00:01
In the case of nitrogen and all - the order of the molecular orbitals is going to be σ1s, σ1s -star, or σ -star, 1s, and then we have π2p, and then σ2p, and then π2p -star, and σ2p -star.
00:42
So one of our options is n2.
00:53
To be paramagnetic, we need to have lone pairs.
00:58
N2 has a total of ten valence electrons, five from each nitrogen.
01:05
If we plug them in, 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, we see that there are no unpaired electrons, so this is not paramagnetic.
01:16
For all of our other options, the order is slightly different.
01:23
We've got 1s, 2, sorry, we've got σ1s, σ1s -star, but then we have σ2p, and the π2p is switched, and this is what it is for all the other options.
01:49
In the case of oxygen, o2, 2-, oxygen has six valence electrons.
02:02
There are two of them, and then there are two additional electrons, so that adds up to 14...