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Title: Physical Chemistry (LibreTexts)
Webpages: 365
Applicable Restrictions: Noncommercial
All licenses found:
- Undeclared: 90.1% (329 pages)
- CC BY-NC-SA 4.0: 3.6% (13 pages)
- CC BY 4.0: 3.3% (12 pages)
- CC BY-SA 4.0: 2.2% (8 pages)
- CC BY-NC-SA 3.0: 0.8% (3 pages)
By Page
- Physical Chemistry (LibreTexts) —
Undeclared
- Front Matter — Undeclared
- 1: The Dawn of the Quantum Theory —
Undeclared
- 1.1: Blackbody Radiation Cannot Be Explained Classically — CC BY 4.0
- 1.2: Quantum Hypothesis Used for Blackbody Radiation Law — Undeclared
- 1.3: Photoelectric Effect Explained with Quantum Hypothesis — CC BY-NC-SA 4.0
- 1.4: The Hydrogen Atomic Spectrum — Undeclared
- 1.5: The Rydberg Formula and the Hydrogen Atomic Spectrum — CC BY-NC-SA 4.0
- 1.6: Matter Has Wavelike Properties — CC BY-NC-SA 4.0
- 1.7: de Broglie Waves can be Experimentally Observed — Undeclared
- 1.8: The Bohr Theory of the Hydrogen Atom — Undeclared
- 1.9: The Heisenberg Uncertainty Principle — Undeclared
- 1.E: The Dawn of the Quantum Theory (Exercises) — Undeclared
- 2: The Classical Wave Equation —
Undeclared
- 2.1: The One-Dimensional Wave Equation — Undeclared
- 2.2: The Method of Separation of Variables — CC BY-NC-SA 4.0
- 2.3: Oscillatory Solutions to Differential Equations — Undeclared
- 2.4: The General Solution is a Superposition of Normal Modes — Undeclared
- 2.5: A Vibrating Membrane — Undeclared
- 2.E: The Classical Wave Equation (Exercises) — Undeclared
- 3: The Schrödinger Equation and a Particle in a Box —
Undeclared
- 3.1: The Schrödinger Equation — Undeclared
- 3.2: Linear Operators in Quantum Mechanics — Undeclared
- 3.3: The Schrödinger Equation is an Eigenvalue Problem — Undeclared
- 3.4: Wavefunctions Have a Probabilistic Interpretation — Undeclared
- 3.5: The Energy of a Particle in a Box is Quantized — Undeclared
- 3.6: Wavefunctions Must Be Normalized — CC BY-NC-SA 4.0
- 3.7: The Average Momentum of a Particle in a Box is Zero — Undeclared
- 3.8: The Uncertainty Principle - Estimating Uncertainties from Wavefunctions — Undeclared
- 3.9: A Particle in a Three-Dimensional Box — Undeclared
- 3.E: The Schrödinger Equation and a Particle in a Box (Exercises) — Undeclared
- 4: Postulates and Principles of Quantum Mechanics —
Undeclared
- 4.1: The Wavefunction Specifies the State of a System — CC BY-NC-SA 4.0
- 4.2: Quantum Operators Represent Classical Variables — Undeclared
- 4.3: Observable Quantities Must Be Eigenvalues of Quantum Mechanical Operators — Undeclared
- 4.4: The Time-Dependent Schrödinger Equation — Undeclared
- 4.5: Eigenfunctions of Operators are Orthogonal — Undeclared
- 4.6: Commuting Operators Allow Infinite Precision — CC BY-NC-SA 3.0
- 4.E: Postulates and Principles of Quantum Mechanics (Exercises) — Undeclared
- 5: The Harmonic Oscillator and the Rigid Rotor —
Undeclared
- 5.1: A Harmonic Oscillator Obeys Hooke's Law — Undeclared
- 5.2: The Equation for a Harmonic-Oscillator Model of a Diatomic Molecule Contains the Reduced Mass of the Molecule — CC BY-NC-SA 4.0
- 5.3: The Harmonic Oscillator Approximates Molecular Vibrations — CC BY 4.0
- 5.4: The Harmonic Oscillator Energy Levels — CC BY-NC-SA 4.0
- 5.5: The Harmonic Oscillator and Infrared Spectra — Undeclared
- 5.6: The Harmonic Oscillator Wavefunctions involve Hermite Polynomials — Undeclared
- 5.7: Hermite Polynomials are either Even or Odd Functions — CC BY-SA 4.0
- 5.8: The Energy Levels of a Rigid Rotor — CC BY-NC-SA 4.0
- 5.9: The Rigid Rotator is a Model for a Rotating Diatomic Molecule — Undeclared
