00:01
So really for higher boiling points, higher boiling points are correlated with stronger intermolecular forces.
00:12
Mainly the boiling point is the point where you're breaking all of your, or the majority are all of your intermolecular forces.
00:20
So it makes sense that if you have a high boiling point, you have very strong intermolecular forces that take a high energy input in terms of temperature to break.
00:29
So mainly we're comparing strength of intermolecular forces here.
00:35
So in our first case, we have, we're comparing the difference between ammonia and methane.
00:42
So the main difference between ammonia and methane is that ammonia has hydrogen bonding, since it contains hydrogen bonded to an electronegative atom, as well as dipole interactions.
00:53
All compounds contain londent dispersion forces, and since ch4 is nonpolar, it also contains london dispersion forces.
01:01
Hydrogen bonding and dipl -dipel -dipal interactions are typically going to sum up to be stronger than london dispersion forces, which is true in this case.
01:10
And ammonia is going to have the higher boiling point.
01:16
In our second part, we have the difference between cs2 and co2.
01:22
So these compounds are both sulfur and oxygen are both relatively electronegative compared to carbon...