Problem: The ground-state electron configuration of a Mn2+ ion is 1s22s22p63s23p63d5. Therefore, Mn2+ isa. paramagnetic with two unpaired electrons.b. paramagnetic with one unpaired electron.c. paramagnetic with five unpaired electrons.d. diamagnetic.e. paramagnetic with three unpaired electrons.

FREE Expert Solution

Recall:

s orbital  can hold a maximum of 2 electrons

p orbitals → can hold a maximum of 6 electrons

d orbitals → can hold a maximum of 10 electrons

f orbitals → can hold a maximum of 14 electrons


Mn2+ ion is 1s22s22p63s23p63d5


To find the number of unpaired electrons, fill up the 3d subshell. All of the electrons in lower energy orbitals are already paired.

3d subshell → 5 electrons

d  → 5 orbitals


When filling up the orbitals, keep in mind:

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Problem Details

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.

d. diamagnetic.

e. paramagnetic with three unpaired electrons.

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