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(C) In $NiCl_{2}$,the oxidation state of $Ni$ is $+2$. The electronic configuration of $Ni^{2+}$ is $[Ar] 3d^{8}$.In the $3d^{8}$ configuration,there

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$2$

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(C) In $NiCl_{2}$,the oxidation state of $Ni$ is $+2$. The electronic configuration of $Ni^{2+}$ is $[Ar] 3d^{8}$.In the $3d^{8}$ configuration,there are $2$ unpaired electrons.When $NiCl_{2}$ is heated with excess $NaCN$ in the presence of a strong oxidizing agent,$Ni^{2+}$ is oxidized to $Ni^{4+}$.The electronic configuration of $Ni^{4+}$ is $[Ar] 3d^{6}$.$CN^-$ is a strong field ligand,which causes pairing of electrons in the $3d$ orbitals.For $d^{6}$ in a strong field,all $6$ electrons pair up in the $t_{2g}$ orbitals,resulting in $0$ unpaired electrons.The change in the number of unpaired electrons = $|0 - 2| = 2$.

An aqueous solution of $NiCl_{2}$ was heated with excess sodium cyanide in the presence of a strong oxidizing agent to form $[Ni(CN)_{6}]^{2-}$. The total change in the number of unpaired electrons on the metal centre is $.....$

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