What type of hybridization is present in $\mathrm{Ni}$ of $\left[\mathrm{Ni}(\mathrm{Cl})_4\right]^{2-}$ and…
What type of hybridization is present in $\mathrm{Ni}$ of $\left[\mathrm{Ni}(\mathrm{Cl})_4\right]^{2-}$ and $\left[\mathrm{Ni}(\mathrm{CN})_4\right]^{2-}$ respectively?
$\mathrm{dsp}^2$ and $\mathrm{dsp}^2$
$\mathrm{sp}^3$ and $\mathrm{dsp}^2$
$\mathrm{dsp}^2$ and $\mathrm{sp}^3$
$\mathrm{sp}^3$ and $\mathrm{sp}^3$
Solution
In $\left[\mathrm{NiCl}_4\right]^{2-} \mathrm{Ni}$ is in +2 oxidation state $\mathrm{Ni}^{+2} \rightarrow[\mathrm{Ar}] 3 \mathrm{~d}^8$
Hybridization involved is $\mathrm{sp}^3$ as participating orbitals are $4 \mathrm{~S}$ \& $4 \mathrm{P}$
$\mathrm{In}\left[\mathrm{NiCN}_4\right]^{2-} \mathrm{Ni}$ is in $2+$ oxidation state. $\mathrm{Ni}^{+2} \rightarrow[\mathrm{Ar}] 3 \mathrm{~d}^8$
$\mathrm{CN}^{-}$is strong field ligand. It causes pairing of $3 \mathrm{~d}$ electrons.
Hybridization
involved is $\mathrm{dsp}^2$ as participating orbitals are $3 \mathrm{~d}, 4 \mathrm{~S}$ and $4 \mathrm{P}$.