- 5.E: The Harmonic Oscillator and the Rigid Rotor (Exercises) — Undeclared
- 6: The Hydrogen Atom —
Undeclared
- 6.1: The Schrödinger Equation for the Hydrogen Atom Can Be Solved Exactly — Undeclared
- 6.2: The Wavefunctions of a Rigid Rotator are Called Spherical Harmonics — CC BY-NC-SA 4.0
- 6.3: The Three Components of Angular Momentum Cannot be Measured Simultaneously with Arbitrary Precision — Undeclared
- 6.4: Hydrogen Atomic Orbitals Depend upon Three Quantum Numbers — Undeclared
- 6.5: s-orbitals are Spherically Symmetric — Undeclared
- 6.6: Orbital Angular Momentum and the p-Orbitals — Undeclared
- 6.7: The Helium Atom Cannot Be Solved Exactly — Undeclared
- 6.E: The Hydrogen Atom (Exercises) — Undeclared
- 7: Approximation Methods —
Undeclared
- 7.1: The Variational Method Approximation — CC BY-NC-SA 3.0
- 7.2: Linear Variational Method and the Secular Determinant — Undeclared
- 7.3: Trial Functions Can Be Linear Combinations of Functions That Also Contain Variational Parameters — Undeclared
- 7.4: Perturbation Theory Expresses the Solutions in Terms of Solved Problems — Undeclared
- 7.E: Approximation Methods (Exercises) — Undeclared
- 8: Multielectron Atoms —
Undeclared
- 8.1: Atomic and Molecular Calculations are Expressed in Atomic Units — CC BY-SA 4.0
- 8.2: Perturbation Theory and the Variational Method for Helium — Undeclared
- 8.3: Hartree-Fock Equations are Solved by the Self-Consistent Field Method — Undeclared
- 8.4: An Electron has an Intrinsic Spin Angular Momentum — Undeclared
- 8.5: Wavefunctions must be Antisymmetric to Interchange of any Two Electrons — Undeclared
- 8.6: Antisymmetric Wavefunctions can be Represented by Slater Determinants — Undeclared
- 8.7: Hartree-Fock Calculations Give Good Agreement with Experimental Data — Undeclared
- 8.8: Term Symbols Gives a Detailed Description of an Electron Configuration — CC BY 4.0
- 8.9: The Allowed Values of J - the Total Angular Momentum Quantum Number — Undeclared
- 8.10: Hund's Rules Determine the Term Symbols of the Ground Electronic States — Undeclared
- 8.11: Using Atomic Term Symbols to Interpret Atomic Spectra — Undeclared
- 8.E: Multielectron Atoms (Exercises) — Undeclared
- 9: Chemical Bonding in Diatomic Molecules —
Undeclared
- 9.1: The Born-Oppenheimer Approximation Simplifies the Schrödinger Equation for Molecules — Undeclared
- 9.2: The H₂⁺ Prototypical Species — Undeclared
- 9.3: The Overlap Integral — Undeclared
- 9.4: Chemical Bond Stability — Undeclared
- 9.5: Bonding and Antibonding Orbitals — Undeclared
- 9.6: A Simple Molecular-Orbital Treatment of H₂ Places Both Electrons in a Bonding Orbital — Undeclared
- 9.7: Molecular Orbitals Can Be Ordered According to Their Energies — Undeclared
- 9.8: Molecular-Orbital Theory Does not Predict a Stable Diatomic Helium Molecule — Undeclared
- 9.9: Electrons Populate Molecular Orbitals According to the Pauli Exclusion Principle — Undeclared
- 9.10: Molecular Orbital Theory Predicts that Molecular Oxygen is Paramagnetic — Undeclared
- 9.11: Photoelectron Spectra Support the Existence of Molecular Orbitals — Undeclared
- 9.12: Molecular-Orbital Theory Also Applies to Heteronuclear Diatomic Molecules — CC BY-NC-SA 3.0
- 9.13: SCF-LCAO-MO Wavefunctions are Molecular Orbitals formed from a Linear Combination of Atomic Orbitals and Whose Coefficients Are Determined Self-Consistently — Undeclared
- 9.14: Molecular Term Symbols Describe Electronic States of Molecules — CC BY 4.0
- 9.15: Molecular Term Symbols Designate Symmetry — Undeclared
- 9.16: Most Molecules Have Excited Electronic States — Undeclared
