VSEPR Theory
| Hybridization | e- groups around center | Bonded pairs | Lone pairs | Geometry | Molecular Shape | Bond Angle |
|---|---|---|---|---|---|---|
| sp | 2 | 2 1 |
0 1 |
Linear | Linear Linear |
180° |
| sp2 | 3 | 3 2 1 |
0 1 2 |
Trigonal planar | Trigonal planar Bent Linear |
120° |
| sp3 | 4 | 4 3 2 1 |
0 1 2 3 |
Tetrahedral | Tetrahedral Trig pyramidal Bent Linear |
109.5° |
| sp3d | 5 | 5 4 3 2 |
0 1 2 3 |
Trigonal bipyramidal |
Trig bipyramidal Seesaw T-Shaped Linear |
90° and 120 |
| sp3d2 | 6 | 6 5 4 |
0 1 2 |
Octahedral | Octahedral Square pyramidal Square planar |
90° |
Electronic Geometry – bonded and lone pairs are the same
Molecular Shape – lone pairs take up less space than bonded pairs
