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VSEPR Theory
Valence Shell Electron Pair Repulsion Theory
Predicts shapes of molecules.
2 atoms bonded to central atom
0 unshared pairs of electrons on the central atom
Linear
sp Hybridization
180 deg
no dipole
3 atoms bonded to central atom
0 unshared pairs of electrons on the central atom
Trigonal Planar
sp² Hybridization
120 deg
no dipole
2 atoms bonded to central atom
1 unshared pairs of electrons on the central atom
Bent
sp² Hybridization
~ 120 deg
has dipole
4 atoms bonded to central atom
0 unshared pairs of electrons on the central atom
Tetrahedral
sp³ Hybridization
109.5 deg
no dipole
3 atoms bonded to central atom
1 unshared pairs of electrons on the central atom
Trigonal Pyramidal
sp³ Hybridization
< 109.5 deg
has dipole
2 atoms bonded to central atom
2 unshared pairs of electrons on the central atom
Bent
sp³ Hybridization
< 109.5 deg
has dipole
Expanded octet:
5 atoms bonded to central atom
0 unshared pairs of electrons on the central atom
Trigonal Bipyramidal
dsp³ Hybridization
90 and 120 deg
no dipole
Expanded octet:
4 atoms bonded to central atom
1 unshared pairs of electrons on the central atom
See-saw
dsp³ Hybridization
90 and 120 deg
has dipole
Expanded octet:
3 atoms bonded to central atom
2 unshared pairs of electrons on the central atom
T-shaped
dsp³ Hybridization
90 and 180 deg
has dipole
Expanded octet:
2 atoms bonded to central atom
3 unshared pairs of electrons on the central atom
Linear
dsp³ Hybridization
180 deg
no dipole
Expanded octet:
6 atoms bonded to central atom
0 unshared pairs of electrons on the central atom
Octehedral
d²sp³ Hybridization
90 deg
no dipole
Expanded octet:
5 atoms bonded to central atom
1 unshared pairs of electrons on the central atom
Square Pyramidal
d²sp³ Hybridization
90 deg
has dipole
Expanded octet:
4 atoms bonded to central atom
2 unshared pairs of electrons on the central atom
Square Planar
d²sp³ Hybridization
90 deg
no dipole
Hybridization
Molecular orbitals.
(s, p, d, f are atomic orbitals.)
Only orbitals that need to be hybridized will be.
σ bonds
Bond that occurs from a direct overlap or orbitals. All single bonds.
π bonds
In double and triple bonds, do not directly overlap.
