The number of unpaired electrons in Mn^{2+} i | vedclass

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(C) The atomic number of $Mn$ is $25$.The electronic configuration of $Mn$ is $[Ar] 3d^5 4s^2$.When $Mn$ forms $Mn^{2+}$ ion, it loses two electrons f

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$5$

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(C) The atomic number of $Mn$ is $25$.The electronic configuration of $Mn$ is $[Ar] 3d^5 4s^2$.When $Mn$ forms $Mn^{2+}$ ion, it loses two electrons from the $4s$ orbital.Thus, the electronic configuration of $Mn^{2+}$ is $[Ar] 3d^5$.In the $3d$ subshell, there are $5$ orbitals, and according to Hund's rule, each orbital will be occupied by one electron.Therefore, there are $5$ unpaired electrons in $Mn^{2+}$ ion.

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

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