Question

Which of the following species represent the example of $ds{p}^2$ -hybridization ?

• A. $[Fe(CN{)}_6{]}^{3-}$
• B. $[Ni(CN{)}_4{]}^{2-}$
• C. $[Zn(N{H}_3{)}_4{]}^{2+}$
• D. $[Fe{F}_6{]}^{3-}$

Answer 1

Answer: (B)

In $Fe(CN{)}_6{]}^{3-}$, and $[Fe{F}_6{]}^{3-}$ there are six ligands, as such $ds{p}^2$-hybridisation is not possible.
For structure of $[Ni(CN{)}_4{]}^{2-}$, see hint to Q. 27 above. In it the state of hybridisation of $N{i}^{2+}$ is $ds{p}^2$.
In $[Zn(N{H}_3{)}_4{]}^{2-},Z{n}^{2+}$ has configuration of $[Ar{]}^{18}3d^{10}$. Thus $ds{p}^2$-hybridisation is not possible