Which of the following transition metal ion c | vedclass

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(D) The magnetic moment $(\mu)$ is given by the formula $\mu = \sqrt{n(n+2)} \ BM$,where $n$ is the number of unpaired electrons.For $\mu = 4.90 \ BM$

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$FeSO_4$

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(D) The magnetic moment $(\mu)$ is given by the formula $\mu = \sqrt{n(n+2)} \ BM$,where $n$ is the number of unpaired electrons.For $\mu = 4.90 \ BM$,we have $\sqrt{n(n+2)} = 4.90$,which implies $n(n+2) \approx 24$,so $n = 4$.In $CoCl_2$,the oxidation state of $Co$ is $+2$. The electronic configuration of $Co^{2+}$ $(Z=27)$ is $[Ar] 3d^7$.In the $3d^7$ configuration,there are $3$ unpaired electrons $(n=3)$,so $\mu = \sqrt{3(5)} = \sqrt{15} \approx 3.87 \ BM$.In $FeSO_4$,the oxidation state of $Fe$ is $+2$. The electronic configuration of $Fe^{2+}$ $(Z=26)$ is $[Ar] 3d^6$.In the $3d^6$ configuration,there are $4$ unpaired electrons $(n=4)$,so $\mu = \sqrt{4(6)} = \sqrt{24} \approx 4.90 \ BM$.Thus,$FeSO_4$ has a magnetic moment of $4.90 \ BM$.

Which of the following transition metal ion compounds has a magnetic moment of $4.90 \ BM$?

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