The boiling point of a substance originates from the molecular structure and intermolecular forces within that substance. The boiling point is the temperature at which the vapor pressure of a liquid equals the atmospheric pressure, causing the liquid to change into a gas. This phenomenon is rooted in the kinetic theory of molecules, which posits that molecules in a liquid are in constant motion and that their kinetic energy increases with temperature.

The boiling point of a substance is influenced by several factors, including the strength of intermolecular forces, the molecular mass, and the presence of impurities. For instance, substances with stronger intermolecular forces, such as hydrogen bonding in water, have higher boiling points than those with weaker forces, like van der Waals forces in methane. Additionally, substances with higher molecular masses generally have higher boiling points due to the increased kinetic energy required to overcome intermolecular forces.

Data from the CRC Handbook of Chemistry and Physics (2016) reveals that the boiling point of water, which is a common solvent, is 100 degrees Celsius at sea level. This value is consistent with the kinetic theory of molecules, as water molecules are held together by strong hydrogen bonds. In contrast, the boiling point of methane, a simple hydrocarbon, is -161.5 degrees Celsius, reflecting its weaker intermolecular forces and lower molecular mass.

In summary, the boiling point of a substance originates from the molecular structure and intermolecular forces, which are governed by the kinetic theory of molecules. The strength of these forces, along with molecular mass and impurities, determines the boiling point of a substance.