Figuring out Intermolecular Forces?

Question

I believe the answer for the first question is hydrogen bonding, but I am not sure about the other ones.

What is the strongest type of intermolecular force in each of the following compounds?

 Dipole-dipole London dispersion Hydrogen bonding  CH₃-O-CH₃

 Dipole-dipole London dispersion Hydrogen bonding  SO₂

 Dipole-dipole London dispersion Hydrogen bonding  CH₃NH₂

 Dipole-dipole London dispersion Hydrogen bonding  PF₅

 Dipole-dipole London dispersion Hydrogen bonding  XeCl₂

Answer 1

There will not be any hydrogen bonding in the first one, CH₃-O-CH₃ because to have H-bonding you need to have a H atoms attached to either a F, O or N atom. Not the case here. But this molecule will exhibit weak dipole-dipole because of the somewhat negative O atom.

In SO2, you have mainly London dispersion because it is non polar

In CH₃NH₂ you have hydrogen bonding because a H atom is bonded to a N atom

In PF₅ you will have London dispersion because there is no H-bonding and the molecule is non polar so there won't be any dipole-dipole.

In XeCl₂ you will have London dispersion because no H-bonding and again, the molecule is non polar so no dipole-dipole interactions.