Question

Does the nature of intermolecular forces change when a substance goes from a solid to a liquid, or from a liquid to a gas? What causes a substance to undergo a phase change?

Short answer

Yes, the nature of intermolecular forces changes when a substance goes from one phase to another. In solids, intermolecular forces are generally stronger; in liquids, they are weaker than in solids, and in gases, they are significantly weaker compared to solids and liquids. Phase changes are primarily caused by changes in temperature and pressure, which influence the strength of intermolecular forces and the kinetic energy of the molecules.

Step-by-step solution

Introduction to Intermolecular Forces

Intermolecular forces are the forces between molecules in a substance. There are several types of intermolecular forces such as van der Waals forces, dipole-dipole interactions, and hydrogen bonding. These forces are weaker than the intramolecular forces (chemical bonds within a molecule).

Solid Phase

In the solid phase, the intermolecular forces are generally stronger, and the molecules are closely packed together. The molecules vibrate around their fixed positions, but they do not move past one another. The strong intermolecular forces hold the molecules in a fixed arrangement, resulting in the substance having a definite shape and volume.

Liquid Phase

In the liquid phase, the intermolecular forces are weaker compared to the solid phase. The molecules are still closely packed, but they have more freedom to move around. They can slide past each other, which allows the liquid to flow and take the shape of its container. The weaker intermolecular forces in the liquid phase are what gives the substance its fluidity.

Gas Phase

In the gas phase, the intermolecular forces are significantly weaker compared to the solid and liquid phases. The molecules are spaced far apart and move freely and randomly, which allows the gas to not only take the shape of its container but also expand to fill the container's entire volume.

Phase Changes and Intermolecular Forces

When a substance transitions from one phase to another, the nature of the intermolecular forces changes as well. For example, when a solid becomes a liquid through melting, the intermolecular forces are weakened, allowing the molecules to move more freely. Similarly, when a liquid becomes a gas through vaporization, the intermolecular forces are weakened even further, allowing the molecules to move around with more freedom.

Factors Causing Phase Change

The most common factors that cause a substance to undergo a phase change are changes in temperature and pressure. When a substance is heated, its molecules gain kinetic energy, which causes them to vibrate or move more rapidly. As the kinetic energy surpasses the strength of the intermolecular forces, the substance undergoes a phase change, such as from a solid to a liquid or from a liquid to a gas. Conversely, when a substance is cooled, its molecules lose kinetic energy, and the intermolecular forces become stronger, resulting in phase changes such as from a gas to a liquid or from a liquid to a solid. Changes in pressure also impact the phase transitions due to variations in the density of the substance and its response to external forces. In conclusion, the nature of intermolecular forces does change when a substance goes from one phase to another, and phase changes are mainly caused by changes in temperature and pressure that influence the strength of intermolecular forces.