# Question #dd0d4

Mar 13, 2017

The hybridization of $\text{P}$ in ${\text{PCl}}_{5}$ is $\text{sp"^3"d}$.

#### Explanation:

The Lewis structure of ${\text{PCl}}_{5}$ is

According to VSEPR theory, a molecule with five bonding pairs must have both a trigonal bipyramidal electron geometry and molecular geometry.

The $\text{P}$ atom needs five orbitals to form the five $\text{P-Cl}$ bonds.

It has a $\text{3s}$ and three $\text{3p}$ orbitals, so it must use one of its $\text{3d}$ orbitals to form the fifth bond.

These orbitals are hybridized to form five $\text{sp"^3"d}$ orbitals that (surprise!) just happen to point in the right directions to form a trigonal bipyramid.