Define the terms boiling point and normal boiling point.

When we talk about the normal boiling point of a substance, we're referring to the specific temperature at which it transforms from a liquid into a gas under very particular conditions. This change occurs only when the atmospheric pressure around the substance is exactly 1 standard atmosphere (1 atm)—the average pressure at sea level on Earth. It's a standardized measure useful for comparing different substances. For example, water's normal boiling point is well-known to be 100°C (212°F) at 1 atm.

Understanding this concept is crucial because the boiling point can change with variations in atmospheric pressure. On a mountaintop, where the pressure is lower, water boils at a temperature lower than 100°C, which affects cooking times and even the taste of food.

Vapor pressure is an indicator of a liquid’s evaporation rate and reflects how molecules escape from the liquid to form a vapor. This pressure is created by the molecules that have escaped the liquid phase and are exerting force on their container.

The vapor pressure of a substance increases with temperature because the molecules move more vigorously and can escape the liquid more easily. When the vapor pressure equals the external pressure, the liquid boils. This equality means that the molecules have enough energy to break free from the liquid’s surface tension and form bubbles within the bulk of the liquid, not just on the surface.

A phase transition is when a substance changes from one state of matter to another, such as from a liquid to a gas during boiling. This transformation occurs due to changes in temperature and pressure, which impact the energy and movements of the particles in a substance.

Boiling is a fascinating example of a phase transition, as it involves a rapid change where liquid molecules suddenly have enough energy to form a vapor. It's essential to recognize that phase transitions are not just about the shifting from one physical state to another, but also about the energy exchange involved in breaking intermolecular forces.

The pressure exerted on a substance by its surroundings is called external pressure. It's an essential factor in determining the boiling point of a liquid, as seen in everyday experiences like cooking at high altitudes.

External pressure affects boiling because it is the pressure that the vapor pressure must overcome for a liquid to boil. High external pressure requires the molecules in the liquid to work harder and increase their kinetic energy to reach the boiling point, resulting in a higher boiling temperature. Conversely, lower external pressure, such as in high altitudes, means that the boiling point will be lower because less energy is required for the liquid molecules to escape into the gaseous phase.