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• Values of Some Physical Constants & Data Tables
• Some Mathematical Formulas & SI Prefixed
• Title Page
• Copyright Page
• Detailed Table of Contents
• Preface
• About the website
• Acknowledgments
• Max Planck
• Chapter 1: The Dawn of the Quantum Theory
• 1-1. Blackbody Radiation Could Not Be Explained by Classical Physics
• 1-2. Planck Used a Quantum Hypothesis to Derive the Blackbody Radiation Law
• 1-3. Einstein Explained the Photoelectric Effect with a Quantum Hypothesis
• 1-4. The Hydrogen Atomic Spectrum Consists of Several Series of Lines
• 1-5. The Rydberg Formula Accounts for All the Lines in the Hydrogen Atomic Spectrum
• 1-6. Louis de Broglie Postulated That Matter Has Wavelike Properties
• 1-7. de Broglie Waves Are Observed Experimentally
• 1-8. The Bohr Theory of the Hydrogen Atom Can Be Used to Derive the Rydberg Formula
• 1-9. The Heisenberg Uncertainty Principle States That the Position and the Momentum of a Particle Ca
• Problems
• MathChapter A: Complex Numbers
• Louis de Broglie
• Chapter 2: The Classical Wave Equation
• 2-1. The One-Dimensional Wave Equation Describes the Motion of a Vibrating String
• 2-2. The Wave Equation Can Be Solved by the Method of Separation of Variables
• 2-3. Some Differential Equations Have Oscillatory Solutions
• 2-4. The General Solution to the Wave Equation Is a Superposition of Normal Modes
• 2-5. A Vibrating Membrane Is Described by a Two-Dimensional Wave Equation
• Problems
• MathChapter B: Probability and Statistics
• Erwin Schrodiner
• Chapter 3: The Schrodinger Equation and a Particle In a Box
• 3-1. The Schrodinger Equation Is the Equation for Finding the Wave Function of a Particle
• 3-2. Classical-Mechanical Quantities Are Represented by Linear Operators in Quantum Mechanics
• 3-3. The Schrodinger Equation Can Be Formulated as an Eigenvalue Problem
• 3-4. Wave Functions Have a Probabilistic Interpretation
• 3-5. The Energy of a Particle in a Box Is Quantized
• 3-6. Wave Functions Must Be Normalized
• 3-7. The Average Momentum of a Particle in a Box Is Zero
• 3-8. The Uncertainty Principle Says That apax > h/2
• 3-9. The Problem of a Particle in a Three-Dimensional Box Is a Simple Extension of the One-Dimension
• Problems
• MathChapter C: Vectors
• Werner Heisenberg
• Chapter 4: Some Postulates and General Principles of Quantum Mechanics
• 4-1. The State of a System Is Completely Specified by its Wave Function
• 4-2. Quantum-Mechanical Operators Represent Classical-Mechanical Variables
• 4-3. Observable Quantities Must Be Eigenvalues of Quantum Mechanical Operators
• 4-4. The Time Dependence of Wave Functions Is Governed by the Time-Dependent Schrodinger Equation
• 4-5. The Eigenfunctions of Quantum Mechanical Operators Are Orthogonal
• 4-6. The Physical Quantities Corresponding to Operators That Commute Can Be Measured Simultaneously
• Problems
• MathChapter D
• E. Bright Wilson, Jr.
