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Chemical Bonding

1. General Principles
2. Molecular Orbital Theory
3. Lewis Theory of Bonding
4. Valence Bond Theory

When molecules share electrons, they form bonds. Atoms can share one, two, or three pairs of electrons, forming single, double, and triple bonds, respectively. Although it is impossible to determine the exact position of the electron, it is possible to calculate the probablity that one will find the electron in a point around the nucleus.

General Principles Covalent Bonds vs Ionic Bonds General Principles Bond Energies Bond Order and Lengths Born Oppenheimer Approximation Covalent Bond Distance, Radius and van der Waals Radius Covalent Bonds Non-Singular Covalent Bonds Electrostatic Potential maps Ionic Bonds Metallic Bonding	Molecular Orbital Theory Molecular Orbital Theory Bonding and antibonding orbitals How to Build Molecular Orbitals MO bonding in F2 and O2 Molecular Orbitals - Example 1: Water Interactive MO: Water
Lewis Theory of Bonding Lewis Theory of Bonding Geometry of Molecules Lewis Structures Lewis Symbols Violations of the Octet Rule Exceptions to the Octet Rule	Valence Bond Theory Contrasting MO and VB theory Valence Bond Theory Hybridization Localized Bonding Resonance Delocalization of Electrons

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Chemical Bonding

Table of contents

General Principles

Molecular Orbital Theory

Lewis Theory of Bonding

Valence Bond Theory