- 9.E: Chemical Bond in Diatomic Molecules (Exercises) — Undeclared
- 10: Bonding in Polyatomic Molecules —
Undeclared
- 10.1: Hybrid Orbitals Account for Molecular Shape — CC BY-NC-SA 4.0
- 10.2: Hybrid Orbitals in Water — Undeclared
- 10.3: BeH₂ is Linear and H₂O is Bent — Undeclared
- 10.4: Photoelectron Spectroscopy — CC BY 4.0
- 10.5: The pi-Electron Approximation of Conjugation — Undeclared
- 10.6: Butadiene is Stabilized by a Delocalization Energy — CC BY-SA 4.0
- 10.7: Benzene and Aromaticity — Undeclared
- 10.E: Bonding in Polyatomic Molecules (Exercises) — Undeclared
- 11: Computational Quantum Chemistry —
Undeclared
- 11.1: Overview of Quantum Calculations — Undeclared
- 11.2: Gaussian Basis Sets — Undeclared
- 11.3: Extended Basis Sets — Undeclared
- 11.4: Orbital Polarization Terms in Basis Sets — Undeclared
- 11.5: The Ground-State Energy of H₂ — Undeclared
- 11.E: Computational Quantum Chemistry (Exercises) — Undeclared
- 12: Group Theory - The Exploitation of Symmetry —
Undeclared
- 12.1: The Exploitation of Symmetry — Undeclared
- 12.2: Symmetry Elements — Undeclared
- 12.3: Symmetry Operations Define Groups — Undeclared
- 12.4: Symmetry Operations as Matrices — Undeclared
- 12.5: The \(C_{3V}\) Point Group — Undeclared
- 12.6: Character Tables — Undeclared
- 12.7: Characters of Irreducible Representations — Undeclared
- 12.8: Using Symmetry to Solve Secular Determinants — Undeclared
- 12.9: Generating Operators — Undeclared
- 12.E: Group Theory - The Exploitation of Symmetry (Exercises) — Undeclared
- 13: Molecular Spectroscopy —
Undeclared
- 13.1: The Electromagnetic Spectrum — Undeclared
- 13.2: Rotations Accompany Vibrational Transitions — CC BY 4.0
- 13.3: Unequal Spacings in Vibration-Rotation Spectra — Undeclared
- 13.4: Unequal Spacings in Pure Rotational Spectra — Undeclared
- 13.5: Vibrational Overtones — CC BY 4.0
- 13.6: Electronic Spectra Contain Electronic, Vibrational, and Rotational Information — Undeclared
- 13.7: The Franck-Condon Principle — Undeclared
- 13.8: Rotational Spectra of Polyatomic Molecules — Undeclared
- 13.9: Normal Modes in Polyatomic Molecules — Undeclared
- 13.10: Irreducible Representation of Point Groups — Undeclared
- 13.11: Time-Dependent Perturbation Theory — CC BY-SA 4.0
- 13.12: The Selection Rule for the Rigid Rotor — Undeclared
- 13.13: The Harmonic Oscillator Selection Rule — Undeclared
- 13.14: Group Theory Determines Infrared Activity — Undeclared
- 13.E: Molecular Spectroscopy (Exercises) — Undeclared
- 14: Nuclear Magnetic Resonance Spectroscopy —
Undeclared
- 14.1: Nuclei Have Intrinsic Spin Angular Momenta — CC BY-SA 4.0
- 14.2: Magnetic Moments Interact with Magnetic Fields — Undeclared
- 14.3: Proton NMR Spectrometers Operate at Frequencies Between 60 MHz and 750 MHz — Undeclared
- 14.4: The Magnetic Field Acting upon Nuclei in Molecules Is Shielded — Undeclared
- 14.5: Chemical Shifts Depend upon the Chemical Environment of the Nucleus — CC BY-SA 4.0
- 14.6: Spin-Spin Coupling Can Lead to Multiplets in NMR Spectra — Undeclared
- 14.7: Spin-Spin Coupling Between Chemically Equivalent Protons is Not Observed — Undeclared
- 14.8: The n+1 Rule Applies Only to First-Order Spectra — Undeclared
- 14.9: Second-Order Spectra Can Be Calculated Exactly Using the Variational Method — Undeclared
- 14.E: Nuclear Magnetic Resonance Spectroscopy (Exercises) — Undeclared
- 15: Lasers, Laser Spectroscopy, and Photochemistry —
CC BY 4.0
- 15.1: Electronically Excited Molecules can Relax by a Number of Processes — Undeclared
