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ISBN 10: 1891389962
ISBN 13: 9781891389962
Author: Donald McQuarrie, John Simon
As the first modern physical chemistry textbook to cover quantum mechanics before thermodynamics and kinetics, this book provides a contemporary approach to the study of physical chemistry. By beginning with quantum chemistry, students will learn the fundamental principles upon which all modern physical chemistry is built. The text includes a special set of “MathChapters” to review and summarize the mathematical tools required to master the material Thermodynamics is simultaneously taught from a bulk and microscopic viewpoint that enables the student to understand how bulk properties of materials are related to the properties of individual constituent molecules. This new text includes a variety of modern research topics in physical chemistry as well as hundreds of worked problems and examples.Translated into French, Italian, Japanese, Spanish and Polish.
Physical Chemistry A Molecular Approach 1st Table of contents:
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
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