Suppose you have two colorless molecular liquids, one boiling at \(-84^{\circ} \mathrm{C},\) the other at \(34^{\circ} \mathrm{C},\) and both at atmospheric pressure. Which of the following statements is correct? For each statement that is not correct, modify the statement so that it is correct. (a) The higher-boiling liquid has greater total intermolecular forces than the lower- boiling liquid. (b) The lower-boiling liquid must consist of nonpolar molecules. (c) The lower- boiling liquid has a lower molecular weight than the higher-boiling liquid. (d) The two liquids have identical vapor pressures at their normal boiling points. (e) At \(-84^{\circ}\) both liquids have vapor pressures of 760 \(\mathrm{mm} \mathrm{Hg}\) .

Understanding how intermolecular forces influence the boiling points of liquids is crucial for comprehending the physical properties of substances. Fundamentally, intermolecular forces are the forces of attraction and repulsion between molecules. They include dipole-dipole interactions, hydrogen bonding, and dispersion forces, also known as London forces.

These forces dictate how tightly molecules are held together in a liquid. A substance with stronger intermolecular forces will require more energy—in the form of heat—to break these attractions and transition from the liquid to the gaseous state, which leads to a higher boiling point. Conversely, weaker intermolecular forces mean that less energy is needed for the molecules to escape into the vapor phase, resulting in a lower boiling point.

The concept of vapor pressure is a core piece in the puzzle of understanding a liquid's boiling point. Vapor pressure is the pressure exerted by the vapor in equilibrium with its liquid phase at a given temperature. The presence of stronger intermolecular forces can reduce a substance's vapor pressure because fewer molecules have the kinetic energy needed to escape into the vapor phase at a given temperature.

A liquid boils when its vapor pressure equals the external pressure, typically atmospheric pressure. Thus, substances with differing boiling points will have different vapor pressures at a given temperature. For example, at a liquid's boiling point, the vapor pressure will be 760 mm Hg, but at any other temperature, the vapor pressures will not be identical unless both substances are at their respective boiling points.

In the context of boiling points and intermolecular forces, molecular weight is another key factor. Generally, molecules with higher molecular weights have more electrons, leading to stronger dispersion forces due to greater polarizability. This typically results in higher boiling points. However, it is not the sole factor determining a substance's boiling point. The type of intermolecular forces (such as hydrogen bonding) can play a far more significant role.

Therefore, while a higher molecular weight can be associated with a higher boiling point through stronger intermolecular forces, it is not an absolute rule. Other types of intermolecular attractions can complicate this picture, as can the shape of the molecule and its ability to pack in the liquid phase.