1. The problem statement, all variables and given/known data The question asks to list all the intermolecular forces operating in each of the two liquids. [itex]H_2O[/itex] [itex]CH_3OH[/itex] 2. Relevant equations N/A 3. The attempt at a solution I'm mostly getting confused about the London Dispersion Force with water, and London Dispersion Force and Dipole-Dipole with Methanol. I know that both of these molecules have a Hydrogen Bond, but I can't seem to pinpoint the other forces. I've googled it and seen several people state that water has all three, and methanol has only LDF and Dipole-Dipole. Drawing the lewis dot diagram of these I just don't see how water can have a LDF, and how methanol can have either an LDF or a Dipole-Dipole. Is it because they are asking for it in a liquid state, and they can orient themselves more freely? Any help is appreciated, or let me know if perhaps I have a concept wrong. Mac *EDIT* Just to add to this, [itex]CH_3F[/itex] would appear to me to have an obvious Hydrogen bond, as you have extreme polar opposites from the Electronegative Fluorine on one side of the molecule, and Hydrogen on the other side. However, it seems from what I've found online that this molecule does not have a hydrogen bond. I think I am definitely missing something. *2nd EDIT* Okay, as for above I see that the Fluorine is not bonded directly with the Hydrogen, so there can not be a Hydrogen Bond. That does not apply to the Methanol though.