Find the species having the magnetic moment v | vedclass

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(D) The magnetic moment is calculated using the formula $\mu = \sqrt{n(n+2)} \ BM$,where $n$ is the number of unpaired electrons.For a magnetic moment

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(D) The magnetic moment is calculated using the formula $\mu = \sqrt{n(n+2)} \ BM$,where $n$ is the number of unpaired electrons.For a magnetic moment of $5.92 \ BM$,we have $\sqrt{n(n+2)} = 5.92$,which implies $n = 5$.$Fe^{3+}$ $([Ar] 3d^5)$ has $5$ unpaired electrons.$Mn^{2+}$ $([Ar] 3d^5)$ has $5$ unpaired electrons.$Cr^{+}$ $([Ar] 3d^5)$ has $5$ unpaired electrons.Since all the given species have $5$ unpaired electrons,they all exhibit a magnetic moment of $5.92 \ BM$.

Find the species having the magnetic moment value of $5.92 \ BM$.

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