Final answer:
Water has stronger intermolecular forces than mercury at room temperature due to the presence of hydrogen bonds in water molecules. These hydrogen bonds contribute to water's high surface tension and heat of vaporization. In contrast, mercury has weaker intermolecular forces known as London dispersion forces.
Step-by-step explanation:
The intermolecular forces in water and mercury are different due to the nature of the molecules. Water molecules can form hydrogen bonds with each other, which are strong intermolecular forces. Mercury, on the other hand, consists of individual atoms that do not form strong intermolecular forces.
Hydrogen bonding, which involves the attraction between a hydrogen atom and an electronegative atom like oxygen, is a strong intermolecular force. It gives water its unique properties, such as high surface tension and heat of vaporization.
In contrast, mercury has weaker intermolecular forces, known as London dispersion forces, which result from temporary fluctuations in electron distribution. These forces are weaker than hydrogen bonds and contribute to lower surface tension and heat of vaporization.