00:01
Okay, we need to draw an m -o diagram for any 2 -plus or the doubly positively charged ion of diatomic neon.
00:17
Well, recall that, you know, in terms of periodic table, we're saying, da -da -da -da -da -carbon, nitrogen, oxygen, fluorineon, right? meaning that this is a row two compound, right? so it's going to be just like, you know, c2, n2, o2, f2, and e2, really.
00:35
That is, we should expect to have, you know, 1s orbitals to overlap, 2s orbitals to overlap, and 2p orbitals that overlap.
00:48
And that's going to be the foundation of our molecular orbital diagram.
00:53
So i've got a template here of exactly that, right? but this is blank, right? so theoretically, you can take something like this and fill it up for any diatomic from row one.
01:07
And here we're going to do any two, right? so what that means is that we're going to have ne plus over here and ne plus over here.
01:16
And the question is, how many electrons should ne plus have? well, neon itself, we know it's a noble gas.
01:25
It should have eight electrons in its valence cell.
01:29
Right so not counting the 1s orbital which is not in its valent shell which we should expect to be full we should expect that any plus has seven electrons right and that's going to be true for either and we should know that its inner shells should also be full right because how would we get to the outer shells right so two electrons in each of the 1s orbitals meaning a total of four electrons in the sigma 1s and sigma star 1s.
01:59
That's sort of besides the point.
02:02
They're there, but they don't do anything.
02:03
They don't increase the bond order, right? okay.
02:08
So now we move on to the important ones.
02:10
Seven electrons that i should fill into ne plus.
02:13
Well, i know i'm going to fill the s orbitals first, one up, one down...