Question

According to the valence bond theory the hybridization of central metal atom is $ds{p}^2$ for which one of the following compounds ?

• A. $N{a}_2\left[NiC{l}_4\right]$
• B. $K_2\left[Ni\right(CN{)}_4]$
• C. $NiC{l}_2.6H_{2}O$
• D. $\left[Ni\right(CO{)}_4]$

Answer 1

The correct option is B $K_2\left[Ni\right(CN{)}_4]$

$Cl$ ligands are weak field so, $NiC{l}_2.6H_{2}O$ and $N{a}_2\left[NiC{l}_4\right]$ form outer orbital complex of $s{p}^3$ hybridisation.

In $\left[Ni\right(CO{)}_4]$, the electronic configuration of $N{i}^0$ is $3d^{10}4s^0$. Hence, its hybridisation will be $s{p}^3$

In $K_2\left[Ni\right(CN{)}_4]$, the CN is strong field ligand so electrons gets paired and form inner orbital complex of $ds{p}^2$ hybridisation.