Question

The hybridisation of $Ni$ centre in $Ni[(PP{h}_3{)}_{2}C{l}_2]$ and $[NiC{l}_4{]}^2$, respectively are

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

Answer 1

Answer: (A)

The oxidation number of $Ni$ in both $[Ni(PP{h}_3{)}_{2}C{1}_2]$ and $[NiC{l}_4{]}^{2-}$ is $+2$.
The electronic configuration of $Ni(II)$ is $[Ar]3d^{8}4s^0$.

As $PP{h}_3$ is a strong ligand, so it forces the electrons to get pair up. $Ni(PP{h}_3{)}_{2}C{l}_2$

As $C{l}^{-}$ is not a strong ligand therefore pairing will not occurs.

Thus, the hybridisation of $Ni$ central atom in $Ni[(PP{h}_3{)}_{2}C{l}_2]$ and $[NiC{l}_4{]}^{2-}$ respectively are $ds{p}^2$ and $s{p}^3$.