Chemical Structure and Bonding

Title Page
Preface to the Second Edition
Preface to the First Edition
Contents
Chapter 1. Atomic Structure
1-1. Rutherford’s Experiments and a Model for Atomic Structure
1-2. Atomic Number and Atomic Mass
1-3. Nuclear Structure
1-4. Bohr Theory of the Hydrogen Atom
1-5. Absorption and Emission Spectra of Atomic Hydrogen
1-6. Ionization Energy of Atomic Hydrogen
1-7. General Bohr Theory for a One-Electron Atom
1-8. Matter Waves
1-9. The Uncertainty Principle
1-10. Atomic Orbitals
1-11. The Wave Equation and the Particle-in-a-Box Problem
The Schrodinger Wave Equation
The Particle in a Box
1-12. The Wave Equation and the Hydrogen Atom
The Quantum Numbers
Quantum Number Specifications of Orbitals
1-13. Many-Electron Atoms
1-14. Effects of Electron-Electron Repulsion in Many-Electron Atoms
1-15. Atomic Energy States and Term Symbols
Energy States in Many-Electron Atoms
Energy States in Many-Electron Atoms Containing Equivalent Electrons
Ground-State Terms for Many-Electron Atoms
Determination of Only the Ground-State Term Symbol
Atomic Energy States and Valence-Orbital Ionization Energies
Questions and Problems
Suggestions for Further Reading
Chapter 2. Atomic and Molecular Properties
2-1 Lewis Structures for Atoms
2-2 Effective Atomic Radii in Molecules
2-3 Ionization Energy and Orbital Configuration
lonization Energies and Periodicity
Ionization Energies of Core Electrons
2-4 Electron Affinity
2-5 Covalent Bonding
2-6 Properties of H₂ and H₂⁺ in a Magnetic Field
2-7 Lewis Structures for Diatomic Molecules
2-8 Ionic Bonding
2-9 Electronegativity
2-10 A Covalent Bond With Ionic Character: The HCI Molecule
2-11 Lewis Structures For Polyatomic Molecules
Methane, Ammonia, and Water
Hydrides of Beryllium and Boron
Ammonium Chloride Molecule
2-12 Molecules With Double and Triple Bonds
2-13 Bonding to Heavier Atoms
2-14 Resonance
2-15 Molecular Geometry
The valence-shell electron-pair repulsion method and molecular geometry
VSEPR Applied To Molecules With Steric Number Greater Than Six
Exceptions to the VSEPR Rules
2-16 The Use of Lewis Structures to Predict Molecular Topology
2-17 Molecular Symmetry
2-18 Polar and Nonpolar Polyatomic Molecules
Questions and Problems
Suggestions for Further Reading
Chapter 3. The Valence Bond and Hybrid Orbital Descriptions of Chemical Bonding
3-1 Valence Bond Theory for the Hydrogen Molecule
3-2 Valence Bond Theory for Hydrogen Fluoride
3-3 Valence Bond Theory for the Water Molecule
3-4 Valence Bond Theory for the Ammonia Molecule
3-5 Valence Bond Theory for Molecules Containing No Lone-Pair Electrons
VB Theory for BeH₂
VB Theory for BH₃
VB Theory for CH₄
VB Theory for PH₅ and SH₆
3-6 Hybrid-Orbital Description of Single and Multiple Bonds in Carbon Compounds
Acetylene
Benzene
3-7 Mathematical Formulation of Hybrid Orbitals
3-8 Structure and Bonding in Boranes
Questions and Problems
Suggestions for Further Reading
Chapter 4. The Molecular-Orbital Theory of Electronic Structure and the Spectroscopic Properties of Diatomic Molecules
4-1 Bonding Theory for H₂⁺
Molecular-Orbital Energy Levels
Refinements in the Molecular-Orbital Treatment of H₂⁺
4-2 Molecular-Orbital Theory and Valence Bond Theory for H₂
4-3 Net Bonding in Molecules with 1s Valence Atomic Orbitals
4-4 Molecular Spectroscopy
4-5 Photoelectron Spectroscopy: An Experimental Method of Studying Molecular Orbitals
4-6 Molecules with s and p Valence Atomic Orbitals
Sigma Orbitals
Pi Orbitals
s-p Sigma Mixing
4-7 Homonuclear Diatomic Molecules
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
Summary
4-8 Term Symbols for Linear Molecules
4-9 Photoelectron Spectra of N₂, O₂, and F₂
Nitrogen
Oxygen and Fluorine
The Photoelectron Spectra of N₂, O₂, and F₂ Core Electrons
4-10 Homonuclear Diatomic Molecules of the Transition Elements
The V₂ Molecule
The Nb₂ Molecule
The Cu₂ Molecule
4-11 Heteronuclear Diatomic Molecules
Hydrogen Fluoride
Carbon Monoxide
Boron Monoftuoride
Bond Properties of Other Heteronuclear Diatomic Molecules and Ions
BO, CN, and CO⁺ (Nine Valence Electrons)
NO⁺, CO, and CN⁻ (Ten Valence Electrons)
NO (Eleven Valence Electrons)
Some Heteronuclear Transition-Metal Molecules
Questions and Problems
Suggestions for Further Reading
Chapter 5. Electronic Structures, Photoelectron Spectroscopy, and the Frontier-Orbital Theory of Reactions of Polyatomic Molecules
5-1 The Simplest Polyatomic Molecule, H₃⁺
5-2 Delocalized Molecular Orbitals for BeH₂ and H₂O
5-3 Delocalized Molecular Orbitals for BH₃ and NH₃
The Borane Molecule
The Ammonia Molecule
5-4 Delocalized Molecular Orbitals for CH₄
5-5 Photoelectron Spectra for the lsoelectronic Sequence Ne, HF, H₂O, NH₃, and CH₄
5-6 Delocalized Molecular Orbitals for CO₂ and XeF₂
Molecular Orbitals for CO₂
The Photoelectron Spectrum of CO₂
Molecular Orbitals for XeF₂
5-7 Molecular-Orbital Theory and Molecular Topology
5-8 Delocalized Molecular Orbitals in Carbon Compounds
Ethylene
Benzene
5-9 The Frontier-Orbital Concept
Proton Affinity and the Frontier-Orbital Concept
The Frontier-Orbital Concept Applied to Reactions of Carbon Monoxide
Symmetry Rules for Chemical Reactions
5-10 Molecular-Orbital Theory for Transition-Metal Molecules Containing One Unsaturated Ligand
5-11 Photoelectron Spectroscopy of Core Electrons
Questions and Problems
Suggestions for Further Reading