Question

Repulsion of electrons within two interacting molecules produces changes in electron distribution. This change in electron distribution creates temporary dipole moments. Which of the following does this explain?

Choose one or more:

A. This explains why the dipole-dipole attractive force between dimethyl ether and acetone does not entirely account for the attractive force between these molecules. B. This explains why ammonia and nitrogen gas exhibit an attractive force between them. C. This explains how the molecules hydrogen fluoride and methanol can exhibit uncharacteristically strong intermolecular forces. D. This explains how two noble gases' molecules can have an attractive force between them. E. This explains why long hydrocarbon chains have relatively high boiling points.

Answer 1

D) This explains how two noble gases molecules can have an attractive force between them.

This force is called as van dar Waals forces.

It plays a fundamental role in fields in as diverse as supramolecular chemistry structural biology .

If no other forces are present, the point at which the force becomes repulsive rather than attractive as two atoms near one another is called the van der Waals contact distance. This results from the electron clouds of two atoms unfavorably coming into contact.[1] It can be shown that van der Waals forces are of the same origin as the Casimir effect, arising from quantum interactions with the zero-point field.[2] The resulting van der Waals forces can be attractive or repulsive.[3] It is also sometimes used loosely as a synonym for the totality of intermolecular forces.[4] The term includes the force between permanent dipoles (Keesom force), the force between a permanent dipole and a corresponding induced dipole (Debye force), and the force between instantaneously induced dipoles