Wiley's Physical Chemistry for JEE (Main & Advanced), 2020

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Cover Half Title Title Page Copyright Page Preface Table of Contents 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 Solved Objective Questions from Previous Year Papers Review Questions Numerical Problems Additional Objective Questions Answers 2 Mole Concept–II 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 2.5 Concept of Equivalent Mass Normality 2.6 Stoichiometry of Redox Reactions and Concept of Gram Equivalents 2.7 Volumetric Analysis Some Terms Used in Volumetric Analysis 2.8 Types of Titrations Redox Titrations Complexometric Titrations Precipitation Titrations Neutralization Titrations 2.9 Applications of Redox Reactions 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 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 4 Solid State 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 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 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 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 6.18 Elementary Idea of Metallic Bonding Electron Sea Model Band Theory or Molecular Orbital Theory 6.19 Weak Forces Repulsive Intermolecular Forces 6.20 Interactions between Ions and Covalent Molecules 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 .H Relationship between .U and .H 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 7.9 Calorimetry △U Measurement △H 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: .cHo) Enthalpy of Atomization (Symbol: .aHo) Enthalpy of Solution (Symbol: .solHo) 7.14 Bond Enthalpy and Bond Dissociation Enthalpy Lattice Enthalpy 7.15 Spontaneity Enthalpy a Criterion for Spontaneity 7.16 Carnot Cycle 7.17 Entropy and Spontaneity Calculation of .S for Different Processes Factors Affecting Entropy Entropy of Physical Changes Entropy of Chemical Changes 7.18 Gibbs Energy and Spontaneity Mathematical Derivation of .G 7.19 Second Law of Thermodynamics 7.20 Gibbs Energy Change and Equilibrium Calculation of .G Gibb’s Helmholtz Equation Chemical Potential of Multicomponent System van ’t Hoff Reaction Isotherm and Equations 7.21 Third Law of Thermodynamics T–S Curves for Different Processes 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 Effect of Adding Catalyst Solved Objective Questions from Previous Year Papers Review Questions Numerical Problems Additional Objective Questions Answers 10 Ionic Equilibrium 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 10.10 pH Calculation of a Mixture of Two Acids or Bases pH of Mixture of Strong Acids in Water 10.11 pH Calculation for Polyprotic Acids 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 pH Calculation of Amphoteric and Amphiprotic Ions 10.13 Buffer Solutions Identification of Buffer pH of Buffer Solutions: Henderson–Hasselbalch Equation Salt Buffer Buffer Capacity Buffer Range 10.14 Acid–Base Titrations 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 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 10.17 Preferential Precipitation of Salts 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 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° cell 11.7 Types of Electrodes 11.8 Concentration Cells Electrode Concentration Cells Electrolyte Concentration Cells Applications of Concentration Cells 11.9 Electrolytic Cells and Electrolysis Faraday’s Laws of Electrolysis Products Formed in Electrolysis Transport (Transference) Number 11.10 Applications of Electrolytic Process Corrosion and its Prevention Electroplating Purification of Metals Electrometallurgy Preparation of Compounds 11.11 Batteries Primary Cells Secondary (Storage) Cells Lithium Batteries Fuel Cells 11.12 Electrical Conductance Metallic Conductors Electrolytic Conductors 11.13 Conductance in Solutions of Electrolytes Interionic Attraction Theory of Conductance Electrical Resistance and Conductance Measurement of the Conductance of Ionic Solutions Molar and Equivalent Conductance Kohlrausch’s Law Applications of Kohlrausch Law of Independent Ionic Migration 11.14 Conductometric Titrations