- 15.2: The Dynamics of Transitions can be Modeled by Rate Equations — Undeclared
- 15.3: A Two-Level System Cannot Achieve a Population Inversion — Undeclared
- 15.4: Population Inversion can be Achieved in a Three-Level System — Undeclared
- 15.5: What is Inside a Laser? — Undeclared
- 15.6: The Helium-Neon Laser — Undeclared
- 15.7: High-Resolution Laser Spectroscopy — Undeclared
- 15.8: Pulsed Lasers Can by Used to Measure the Dynamics of Photochemical Processes — Undeclared
- 15.E: Lasers, Laser Spectroscopy, and Photochemistry (Exercises) — Undeclared
- 16: The Properties of Gases —
Undeclared
- 16.1: All Dilute Gases Behave Ideally — Undeclared
- 16.2: van der Waals and Redlich-Kwong Equations of State — Undeclared
- 16.3: A Cubic Equation of State — Undeclared
- 16.4: The Law of Corresponding States — Undeclared
- 16.5: The Second Virial Coefficient — Undeclared
- 16.6: The Repulsive Term in the Lennard-Jones Potential — Undeclared
- 16.7: Van der Waals Constants in Terms of Molecular Parameters — Undeclared
- 16.E: The Properties of Gases (Exercises) — Undeclared
- 17: Boltzmann Factor and Partition Functions —
Undeclared
- 17.1: The Boltzmann Factor — Undeclared
- 17.2: The Thermal Boltzman Distribution — Undeclared
- 17.3: The Average Ensemble Energy — Undeclared
- 17.4: Heat Capacity at Constant Volume — Undeclared
- 17.5: Pressure in Terms of Partition Functions — Undeclared
- 17.6: Partition Functions of Distinguishable Molecules — Undeclared
- 17.7: Partition Functions of Indistinguishable Molecules — Undeclared
- 17.8: Partition Functions can be Decomposed — Undeclared
- 17.E: Boltzmann Factor and Partition Functions (Exercises) — Undeclared
- 18: Partition Functions and Ideal Gases —
Undeclared
- 18.1: Translational Partition Functions of Monotonic Gases — Undeclared
- 18.2: Most Atoms are in the Ground Electronic State — Undeclared
- 18.3: The Energy of a Diatomic Molecule Can Be Approximated as a Sum of Separate Terms — Undeclared
- 18.4: Most Molecules are in the Ground Vibrational State — Undeclared
- 18.5: Most Molecules are Rotationally Excited at Ordinary Temperatures — Undeclared
- 18.6: Rotational Partition Functions of Diatomic Gases — Undeclared
- 18.7: Vibrational Partition Functions of Polyatomic Molecules — Undeclared
- 18.8: Rotational Partition Functions of Polyatomic Molecules — Undeclared
- 18.9: Molar Heat Capacities — Undeclared
- 18.10: Ortho and Para Hydrogen — Undeclared
- 18.11: The Equipartition Principle — Undeclared
- 18.E: Partition Functions and Ideal Gases (Exercises) — Undeclared
- 19: The First Law of Thermodynamics —
Undeclared
- 19.1: Overview of Classical Thermodynamics — Undeclared
- 19.2: Pressure-Volume Work — Undeclared
- 19.3: Work and Heat are not State Functions — Undeclared
- 19.4: Energy is a State Function — Undeclared
- 19.5: An Adiabatic Process is a Process in which No Energy as Heat is Transferred — Undeclared
- 19.6: The Temperature of a Gas Decreases in a Reversible Adiabatic Expansion — Undeclared
- 19.7: Work and Heat Have a Simple Molecular Interpretation — Undeclared
- 19.8: Pressure-Volume Work — Undeclared
- 19.9: Heat Capacity is a Path Function — Undeclared
- 19.10: Relative Enthalpies Can Be Determined from Heat Capacity Data and Heats of Transition — Undeclared
- 19.11: Enthalpy Changes for Chemical Equations are Additive — Undeclared
- 19.12: Heats of Reactions Can Be Calculated from Tabulated Heats of Formation — Undeclared
- 19.13: The Temperature Dependence of ΔH — Undeclared
- 19.E: The First Law of Thermodynamics (Exercises) — Undeclared
- Enthalpy is a State Function — Undeclared
