Question

Among $\left[Ni\right(CO{)}_4],[Ni(CN{)}_4{]}^{2-},[NiC{l}_4{]}^{2-}$ species, the hybridization states at the Ni atom are, respectively (Atomic Number of Ni = 28) :

• A. $ds{p}^2,s{p}^3,s{p}^3$
• B. $s{p}^3,ds{p}^2,ds{p}^2$
• C. $s{p}^3,ds{p}^2,s{p}^3$
• D. $s{p}^3,s{p}^3,ds{p}^2$

Answer 1

Answer: (C)

$s{p}^3,ds{p}^2,s{p}^3$

Option (C) is correct.

Outermost electronic configuration of $\left[Ni\right(CO{)}_4]$ complex is $3d^8,4s^2$ and $CO$ is a strong ligand thus electrons get paired up and shows $s{p}^3$ hybridisation.

Outermost electronic configuration of $\left[Ni\right(CN{)}_4{]}^{2-}$ complex is $3d^8$ and $CN$ is a strong ligand thus electrons get paired up but one $d$ orbital is empty and shows $ds{p}^2$ hybridisation.

Outermost electronic configuration of $\left[Ni\right(Cl{)}_4{]}^{2-}$ complex is $3d^8,4s^2$ and $Cl$ is a weak ligand thus electrons does not paired up and shows $s{p}^3$ hybridisation.