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?

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 \(4 \mathrm{P}\).