- 20: Entropy and The Second Law of Thermodynamics —
Undeclared
- 20.1: Energy Does not Determine Spontaneity — Undeclared
- 20.2: Nonequilibrium Isolated Systems Evolve in a Direction That Increases Their Energy Dispersal — Undeclared
- 20.3: Unlike heat, Entropy is a State Function — Undeclared
- 20.4: The Second Law of Thermodynamics — Undeclared
- 20.5: The Famous Equation of Statistical Thermodynamics is S=k ln W — Undeclared
- 20.6: We Must Always Devise a Reversible Process to Calculate Entropy Changes — Undeclared
- 20.7: Thermodynamics Provides Insight into the Conversion of Heat into Work — Undeclared
- 20.8: Entropy Can Be Expressed in Terms of a Partition Function — Undeclared
- 20.9: The Statistical Definition of Entropy is Analogous to the Thermodynamic Definition — Undeclared
- 20.E: Entropy and The Second Law of Thermodynamics (Exercises) — Undeclared
- 21: Entropy and the Third Law of Thermodynamics —
Undeclared
- 21.1: Entropy Increases With Increasing Temperature — Undeclared
- 21.2: The 3rd Law of Thermodynamics Puts Entropy on an Absolute Scale — Undeclared
- 21.3: The Entropy of a Phase Transition can be Calculated from the Enthalpy of the Phase Transition — Undeclared
- 21.4: The Debye Function is Used to Calculate the Heat Capacity at Low Temperatures — Undeclared
- 21.5: Practical Absolute Entropies Can Be Determined Calorimetrically — Undeclared
- 21.6: Practical Absolute Entropies of Gases Can Be Calculated from Partition Functions — Undeclared
- 21.7: Standard Entropies Depend Upon Molecular Mass and Structure — Undeclared
- 21.8: Spectroscopic Entropies sometimes disgree with Calorimetric Entropies — Undeclared
- 21.9: Standard Entropies Can Be Used to Calculate Entropy Changes of Chemical Reactions — Undeclared
- 21.E: Entropy and the Third Law of Thermodynamics (Exercises) — Undeclared
- 22: Helmholtz and Gibbs Energies —
Undeclared
- 22.1: Helmholtz Energy — Undeclared
- 22.2: Gibbs Energy Determines the Direction of Spontaneity at Constant Pressure and Temperature — Undeclared
- 22.3: The Maxwell Relations — Undeclared
- 22.4: The Enthalpy of an Ideal Gas is Independent of Pressure — Undeclared
- 22.5: Thermodynamic Functions have Natural Variables — Undeclared
- 22.6: The Standard State for a Gas is an Ideal Gas at 1 Bar — Undeclared
- 22.7: The Gibbs-Helmholtz Equation — Undeclared
- 22.8: Fugacity Measures Nonideality of a Gas — Undeclared
- 22.E: Helmholtz and Gibbs Energies (Exercises) — Undeclared
- 23: Phase Equilibria —
Undeclared
- 23.1: A Phase Diagram Summarizes the Solid-Liquid-Gas Behavior of a Substance — Undeclared
- 23.2: Gibbs Energies and Phase Diagrams — Undeclared
- 23.3: The Chemical Potentials of a Pure Substance in Two Phases in Equilibrium — Undeclared
- 23.4: The Clausius-Clapeyron Equation — CC BY 4.0
- 23.5: Chemical Potential Can be Evaluated From a Partition Function — Undeclared
- 23.E: Phase Equilibria (Exercises) — Undeclared
- 24: Solutions I- Liquid-Liquid Solutions —
Undeclared
- 24.1: Partial Molar Quantities in Solutions — Undeclared
- 24.2: The Gibbs-Duhem Equation — Undeclared
- 24.3: Chemical Potential of Each Component Has the Same Value in Each Phase in Which the Component Appears — Undeclared
- 24.4: Ideal Solutions obey Raoult's Law — Undeclared
- 24.5: Most Solutions are Not Ideal — Undeclared
- 24.6: Vapor Pressures of Volatile Binary Solutions — Undeclared
- 24.7: Activities of Nonideal Solutions — Undeclared
- 24.8: Activities are Calculated with Respect to Standard States — Undeclared