• Chapter 5: The Harmonic Oscillator and the Rigid Rotator: Two Spectroscropic Models
• 5-1. A Harmonic Oscillator Obeys Hooke’s Law
• 5-2. The Equation for a Harmonic-Oscillator Model of a Diatomic Molecule Contains the Reduced Mass o
• 5-3. The Harmonic-Oscillator Approximation Results from the Expansion of an Internuclear Potential A
• 5-4. The Energy Levels of a Quantum-Mechanical Harmonic Oscillator Are Ev = nw(v +1/2) with v = 0, I
• 5-5. The Harmonic Oscillator Accounts for the Infrared Spectrum of a Diatomic Molecule
• 5-6. The Harmonic-Oscillator Wave Functions Involve Hermite Polynomials
• 5-7. Hermite Polynomials Are Either Even or Odd Functions
• 5-8. The Energy Levels of a Rigid Rotator Are E = h2 J(J + 1)/2I
• 5-9. The Rigid Rotator Is a Model for a Rotating Diatomic Molecule
• Problems
• Niels Bohr
• Chapter 6: The Hydrogen Atom
• 6-1. The Schrodinger Equation for the Hydrogen Atom Can Be Solved Exactly
• 6-2. The Wave Functions of a Rigid Rotator Are Called Spherical Harmonics
• 6-3. Precise Values of the Three Components of Angular Momentum Cannot Be Measured Simultaneously
• 6-4. Hydrogen Atomic Orbitals Depend upon Three Quantum Numbers
• 6-5. s Orbitals Are Spherically Symmetric
• 6-6. There Are Three p Orbitals for Each Value of the Principal Quantum Number, n > 2
• 6-7. The Schrodinger Equation for the Helium Atom Cannot Be Solved Exactly
• Problems
• MathChapter E: Determinants
• Douglas Hartree
• Chapter 7: Approximation Methods
• 7-1. The Variational Method Provides an Upper Bound to the Ground-State Energy of a System
• 7-2. A Trial Function That Depends Linearly on the Variational Parameters Leads to a Secular Determi
• 7-3. Trial Functions Can Be Linear Combinations of Functions that Also Contain Variational Parameter
• 7-4. Perturbation Theory Expresses the Solution to One Problem in Terms of Another Problem Solved Pr
• Problems
• Charlotte E. Moore
• Chapter 8: Multielectron Atoms
• 8-1. Atomic and Molecular Calculations Are Expressed in Atomic Units
• 8-2. Both Perturbation Theory and the Variational Method Can Yield Excellent Results for Helium
• 8-3. Hartree-Fock Equations Are Solved by the Self-Consistent Field Method
• 8-4. An Electron Has An Intrinsic Spin Angular Momentum
• 8-5. Wave Functions Must Be Antisymmetric in the Interchange of Any Two Electrons
• 8-6. Antisymmetric Wave Functions Can Be Represented by Slater Determinants
• 8-7. Hartree-Fock Calculations Give Good Agreement with Experimental Data
• 8-8. A Term Symbol Gives a Detailed Description of an Electron Configuration
• 8-9. The Allowed Values of J are L + S, L + S- I, … , IL- Sl
• 8-10. Hund’s Rules Are Used to Determine the Term Symbol of the Ground Electronic State
• 8-11. Atomic Term Symbols Are Used to Describe Atomic Spectra
• Problems
• Robert S. Mulliken
• Chapter 9: The Chemical Bond: Diatomic Molecules
• 9-1. The Born-Oppenheimer Approximation Simplifies the Schrodinger Equation for Molecules
• 9-2. H2 Is the Prototypical Species of Molecular-Orbital Theory
• 9-3. The Overlap Integral Is a Quantitative Measure of the Overlap of Atomic Orbitals Situated on Di
• 9-4. The Stability of a Chemical Bond Is a Quantum-Mechanical Effect
• 9-5. The Simplest Molecular Orbital Treatment of H2 Yields a Bonding Orbital and an Antibonding Orbi
• 9-6. A Simple Molecular-Orbital Treatment of H2 Places Both Electrons in a Bonding Orbital
• 9-7. Molecular Orbitals Can Be Ordered According to Their Energies
• 9-8. Molecular-Orbital Theory Predicts that a Stable Diatomic Helium Molecule Does Not Exist
• 9-9. Electrons Are Placed into Molecular Orbitals in Accord with the Pauli Exclusion Principle
• 9-10. Molecular-Orbital Theory Correctly Predicts that Oxygen Molecules Are Paramagnetic
• 9-11. Photoelectron Spectra Support the Existence of Molecular Orbitals
• 9-12. Molecular-Orbital Theory Also Applies to Heteronuclear Diatomic Molecules
• 9-13. An SCF-LCAO-MO Wave Function Is a Molecular Orbital Formed from a Linear Combination of Atomic
• 9-14. Electronic States of Molecules Are Designated by Molecular Term Symbols
• 9-15. Molecular Term Symbols Designate the Symmetry Properties of Molecular Wave Functions
• 9-16. Most Molecules Have Excited Electronic States
• Problems
• Linus Pauling
• Chapter 10: Bonding in Polyatomic Molecules
• 10-1. Hybrid Orbitals Account for Molecular Shape
• 10-2. Different Hybrid Orbitals Are Used for the Bonding Electrons and the Lone Pair Electrons in Wa
• 10-3. Why is BeH2 Linear and H20 Bent?
