Question

What is the magnetism of O2+2, and how many unpaired electrons does it possess?
1. paramagnetic; 3
2. diamagnetic; 2
3. diamagnetic; 0
4. paramagnetic; 1
5. paramagnetic; 4
6. paramagnetic; 2
7. diamagnetic; 1

Answer 1

The molecule is diamagnetic with zero unpaired electrons.

In order to determine the magnetism of the O2^2+ ion, we must have to write the molecular orbital configuration and fill its electrons into molecular orbitals. There are 14 electrons in the molecule. Its molecular orbital configuration is;

σ1s2, σ*1s2, σ2s2, σ*2s2, σ2px2 π2py2 π2pz2

We can see from the molecular orbital configuration of the molecule that the molecule is diamagnetic with zero unpaired electrons.

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