Which of the following species represent the example of dsp^2 hybridization ? (a) [Fe(CN)6]^(3+) (b) [Ni(CN)4]^(2+)

Question

Which of the following species represent the example of \(d s p^{2}\) hybridization?

(a) \([\mathrm{Fe}(\mathrm{CN}) 6]^{3-}\)

(b) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\)

(c) \(\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}\)

(d) \([\mathrm{Co}(\mathrm{CN}) 6]^{3-}\)

Answer 1

Correct option is (b) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\)

\(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) exhibit dsp² geometry and hence sqaure planar geometry. Due to strong field ligand CN^- electrons get paired in 3d orbitals.