In terms of structure and bonding explain why the boiling point of magnesium is much higher than that of bromine?

Bromine is molecular, existing as Br2 molecules, wheras magnesium is metallic and therefore exists in a large macromolecular structure. In bromine there are strong INTERmolecular covalent bonds, but only weak INTRAmolecular Van der Waals forces. It is these weak INTRAmolecular forces that must be overcome for bromine to boil. Magnesium exists as a large macromolecular structure (ie.a large interconnected lattice NOT molecules) with strong metallic bonds between the Magnesium ions and the sea of delocalised electrons. In orser for magnesium to boil these strong metallic bonds must be broken. It takes more energy (in the form of heat) to overcome the stronger metallic bonds in magnesium than the weaker INTRAmolecular Van der Waals forces in bromine, therefore magnesium has a higher boiling point than bromine.

Answered by Edwina B. Chemistry tutor

24469 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Explain why the ionisation energies tend to increase across a period


State and explain the trend in boiling points of chlorine, bromine, and iodine


Why is cyclohexene able to react with bromine water, but Benzene isn't


Give the IUPAC name of CH3CH2CH2CH2CH(OH)CN


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