What describes the intermolecular forces in simple molecular structures?

The intermolecular forces in simple molecular structures, such as those found in substances like nitrogen (N₂) and carbon dioxide (CO₂), are indeed very weak. These forces, known as van der Waals forces or London dispersion forces, arise due to temporary dipoles that occur when the electron distribution within molecules becomes uneven.

Because these forces are weak, simple molecular structures tend to have lower boiling and melting points compared to ionic or metallic compounds, which are held together by much stronger bonds. The weak intermolecular forces allow these substances to exist as gases or liquids at room temperature and means that they can easily be separated from one another when energy is added, such as through heating.

In contrast, very strong intermolecular forces would imply that the substances would have high boiling and melting points, which is not the case for simple molecular substances. Moderate forces would not fully capture the essence of the weak attraction present. Finally, non-existent forces would suggest that the molecules do not exert any attraction toward each other, which is incorrect as they do exhibit some degree of attraction, albeit weak. Thus, the characterization of these forces as very weak accurately reflects their nature in simple molecular structures.