🤓 Based on our data, we think this question is relevant for Professor Oppenheim's class at University of Colorado at Colorado Springs.
The ground-state electron configuration of a Mn2+ ion is 1s22s22p63s23p63d5. Therefore, Mn2+ is
a. paramagnetic with two unpaired electrons.
b. paramagnetic with one unpaired electron.
c. paramagnetic with five unpaired electrons.
e. paramagnetic with three unpaired electrons.
We have to determine if Mn2+ ion is paramagnetic or diamagnetic and how many unpaired electrons it has.
Manganese is a transition metal that belongs to group 7B.
The given electronic configuration of Mn2+ ion is:
1s2 2s2 2p6 3s2 3p6 3d5
An orbital which is completely filled cannot contain any unpaired electrons as all of the electrons in a full orbital have to be paired.
This means there will no unpaired electrons in orbitals from 1s to 3p since they are all filled and all of the electrons contained within will be paired.
An orbital, which is partially-filled, can have unpaired electrons.