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AS 020 09-Jul-12

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BASIC IDEAS Shapes of molecules and ions depends on total number of electron pairs around the central atom. Two types of electron pairs: Bonding pairs (i.e. e - ’s in a covalent bond) Non-bonding pairs (i.e. lone pairs) These electron pairs repel as far as possible (but lone pairs repel more than bonding pairs).

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https://people.ok.ubc.ca/wsmcneil/vsepr.htm Very useful website (all rotateable)

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2 ELECTRON PAIRS electron pairs bonding pairs lone pairsshape 220linear

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2 bonding pairs linear

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3 ELECTRON PAIRS electron pairs bonding pairs lone pairsshape 330Trigonal planar 321Bent (V-shape)

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3 bonding pairs Trigonal planar

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2 bonding pair + 1 lone pair Bent

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4 electron pairs tetrahedral

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3 electron pairs + 1 lone pair trigonal pyramid

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2 bonding pairs + 2 lone pairs bent

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4 ELECTRON PAIRS electron pairs bonding pairs lone pairsshape 440Tetrahedral 431Pyramidal 422Bent (V-shape)

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5 ELECTRON PAIRS electron pairs bonding pairs lone pairsshape 550 Trigonal bipyramidal 541 532 Trigonal planar or T-shape

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5 electron pairs Trigonal bipyramidal

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4 bonding pairs + 1 lone pair Seesaw

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3 bonding pairs + 2 lone pairs T-shape

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6 ELECTRON PAIRS electron pairs bonding pairs lone pairsshape 660Octahedral 651 Distorted square pyramid 642Square planar

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6 electron pairs octahedral

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5 bonding pairs + 1 lone pairs square pyramid

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4 bonding pairs + 2 lone pairs square planar

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http://www.lsbu.ac.uk/php-cgiwrap/biology/pfpb.php3?page=http://www.lsbu.ac.uk/biology/biolchem/shapes.html

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