Table of Contents Last updated Save as PDF Page ID204674 This text is an introduction to physical chemistry that emphasizes experimental and theoretical aspects of chemical thermodynamics, chemical and physical equilibrium, and kinetics.1: Enery Levels and Spectroscopy1.1: Electromagnetic Radiation1.2: The Wave Theory of Light1.3: Bohr's Theory of the Hydrogen Emission Spectrum1.4: Hydrogen's Atomic Emission Spectrum1.5: The Schrödinger Wave Equation1.6: Particle in a One-Dimensional Box1.7: Electronic Spectroscopy1.8: The Harmonic Oscillator Approximates Vibrations1.9: The Harmonic Oscillator and Infrared Spectra1.10: Microwave Spectroscopy2: Atomic Structure2.1: Many-Electron Atoms and the Periodic Table2.2: Quantum-Mechanical Tunneling3: Chemical Bond3.1: Lewis Structures3.2: Valence Bond Theory3.3: Hybridization of Atomic Orbitals3.4: Molecular Orbital Theory3.5: Diatomic Molecules4: Gases4.1: The Perfect Gas4.2: Real Gases (Deviations From Ideal Behavior)4.3: The Repulsive Term in the Lennard-Jones Potential5: Boltzmann5.1: The Boltzmann Factor5.2: The Thermal Boltzman Distribution5.3: The Average Ensemble Energy5.4: Heat Capacity at Constant Volume5.5: Partition Functions can be Decomposed5.6: Translational Partition Functions of Monotonic Gases5.7: Most Atoms are in the Ground Electronic State5.8: The Energy of a Diatomic Molecule Can Be Approximated as a Sum of Separate Terms5.9: Most Molecules are in the Ground Vibrational State5.10: Most Molecules are Rotationally Excited at Ordinary Temperatures5.11: Rotational Partition Functions of Diatomic Gases6: The First Law6.1: Internal Energy6.2: Enthalpy6.3: Thermochemistry7: Entropy and the Second Law7.1: A System and Its Surroundings7.2: The Second Law of Thermodynamics7.3: We Must Always Devise a Reversible Process to Calculate Entropy Changes7.4: The Statistical Interpretation of Entropy7.5: Entropy Can Be Expressed in Terms of a Partition Function8: The Third Law8.1: Heat Capacity as A Function of Temperature8.2: Evaluating Entropy Changes Using Thermochemical Cycles8.3: The Third Law of Thermodynamics9: Helmholtz and Gibbs Energies9.1: Helmholtz Energy9.2: Gibbs Energy9.3: The Maxwell Relations9.4: The Enthalpy of an Ideal Gas9.5: Gibbs-Helmholtz Relation (Gibbs Energy-Chang)9.6: The Gibbs-Helmholtz Equation10: Phase Equilibria10.1: A Phase Diagram Summarizes the Solid-Liquid-Gas Behavior of a Substance10.2: Gibbs Energies and Phase Diagrams10.3: The Chemical Potentials of a Pure Substance in Two Phases in Equilibrium10.4: The Clausius-Clapeyron Equation11: Solutions I- Liquid-Liquid Solutions11.1: Partial Molar Quantities in Solutions11.2: The Gibbs-Duhem Equation11.3: Chemical Potential of Each Component Has the Same Value in Each Phase in Which the Component Appears11.4: Ideal Solutions obey Raoult's Law11.5: Most Solutions are Not Ideal11.6: Vapor Pressures of Volatile Binary Solutions11.7: Activities of Nonideal Solutions12: Chemical Equilibriium12.1: The Standard Gibbs Free Energy Change and Equilibrium in Ideal Gas Reactions12.2: Equilibrium Results when Gibbs Energy is Minimized12.3: The Equilibrium Constant12.4: Calculating an Equilibrium Constant, Kp, with Partial Pressures12.5: The Van't Hoff Equation13: Kinetic Theory of Gases13.1: The Distribution of Molecular Speeds Is Given by the Maxwell-Boltzmann Distribution13.2: Collision Theory13.3: The Rate of a Gas-Phase Chemical Reactions14: Chemical Kinetics Rate Laws14.1: The Time Dependence of a Chemical Reaction Is Described by a Rate Law14.2: First-Order Reactions Show an Exponential Decay of Reactant Concentration with Time14.3: Different Rate Laws Predict Different Kinetics14.4: Arrhenius Equation14.5: Eyring equation15: Reaction mechanisms15.1: Elementary Steps15.2: The Steady-State Approximation15.3: The Lindemann Mechanism15.4: Some Reaction Mechanisms Involve Chain Reactions15.5: A Catalyst Affects the Mechanism and Activation Energy15.6: The Michaelis-Menten Mechanism for Enzyme CatalysisBack MatterIndexGlossary
