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(B) The atomic number of iron $(Fe)$ is $26$. The electronic configuration of $Fe$ is $[Ar] 3d^6 4s^2$. When $Fe$ forms a ferrous ion $(Fe^{2+})$,it l

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$4$

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(B) The atomic number of iron $(Fe)$ is $26$. The electronic configuration of $Fe$ is $[Ar] 3d^6 4s^2$. When $Fe$ forms a ferrous ion $(Fe^{2+})$,it loses two electrons from the $4s$ orbital. The electronic configuration of $Fe^{2+}$ becomes $[Ar] 3d^6$. In the $3d$ subshell,there are $5$ orbitals. According to Hund's rule,the $6$ electrons are filled as: one electron in each of the $5$ orbitals and the $6^{th}$ electron pairs up in the first orbital. Thus,there are $4$ unpaired electrons in the $Fe^{2+}$ ion.

What is the number of unpaired electrons in a ferrous ion $(Fe^{2+})$?

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