• 10-4. Photoelectron Spectroscopy Can Be Used to Study Molecular Orbitals
• 10-5. Conjugated Hydrocarbons and Aromatic Hydrocarbons Can Be Treated by a pi-Electron Approximatio
• 10-6. Butadiene Is Stabilized by a Delocalization Energy
• Problems
• John Pople
• Chapter 11: Computational Quantum Chemistry
• 11-1. Gaussian Basis Sets Are Often Used in Modern Computational Chemistry
• 11-2. Extended Basis Sets Accurately Account for the Size and Shape of Molecular Charge Distribution
• 11-3. Asterisks in the Designation of a Basis Set Denote Orbital Polarization Terms
• 11-4. The Ground-State Energy of H2 Can Be Calculated Essentially Exactly
• 11-5. GAUSSIAN 94 Calculations Provide Accurate Information About Molecules
• Problem
• Math Chapter F: Matrices
• Buckminsterfullerene
• Chapter 12: Group Theory: The Exploitation of Symmetry
• 12-1. The Exploitation of the Symmetry of a Molecule Can Be Used to Significantly Simplify Numerical
• 12-2. The Symmetry of Molecules Can Be Described by a Set of Symmetry Elements
• 12-3. The Symmetry Operations of a Molecule Form a Group
• 12-4. Symmetry Operations Can Be Represented by Matrices
• 12-5. The C3v Point Group Has a Two-Dimensional Irreducible Representation
• 12-6. The Most Important Summary of the Properties of a Point Group Is Its Character Table
• 12-7. Several Mathematical Relations Involve the Characters of Irreducible Representations
• 12-8. We Use Symmetry Arguments to Predict Which Elements in a Secular Determinant Equal Zero
• 12-9. Generating Operators Are Used to Find Linear Combinations of Atomic Orbitals That Are Bases fo
• Problems
• Gerhard Herzberg
• Chapter 13: Molecular Spectroscopy
• 13-1. Different Regions of the Electromagnetic Spectrum Are Used to Investigate Different Molecular
• 13-2. Rotational Transitions Accompany Vibrational Transitions
• 13-3. Vibration-Rotation Interaction Accounts for the Unequal Spacing of the Lines in the P and R Br
• 13-4. The Lines in a Pure Rotational Spectrum Are Not Equally Spaced
• 13-5. Overtones Are Observed in Vibrational Spectra
• 13-6. Electronic Spectra Contain Electronic, Vibrational, and Rotational Information
• 13-7. The Franck-Condon Principle Predicts the Relative Intensities of Vibronic Transitions
• 13-8. The Rotational Spectrum of a Polyatomic Molecule Depends Upon the Principal Moments of Inertia
• 13-9. The Vibrations of Polyatomic Molecules Are Represented by Normal Coordinates
• 13-10. Normal Coordinates Belong to Irreducible Representations of Molecular Point Groups
• 13-11. Selection Rules Are Derived from Time-Dependent Perturbation Theory
• 13-12. The Selection Rule in the Rigid-Rotator ApproximationIs DJ= ±1
• 13-13. The Harmonic-Oscillator Selection Rule Is Dv = ±1
• 13-14. Group Theory Is Used to Determine the Infrared Activity of Normal Mode Vibrations
• Problems
• Richard R. Ernst
• Chapter 14: Nuclear Magnetic Resonance Spectroscopy
• 14-1. Nuclei Have Intrinsic Spin Angular Momenta
• 14-2. Magnetic Moments Interact with Magnetic Fields
• 14-3. Proton NMR Spectrometers Operate at Frequencies Between 60 MHz and 750 MHz
• 14-4. The Magnetic Field Acting upon Nuclei in Molecules Is Shielded
• 14-5. Chemical Shifts Depend upon the Chemical Environment of the Nucleus
• 14-6. Spin-Spin Coupling Can Lead to Multiplets in NMR Spectra
• 14-7. Spin-Spin Coupling Between Chemically Equivalent ProtonsIs Not Observed
• 14-8. The n+1 Rule Applies Only to First-Order Spectra
• 14-9. Second-Order Spectra Can Be Calculated Exactly Using the Variational Method
• Problems
• Richard N. Zare
• Chapter 15: Lasers, Laser Spectroscopy, and Photochemistry
• 15-1. Electronically Excited Molecules Can Relax by a Number of Processes
• 15-2. The Dynamics of Spectroscopic Transitions Between the Electronic States of Atoms Can Be Modele
• 15-3. A Two-Level System Cannot Achieve a Population Inversion
• 15-4. Population Inversion Can Be Achieved in a Three-Level System
• 15-5. What is Inside a Laser?
