Which of the following has a magnetic moment | vedclass

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(A) 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 = 1.73 \,

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$[Cu(NH_3)_4]^{2+}$

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(A) 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 $\mu = 1.73 \, B.M.$,we have $\sqrt{n(n+2)} = 1.73$,which implies $n = 1$.$1$. In $[Cu(NH_3)_4]^{2+}$,$Cu$ is in $+2$ oxidation state ($3d^9$ configuration). It has $1$ unpaired electron $(n=1)$. Thus,$\mu = \sqrt{1(1+2)} = \sqrt{3} = 1.73 \, B.M.$$2$. In $[Ni(CN)_4]^{2-}$,$Ni$ is in $+2$ oxidation state $(3d^8)$. Due to the strong field ligand $CN^-$,electrons pair up,resulting in $n=0$.$3$. In $TiCl_4$,$Ti$ is in $+4$ oxidation state $(3d^0)$,so $n=0$.$4$. In $[CoCl_6]^{4-}$,$Co$ is in $+2$ oxidation state $(3d^7)$. With a weak field ligand $Cl^-$,it has $3$ unpaired electrons $(n=3)$.

Which of the following has a magnetic moment of $1.73 \, B.M.$?

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