Explain the unusually high boiling point of HF

  • Due to the high electronegativity of flourine hydrogen bonds can be formed between HF molecules. - Hydrogen bonds require more energy to break that London Forces. - The other halogens are not as electronegative and so other hydrogen halides cannot form hydrogen bonds between molecules. Only London Forces are formed. - Therefore more energy is required to break the intermolecular forces in HF than the other hydrogen halides and so it has a higher boiling point. 
Answered by Chloe G. Chemistry tutor

27895 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

State and explain the trend in melting points of diamond, iodine and hydrogen fluoride.


Balance the following redox equation: PbO2 + SO32- ==> Pb2+ + SO42-


How do you form a Born-Haber cycle?


Explain why Br2 has a higher melting point than Cl2


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 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences