Shapes of Molecules (valence shell electron pair repulsion theory - VSEPRT)

Rob Pettit
Mind Map by Rob Pettit, updated more than 1 year ago
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3 Chemistry Mind Map on Shapes of Molecules (valence shell electron pair repulsion theory - VSEPRT), created by Rob Pettit on 04/19/2015.
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Shapes of Molecules (valence shell electron pair repulsion theory - VSEPRT)
1 Identify the central atom.
1.1 Draw a dot/cross diagram to show bonding.
1.1.1 Count the number of electrons in the outer valence shell of the central atom.
1.1.1.1 Count how many electrons the other atoms contribute to the bonding.
1.1.1.1.1 Add them up and divide by 2 to give the number of electron pairs
1.1.1.1.1.1 These will arrange themselves to minimise the repulsion between them.
1.1.1.1.1.1.1 There are set geometries for given numbers of electron pairs.
1.1.1.1.1.1.2 Lone pair - Lone pair
1.1.1.1.1.1.2.1 Greatest repulsion
1.1.1.1.1.1.2.2 Lone Pair - Bond pair
1.1.1.1.1.1.2.2.1 Bond pair - Bond pair
1.1.1.1.1.1.2.2.1.1 Least repulsion
2 2/0 - Linear - 180
2.1 2/1 - V bent - 120
2.1.1 2/2 - V bent - 104.5
2.1.1.1 Water - H2O
3 3/0 - TrPl - 120
3.1 3/1 - TrPy - 107.8
3.1.1 3/2 - Tee- 90
3.1.1.1 Chlorine trifluoride - ClF3
3.1.2 Ammonia - NH3
3.2 Boron trifluoride - BF3
4 4/0 - TeHe - 109.5
4.1 4/1
4.1.1 4/2 - SqPl - 90
5 5/0 - TrBi - 90/120
5.1 Phosphorus pentachloride - PCl5
6 6/0 - Oct - 90
6.1 sulfur hexafluoride - SF6
7 2/0 means 2 atoms and 0 lone pairs around central atom. 4/2 means means 4 atome and 2 lone pairs around central atom.
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