The observed magnetic moment of the complex [ | vedclass

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(A) The magnetic moment $\mu = \sqrt{n(n+2)} \ BM$. Given $\mu = 6.06 \ BM$,which corresponds to $n = 5$ unpaired electrons. For $Mn$ $(Z=25)$,the ele

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$4$

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(A) The magnetic moment $\mu = \sqrt{n(n+2)} \ BM$. Given $\mu = 6.06 \ BM$,which corresponds to $n = 5$ unpaired electrons. For $Mn$ $(Z=25)$,the electronic configuration is $[Ar] 3d^5 4s^2$. To have $5$ unpaired electrons in the complex,$Mn$ must be in the $+2$ oxidation state $(Mn^{2+})$,which has the configuration $[Ar] 3d^5$. Let the oxidation state of $Mn$ be $y$. The charge on the complex is given by $y + 6 	imes (-1) = -x$. Since $y = +2$,we have $2 - 6 = -x$,which gives $-4 = -x$,so $x = 4$.

The observed magnetic moment of the complex $[Mn(NCS)_6]^{x-}$ is $6.06 \ BM$. The numerical value of $x$ is $.......$.

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