The force attraction of the molecule in volatile liquid
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Volatility of a Liquid
With sufficient kinetic energy, most liquids can become gases through the process of vaporization. Whether or not a liquid will vaporize depends upon the chemical properties of the liquid. Volatile liquids, including ethanol, vaporize with relative ease. Scientists commonly use the boiling point of a liquid as the measure of volatility.
Volatile liquids have low boiling points.
A liquid with a low boiling point will begin to boil faster than liquids with higher boiling points.
Much less energy (in the form of heat) is required to break the intermolecular bonds of a volatile liquid than those of liquids having higher boiling points.
Once enough energy is supplied to break apart the bonds between molecules, the molecules are free to expand and escape the liquid surface in the form of a gas.
Chemical Bonds contribute to volatility
The major attractive forces between molecules in a liquid are called hydrogen bonds. Less hydrogen bonding is expected between molecules of a volatile liquid compared with other less volatile liquids. With fewer hydrogen bonds holding volatile compounds in the liquid state, only minimal energy is required to break the bonds and allow the molecules to drift apart and escape from the surface of the liquid as a gas.