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Difference (from prior major revision)
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Changed: 21c21
Changed: 31c31
| VSPER & Geometry Table |
| #pairs of electron around central atom |
# lone pair on central atom |
#single bonds |
Hybrid. |
Formula |
Name of shape |
Bond angle |
| 2 |
0 |
2 |
sp |
YX2 |
Linear |
180 |
| 3 |
0 |
3 |
sp2 |
YX3 |
Trigonal planar |
120 |
| 4 |
0 |
4 |
sp3 |
Y X4 |
Tetrahedral |
109.5 |
| 4 |
1 |
3 |
sp3 |
Y X3 |
Pyramidal |
107.0 |
| 4 |
2 |
2 |
sp3 |
Y X2 |
Bent |
104.5 |
| 5 |
0 |
5 |
dsp3 |
Y X5 |
Trigonal bipyramidal |
90, 120 |
| 6 |
0 |
6 |
d2sp3 |
Y X6 |
Octahedral |
90,90 |
Notes:
- Two atoms bonding will always give linear geometry
- Hybridization is only on the central atom.
- All compounds with multiple bonds (i.e. double bonds) have a planar geometry
- C,N,O,F (sometime P,S,Cl) are the most common elements that form multiple bonds
- Compounds that have the potential to have d-orbitals (this excludes C,N,O,F) can exceed the Octet Rule/ Rule of 8.
- For compounds w/elements in 3rd energy (row) and higher, look for Lewis Dot Structure with single bonding first before more complex structure w/double bonds.
- The simple way of determining the Hybridization on the Central atom:
- Add up the number of outside atoms that central atom is bonding with.
- Add up the number of lone pairs on central atom
- Add together to get number.
- This number is number of Hybridized orbital
- Example CH4
- Central atom is bonded to 4 outside atoms and no lone pair so hybridization is sp3 where there are 4 of them.