Final answer:
A volatile liquid quickly evaporates and transitions into the gas phase due to high vapor pressure and low boiling point, influenced by temperature and weak intermolecular interactions.
Step-by-step explanation:
A volatile liquid is one that evaporates quickly so it transitions easily into the gas phase. When a liquid is in an open container, the molecules that escape into the vapor phase will diffuse through the gas phase away from the container, leading to continuous evaporation until the liquid has effectively 'disappeared.' The rate of evaporation is influenced by the liquid's vapor pressure and the temperature. Volatile liquids have high vapor pressures and tend to evaporate readily, making them transition more easily to the gas phase. For example, substances like diethyl ether, acetone, and gasoline are considered volatile. In contrast, substances with lower vapor pressures, such as mercury, ethylene glycol, and motor oil, are nonvolatile and evaporate more slowly.
Volatile substances are characterized by low boiling points and weak intermolecular interactions, while nonvolatile substances have higher boiling points signifying stronger intermolecular forces. The liquid state of matter is itself more energetic than a solid but less than a gas, allowing liquid molecules to move more freely compared to solids. The phase a substance is in is determined by the balance between particle energy and intermolecular forces, where temperature plays a critical role in defining the stable state of matter.