The intermolecular interaction that is dependent on the inverse cube of the distance between the molecules is:
A. ion-ion interaction
B. ion-dipole interaction
C. London force
D. hydrogen bond

Hint: The hydrogen bond is an example of a dipole-dipole interaction and it is an example of an electrostatic force between a covalently bonded hydrogen atom of one molecule and an electronegative atom.

Complete step by step answer:
The strength of the hydrogen atom is inversely proportional to the cube of the distance between the molecules. This makes it a type of weak force of attraction whose bond strength ranges between 8-42 kJ/mol. But, the overall strength of the hydrogen bond is greater than the van der waal’s force of attraction. In the case of other forces provided in the various options in the question, we find that according to their strength, none is inversely proportional to the cube of distance between the molecules. In dipole-dipole interaction, the major role is played by the electronegativity of the adjacent atoms along with the covalently bonded hydrogen atom present at a nearby location. The formation of feeble charges causes the formation of very weak bonds. The hydrogen bond is of two types:
(i) Intermolecular hydrogen bond- The H-bond between two or more molecules of either the same or different compounds.
(ii) Intramolecular hydrogen bond- H-bond formed between the molecules of the same compound.

Thus, the correct option is (D) hydrogen bond.

Note:
Here, in this question, one must have to understand that the higher the order of distance of separation of molecules, the lower the strength of the attractive forces or the lower the interaction among the molecules is.