Which of the following will have a spin-only | vedclass

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

Vedclass · Accepted Answer

$[NiCl_4]^{2-}$

Vedclass · Answer

(C) The spin-only magnetic moment $\mu$ is given by the formula $\mu = \sqrt{n(n+2)} \ BM$,where $n$ is the number of unpaired electrons.For $\mu = 2.86 \ BM$,we have $\sqrt{n(n+2)} \approx 2.86$,which implies $n(n+2) \approx 8$,so $n = 2$.In $[NiCl_4]^{2-}$,$Ni$ is in the $+2$ oxidation state ($3d^8$ configuration).For $Ni^{2+}$ $(3d^8)$,the electrons are arranged as $t_{2g}^6 e_g^2$ in a tetrahedral field,resulting in $n = 2$ unpaired electrons.Thus,$\mu = \sqrt{2(2+2)} = \sqrt{8} \approx 2.83 \ BM$,which matches the given value.

Which of the following will have a spin-only magnetic moment of $2.86 \ BM$?

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