Question

The hybridization of $IC{l}_2^{-}$ and $Cl{O}_4^{-}$, respectively are:

• A. $s{p}^3{d}^2$ , $s{p}^3$
• B. $s{p}^2$ , $s{p}^{3}d$
• C. $s{p}^{3}d$ , $s{p}^3$
• D. None of these

Answer 1

Answer: (C)

$s{p}^{3}d$ , $s{p}^3$

$H=\frac{1}{2}[V+M-C+A]$

where,
H= Number of orbitals involved in hybridization.
V=Valence electrons of the central atom.
M- Number of monovalent atoms linked to the central atom.
C= Charge of a cation.
A= Charge of the anion.

Consider the hybridization and shape of the options:

A) $IC{l}_2^{-}$

$H=\frac{1}{2}[7+2+1]=5$.

$\Rightarrow s{p}^{3}d$ hybridized state.
Linear in shape

B) $Cl{O}_4^{-}$

$H=\frac{1}{2}[7+1]=4$.

$\Rightarrow s{p}^3$ hybridized state.
Tetrahedral in shape.

So, the correct option is $C$