057_Ho_5_RG_2_07 - Chem 057 J. Walcott CENTER FOR LEARNING...

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Chem 057 CENTER FOR LEARNING AND TEACHING Handout #5 J. Walcott LEARNING STRATEGIES CENTER Fall 2007 Review Guide #2 Lecture: 8/27/07 – 8/31/07: Chapter 1 I. Lewis Structures and Formal Charges Please refer to Review Guide #1 for the general procedure for writing Lewis structures and for calculating formal charges on atoms. II. Molecular Shapes/Bonding A. Molecular Orbital (MO) Theory When two atomic orbitals come together they will form a bond if the energy of the molecule created is lower than the energy of the individual atoms. Electrons in orbitals with wavefunctions having constructive overlap are in bonding molecular orbitals . Electrons in orbitals with wavefunctions having destructive overlap (cancellation of the wave in the region of overlap producing a node) are in anti-bonding molecular orbitals . Chemical bonding can occur when there is a net decrease in bonding energy. B. VSEPR theory 1. From the Lewis structures with single, double or triple bonds, we can predict bond angles using the VSEPR (valence-shell electron-pair repulsion) model. According to the VSEPR model, the outer shell valence electrons may form single, double or triple bonds, or they may be unshared. Each situation creates a negatively charged region of space. Because like charges repel each other, the regions of electron density around an atom
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This note was uploaded on 09/12/2008 for the course CHEM 057 taught by Professor Walcott, j during the Fall '07 term at Cornell University (Engineering School).

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057_Ho_5_RG_2_07 - Chem 057 J. Walcott CENTER FOR LEARNING...

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