Question

The hybridization of P in solid PCl5 is

Answer 1

VSEPR theory predicts that PCl5 should have a trigonal bipyramidal structure, which corresponds to an sp3d hybridization. We usually show the P-Cl bond as being formed by the overlap of a phosphorus sp3d orbital with a \chlorine 3p orbital.
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Answer 2

Answer: The hybridization of $PCl_5$ is $sp^3d$

Explanation:

The equation used to calculate hybridization follows:

$\text{Number of electron pair}=\frac{1}{2}[V+N-C+A]$

where,

V = number of valence electrons present in central atom

N = number of monovalent atoms bonded to central atom

C = charge of cation

A = charge of anion

For the given compound, $PCl_5$

We know that:

$V=5\\N=5\\C=0\\A=0$

Putting values in above equation, we get:

$\text{Number of electron pair}=\frac{[5+5]}{2}=5$

The number of electron pair are coming out to be 5. This means that the hybridization will be $sp^3d$ and the electronic geometry of the molecule will be trigonal bipyramidal.

Hence, the hybridization of $PCl_5$ is $sp^3d$