Final answer:
The statement regarding molecules at the surface of a liquid exerting vapor pressure if they have enough kinetic energy is true. Vapor pressure is influenced by the molecular intermolecular forces and temperature, with stronger forces leading to lower vapor pressures, and higher temperatures resulting in higher vapor pressures.
Step-by-step explanation:
The statement that molecules at the surface of a liquid, if they possess enough kinetic energy, can escape to the gas state and that a liquid will exert a vapor pressure is true. The magnitude of the vapor pressure is indeed determined by the strength of the intermolecular forces within the liquid and the temperature of the sample. A substance with relatively strong intermolecular attractive forces will have a lower vapor pressure because these forces tend to hold the molecules together, making it harder for them to escape into the vapor phase.
On the other hand, substances with weak intermolecular forces tend to have a higher vapor pressure since these molecules can escape into the gas phase more easily. The temperature of the liquid also plays a crucial role; at higher temperatures, the average kinetic energy of the molecules increases, and thus a greater number of molecules have sufficient energy to vaporize. This leads to an increase in vapor pressure with temperature.