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Magnetic moment of $\left[\mathrm{MnCl}_4\right]^{2-}$ is $5.92 \mathrm{BM}$. Explain giving reason present.
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Verified Answer
In $\left[\mathrm{MnCl}_4\right]^{2-}, \mathrm{Mn}^{2+}$ has $\mathrm{sp}^3$ hybridisation as shown below.
i.e. It has 5 unpaired electrons. Thus magnetic moment is
$$
\sqrt{\mathrm{n}(\mathrm{n}+2)}=\sqrt{5(5+2)}=5.92 \mathrm{BM}
$$
i.e. It has 5 unpaired electrons. Thus magnetic moment is
$$
\sqrt{\mathrm{n}(\mathrm{n}+2)}=\sqrt{5(5+2)}=5.92 \mathrm{BM}
$$
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