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| Question | Answer |
| Linear | -2 electron pairs -3 atoms -180 degree bond angles Example: Carbon Dioxide |
| Trigonal Planar | -3 electron pairs -4 atoms -120 degree bond angles Example: Boron Trifluoride |
| Tetrahedral | -4 electron pairs -5 atoms -109.5 degree bond angles Example: Methane |
| Trigonal Bipyramid | -5 electron pairs -6 atoms -180 degree and 120 degree bond angles Example: Phosphorous Pentachloride |
| Octahedral | -6 electron pairs -7 atoms -90 degree bond angles Example: Sulfur Hexafluoride |
| Lone pairs | -A pair of electrons that are not involved in a (covalent) bond. -There is more repulsion made by lone pairs than bonding pairs as they are closer. -They are worth 2.5 degree per lone pair. Example: Water |
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