From what i currently understand, Chlorine is more electronegative than iodine. So the force of the dipole dipole forces should be higher and therefore the boiling point should be much higher. I also understand that London dispersion forces increase with increasing molar mass (due to the number of electrons within the element). However, i was also informed that the dipole dipole forces are much stronger than that of London dispersion forces. So to sum it up, shouldn't HCl have a higher boiling point than HI? Clearly something is wrong with my logic because the order boiling points is: HI>HBr>HCl. Can someone please explain this? Thank you very much!!