shapes of molecules in class fc
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8 Terms
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electron pair repulsion theory
e- pair repel as far as possible
lone pairs repel more than bonding pair (closer to nucleus)
2
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tetrahedral
bonding pair: 4
lone pair: 0
bond angle: 109.5
eg. CH4 methane
3
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pyramidal
bonding pair: 3
lone pair: 1
bond angle: 107°
eg. NH3
4
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non linear
bonding pairs: 2
lone pairs: 2
bond angle: 104.5°
eg. H2O
5
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trigonal planar
bonding pairs: 3
lone pairs: 0
bond angle: 120°
eg. BF3
6
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octohedral
bonding pairs: 6
lone pairs: 0
bond angles: 90°
eg. SF6
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linear
bonding regions: 2
lone pairs: 0
bond angle: 180°
eg. CO2
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expansion of the octet
makes more bonds than it should
non metals EXCEPT oxygen, nitrogen, fluorine
breaking apart the lone pairs
eg. sulfur can make 6 bonds
Note 
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