Which of the following elements in their resp | vedclass

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

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$Zn^{2+}$

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(B) The spin only magnetic moment is given by the formula $\mu = \sqrt{n(n+2)} 	ext{ BM}$,where $n$ is the number of unpaired electrons.For a species to have no spin only magnetic moment,it must have $n = 0$ (i.e.,all electrons are paired).Let us analyze the electronic configurations:$1. Cu^{2+} (Z=29): [Ar] 3d^9$. It has $1$ unpaired electron.$2. Zn^{2+} (Z=30): [Ar] 3d^{10}$. It has $0$ unpaired electrons.$3. Ti^{3+} (Z=22): [Ar] 3d^1$. It has $1$ unpaired electron.$4. V^{3+} (Z=23): [Ar] 3d^2$. It has $2$ unpaired electrons.Since $Zn^{2+}$ has $0$ unpaired electrons,its spin only magnetic moment is $0$.

Which of the following elements in their respective oxidation states does not develop spin only magnetic moment? $[Ti (Z=22), Zn(Z=30), V(Z=23), Cu(Z=29)]$

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