Strong Acid vs. Strong Base Weak Base vs. Strong Acid Weak Acid vs. Strong Base Mixture of Acids vs. Strong Base AgNO3 vs. NaCl Solved Objective Questions from Previous Year Papers Review Questions Numerical Problems Additional Objective Questions Answers 12 Chemical Kinetics 12.1 Rate of a Chemical Reaction Average and Instantaneous Rates 12.2 Factors Influencing Rate of a Reaction 12.3 Differential Rate Expression and Rate Constant 12.4 Elementary and Complex Reactions 12.5 Molecularity of a Reaction 12.6 Order of a Reaction Units of Rate Constant 12.7 Calculations of Order and Molecularity Based on Reaction Mechanisms 12.8 Pseudo Order Reactions 12.9 Integrated Rate Equations Zero Order Reactions First Order Reactions Second Order Reactions Third Order Reactions Higher nth Order Reactions Replacement of Concentration Terms by other Variables in First Order Reactions 12.10 Half-Life of Reactions and Radioactivity Radioactivity 12.11 Derivation of Rate Laws for Complex Reactions Using Integrated Rate Equations Consecutive or Sequential Reactions Parallel Reactions Reversible or Opposing Reactions 12.12 Determination of Order of Simple Reactions – Experimental Methods 12.13 Effect of Temperature – Arrhenius Theory Activated Complex Theory and Concept of Activation Energy Arrhenius Equation and Calculation of Activation Energy 12.14 Effect of Catalyst 12.15 Collision Theory Limitation of Collision Theory Rising Temperature Increases Reaction Rate Solved Objective Questions from Previous Year Papers Review Questions Numerical Problems Additional Objective Questions Answers 13 Surface Chemistry 13.1 Adsorption Adsorption and Related Phenomena Adsorption Mechanism Physisorption and Chemisorption 13.2 Factors Affecting Adsorption Adsorption of Gases on Solids Adsorption of Solids from Solutions 13.3 Adsorption Isotherms Freundlich Adsorption Isotherm Langmuir Adsorption Isotherm Multilayer Adsorption 13.4 Some Applications of Adsorption 13.5 Catalysis Characteristics of Catalysts 13.6 Types of Catalytic Reactions 13.7 Theory of Heterogeneous Catalysis 13.8 Shape-Selective Catalysis by Zeolites 13.9 Enzyme Catalysis Characteristic Features of Enzymes Mechanism of Enzyme Catalysis 13.10 Catalysts in Industry 13.11 Colloids Types of Colloids Mechanism of Micelle Formation 13.12 Preparation of Colloids Dispersion Methods Condensation Methods 13.13 Purification of Colloidal Solutions 13.14 Properties of Colloidal Solutions 13.15 Coagulation or Precipitation and Hardy–Schulze Rule Coagulation of Lyophobic Sols Coagulation of Lyophilic Sols Hardy–Schulze Rule 13.16 Protection of Colloids 13.17 Emulsions Emulsification and De-Emulsification 13.18 Role of Colloids in Natural Phenomena and in Industry Industrial Applications of Colloids Solved Objective Questions from Previous Year Papers Review Questions Numerical Problems Additional Objective Questions Answers 14 Nuclear Chemistry 14.1 Radioactivity Theory of Nuclear Disintegration 14.2 Structure of Atom 14.3 Stability of Nucleus Forces in the Nucleus Stability 14.4 Modes of Radioactive Decay Alpha Decay Beta Decay Gamma Emission Spontaneous Fission 14.5 Decay Mechanism in Neutron-Rich and Neutron-Poor Nuclides 14.6 Binding Energy and Nuclear Stability 14.7 The Kinetics of Radioactive Decay Radioactive Nuclei Decay by First-Order Kinetics Half-Life Period Average Life 14.8 Radioactive Equilibrium Parallel Decay 14.9 Activity of Radioactive Substances, Detection and Units of Radioactivity Detection of Radioactivity Units of Radioactivity 14.10 Natural vs. Induced Radioactivity Natural Radioactivity Radioactive Series Induced Radioactivity 14.11 Transmutation Transmutation for Nuclear Synthesis 14.12 Nuclear Reactions Nuclear Fission Nuclear Fusion 14.13 Biological Effects of Radiation Biological Effects of Ionizing Radiation 14.14 Applications of Radioactivity Dating by Radioactive Decay Nuclear Medicine Solved Objective Questions from Previous Year Papers Review Questions Numerical Problems Additional Objective Questions Answers Appendix A Appendix B JEE (ADVANCED) 2018PAPER I (CHEMISTRY) JEE Main 2019 Index Back Cover