00:01
So in the lewis model, when we see two bonds being formed between two atoms, a double bond, all we see is just four electrons are shared between them instead of two.
00:11
But in the valence bond theory, we see a little bit better of a picture.
00:16
I'm going to take an example of ethylene, which is c2h4.
00:23
And if we draw this out, we see if there's a double bond between the carbons.
00:29
And then since they each have four bonds, they each get two more.
00:31
More hydrogen atoms here.
00:41
So these two bonds here are not identical.
00:44
If we look at the number of things that this carbon atom here is bonded to, it's only three.
00:51
So we know that it has to be sp2 hybridized because it's going to form three sigma bonds and we want them all to be the same energy.
01:01
So this is only as one s orbital...