Intermolecular Forces

Ion-Dipole Forces
The attraction between an ion and a pole of a polar molecule(dipole).
BE(Bond Energy) = 40-600 kJ/mol

Dipole-Dipole Forces
The attraction between oppositely charged poles of polar molecules.
BE = 5-25 kJ/mol

Hydrogen Bond
When an H atom is bound to a small and highly electronegative atom with lone pairs (N,O or F) the electrons are drawn away from the H atom making this particular covalent bond very polar. The H atom has a relatively strong + charge and the N, O or F atom has a relatively strong - charge. The + H atom of one of these molecules forms very strong bonds with the - N, O or F atom of another of the molecules. The H atom is specifically attracted to the lone pairs of electrons of the N, O and F atoms.
BE = 10-40 kJ/mol

Charge-Induced Dipoles
Lone pair electrons are in constant motion around their atom in what we picture as a cloud of negative charge. A nearby electric field can distort the cloud by pulling it towards a positive charge or pushing it away from a negative charge. This distortion results in a temporary induced dipole in the electrons molecule.
Ion-induced dipole and dipole-induced dipole are two examples of this.
Ion-induced dipole BE = 3-15 kJ/mol
Dipole-induced dipole BE = 2-10 kJ/mol

Dispersion Forces
Momentary oscillations of electron charge can create an instantaneous dipole within an atom which in turn induces dipoles in neighboring atoms. This happens all throughout a substance so all the molecules in a substance are slightly attracted to each other.
Also known as instantaneous dipole-induced dipole forces.
BE = 0.05-40 kJ/mol