- 24.9: Gibbs Energy of Mixing of Binary Solutions in Terms of the Activity Coefficient — Undeclared
- 24.E: Solutions I- Liquid-Liquid Solutions (Exercises) — Undeclared
- 25: Solutions II - Solid-Liquid Solutions —
Undeclared
- 25.1: Raoult's and Henry's Laws Define Standard States — Undeclared
- 25.2: The Activities of Nonvolatile Solutes — Undeclared
- 25.3: Colligative Properties Depend only on Number Density — Undeclared
- 25.4: Osmotic Pressure can Determine Molecular Masses — Undeclared
- 25.5: Electrolytes Solutions are Nonideal at Low Concentrations — Undeclared
- 25.6: The Debye-Hückel Theory — Undeclared
- 25.7: Extending Debye-Hückel Theory to Higher Concentrations — Undeclared
- 25.8: Homework Problems — Undeclared
- 26: Chemical Equilibrium —
Undeclared
- 26.1: Equilibrium Results when Gibbs Energy is Minimized — Undeclared
- 26.2: An Equilibrium Constant is a Function of Temperature Only — Undeclared
- 26.3: Standard Gibbs Energies of Formation Can Be Used to Calculate Equilibrium Constants — Undeclared
- 26.4: Gibbs Energy of a Reaction vs. Extent of Reaction is a Minimum at Equilibrium — CC BY 4.0
- 26.5: Reaction Quotient and Equilibrium Constant Ratio Determines Reaction Direction — CC BY 4.0
- 26.6: The Sign of ΔG and not ΔG° Determines the Direction of Reaction Spontaneity — Undeclared
- 26.7: The van 't Hoff Equation — Undeclared
- 26.8: Equilibrium Constants in Terms of Partition Functions — CC BY-SA 4.0
- 26.9: Molecular Partition Functions and Related Thermodynamic Data Are Extensively Tabulated — Undeclared
- 26.10: Real Gases Are Expressed in Terms of Partial Fugacities — Undeclared
- 26.11: Thermodynamic Equilibrium Constants Are Expressed in Terms of Activities — Undeclared
- 26.12: Activities are Important for Ionic Species — Undeclared
- 26.13: Homework Problems — Undeclared
- 27: The Kinetic Theory of Gases —
Undeclared
- 27.1: The Average Translational Kinetic Energy of a Gas — Undeclared
- 27.2: The Gaussian Distribution of One Component of the Molecular Velocity — Undeclared
- 27.3: The Distribution of Molecular Speeds is Given by the Maxwell-Boltzmann Distribution — Undeclared
- 27.4: The Frequency of Collisions with a Wall — Undeclared
- 27.5: The Maxwell-Boltzmann Distribution Has Been Verified Experimentally — Undeclared
- 27.6: Mean Free Path — CC BY-NC-SA 4.0
- 27.7: Rates of Gas-Phase Chemical Reactions — Undeclared
- 27.E: The Kinetic Theory of Gases (Exercises) — Undeclared
- 28: Chemical Kinetics I - Rate Laws —
Undeclared
- 28.1: The Time Dependence of a Chemical Reaction is Described by a Rate Law — Undeclared
- 28.2: Rate Laws Must Be Determined Experimentally — Undeclared
- 28.3: First-Order Reactions Show an Exponential Decay of Reactant Concentration with Time — Undeclared
- 28.4: Different Rate Laws Predict Different Kinetics — Undeclared
- 28.5: Reactions can also be Reversible — Undeclared
- 28.6: The Rate Constants of a Reversible Reaction Can Be Determined Using Relaxation Techniques — Undeclared
- 28.7: Rate Constants Are Usually Strongly Temperature Dependent — Undeclared
- 28.8: Transition-State Theory Can Be Used to Estimate Reaction Rate Constants — Undeclared
- 28.E: Chemical Kinetics I - Rate Laws (Exercises) — Undeclared
- 29: Chemical Kinetics II- Reaction Mechanisms —
Undeclared
- 29.1: A Mechanism is a Sequence of Elementary Reactions — Undeclared
- 29.2: The Principle of Detailed Balance — Undeclared
- 29.3: Multiple Mechanisms are often Indistinguishable — Undeclared
- 29.4: The Steady-State Approximation — Undeclared
- 29.5: Rate Laws Do Not Imply Unique Mechanism — Undeclared
