Why does silicon dioxide have a higher melting point than sulphur?

Silicon dioxide (SiO2) has a macromolecular structure. This means that it forms thousands of covalent bonds between its silicon and oxygen subunits. Sulphur trioxide (SO3), meanwhile, has a simple covalent structure, with no other bonds between molecules. Where SiO2 has strong covalent bonds between molecules, SO3 only has weak van der waals intermolecular forces holding its molecules together. Since covalent bonds require more energy to overcome than van der waals, SiO2 requires a higher temperature than SO3 to melt, thus SiO2 has a higher melting point.

JL
Answered by Jacob L. Chemistry tutor

28724 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Can you explain acylation?


Explain why hydrogen bonding occurs between water molecules


How does free radical substitution work?


What is a chiral carbon and optical isomerism?


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

MyTutor is part of the IXL family of brands:

© 2025 by IXL Learning