00:02
Hi there.
00:03
In this question, i went ahead and sketch this molecule out showing the actual carbons and the hydrogens.
00:12
And what we are interested in is the type of orbital overlap that forms this bond right here.
00:19
Okay, so that's going to form between what i'm just arbitrarily calling carbon one and carbon two, the two carbons that i'm interested in.
00:29
So looking first at carbon one, we see that carbon one has four atoms bonded to it, and it has zero blown pairs.
00:52
That means we need a total of four equal energy orbitals.
01:05
And equal energy orbitals are perhaps better known as hybrid orbitals.
01:18
The way to form hybrid orbitals is by taking the s orbital from the valent shell and blending it with three, or all three actually, of the p orbitals because one s and three of the p orbitals added together gives us a total of four equal energy orbitals.
01:40
So the first carbon is going to have sp3 hybridization...