A transition metal (M) among Mn, Cr, Co and F | vedclass

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(B) The standard electrode potential $(M^{3+}/M^{2+})$ values for the given metals are: $Mn^{3+}/Mn^{2+} = +1.57 \ V$,$Cr^{3+}/Cr^{2+} = -0.41 \ V$,$C

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(B) The standard electrode potential $(M^{3+}/M^{2+})$ values for the given metals are: $Mn^{3+}/Mn^{2+} = +1.57 \ V$,$Cr^{3+}/Cr^{2+} = -0.41 \ V$,$Co^{3+}/Co^{2+} = +1.97 \ V$,$Fe^{3+}/Fe^{2+} = +0.77 \ V$. Among these,$Co$ has the highest standard electrode potential. The complex is $[Co(CN)_6]^{4-}$. In this complex,the oxidation state of $Co$ is $+2$. The electronic configuration of $Co^{2+}$ is $[Ar] 3d^7$. $CN^-$ is a strong field ligand,causing pairing of electrons. According to Crystal Field Theory,for an octahedral complex with $d^7$ configuration and strong field ligand,the distribution is $t_{2g}^6 e_g^1$. Therefore,the number of electrons in the $e_g$ orbital is $1$.

$A$ transition metal $(M)$ among $Mn, Cr, Co$ and $Fe$ has the highest standard electrode potential $(M^{3+} / M^{2+})$. It forms a metal complex of the type $[M(CN)_6]^{4-}$. The number of electrons present in the $e_g$ orbital of the complex is $.........$

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