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 depicts a gaseous diatomic element. Diatomic elements are non - polar (e.g., $H_2$, $N_2$). Non - polar molecules have London dispersion forces, which are due to temporary fluctuating dipoles in molecular electron clouds. The model doesn't show this. Hydrogen bonds occur between molecules with $N - H$, $O - H$ or $F - H$ bonds. There are no ions present for ion - induced dipole interactions, and non - polar diatomic molecules don't 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.