Chem energy question (intermolecular forces?) ?

Question

Comparing the energies of the following intermolecular forces on a kJ/mol basis, which would normally have the highest energy (i.e., be the strongest force)?
Answer
Question 5 answers
A. dipole-dipole
B. ion-induced dipole
C. ion-dipole
D. dispersion
E. dipole-induced dipole

Answer 1

A quiz question I believe.

Homework or Chemistry might be a better category.

I feel you should do this on your own.

Answer 2

a)Hydrogen bonding is present in water, to a lesser extent in ammonia, and not at all in methane. When hydrogen bonding is present, more energy must be invested to overcome the intermolecular forces. b)At 25C and 1 atm. chlorine is a gas, bromine a liquid, and iodine a solid because of the Van der Waal's force (London dispersion force) which increases with mass. Chlorine, the lighest of the three, is in a gaseous phase because less energy was required to overcome the Van der Waal's force. c)calcium oxide melts at a much higher temperature than does potassium chloride because calcium oxide has a much higher lattice energy due to the high charges of Ca and O (2and -2 respectively) vs. the charges of KCL (1 and -1 on the ions respectively). d) ethanol is a liquid rather than a gas because unlike propane, ethanol contains an O-H group giving it hydrogen bonding which explains the higher boiling point of ethanol.