]

Buffer Range [JEE (A) only]

10.14 Acid–Base Titrations [JEE (A) only]

Strong Acid vs. Strong Base

Weak Acid vs. Strong Base

Weak Base vs. Strong Acid

Titration Curves for Diprotic Acids

10.15 Theory of Indicators [JEE (A) only]

Working of Indicators

Ostwald and Quinoid Selection of Indicators

10.16 Solubility Equilibria of Sparingly Soluble Salts

Solubility Product Constant

Calculation of Solubility of Salts

Effect of Common Ion on Solubility

Effect of Hydrolysis on Solubility

Effect of pH on Solubility [JEE (A) only]

10.17 Preferential Precipitation of Salts [JEE (A) only]

10.18 Applications of Solubility Product

Solved Objective Questions from Previous Year Papers

Review Questions

Numerical Problems

Additional Objective Questions

Answers

11 Electrochemistry

11.1 Electrochemical Cells

Galvanic Cell

11.2 Electrode Potential

Oxidation and Reduction Potential

Potential of a Cell or EMF

Reversible and Irreversible Cells

Electrochemical Conventions

11.3 Measurement of Electrode Potential

Some Reference Electrodes [JEE (A) only]

Electrochemical Series

11.4 Thermodynamics of a Cell

Cell Potential and Gibbs Energy Change

Calculation of Cell Potential and Other Thermodynamic Parameters

11.5 Nernst Equation

Equilibrium Constant from Nernst Equation

Applications of Nernst Equation

11.6 Calculation of E.

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