Physical Chemistry

Every chemist should own a copy of this uniquely thorough yet incisive treatment of the basic principles of physical chemistry. Written by three eminent physical chemists, the second edition of this exceptional work is the most lucid and comprehensive physical chemistry reference available.
The authors present the fundamentals of the three major areas of physical chemistry--the microscopic structure of matter, the equilibrium properties of systems, and the physical and chemical kinetics of transformations of systems--in a logical sequence, from the simple to the complex. Beginning with
atomic and molecular structure, they progress to properties of condensed matter, to statistical and thermodynamic properties of systems in equilibrium, and then to transport phenomena and chemical reaction processes. The book's mathematical level begins with elementary calculus and rises to the use
of simple properties of partial differential equations and the special functions that enter into their solutions. The conceptual structure of physical chemistry is emphasized throughout and appendices develop the details of the mathematical tools as they are needed.
This new edition features:
DT In-depth and illuminating presentation of conceptual arguments
DT No shortcuts--derives whole formulas
DT 100 new problems
DT New material on nuclear magnetic resonance
DT Expanded treatment of linear and nonlinear irreversible processes and thermodynamics
DT A completely revised treatment of electrode kinetics
DT Many updates throughout
DT Several vignettes--written by leaders in the field--that cover topics at the cutting edge of physical chemistry research

The authors' goal is the presentation of the three major areas of physical chemistry: molecular structure, the equilibrium properties of systems, and the kinetics of transformations of systems. The theoretical foundations of these subjects are, respectively, quantum mechanics, thermodynamics and equilibrium statistical mechanics, and chemical kinetics and kinetic theory. These theories, firmly based on experimental findings, constitute the structure required for the understanding of past accomplishments and the basis for recognition and development of significant new areas in physical chemistry. The presentation of the theories of physical chemistry requires careful discussions at several levels of exposition. The authors' approach aims toward depth of understanding of fundamentals more than toward breadth of recognition of the multitude of activities that go on under the name of physical chemistry. The organization of the book, with its three principal sections, should make this clear. The mathematical level begins with elementary calculus, and rises to the use of simple properties of partial differential equations and the special functions that enter into their solutions. The authors' intention is to keep the reader's mind on the scienc rather than on the mathematics, especially at the beginning. This procedure also corresponds to the pattern, followed by many students, of taking physical chemistry and advanced calculus concurrently. Appendices develop the details of the mathematical tools as they are needed. The text discussion contains more material than can be covered in the traditional one-year physical chemistry sequence; it is designed to fulfill the dual purpose of providing a clear and incisive treatment of fundamental principles at a level accessible to all students while broadening the perspectives and challenging the minds of the best students. Individual instructors will wish to make their own selections of material for inclusion and exclusion, respectively.

