lecture11 - Molecular geometry Chem 1A Lecture 11: Beyond...

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Unformatted text preview: Molecular geometry Chem 1A Lecture 11: Beyond Lewis structures Many of the interesting properties of water result from its shape and cannot be predicted from the Lewis structure. Lewis structures are useful for keeping track of the number and placement of electrons in a molecule. They do not tell us anything about the geometry. O H H O H H Beyond Lewis structures Many of the interesting properties of water result from its shape and cannot be predicted from the Lewis structure. Lewis structures are useful for keeping track of the number and placement of electrons in a molecule. They do not tell us anything about the geometry. O H H O H H Molecules are more exciting in 3D! C H H H H VSEPR theory V alence S hell E lectron P air R epulsion Because electrons are negatively charged, they repel each other. In a molecule, bonds and lone pairs stay as far apart as possible. Valence electrons Number of dots = number of valence electrons Only valence electrons participate in bonding. VSEPR theory - rules The arrangement of bonds and lone pairs around the central atom is controlled by electrostatic repulsion. Double and triple bonds can be treated approximately like single bonds. If a molecule has resonance structures, VSEPR can be applied to all of them. Arrange all bonds and lone pairs as far apart as possible. Lone pairs have more repulsion than bonds, causing distortion in the structure. Linear molecule - AB 2 Examples: BeCl 2 , CO 2 , HCN C N H O O C Be Cl Cl Bond angles all 180 Trigonal planar molecule - AB...
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This note was uploaded on 02/25/2012 for the course CHEM 1A 40030 taught by Professor Borovick during the Fall '10 term at UC Irvine.

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lecture11 - Molecular geometry Chem 1A Lecture 11: Beyond...

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