The electronic configuration of the central a | vedclass

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(D) $1$. In the complex $[MnO_4]^{2-}$,the oxidation state of $Mn$ is calculated as: $x + 4(-2) = -2$,which gives $x = +6$. $2$. The electronic config

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$e^1 \, t_2^0$

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(D) $1$. In the complex $[MnO_4]^{2-}$,the oxidation state of $Mn$ is calculated as: $x + 4(-2) = -2$,which gives $x = +6$. $2$. The electronic configuration of $Mn$ $(Z=25)$ is $[Ar] 3d^5 4s^2$. $3$. The electronic configuration of $Mn^{6+}$ is $[Ar] 3d^1$. $4$. In a tetrahedral complex like $[MnO_4]^{2-}$,the $d$-orbitals split into $e$ (lower energy) and $t_2$ (higher energy) sets. $5$. The single $d$-electron occupies the lower energy $e$ orbital. $6$. Therefore,the configuration is $e^1 \, t_2^0$.

$I$	$II$
$(a). [Cr(H_2O)_6]^{2+}$	$[Cr(H_2O)_6]^{3+}$
$(b). [Fe(H_2O)_6]^{3+}$	$[Fe(CN)_6]^{3-}$
$(c). [Fe(CN)_6]^{3-}$	$[Ru(CN)_6]^{3-}$
$(d). [NiF_6]^{4-}$	$[NiF_6]^{2-}$

The electronic configuration of the central atom of the complex $[MnO_4]^{2-}$ is:

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