If an oxide of manganese has a value of magne | vedclass

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(B) The magnetic moment is given by the formula $\mu = \sqrt{n(n+2)} \ BM$,where $n$ is the number of unpaired electrons.Given $\mu = 4.9 \ BM$,we hav

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$Mn_2O_3$

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(B) The magnetic moment is given by the formula $\mu = \sqrt{n(n+2)} \ BM$,where $n$ is the number of unpaired electrons.Given $\mu = 4.9 \ BM$,we have $\sqrt{n(n+2)} = 4.9$,which implies $n(n+2) \approx 24$,so $n = 4$.For $MnO$,$Mn$ is in $+2$ oxidation state $(3d^5)$,having $5$ unpaired electrons.For $Mn_2O_3$,$Mn$ is in $+3$ oxidation state $(3d^4)$,having $4$ unpaired electrons.For $Mn_2O_7$,$Mn$ is in $+7$ oxidation state $(3d^0)$,having $0$ unpaired electrons.For $MnO_2$,$Mn$ is in $+4$ oxidation state $(3d^3)$,having $3$ unpaired electrons.Since $Mn^{3+}$ has $4$ unpaired electrons,the oxide is $Mn_2O_3$.

If an oxide of manganese has a value of magnetic moment $( \mu )$ of $4.9 \ BM$,then which oxide would it be?

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