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(D) The complex $\left[ Co(CN)_6 \right]^{3-}$ contains $Co^{3+}$ as the central metal ion.The atomic number of $Co$ is $27$. The electronic configura

Vedclass · Accepted Answer

$t_{2g}^6 e_g^0$

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(D) The complex $\left[ Co(CN)_6 \right]^{3-}$ contains $Co^{3+}$ as the central metal ion.The atomic number of $Co$ is $27$. The electronic configuration of $Co$ is $[Ar] 3d^7 4s^2$.For $Co^{3+}$,the electronic configuration is $[Ar] 3d^6$.$CN^-$ is a strong field ligand,which causes the pairing of electrons in the $d$-orbitals.In an octahedral field,the $d$-orbitals split into $t_{2g}$ and $e_g$ sets.Since $CN^-$ is a strong field ligand,all $6$ electrons of $Co^{3+}$ $(3d^6)$ will occupy the $t_{2g}$ orbitals,resulting in the configuration $t_{2g}^6 e_g^0$.Therefore,the correct option is $D$.

$I$. $NCS^{-}$	$II$. $S^{2-}$
$III$. $en$	$IV$. $SCN^{-}$

The electronic configuration of the central metal atom/ion in $\left[ Co(CN)_6 \right]^{3-}$ is

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