Question

What is the ground-state electron configuration for the Mn4+ ion and is it paramagnetic or diamagnetic?

Group of answer choices

[Ar] 3d2, paramagnetic

[Kr] 5s2, paramagnetic

[Ar] 3d3, paramagnetic

[Ar] 4s2 3d5, paramagnetic

[Ar] 3d3, diamagnetic

[Ar] 3d2, diamagnetic

[Ar] 4s2 3d5, diamagnetic

Answer 1

Answer:

[Ar] 4s2 3d5 paramagnetic

Explanation:

Answer 2

The option that shows the correct ground state electron configuration of Mn⁴⁺ and whether paramagnetic or diamagnetic is;

Option C; [Ar]3d³ and paramagnetic

We want to find the ground state configuration of the ion Mn⁴⁺

Now, the electronic configuration of Mn which is manganese is normally written as;

[Ar]3d⁵4s²

• Now, the ion we are given Mn⁴⁺ tells us that it has lost 4 electrons and the new configuration at its' ground state is; [Ar]3d³

• Now, we see that there are now 3 numbers of 3d orbitals and so the 3d orbital is not full and as such has unpaired electrons and is therefore paramagnetic.

In conclusion, the ground state electron configuration is [Ar]3d³ and is paramagnetic.

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