• 15-6. The Helium-Neon Laser Is an Electrical-Discharge Pumped, Continuous-Wave, Gas-Phase Laser
• 15-7. High-Resolution Laser Spectroscopy Can Resolve Absorption Lines that Cannot Be Distinguished b
• 15-8. Pulsed Lasers Can Be Used to Measure the Dynamics of Photochemical Processes
• Problems
• MathChapter G: Numerical Methods
• Johannes Diderik van der Waals
• Chapter 16: The Properties of Gases
• 16-1. All Gases Behave Ideally If They Are Sufficiently Dilute
• 16-2. The van der Waals Equation and the RedIich-Kwong Equation Are Examples of Two-Parameter Equati
• 16-3. A Cubic Equation of State Can Describe Both the Gaseous and Liquid States
• 16-4. The van der Waals Equation and the Redlich-Kwong Equation Obey the Law of Corresponding States
• 16-5. Second Virial Coefficients Can Be Used to Determine Intermolecular Potentials
• 16-6. London Dispersion Forces Are Often the Largest Contribution to the r-6 Term in the Lennard-Jan
• 16-7. The van der Waals Constants Can Be Written in Terms of Molecular Parameters
• Problems
• MathChapter H: Partial Differentiation
• Ludwig Boltzmann
• Chapter 17: The Boltzmann Factor and Partition Functions
• 17-1. The Boltzmann Factor Is One of the Most Important Quantities in the Physical Sciences
• 17-2. The Probability That a System in an Ensemble Is in the State j with Energy Ej (N, V) Is Propor
• 17-3. We Postulate That the Average Ensemble Energy Is Equal to the Observed Energy of a System
• 17-4. The Heat Capacity at Constant Volume Is the Temperature Derivative of the Average Energy
• 17-5. We Can Express the Pressure in Terms of a Partition Function
• 17-6. The Partition Function of a System of Independent, Distinguishable Molecules Is the Product of
• 17-7. The Partition Function of a System of Independent, Indistinguishable Atoms or Molecules Can Us
• 17-8. A Molecular Partition Function Can Be Decomposed into Partition Functions for Each Degree of F
• Problems
• MathChapter I: Series and Limits
• William Francis Giauque
• Chapter 18: Partition Functions and Ideal Gases
• 18-1. The Translational Partition Function of an Atom in a Monatomic Ideal Gas is (2pimkBT / h2)3/2
• 18-2. Most Atoms Are in the Ground Electronic State at Room Temperature
• 18-3. The Energy of a Diatomic Molecule Can Be Approximated as a Sum of Separate Terms
• 18-4. Most Molecules Are in the Ground Vibrational State at Room Temperature
• 18-5. Most Molecules Are in Excited Rotational States at Ordinary Temperatures
• 18-6. Rotational Partition Functions Contain a Symmetry Number
• 18-7. The Vibrational Partition Function of a Polyatomic Molecule Is a Product of Harmonic Oscillato
• 18-8. The Form of the Rotational Partition Function of a Polyatomic Molecule Depends Upon the Shape
• 18-9. Calculated Molar Heat Capacities Are in Very Good Agreement with Experimental Data
• Problems
• James Prescott Joule
• Chapter 19: The First Law of Thermodynamics
• 19-1. A Common Type of Work Is Pressure-Volume Work
• 19-2. Work and Heat Are Not State Functions, but Energy Is a State Function
• 19-3. The First Law of Thermodynamics Says the Energy Is a State Function
• 19-4. An Adiabatic Process Is a Process in Which No Energy as Heat Is Transferred
• 19-5. The Temperature of a Gas Decreases in a Reversible Adiabatic Expansion
• 19-6. Work and Heat Have a Simple Molecular Interpretation
• 19-7. The Enthalpy Change Is Equal to the Energy Transferred as Heat in a Constant-Pressure Process
• 19-8. Heat Capacity Is a Path Function
• 19-9. Relative Enthalpies Can Be Determined from Heat Capacity Data and Heats of Transition
• 19-10. Enthalpy Changes for Chemical Equations Are Additive
• 19-11. Heats of Reactions Can Be Calculated from Tabulated Heats of Formation
• 19-12. The Temperature Dependence of DrH Is Given in Terms of the Heat Capacities of the Reactants a
