1. The problem statement, all variables and given/known data QUESTION: Methane (CH4) is a gas at room temperature and pressure while water is a liquid. In both molecules hydrogen atoms are bonded to a non-metal element. Water also has a much higher heat of vaporization than methane even though the molecular weights of these two molecules aren't that different. I am to: -account for these differences by describing the bonding between atoms within these two molecules, and the bonding and intermolecular interactions between molecules in each. -indicate how electronegativity differences between the elements, and geometry of the molecules, are both important. -explain what hydrogen bonding is. -indicate what is happening on the molecular level when water boils, and what kind of bonds or interactions need to be broken. 3. The attempt at a solution This question contains many little ones! I believe that hydrogen bonding involves dipole forces. I assume that in order to indicate how electronegativity differs between the elements, I would use the elements of methane (CH4). I really need a lot of help on this. Hopefully it makes sense to someone out there!! Thanks!