Question

Which of the following species represent the example of $dsp^2$ -hybridization ?

• A. $[Fe(CN)_6]^{3-}$
• B. $[Ni(CN)_4]^{2-}$
• C. $[Zn(NH_3)_4]^{2+}$
• D. $[FeF_6]^{3-}$

Answer 1

Answer: (B)

$[Ni(CN)_4]^{2-}$

Answer 2

In $Fe(CN)_6]^{3-}$, and $[FeF_6]^{3-}$ there are six ligands, as such $dsp^2$-hybridisation is not possible. For structure of $[Ni(CN)_4]^{2-}$, see hint to 27 above. In it the state of hybridisation of $Ni^{2+}$ is $dsp^2$. In $[Zn(NH_3)_4]^{2-} \, ,Zn^{2+}$ has configuration of $[Ar]^{18} \,3d^{10}$. Thus $dsp^2$-hybridisation is not possible