00:01
In this video, we want to determine which of the molecules listed has only london dispersion forces, meaning that we want compounds that are non -polar.
00:11
So let's go through the compound.
00:12
So we have hf, which consists of a hydrogen bonded to a fluorine, and fluorine is really electroneg and withdraws electrons.
00:21
So it's polar, so no, it has more than just london dispersion forces.
00:27
Then we can consider water, which looks like this, and oxygen is really electronegative and draws electrons away from high.
00:36
Hydrogen.
00:37
We know that there's a net dipole because that's what allows for this species to hydrogen bond.
00:42
So i'll just put an x next to each one of them that we've already considered.
00:48
All right.
00:48
Then we have nh3.
00:52
Similarly, nh3 has really polar bonds and a net dipole.
00:56
It's also capable of hydrogen bonding.
00:59
Nitrogen withdraws the electrons, so nope.
01:02
All right.
01:04
Bh3.
01:05
All right, boron is an exception to the octet rule, so it only needs six valence electrons.
01:09
Meaning that if there's three hydrogens, each can form one bond, no loan pairs...