(A – r) ; (B – p, r) ; (C – p, q, r) ; (D – p, r) ; (E – p, r, s).

Br 2 is non-polar in nature. All molecules experience London dispersion forces which results from the motion of electrons.

HF has hydrogen bonding in liquid as well as in solid state. HF molecules also experience dispersion forces.

Ion-dipole forces are found in the solutions of ionic compounds in polar solvent where solvated species such as Na(OH 2 ) x+ and F(H 2 O) y– exist. Hydrogen bond exist between water molecules. In addition they also experience dispersion London forces.

CH 3 NH 2 is a polar molecule that can form hydrogen bonds. In addition, it has dispersion forces.

(E) Induced dipole-dipole interaction exists between non-polar molecules and polar molecules such as clathrate compound of Xe gas with water, when water is frozen under a high pressure of the gas. They have formulae approximating to 6H 2 O : 1 gas atom (i.e. Xe.6H 2 O).

In addition, Xe.6H 2 O has H-bonding and dispersion forces.