Intermolecular Forces

Solid vs Liquid vs Gas

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.