- 29.6: The Lindemann Mechanism — Undeclared
- 29.7: Some Reaction Mechanisms Involve Chain Reactions — Undeclared
- 29.8: A Catalyst Affects the Mechanism and Activation Energy — Undeclared
- 29.9: The Michaelis-Menten Mechanism for Enzyme Catalysis — Undeclared
- 29.E: Chemical Kinetics II- Reaction Mechanisms (Exercises) — Undeclared
- 30: Gas-Phase Reaction Dynamics —
Undeclared
- 30.1: The Rate of Bimolecular Gas-Phase Reaction Can Be Estimated Using Hard-Sphere Collision Theory and an Energy-Dependent Reaction Cross Section — Undeclared
- 30.2: A Reaction Cross Section Depends Upon the Impact Parameter — Undeclared
- 30.3: The Rate Constant for a Gas-Phase Chemical Reaction May Depend on the Orientations of the Colliding Molecules — Undeclared
- 30.4: The Internal Energy of the Reactants Can Affect the Cross Section of a Reaction — Undeclared
- 30.5: A Reactive Collision Can Be Described in a Center-of-Mass Coordinate System — Undeclared
- 30.6: Reactive Collisions Can be Studied Using Crossed Molecular Beam Machines — CC BY-SA 4.0
- 30.7: Reactions Can Produce Vibrationally Excited Molecules — Undeclared
- 30.8: The Velocity and Angular Distribution of the Products of a Reactive Collision — Undeclared
- 30.9: Not All Gas-Phase Chemical Reactions are Rebound Reactions — Undeclared
- 30.10: The Potential-Energy Surface Can Be Calculated Using Quantum Mechanics — Undeclared
- 30.E: Gas-Phase Reaction Dynamics (Exercises) — Undeclared
- 31: Solids and Surface Chemistry —
Undeclared
- 31.1: The Unit Cell is the Fundamental Building Block of a Crystal — Undeclared
- 31.2: The Orientation of a Lattice Plane is Described by its Miller Indices — Undeclared
- 31.3: The Spacing Between Lattice Planes Can Be Determined from X-Ray Diffraction Measurements — Undeclared
- 31.4: The Total Scattering Intensity is Related to the Periodic Structure of the Electron Density in the Crystal — CC BY 4.0
- 31.5: The Structure Factor and the Electron Density Are Related by a Fourier Transform — CC BY-NC-SA 4.0
- 31.6: Atoms and Molecules can Physisorb or Chemisorb to a Surface — Undeclared
- 31.7: Isotherms are Plots of Surface Coverage as a Function of Gas Pressure at Constant Temperature — Undeclared
- 31.8: Using Langmuir Isotherms to Derive Rate Laws for Surface-Catalyzed Gas-Phase Reactions — Undeclared
- 31.9: The Structure of a Surface is Different from that of a Bulk Solid — Undeclared
- 31.10: The Haber-Bosch Reaction Can Be Surface Catalyzed — Undeclared
- 31.E: Homework Problems — Undeclared
- 32: Math Chapters —
Undeclared
- 32.1: Complex Numbers — Undeclared
- 32.2: Probability and Statistics — Undeclared
- 32.3: Vectors — Undeclared
- 32.4: Spherical Coordinates — Undeclared
- 32.5: Determinants — Undeclared
- 32.6: Matrices — Undeclared
- 32.7: Numerical Methods — Undeclared
- 32.8: Partial Differentiation — Undeclared
- 32.9: Series and Limits — Undeclared
- 32.10: Fourier Analysis — Undeclared
- 32.11: The Binomial Distribution and Stirling's Appromixation — Undeclared
- Reference Tables —
Undeclared
- 10. Spherical Harmonic Wavefunctions — Undeclared
- Appendix 10: Solubility Products — Undeclared
- Table 1 Regions of the Electromagnetic Spectrum — Undeclared
- Table 2. Characteristics of Electromagnetic Radiation — Undeclared
- Table 5. Some Units Commonly Used in Quantum Chemistry — Undeclared
- Table 8 — Undeclared
- Table 9. The Greek Alphabet — Undeclared
- Table 11 Radial functions for one-electron atoms and ions. — Undeclared
- Table 14. The ground-state electron configurations of the elements. — Undeclared
- Back Matter — Undeclared