What can be said about intermolecular forces between gas molecules?

Intermolecular forces between gas molecules are typically weak and not significant at normal conditions, which is why the choice indicating this is correct. In gases, the molecules are far apart compared to liquids or solids, leading to a minimal influence of attractive or repulsive interactions.

At standard temperature and pressure, the kinetic energy of gas molecules is significantly higher than the energy associated with intermolecular forces. As a result, gas molecules move freely and independently, allowing gases to expand to fill their containers. This characteristic of gases explains why intermolecular forces are generally negligible under typical conditions.

In contrast to this correct option, strong intermolecular forces are more relevant in solids and liquids, where the molecules are closer together and can interact more significantly. The suggestion that intermolecular forces are the same in liquids does not apply, as liquids have much stronger forces due to their closer arrangement. High pressures can lead to increased intermolecular interactions, but this is not the norm for gases under typical conditions.