• Problems
• MathChapter J: The Binomial Distribution and Stirling’s Approximation
• Rudolf Clausius
• Chapter 20: Entropy and the Second Law of Thermodynamics
• 20-1. The Change of Energy Alone Is Not Sufficient to Determine the Direction of a Spontaneous Proce
• 20-2. Nonequilibrium Isolated Systems Evolve in a Direction That Increases Their Disorder
• 20-3. Unlike Qrev, Entropy Is a State Function
• 20-4. The Second Law of Thermodynamics States That the Entropy of an Isolated System Increases as a
• 20-5. The Most Famous Equation of Statistical Thermodynamics Is S= kB ln W
• 20-6. We Must Always Devise a Reversible Process to Calculate Entropy Changes
• 20-7. Thermodynamics Gives Us Insight into the Conversion of Heat into Work
• 20-8. Entropy Can Be Expressed in Terms of a Partition Function
• 20-9. The Molecular Formula S= kB In W Is Analogous to the Thermodynamic Formula dS = Sqrev/T
• Problems
• Walther Nernst
• Chapter 21: Entropy and the Third Law of Thermodynamics
• 21-1. Entropy Increases with Increasing Temperature
• 21-2. The Third Law of Thermodynamics Says That the Entropy of a Perfect Crystal Is Zero at 0 K
• 21-3. DtrsS = DtrsHf/Ttrs at a Phase Transition
• 21-4. The Third Law of Thermodynamics Asserts That Cp –> 0 as T –> 0
• 21-5. Practical Absolute Entropies Can Be Determined Calorimetrically
• 21-6. Practical Absolute Entropies of Gases Can Be Calculated from Partition Functions
• 21-7. The Values of Standard Molar Entropies Depend Upon Molecular Mass and Molecular Structure
• 21-8. The Spectroscopic Entropies of a Few Substances Do Not Agree with the Calorimetric Entropies
• 21-9. Standard Entropies Can Be Used to Calculate Entropy Changes of Chemical Reactions
• Problems
• Hermann von Helmholtz
• Chapter 22: Helmholtz and Gibbs Energies
• 22-1. The Sign of the Helmholtz Energy Change Determines the Direction of a Spontaneous Process in a
• 22-2. The Gibbs Energy Determines the Direction of a Spontaneous Process for a System at Constant Pr
• 22-3. Maxwell Relations Provide Several Useful Thermodynamic Formulas
• 22-4. The Enthalpy of an Ideal Gas Is Independent of Pressure
• 22-5. The Various Thermodynamic Functions Have Natural Independent Variables
• 22-6. The Standard State for a Gas at Any Temperature Is the Hypothetical Ideal Gas at One Bar
• 22-7. The Gibbs-Helmholtz Equation Describes the Temperature Dependence of the Gibbs Energy
• 22-8. Fugacity Is a Measure of the Nonideality of a Gas
• Problems
• Josiah Willard Gibbs
• Chapter 23: Phase Equilibria
• 23-1. A Phase Diagram Summarizes the Solid-Liquid-Gas Behavior of a Substance
• 23-2. The Gibbs Energy of a Substance Has a Close Connection to Its Phase Diagram
• 23-3. The Chemical Potentials of a Pure Substance in Two Phases in Equilibrium Are Equal
• 23-4. The Clausius-Clapeyron Equation Gives the Vapor Pressure of a Substance As a Function of Tempe
• 23-5. Chemical Potential Can Be Evaluated From a Partition Function
• Problems
• Joel Hildebrand
• Chapter 24: Solutions I: Liquid-Liquid Solutions
• 24-1. Partial Molar Quantities Are Important Thermodynamic Properties of Solutions
• 24-2. The Gibbs-Duhem Equation Relates the Change in the Chemical Potential of One Component of a So
• 24-3. At Equilibrium, the Chemical Potential of Each Component Has the Same Value in Each Phase in W
• 24-4. The Components of an Ideal Solution Obey Raoult’s Law for AII Concentrations
• 24-5. Most Solutions Are Not Ideal
• 24-6. The Gibbs-Duhem Equation Relates the Vapor Pressures of the Two Components of a Volatile Binar
• 24-7. The Central Thermodynamic Quantity for Nonideal Solutions Is the Activity
• 24-8. Activities Must Be Calculated with Respect to Standard States
• 24-9. We Can Calculate the Gibbs Energy of Mixing of Binary Solutions in Terms of the Activity Coeff
• Problems
• Peter Debye
• Chapter 25: Solutions II: Solid-Liquid Solutions
• 25-1. We Use a Raoult’s Law Standard State for the Solvent and a Henry’s Law Standard State for the
• 25-2. The Activity of a Nonvolatile Solute Can Be Obtained from the Vapor Pressure of the Solvent
• 25-3. Colligative Properties Are Solution Properties That Depend Only Upon the Number Density of Sol
• 25-4. Osmotic Pressure Can Be Used to Determine the Molecular Masses of Polymers
• 25-5. Solutions of Electrolytes Are Nonideal at Relatively Low Concentrations
• 25-6. The Debye-Huckel Theory Gives an Exact Expression for In Y±for Very Dilute Solutions
• 25-7. The Mean Spherical Approximation Is an Extension of the Debye-Huckel Theory to Higher Concentr
• Problems
• Gilbert Newton Lewis
• Chapter 26: Chemical Equilibrium
• 26-1. Chemical Equilibrium Results When the Gibbs Energy Is a Minimum with Respect to the Extent of
• 26-2. An Equilibrium Constant Is a Function of Temperature Only
• 26-3. Standard Gibbs Energies of Formation Can Be Used to Calculate Equilibrium Constants
• 26-4. A Plot of the Gibbs Energy of a Reaction Mixture Against the Extent of Reaction Is a Minimum a
• 26-5. The Ratio of the Reaction Quotient to the Equilibrium Constant Determines the Direction in Whi
• 26-6. The Sign of DrG And Not That of DrGc Determines the Direction of Reaction Spontaneity
• 26-7. The Variation of an Equilibrium Constant with Temperature Is Given by the Van’t Hoff Equation
• 26-8. We Can Calculate Equilibrium Constants in Terms of Partition Functions
• 26-9. Molecular Partition Functions and Related Thermodynamic Data Are Extensively Tabulated
• 26-10. Equilibrium Constants for Real Gases Are Expressed in Terms of Partial Fugacities
• 26-11. Thermodynamic Equilibrium Constants Are Expressed in Terms of Activities
• 26-12. The Use of Activities Makes a Significant Difference in Solubility Calculations Involving Ion
• Problems
• James Clerk Maxwell
• Chapter 27: The Kinetic Theory of Gases
• 27-1. The Average Translational Kinetic Energy of the Molecules in a Gas Is Directly Proportional to
• 27-2. The Distribution of the Components of Molecular Speeds Are Described by a Gaussian Distributio
• 27-3. The Distribution of Molecular Speeds Is Given by the Maxwell-Boltzmann Distribution
• 27-4. The Frequency of Collisions that a Gas Makes with a Wall Is Proportional to its Number Density
• 27-5. The Maxwell-Boltzmann Distribution Has Been Verified Experimentally
• 27-6. The Mean Free Path Is the Average Distance a Molecule Travels Between Collisions
• 27-7. The Rate of a Gas-Phase Chemical Reaction Depends Upon the Rate of Collisions in Which the Rel
• Problems
• Svante Arrhenius
• Chapter 28: Chemical Kinetics 1: Rate Laws
• 28-1. The Time Dependence of a Chemical Reaction Is Described by a Rate Law
• 28-2. Rate Laws Must Be Determined Experimentally
• 28-3. First-Order Reactions Show an Exponential Decay of Reactant Concentration with Time
• 28-4. The Rate Laws for Different Reaction Orders Predict Different Behaviors for Time-Dependent Rea
• 28-5. Reactions Can Also Be Reversible
• 28-6. The Rate Constants of a Reversible Reaction Can Be Determined Using Relaxation Methods
• 28-7. Rate Constants Are Usually Strongly Temperature Dependent
• 28-8. Transition-State Theory Can Be Used to Estimate Reaction Rate Constants
• Problems
• Sherwood Rowland, Mario J. Molina, Paul J. Crutzen
• Chapter 29: Chemical KineticsII: Reaction Mechanisms
• 29-1. A Mechanism Is a Sequence of Single-Step Chemical Reactions Called Elementary Reactions
• 29-2. The Principle of Detailed Balance States that when a Complex Reaction Is at Equilibrium, the R
• 29-3. When Are Consecutive and Single-Step Reactions Distinguishable?
