Question

In the reaction $2PC{l_5} \rightleftharpoons PCl_4^ + + PCl_6^ -$ , the change in the hybridization is from:
A. $s{p^3}d$ to $s{p^3}$ and $s{p^3}{d^2}$
B. $s{p^3}d$ to $s{p^2}$ and $s{p^3}$
C. $s{p^3}d$ to $s{p^3}{d^2}$ and $s{p^3}{d^3}$
D. $s{p^3}{d^2}$ to $s{p^3}$ and $s{p^3}d$

Answer 1

Hybridization occurs when an atom bonds using electrons from both s and p orbitals, creating an imbalance in the energy level of the electrons. To equalize these energy levels, the s and p orbitals involved are combined to create hybrid orbitals. Hybridization is a key concept in valence bond theory, but alternate models are proposed in molecular orbital theory. It was introduced by the molecular structure when the valence bond theory failed to correctly predict them.

Complete answer:
The hybridization form is determined by the equalized energy level of s and p orbitals which is involved to create hybrid orbitals. $s{p^3}$ hybridization can explain the tetrahedral structure of molecules. In it, the 2s orbitals and all three of the 2p orbitals hybridize to form four sp orbitals.
$PC{l_5}$ contains $s{p^3}d$ hybridized with trigonal bipyramidal. In $PCl_4^ +$ has $s{p^3}$ and $PCl_6^ -$ contains $s{p^3}{d^2}$ hybridization with the shape of an octahedral.
As we see the reaction, we know that the hybridization of each salt of phosphorus contains different shapes.

Hence, option (A) is the correct answer.

Note:
Hybridization happens when atomic orbitals mix to form a new atomic orbital. The new orbital can hold the same total number of electrons as the old ones. The properties and energy of the new, hybridized orbital are an average of the original unhybridized orbitals. The concept of hybridization was introduced by the best explanation for the fact that all the C-H bonds in molecules.