Number of unpaired electrons in Mn^{2+} is | vedclass

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Question

(B) 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

Vedclass · Accepted Answer

$5$

Vedclass · Answer

(B) 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. The electronic configuration of $Mn^{2+}$ becomes $[Ar] 3d^5$. In the $3d$ subshell,there are $5$ orbitals,and according to Hund's rule,each orbital will be singly occupied. Therefore,there are $5$ unpaired electrons in $Mn^{2+}$.

Number of unpaired electrons in $Mn^{2+}$ is

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