In Chemistry class it's easy for teachers to get so bogged down in the details of whatever vocabulary-packed topic you happen to be studying that the "big picture" goes unnoticed: ultimately, everything in chemistry is about bouncy little magnets (atoms and molecules) either sticking together (solid) or rattling apart (liquid and gas).
Dipole-Dipole & Hydrogen Bonding
These are the stronger type of intermolecular force, and are the reason that water and alcohols are liquids at room temperature. This video covers what these forces are, why they matter, and how to spot them.
London Dispersion Forces & Induced Dipoles
If you're looking at a molecule and can't figure it out the IMF's because it's not ionic or polar or dipole-dipole or hydrogen bonding or... Well, there's always London Forces! Literally, every molecule has London forces, so if all else fails, it's your default answer.
Bond Types In Solids
Ionic, Metallic, and Network Covalent bonds aren't technically "intermolecular" because they don't involve molecules, just atoms. Yet they tend to show up in the IMF chapter anyways (along with dipole-dipole, London, etc) because they have to do with why atoms form these particular types of solids. Also emphasized are the melting point and electrical properties of these types of solids, since these are common test questions.
If you do not have an account, you should get one, because it is awesome! You can save a playlist for each test or each chapter, and save your "greatest hits" into a "watch right before the final" list (not that we recommend cramming, but when in Rome...)