To form a gas, the molecules of a liquid must overcome the intermolecular forces of attraction that bind them in the liquid state. As these forces of attraction become stronger, what happens to the boiling point?
the boiling point:increases, decreases, or remains constant
Number of molecules increases
stay the same
To understand the relationship between the strength of intermolecular forces and the boiling point of a liquid, we need to consider that boiling occurs when the vapor pressure of the liquid is equal to the atmospheric pressure.
When the intermolecular forces of attraction between the molecules in a liquid are strong, it requires more energy to overcome these forces and transition into the gas phase. Consequently, the liquid has a higher boiling point because higher temperatures are needed to provide the necessary energy for the molecules to break free from their arrangement in the liquid phase.
On the other hand, if the intermolecular forces of attraction are weak, it takes less energy to overcome these forces, and the liquid molecules can transition more easily into the gas phase. Thus, a liquid with weaker intermolecular forces will have a lower boiling point because less temperature is needed to reach the vapor pressure required for boiling.
In summary, as the intermolecular forces of attraction become stronger, the boiling point of the liquid increases. Conversely, if these forces become weaker, the boiling point decreases.