Which element from the following does NOT exh | vedclass

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(D) The magnetic moment of an ion is given by the formula $\mu = \sqrt{n(n+2)} 	ext{ BM}$,where $n$ is the number of unpaired electrons.For an ion to

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$Zn$

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(D) The magnetic moment of an ion is given by the formula $\mu = \sqrt{n(n+2)} 	ext{ BM}$,where $n$ is the number of unpaired electrons.For an ion to exhibit a magnetic moment,it must have at least one unpaired electron $(n > 0)$.Let us analyze the electronic configuration of the given elements in their $+2$ oxidation state:$1$. $Mn^{2+}$: $[Ar]3d^5$ $(n = 5)$$2$. $Co^{2+}$: $[Ar]3d^7$ $(n = 3)$$3$. $Fe^{2+}$: $[Ar]3d^6$ $(n = 4)$$4$. $Zn^{2+}$: $[Ar]3d^{10}$ $(n = 0)$Since $Zn^{2+}$ has a completely filled $3d$ subshell,it has $0$ unpaired electrons. Therefore,it does not exhibit a magnetic moment.

Which element from the following does $NOT$ exhibit a magnetic moment in the $+2$ oxidation state?

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