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(A) The magnetic moment $\mu$ is given by $\sqrt{n(n+2)} \ BM$,where $n$ is the number of unpaired electrons. For $\mu = 1.73 \ BM$,$n$ must be $1$.$(

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$CuI$

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(A) The magnetic moment $\mu$ is given by $\sqrt{n(n+2)} \ BM$,where $n$ is the number of unpaired electrons. For $\mu = 1.73 \ BM$,$n$ must be $1$.$(1)$ $CuI$: In $CuI$,$Cu$ is in the $+1$ oxidation state $(Cu^{+})$. The electronic configuration of $Cu^{+}$ is $[Ar]3d^{10}$,which has $0$ unpaired electrons. Thus,$\mu = 0 \ BM$.$(2)$ $\left[Cu(NH_{3})_{4}\right]Cl_{2}$: Here,$Cu$ is in the $+2$ oxidation state $(Cu^{2+})$. The electronic configuration of $Cu^{2+}$ is $[Ar]3d^{9}$,which has $1$ unpaired electron. Thus,$\mu = \sqrt{1(1+2)} = 1.73 \ BM$.$(3)$ $O_{2}^{+}$: Total electrons = $15$. Molecular orbital configuration: $\sigma_{1s}^{2} \sigma_{1s}^{*2} \sigma_{2s}^{2} \sigma_{2s}^{*2} \sigma_{2pz}^{2} \pi_{2px}^{2} \pi_{2py}^{2} \pi_{2px}^{*1}$. It has $1$ unpaired electron. Thus,$\mu = 1.73 \ BM$.$(4)$ $O_{2}^{-}$: Total electrons = $17$. Molecular orbital configuration: $\sigma_{1s}^{2} \sigma_{1s}^{*2} \sigma_{2s}^{2} \sigma_{2s}^{*2} \sigma_{2pz}^{2} \pi_{2px}^{2} \pi_{2py}^{2} \pi_{2px}^{*2} \pi_{2py}^{*1}$. It has $1$ unpaired electron. Thus,$\mu = 1.73 \ BM$.Therefore,$CuI$ does not have a magnetic moment of $1.73 \ BM$.

Which one of the following species does not have a magnetic moment of $1.73 \ BM$ (spin only value)?

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