Calculate the magnetic moment of a divalent i | vedclass

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(D) The atomic number of the element is $25$, which corresponds to Manganese $(Mn)$.Its electronic configuration is $[Ar] 3d^{5} 4s^{2}$.A divalent io

Vedclass · Accepted Answer

$5.92$

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(D) The atomic number of the element is $25$, which corresponds to Manganese $(Mn)$.Its electronic configuration is $[Ar] 3d^{5} 4s^{2}$.A divalent ion $(Mn^{2+})$ is formed by losing two electrons from the $4s$ orbital, resulting in a $3d^{5}$ configuration.This configuration has $n = 5$ unpaired electrons.The magnetic moment $(\mu)$ is calculated using the spin-only formula: $\mu = \sqrt{n(n+2)} \, BM$.Substituting $n = 5$: $\mu = \sqrt{5(5+2)} = \sqrt{35} \approx 5.92 \, BM$.

Calculate the magnetic moment of a divalent ion in aqueous solution if its atomic number is $25$. (in $BM$)

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