Which of the following indicates the exsistence of stron intermolecular forces of attraction in a liquid?
a very low boiling point
a very low vapor pressure
a very low critical pressure
a very low viscosity
a very low heat of vaporization
A very low vapor pressure means the molecules have a tough time separating from each other from the liquid to the vapor state. The molecules are hanging together.
A very low vapor pressure indicates the presence of strong intermolecular forces of attraction in a liquid.
The correct answer is "a very low vapor pressure."
To determine which choice indicates the existence of strong intermolecular forces of attraction in a liquid, we need to understand the relationship between intermolecular forces and the physical properties of liquids.
Intermolecular forces are the attractive forces between molecules in a substance. They can be categorized into different types, such as dipole-dipole interactions, hydrogen bonding, or London dispersion forces. These forces play a crucial role in determining the physical properties of substances, including boiling point, vapor pressure, critical pressure, viscosity, and heat of vaporization.
Vapor pressure is the pressure exerted by a vapor when it is in dynamic equilibrium with its liquid phase. It is directly related to the strength of intermolecular forces. If the intermolecular forces are weak, the molecules will easily escape from the liquid phase and form a vapor, resulting in a high vapor pressure. Conversely, if the intermolecular forces are strong, it will be harder for the molecules to escape from the liquid, leading to a lower vapor pressure.
Therefore, a very low vapor pressure indicates that there are strong intermolecular forces of attraction in the liquid. This suggests that the molecules are tightly held together, making it difficult for them to escape and form a vapor.