1.1 - Development of the Atomic Theory: Relative Atomic Weights
1.2 - Atomic Magnitudes
1.3 - The Charge-to-Mass Ratio of the Electron: Thomson's Method
1.4 - The Charge of the Electron: Millikan's Method
1.5 - Mass Spectrometry
1.6 - The Atomic Mass Scale and the Mole
1.7 - The Periodic Table
2.1 - The Franck-Hertz Experiment
2.2 - The Photoelectric Effect
2.3 - x Rays and Matter
2.4 - The Emission Spectra of Atoms
2.5 - The Nuclear Atom
2.6 - The Problem of Black-Body Radiation
2.7 - The Concept of Action
2.8 - The Harmonic Oscillator
2.9 - Action Quantized: The Heat Capacity of Solids
2.10 - Some Orders of Magnitude
2.11 - Bohr's Model of the Atom
3.1 - The de Broglie Hypothesis
3.2 - The Nature of Waves
3.3 - Dispersion Relations and Wave Equations: The Free Particle
3.4 - Operators
3.5 - Eigenfunctions and Eigenvalues
3.6 - The Particle in a One-Dimensional Box
3.7 - The Interdeterminacy or Uncertainty Principle
3.8 - Expectation Values; Summary of Postulates
3.9 - Particles in Two- and Three-Dimensional Boxes
3.10 - Particles in Circular Boxes
3.11 - Particles in Spherical Boxes
3.12 - The Rigid Rotor
4.1 - Finite Potential Barriers
4.2 - The Quantum Mechanical Harmonic Oscillator
4.3 - The Hydrogen Atom
4.4 - The Shapes of Orbitals
4.5 - Transitions Between Energy Levels
5.1 - Electron Spin; Magnetic Phenomena
5.2 - The Pauli Exclusion Principle; the Aufbau Principle
5.3 - Electronic Configuration of Atoms
5.4 - Calculation of Atomic Structures
5.5 - Atomic Structure and Periodic Behavior
5.6 - Term Splitting and the Vector Model
5.7 - Fine Structure and Spin—Orbit Interactions
6.1 - Bonding Forces Between Atoms
6.2 - The Simplest Molecule: The Hydrogen Molecule-Ion, H2+
6.3 - H2+: Molecular Orbitals and the LCAO Approximation
6.4 - H2+: Obtaining the Energy Curve
6.5 - H2+: Correlation of Orbitals; Excited States
6.6 - The H2 Molecule: Simple MO Description
6.7 - Symmetry Properties of Identical Particles
6.8 - H2: The Valence BOnd Representation
6.9 - H2: Beyond the Simple MO and VB Approximations
6.10 - H2: Excited Electronic States
7.1 - Vibrations of Diatomic Molecules
7.2 - Rotations of Diatomic Molecules
7.3 - Spectra of Diatomic Molecules
7.4 - The Ionic Bond
7.5 - Homonuclear Diatomic Molecules: Molecular Orbitals and Orbital Correlation
7.6 - Homonuclear Diatomic Molecules: Aufbau Principle and the Structure of First-Row Molecules
7.7 - Introduction to Heteronuclear Diatomic Molecules: Electronegativity
7.8 - Bonding in LiH: Crossing and Noncrossing Potential Curves
7.9 - Other First-Row Diatomic Hydrides
7.10 - Isoelectronic and Other Series
8.1 - Electronic Structure and Geometry in the Simplest Cases: H3 and H3+
8.2 - Dihydrides: Introduction to the Water Molecule
8.3 - Hybrid Orbitals
8.4 - Delocalized Orbitals in H2O: The General MO Method
8.5 - Bonding in More Complex Triatomic Molecules
8.6 - Normal Coordinates and Modes of Vibration
8.7 - A Solvable Example: The Vibrational Modes of CO2
8.8 - Transition and Spectra of Polyatomic Molecules
9.1 - Small Molecules
9.2 - Catenated Carbon Compounds; Transferability
9.3 - Other Extended Structures
9.4 - Some Steric Effects
9.5 - Complex Ions and Other Coordination Compounds: Simple Polyhedra
9.6 - Chirality and Optical Rotation
9.7 - Chiral and Other Complex Ions
9.8 - Magnetic Properties of Complexes
9.9 - Electronic Structure of Complexes
10.1 - Long-Range Forces: Interactions Between Charge Distributions
10.2 - Empirical Intermolecular Potentials
10.3 - Weakly Associated Molecules
11.1 - Some General Properties of Solids
11.2 - Space Lattices and Crystal Symmetry
11.3 - x Ray Diffraction from Crystals: The Bragg Model
11.4 - The Laue Model
11.5 - Determination of Crystal Structures
11.6 - Techniques of Diffraction
11.7 - Molecular Crystals
11.8 - Structures of Ionic Crystals
11.9 - Binding Energy of Ionic Crystals
11.10 - Covalent Solids
11.11 - The Free-Electron Theory of Metals
11.12 - The Band Theory of Solids
11.13 - Conductors, Insulators, and Semicondutors
11.14 - Other Forms of Condensed Matter
12.1 - The Perfect Gas: Definition and Elementary Model
12.2 - The Perfect Gas: A General Relation Between Pressure and Energy
12.3 - Some Comments About Thermodynamics
12.4 - Temperature and the Zeroth Law of Thermodynamics
12.5 - Empirical Temperature: The Perfect Gas Temperature Scale
12.6 - Comparison of the Microscopic and Macroscopic Approaches
13.1 - Microscopic and Macroscopic Energy in a Perfect Gas
13.2 - Description of Thermodynamic States
13.3 - The Concept of Work in Thermodynamics
13.4 - Intensive and Extensive Variables
13.5 - Quasi-static and Reversible Processes
13.6 - The First Law: Energy and Heat
13.7 - Some Historical Notes
13.8 - Microscopic Interpretation of Internal Heat and Energy
13.9 - Constraints, Work, and Equilibrium
14.1 - Heat Capacity and Enthalpy
14.2 - Energy and Enthalpy Changes in Chemical Reactions
14.3 - Thermochemistry of Physical Processes
14.4 - Introduction to Phase Changes
14.5 - Standard States
14.6 - Thermochemistry of Solutions
14.7 - Molecular Interpretation of Physical Processes
14.8 - Bond Energies
14.9 - Some Energy Effects in Molecular Structures
14.10 - Lattice Energies of Ionic Crystals
15.1 - The Relationship Between Average Propertis and Molecular Motion in an N-Molecule System: Time Averages and Ensemble Averages
15.2 - Ensembles and Probability Distributions
15.3 - Some Properties of a System with Many Degrees of Freedom: Elements of the Statistical Theory of Matter at Equilibrium
15.4 - The Influences of Constraints on the Density of States
15.5 - The Entropy: A Potential Function for the Equilibrium State
16.1 - The Second Law of Thermodynamics
16.2 - The Existence of an Engropy Function for Reversible Processes
16.3 - Irreversible Processes: The Second Law Interpretation
16.4 - The Clausius and Kelvin Statements Revisited
16.5 - The Second Law as an Inequality
16.6 - Some Relationships Between the Microscopic and Macroscopic Theories
17.1 - Choice of Independent Variables
17.2 - The Available Work Concept
17.3 - Entropy Changes in Reversible Processes
17.4 - Entropy Changes in Irreversible Processes
17.5 - Entropy Changes in Phase Transitions
18.1 - The Magnitude of the Entropy at T=0
18,2 - The Unattainability of Absolute Zero
18.3 - Experimental Verification of the Third Law
19.1 - Properties of the Equilibrium State of a Pure Substance
19.2 - Alternative Descriptions of the Equilibrium State for Different External Constraints
19.3 - The Stability of the Equilibrium State of a One-Component System
19,4 - The Equilibrium State in a Multicomponent System
19.5 - Chemical Equilibrium
19.6 - Thermodynamic Weight: Further Connections Between Thermodynamics and Microscopic Structure
19.7 - An Application of the Canonical Ensemble: The Distribution of Molecular Speeds in a Perfect Gas
20.1 - General Form of the Equation of Continuity
20.2 - Conservation of Mass and the Diffusion Equation
20.3 - Conservation of Momentum and the Navier-Stokes Equation
20.4 - Conservation of Energy and the Second Law of Thermodynamics
20.5 - Linear Transport