Physical chemistry

With its clear explanations and practical pedagogy, Physical Chemistry is less intimidating to students than other texts, without sacrificing the mathematical rigor and comprehensiveness necessary for a junior-level physical chemistry course. The text's long-standing reputation for accessible writing provides clear instruction and superior problem-solving support for students.

Note: Each chaper concludes with Key Equations, Problems, and Suggested Reading

1 The Nature of Physical Chemistry and the Kinetic Theory of Gases

1.1 The Nature of Physical Chemistry

1.2 Some Concepts from Classical Mechanics

1.3 Systems, States, and Equilibrium

1.4 Thermal Equilibrium

1.5 Pressure and Boyle's Law Biography: Robert Boyle

1.6 Gay-Lussac's (Charles's) Law

1.7 The Ideal Gas Thermometer

1.8 The Equation of State for an Ideal Gas

1.9 The Kinetic-Molecular Theory of Ideal Gases

1.10 The Barometric Distribution Law

1.11 The Maxwell Distribution of Molecular Speeds and Translational Energies

1.12 Real Gases

1.13 Equations of State

1.14 The Virial Equation Appendix: Some Definite and Indefinite Integrals Often Used in Physical Chemistry

2 The First Law of Thermodynamics

2.1 Origins of the First Law

2.2 States and State Functions

2.3 Equilibrium States and Reversibility

2.4 Energy, Heat, and Work

2.5 Thermochemistry

2.6 Ideal Gas Relationships

2.7 Real Gases

3 The Second and Third Laws of Thermodynamics Biography: Rudolph Julius Emmanuel Clausius

3.1 The Carnot Cycle

3.2 Irreversible Processes

3.3 Molecular Interpretation of Entropy

3.4 The Calculation of Entropy Changes

3.5 The Third Law of Thermodynamics

3.6 Conditions for Equilibrium

3.7 The Gibbs Energy

3.8 Some Thermodynamic Relationships

3.9 The Gibbs-Helmholtz Equation

3.10 Thermodynamic Limitations to Energy Conversion

4 Chemical Equilibrium Biography: Jacobus Henricus van't Hoff

4.1 Chemical Equilibrium Involving Ideal Gases

4.2 Equilibrium in Nonideal Gaseous Systems

4.3 Chemical Equilibrium in Solution

4.4 Heterogeneous Equilibrium

4.5 Tests for Chemical Equilibrium

4.6 Shifts of Equilibrium at Constant Temperature

4.7 Coupling of Reactions

4.8 Temperature Dependence of Equilibrium Constants

4.9 Pressure Dependence of Equilibrium Constants

5 Phases and Solutions

5.1 Phase Recognition

5.2 Vaporization and Vapor Pressure

5.3 Classification of Transitions in Single-Component Systems

5.4 Ideal Solutions: Raoult's and Henry's Laws

5.5 Partial Molar Quantities

5.6 The Chemical Potential

5.7 Thermodynamics of Solutions

5.8 The Colligative Properties

6 Phase Equilibria

6.1 Equilibrium Between Phases

6.2 One-Component Systems

6.3 Binary Systems Involving Vapor

6.4 Condensed Binary Systems

6.5 Thermal Analysis

6.6 More Complicated Binary Systems

6.7 Crystal Solubility: The Krafft Boundary and Krafft Eutectic

6.8 Ternary Systems

7 Solutions of Electrolytes

7.1 Faraday's Laws of Electrolysis Biography: Michael Faraday

7.2 Molar Conductivity

7.3 Weak Electrolytes: The Arrhenius Theory Biography: Svante August Arrhenius

7.4 Strong Electrolytes

7.5 Independent Migration of Ions

7.6 Transport Numbers

7.7 Ion Conductivities

7.8 Thermodynamics of Ions

7.9 Theories of Ions in Solution

7.10 Activity Coefficients

7.11 Ionic Equilibria

7.12 Ionization of Water

7.13 The Donnan Equilibrium

8 Electrochemical Cells

8.1 The Daniell Cell

8.2 Standard Electrode Potentials

8.3 Thermodynamics of Electrochemical Cells

8.4 Types of Electrochemical Cells

8.5 Applications of emf Measurements

8.6 Fuel Cells

8.7 Photogalvanic Cells

8.8 Batteries, Old and New

9 Chemical Kinetics I. The Basic Ideas

9.1 Rates of Consumption and Formation

9.2 Rate of Reaction

9.3 Empirical Rate Equations

9.4 Analysis of Kinetic Results

9.5 Techniques for Very Fast Reactions

9.6 Molecular Kinetics

9.7 The Arrhenius Equation

9.8 Potential-Energy Surfaces

9.9 The Preexponential Factor Biography: Henry Eyring

9.10 Reactions in Solution

9.11 Reaction Dynamics

10 Chemical Kinetics II. Composite Mechanisms

