The Boiling Point: Factors Affecting the Boiling Point of a Compound

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The theory of boiling point of a compound
The molecule in a liquid are closely packed together which consists of several random
movements which are in constant motion. During heating, the temperature is equally increases
creating increase in kinetic energy which in turn increases the molecular random motion. Due
high intensity, such heat weakens the forces of attraction making liquid molecules to become
free and mobile hence forming a vapour. The boiling point therefore varies depending on the
atmospheric pressure on the environment. Liquids at low atmospheric pressure have low boiling
point while liquids at high atmospheric pressure have high boiling point. From the above
explanation, boiling point can be defined as;
The boiling point of a substance refers to the process by which liquid substance is changed into
gaseous state. The liquid therefore changes into vapour by the process of evaporation. Through
this process of evaporation, the liquid substance will be transformed into vapour which escape to
the surrounding (Vogel, 2013).
Normal boiling point of a compound is the evidence of volatility of such a substance. A
compound is said to be less volatile if its boiling point is high. On the other hand, a compound is
said to be highly volatile if it has a lower boiling point. It is therefore clear that at high
temperature, in a situation where a compound’s boiling point is low it will vaporise into the
atmosphere whereas if a compound’s boiling point is high it forms liquid or solid. This is greatly
evidenced by the strength of intermolecular forces in the bonding structure of the compound.
The intermolecular forces have several effects on boiling point of a compound which depends on
the functional group that exists in its molecular structure (Haynes, 2014).
The length of carbon chain has a greater effect on the boiling point of a compound.