Which of the following complexes has a magnet | vedclass

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(B) The magnetic moment $\mu$ is given by the formula $\mu = \sqrt{n(n+2)} \ B.M.$,where $n$ is the number of unpaired electrons.For $\mu = 2.82 \ B.M

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$[NiCl_4]^{2-}$

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(B) The magnetic moment $\mu$ is given by the formula $\mu = \sqrt{n(n+2)} \ B.M.$,where $n$ is the number of unpaired electrons.For $\mu = 2.82 \ B.M.$,$n$ must be $2$.In $[NiCl_4]^{2-}$,the oxidation state of $Ni$ is $+2$. The electronic configuration of $Ni^{2+}$ is $3d^8$.Since $Cl^-$ is a weak field ligand,it does not cause pairing of electrons in the $3d$ orbitals.Thus,the $3d^8$ configuration has $2$ unpaired electrons $(n=2)$.Therefore,$\mu = \sqrt{2(2+2)} = \sqrt{8} \approx 2.82 \ B.M.$

Which of the following complexes has a magnetic moment of $2.82 \ B.M.$?

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