I Chapter 8 Advanced Theories of Covalent Bonding A Bonding...

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I. Chapter 8 - Advanced Theories of Covalent Bonding A. Bonding Theories 1. Lewis Structures and VSPER models do a good job of depicting the arrangement of the atoms accurately around the central atoms 2. But they do not explain how bonds are formed or why carbon forms four separate, but equal, bonds from it valence electron 3. Two quantum mechanical descriptions of chemical bonding a) Valence Bonding (VB) theory (1) Describes the bonding in molecule using atomic orbitals (AOs) (2) Explains bonding through localized overlap of AOs b) Molecular Orbital (MO) theory (1) Describes the bonding in molecules using molecular orbits (2) Explains bonding using electron orbitals delocalized over the entire molecule B. Valence Bond theory 1. Basic Principles a) A covalent bond forms when the partially filled (one electron) atomic orbitals of two atoms overlap b) The overlapping region becomes occupied by the two electrons (one from each atom) c) The two electrons (with opposing spins) can be described by two wave wave functions that are in phase with each other, thus increasing the amplitude of the wave function where the orbitals overlap 2. Themes a) The set of overlapping orbitals ahs a max or two electrons which must have opposing spins b) The greater the overlap, the stronger the bond and the more stable 3. Orbital shapes and Overlap a) The covalent bond between hydrogen atosm occurs when the two 1s orbitals overplay and share electrons b)
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