• 29-4. The Steady-State Approximation Simplifies Rate Expressions by Assuming that d[l]/dt = 0, where
• 29-5. The Rate Law for a Complex Reaction Does Not Imply a Unique Mechanism
• 29-6. The Lindemann Mechanism Explains How Unimolecular Reactions Occur
• 29-7. Some Reaction Mechanisms Involve Chain Reactions
• 29-8. A Catalyst Affects the Mechanism and Activation Energy of a Chemical Reaction
• 29-9. The Michaelis-Menten Mechanism Is a Reaction Mechanismfor Enzyme Catalysis
• Problems
• Yuan T. Lee, Dudley Herschbach, John c. Polanyi
• Chapter 30: Gas-Phase Reaction Dynamics
• 30-1. The Rate of a Bimolecular Gas-Phase Reaction Can Be Calculated Using Hard-Sphere Collision The
• 30-2. A Reaction Cross Section Depends Upon the Impact Parameter
• 30-3. The Rate Constant for a Gas-Phase Chemical Reaction May Depend on the Orientations of the Coll
• 30-4. The Internal Energy of the Reactants Can Affect the Cross Section of a Reaction
• 30-5. A Reactive Collision Can Be Described in a Center-of-Mass Coordinate System
• 30-6. Reactive Collisions Can Be Studied Using Crossed Molecular Beam Machines
• 30-7. The Reaction F(g) + D2(g) => DF(g) + D(g) Can Produce Vibrationally Excited DF(g) Molecules
• 30-8. The Velocity and Angular Distribution of the Products of a Reactive Collision Provide a Molecu
• 30-9. Not All Gas-Phase Chemical Reactions Are Rebound Reactions
• 30-10. The Potential-Energy Surface for the Reaction F(g) + D2(g) => DF(g) + D(g) Can Be Calculated
• Problems
• Dorothy Crowfoot Hodgkin
• Chapter 31: Solids and Surface Chemistry
• 31-1. The Unit Cell Is the Fundamental Building Block of a Crystal
• 31-2. The Orientation of a Lattice Plane Is Described by its Miller Indices
• 31-3. The Spacing Between Lattice Planes Can Be Determined from X-Ray Diffraction Measurements
• 31-4. The Total Scattering Intensity Is Related to the Periodic Structure of the Electron Density in
• 31-5. The Structure Factor and the Electron Density Are Related by a Fourier Transform
• 31-6. A Gas Molecule Can Physisorb or Chemisorb to a Solid Surface
• 31-7. Isotherms Are Plots of Surface Coverage as a Function of Gas Pressure at Constant Temperature
• 31-8. The Langmuir Adsorption Isotherm Can Be Used to Derive Rate Laws for Surface-Catalyzed Gas-Pha
• 31-9. The Structure of a Surface Is Different from that of a Bulk Solid
• 31-10. The Reaction Between H2(g) and N2(g) to Produce NH3(g) Can Be Surface Catalyzed
• Problems
• Answers to the Numerical Problems
• Illustration Credits
• Index