What is the relationship between vapor pressure and atmospheric pressure during boiling?

During boiling, a liquid transitions to its gaseous state, and this process occurs when the liquid's vapor pressure equals the atmospheric pressure exerted on it. At this point, bubbles of vapor can form throughout the liquid, rather than just at the surface, allowing the liquid to boil.

When a substance boils, it changes from a liquid to a vapor, which implies that there is sufficient energy present to overcome intermolecular forces. For this to happen throughout the entire body of the liquid, the vapor pressure must reach a point where it matches atmospheric pressure. Only at this point do the conditions allow for bubble formation and the subsequent boiling of the liquid. Therefore, the relationship between vapor pressure and atmospheric pressure during boiling is that they become equal.

While it’s important to note that vapor pressure can fluctuate based on temperature (with higher temperatures yielding higher vapor pressures), during boiling, the critical factor is that these pressures balance out. This understanding plays a fundamental role in concepts such as phase changes and thermodynamics in chemistry.