Question

In $PC{l}_5$, phosphorus is in $s{p}^{3}d$ hybridized state but all its five bonds are not equivalent. Justify your option with reason.

Answer 1

* Generally, all the hybridized orbitals are in the same size and shape.

* In $PC{l}_{5}moleculePiss{p}^{3}d$ hybridized
and five $s{p}^{3}d$ hybridized orbitals are
overlapping with five chlorine $2p$
orbitals.

* $PC{l}_5$ molecules have trigonal bipyramidal geometry in which the central atom $P$ is
linked with three $P-Cl$ equatorial bonds
and two axial $P-Cl$ bonds.

* The 3 equatorial bonds are equivalent. While the two $P-Cl$ axial bonds are longer than equatorial bonds.

* This is due to the fact that the axial bond pairs suffer more repulsion as compared to equatorial bonds.