VSEPR - VSEPR The shapes of covalently bonded molecules and...

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VSEPR The shapes of covalently bonded molecules and ions can be determined by considering the number of electron pairs around the central atom. The electron pairs repel one another and try to get as far apart as possible. This theory is called Valence Shell Electron Pair Repulsion theory or VSEPR. There are some standard shapes for specific numbers of electron pairs and some simple deviations from this theory when non-bonding pairs are present around the central atom. A non-bonding pair will repel more strongly than a bonding pair. When comparing bond angles it can be seen that this has the effect of altering the bond angles and the shape of molecules that have a similar total number of electron pairs around the central atom.
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Number of pairs around central atom Full description of the molecule BONDING NON- BONDING (LONE) Example Bond Angles in o Arrangement of electron Pairs Geometry of Atoms 3D Shape Type 2 0 BeCl 2 180 Linear Linear AB 2 3 0 BF 3 120 Trigonal planar Trigonal planar AB 3 4
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This note was uploaded on 08/22/2011 for the course CHEMISTRY 101 taught by Professor Staff during the Spring '11 term at Middlesex CC.

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VSEPR - VSEPR The shapes of covalently bonded molecules and...

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