Nitrogen, oxygen, and chlorine:

In an organic structures Nitrogen, oxygen and chlorine atoms can as well be sp³ hybridized. Nitrogen contains five valence electrons in the second shell of it. Later than the hybridization, it will have 3 half-filled sp³ orbitals and can make three bonds. Oxygen comprises six valence electrons. Later than the hybridization, it will comprise two half-?lled sp³ orbitals and will make two bonds. Chlorine contains 7 valence electrons. After hybridization, it will contain one half- filled sp³ orbital and will make one bond.

The four sp³ orbitals for these three atoms create a tetrahedral arrangement along with one or more of the orbitals occupied through a lone pair of electrons. Referring the atoms alone, nitrogen creates a pyramidal shape in which the bond angles are little less than 109.5^o (c. 107^o). This compression of the bond angles is because of the orbital consisting of the lone pair of electrons that demands a little greater amount of space than a bond. Oxygen creates an angled or bent shape in which two lone pairs of electrons compress the bond angle from 109.5^o to c. 104^o.