Which of the following is true regarding the behavior of gas particles?

The behavior of gas particles is best characterized by their constant motion. This property is a fundamental aspect of gas laws and the kinetic molecular theory, which states that gas molecules are in continuous, random motion, colliding with one another and the walls of their container. This constant movement contributes to the pressure exerted by the gas, as these collisions occur frequently and with varying energy, depending on the temperature of the gas.

In contrast, other options suggest behaviors that don't accurately describe gas particles. For instance, gas particles do not move in an orderly fashion; rather, their motion is described as random and chaotic. Additionally, gas particles occupy a relatively large amount of space, but their own volume is considered negligible compared to the distance between particles, meaning they have no significant volume. Finally, gas particles do not require high temperatures to move; they are always in motion, even at low temperatures, though this motion slows as temperature decreases. Thus, the idea that gas particles can only move at high temperatures is a misunderstanding of gas behavior.