Here it says to identify the major type of intermolecular force between the particles of each of the following. So first, we're starting out with N₂. N₂ is two nitrogens bonded together, and if we assume we are in a container filled with N₂ and they are all N₂, they are all nonpolar because they are the same exact element bonded to each other. They share electrons equally and perfectly with one another. Because they are nonpolar, their major force is London dispersion, aka dispersion forces, aka van der Waals forces.

The next one, CH₃OH. The important thing here is that we have an O here, and right next to it is an H. When you have hydrogen connected to F, O, or N, it is hydrogen bonded.

The next one, CH₃Cl. If we were to draw this, we have carbon in the center connected to 3 hydrogens and then connected to a chlorine. For those of you who remember my videos on molecular polarity, we would know that this is not a perfect shape. A perfect shape would mean that all the surrounding elements are the same, but they are not. Three are hydrogens and one is a chlorine. Because it's not a perfect shape, it is a polar molecule. It's a polar covalent molecule, so its major force is dipole-dipole.

And then finally, we have KCl, which is an ionic compound. And we just said that this CH₃OH, which is called methanol, had hydrogen bonding, which is a polar force. So you have an ionic compound with a polar compound. So this would be ion-dipole.

So, remember, to be able to successfully identify all the intermolecular forces, it's going to require you remember some of our earlier topics when it comes to molecular polarity, when it comes to dipole moments. So if you haven't watched those videos or it's been a while, I suggest you go back and take a look because knowing the polarity of these compounds is sometimes key to determining the correct intermolecular force.