9.1: The Born-Oppenheimer Approximation Simplifies the Schrödinger 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 Different Atoms
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 Orbital
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 Orbitals and Whose Coefficients Are Determined Self-Consistently
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