The number of unpaired electrons in the Fe^{2 | vedclass

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(B) The atomic number of $Fe$ is $26$. The electronic configuration of $Fe$ is $[Ar] \, 3d^6 \, 4s^2$.When $Fe$ forms the $Fe^{2+}$ ion,it loses two e

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$4$

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

The number of unpaired electrons in the $Fe^{2+}$ ion is

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