Question

the diagram above is a molecular model of a gaseous diatomic element that is just above its boiling point. intermolecular forces between the gas molecules will cause them to condense into the liquid phase if the temperature is lowered. which of the following best describes how the model is limited in its depiction of the phenomenon?
a it does not show how hydrogen bonds are constantly forming, breaking, and reforming, which results in a net force of attraction between the molecules.
b it does not show how the interactions between ions and the induced molecular dipoles result in a net force of attraction between the molecules.
c it does not show how the interacting permanent dipoles of the molecules result in a net force of attraction between the molecules.
d it does not show how the temporary fluctuating dipoles of the molecular electron clouds result in a net force of attraction between the molecules.

Explanation:

The model is of a non - polar diatomic gas just above its boiling point. Non - polar molecules experience London dispersion forces which are due to temporary fluctuating dipoles in the molecular electron clouds. The model does not show this aspect of intermolecular forces. Hydrogen bonds require hydrogen bonded to a highly electronegative atom, which is not applicable here. There are no ions present so ion - induced dipole interactions are not relevant. And non - polar diatomic molecules do not have permanent dipoles.

Answer:

D. It does not show how the temporary fluctuating dipoles of the molecular electron clouds result in a net force of attraction between the molecules.