10.1 Evidence for a Composite Mechanism

10.2 Types of Composite Reactions

10.3 Rate Equations for Composite Mechanisms

10.4 Rate Constants, Rate Coefficients, and Equilibrium Constants

10.5 Free-Radical Reactions

10.6 Photochemical Reactions

10.7 Radiation-Chemical Reactions

10.8 Explosions

10.9 Catalysis

10.10 Reactions in Solution: Some Special Features

10.11 Mechanisms of Polymerization in Macromolecules

10.12 Kinetics of Polymerization

10.13 Induction Periods, Oscillations, and Chaos

10.14 Electrochemical Dynamics

11 Quantum Mechanics and Atomic Structure

11.1 Electromagnetic Radiation and the Old Quantum Theory

11.2 Bohr's Atomic Theory

11.3 The Foundations of Quantum Mechanics

11.4 Schr?dinger's Wave Mechanics

11.5 Quantum-Mechanical Postulates

11.6 Quantum Mechanics of Some Simple Systems

11.7 Quantum Mechanics of Hydrogenlike Atoms

11.8 Physical Significance of the Orbital Quantum Numbers

11.9 Angular Momentum and Magnetic Moment

11.10 The Rigid Linear Rotor

11.11 Spin Quantum Numbers

11.12 Many-Electron Atoms

11.13 Approximate Methods in Quantum Mechanics

12 The Chemical Bond Biography: Gilbert Newton Lewis

12.1 The Hydrogen Molecular-Ion, H2+

12.2 The Hydrogen Molecule

12.3 H?ckel Theory for More Complex Molecules

12.4 Valence-Bond Theory for More Complex Molecules

12.5 Symmetry in Chemistry

12.6 Symmetry of Molecular Orbitals Appendix: Character Tables

13 Foundations of Chemical Spectroscopy

13.1 Emission and Absorption Spectra

13.2 Atomic Spectra Biography: Gerhard Herzberg

13.3 Pure Rotational Spectra of Molecules

13.4 Vibrational-Rotational Spectra of Molecules

13.5 Raman Spectra

13.6 Electronic Spectra of Molecules Appendix: Symmetry Species Corresponding to Infrared and Raman Spectra

14 Some Modern Applications of Spectroscopy

14.1 Laser Spectroscopy

14.2 Spectral Line Widths

14.3 Types of Lasers

14.4 Laser Techniques for Chemistry

14.5 Magnetic Spectroscopy

14.6 Nuclear Magnetic Spectroscopy

14.7 Electron Magnetic Resonance (EMR)

14.8 M?ssbauer Spectroscopy

14.9 Photoelectron Spectroscopy

14.10 Photoacoustic Spectroscopy

14.11 Chiroptical Methods

14.12 Mass Spectrometry

15 Statistical Mechanics

15.1 Forms of Molecular Energy Biography: Ludwig Boltzmann

15.2 Principles of Statistical Mechanics

15.3 The Partition Function

15.4 Thermodynamic Quantities from Partition Functions

15.5 The Partition Function for Some Special Cases

15.6 The Internal Energy, Enthalpy, and Gibbs Energy Functions

15.7 The Calculation of Equilibrium Constants

15.8 Transition-State Theory

15.9 The Approach to Equilibrium

15.10 The Canonical Ensemble

16 The Solid State

16.1 Crystal Forms and Crystal Lattices

16.2 X-Ray Crystallography

16.3 Experimental Methods Biography: Dorothy Crowfoot Hodgkin

16.4 Theories of Solids

16.5 Statistical Thermodynamics of Crystals: Theories of Heat Capacities

16.6 Electrical Conductivity in Solids

16.7 Optical Properties of Solids

17 The Liquid State

17.1 Liquids Compared with Dense Gases

17.2 Liquids Compared with Solids

17.3 Intermolecular Forces

17.4 Theories and Models of Liquids

17.5 Water, the Incomparable Liquid

17.6 The Hydrophobic Effect

18 Surface Chemistry and Colloids

18.1 Adsorption

18.2 Adsorption Isotherms

18.3 Thermodynamics and Statistical Mechanics of Adsorption

18.4 Chemical Reactions on Surfaces

18.5 Surface Heterogeneity

18.6 The Structure of Solid Surfaces and of Adsorbed Layers

18.7 Surface Tension and Capillarity

18.8 Liquid Films on Surfaces Biography: Agnes Pockels

18.9 Colloidal Systems

19 Transport Properties

19.1 Viscosity

19.2 Diffusion

19.3 Sedimentation

Appendix A Units, Quantities, and Symbols: The SI/IUPAC Recommendations

Appendix B Physical Constants

Appendix C Some Mathematical Relationships

Appendix D Standard Enthalpies, Entropies, and Gibbs Energies of Formation

Appendix E Character Tables for Some Important Symmetry Groups in Chemistry Answers to Problems

Index

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On Order

Summary

Summary

Table of Contents