00:01
So for this question you're trying to figure out which type of hybridization will form the strongest sigma bond.
00:12
So the rule of note is that it will have a shorter, hence a stronger bond, or stronger, stronger sigma bond, right, the closer it is to the nucleus.
00:45
And what affects that is the s character of the hybrid orbital.
00:57
So the more s character that hybrid has, the shorter and stronger that bond will be.
01:14
Right, if you think about electrons in an s orbital versus a p orbital, the ones in the s orbital are closer, right, to the nucleus than the p.
01:25
So since they're closer to the nucleus, they're going to have a shorter and stronger bond.
01:34
So which of these hybrid orbitals has the most s character? so, right, when we think about it, when we're looking at the sp3 hybrid orbital, right, say we have our, you know, our 2s and our 2p orbitals, and we have two electrons in the s and then two electrons in the 2p.
02:18
To form that hybrid, one of these s electrons is going to fill that empty orbital.
02:29
So then we're going to have one electron in each orbital.
02:36
So if we look at the sp3, right, we lost this s electron and it went into the p orbital.
02:42
So we have less s character and more p, right, we have one electron in an s orbital basically and three in a p orbital...