Nitrogen - sp³ hybridization

The nitrogen atom also hybridizes in the sp² arrangement, but differs from carbon in that there is a "lone pair" of electron left on the nitrogen that does not participate in the bonding. The geometry about nitrogen with three bonded ligands is therefore trigonal pyramidal.

Nitrogen -sp² hybridization

Nitrogen will also hybridize sp² when there are only two atoms bonded to the nitrogen (one single and one double bond). Just as for sp³ nitrogen, a pair of electrons is left on the nitrogen as a lone pair. The resulting geometry is bent with a bond angle of 120 degrees.

Oxygen - sp³hybridization

Oxygen bonded to two atoms also hybridizes as sp³. There are two lone pairs of electrons located on the oxygen atom (not shown) and the resulting geometry is bent with a bond angle ~109 degrees. Note that in acetic acid one of the oxygen atoms is bonded to only one atom. We therefore do not have to consider the geometry (or hybridization) around that particular atom.

Sulfur - sp³ hybridization

The geometry of sulfur compounds is essentially the same as for oxygen compounds with sp³  hybridization found with two atoms bonded to sulfur.