Explain the trend in boiling points between HF, HCl and HBr.

There are two themes in this answer. The first being the hydrogen bonding potential of HF and the second being the difference in size of the of the halide ions. Fluorine is one of three elements that can form hydogen bonds (as well as N and O). HF can both donate and recieve a hydrogen bond and the network this creates requires energy to break before the molecules themselves can be given enough kinetic energy to transfer into the gas phase. Hence this has the highest boiling point of the three. Bromine is a larger ion than chlorine and thus has stronger Van der Waals forces. Larger amounts of energy (a higher temperature) are required to break these interactions and so the boiling point of HBr is higher than HCl.

Answered by Thomas S. Chemistry tutor

42767 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Sort the following compounds in order of increasing boiling point and explain your reasoning: hydrogen, hydrogen fluoride and hydrogen bromide


What happens upon the addition of NaOH solution (OH- ions) to a pink solution of cobalt chloride? Include equation(s) in your answer.


State and explain the general trend in first ionization energy as you move across the period from left to right.


What factors affect the equilibrium position and in what way?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2024

Terms & Conditions|Privacy Policy
Cookie Preferences