Which statement about intermolecular forces in liquids is false? 1. the stronger the intermolecular forces, the greater the molar heat of vaporization. 2. the weaker the intermolecular forces, the lower the surface tension. 3. the weaker the intermolecular forces, the more rapid the evaporation rate. 4. the stronger the intermolecular forces, the lower the boiling point. 5. the greater the intermolecular forces, the lower the vapor pressure.

Option (4) is the correct answer.

Explanation:

When molecules of a substance are held together by strong intermolecular forces of attraction then in order to separate the molecules we need to provide great amount of heat to the substance.

This means greater is the  intermolecular forces, the greater the molar heat of vaporization.

When molecules beneath the surface of a liquid tends to attract the molecules present at the surface then a force is exerted at the surface of the molecules of the liquid which is known as surface tension.

Hence, weaker the intermolecular forces, the lower the surface tension.

When there is weaker intermolecular forces present in a substance then its molecules are able to move freely. Hence, the more rapid will be the evaporation rate of the substance.

Also, more is the intermolecular forces more heat will be required to break the bonds within molecules in order to change the state of substance. Hence, more will be the boiling point of substance.

Therefore, the statement stronger the intermolecular forces, the lower the boiling point, is false.

The pressure exerted by a gas on the surface of a liquid is defined as the vapor pressure.

Hence, the greater the intermolecular forces, the lower the vapor pressure.

Thus, we can conclude that the statement stronger the intermolecular forces, the lower the boiling point is false about intermolecular forces in liquids.

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