00:01
When we have two hydrocarbons, like in part a, that only have dispersion forces, hydrocarbons only have dispersion forces, the one with more carbons or greater molar mass is going to have the higher boiling point.
00:16
So out of ch3, h8, and ch4, h10, this will have the higher boiling point.
00:36
Then if we're comparing two species that are about the same molar mass, but one has, dipyl dipyl diphyl -ythor, that being diethyl ether, and one has hydrogen bonding, that being butanol, because hydrogen bonding is a stronger intermolecular force than dipole -dipole, then one butanol will have the higher boiling point.
01:08
Then if we look at s .o .2 versus s .o .3, ends up taking on a trigonal planar geometry, kind of suggesting that the dipole forces cancel, but it also has a greater molar mass than so2, and that wins...