Question

The hybridisations of $Ni(CO{)}_4$ and $[Cr(H_{2}O{)}_6^2{]}^{+}$ respectively, are

• A. $s{p}^3$ and $d^{3}s{p}^2$
• B. $ds{p}^2$ and $d^{2}s{p}^3$
• C. $s{p}^3$ and $d^{2}s{p}^3$
• D. $ds{p}^2$ and $s{p}^3{d}^2$

Answer 1

Answer: (C)

The oxidation state of $Ni$ in $Ni(CO{)}_4$ is $O$. It’s electronic configuration will be $[Ar]3d^{8}4s^2$

As $CO$ is a strong field ligand, pairing of electrons will occur.

The oxidation state of $Cr$ in $[Cr(H_{2}O{)}_6{]}^{2+}$ is $+2$. It’s electronic configuration will $[Ar]3d^{4}4s^0$.

As $H_{2}O$ is also a strong field ligand, pairing of electrons will occur.