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.

List-$I$	List-$II$
$(1)$ $Ti^+$	$(A)$ $(n-1)d^4ns^2$
$(2)$ $_{30}Zn$	$(B)$ $(n-1)d^{10}ns^1$
$(3)$ $_{24}Cr$	$(C)$ $(n-1)d^2ns^0$
$(4)$ $_{29}Cu$	$(D)$ $(n-1)d^5ns^1$
	$(E)$ $(n-1)d^0ns^2$
	$(F)$ $(n-1)d^{10}ns^2$

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

Similar Questions

Which of the following groups of transition metals is known as coinage metals?

Match the elements in List-$I$ with their electronic configurations in List-$II$.

List-$I$ List-$II$

$(1)$ $Ti^+$ $(A)$ $(n-1)d^4ns^2$

$(2)$ $_{30}Zn$ $(B)$ $(n-1)d^{10}ns^1$

$(3)$ $_{24}Cr$ $(C)$ $(n-1)d^2ns^0$

$(4)$ $_{29}Cu$ $(D)$ $(n-1)d^5ns^1$

$(E)$ $(n-1)d^0ns^2$

$(F)$ $(n-1)d^{10}ns^2$

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