Explain why Silicon Dioxide has a higher melting point than Sulfur Trioxide.

Silicon Dioxide has a macromolecular/giant covalent structure which means it has covalent bonds between all atoms in its structure. Sulfur Trioxide has a simple molecular structure meaning it has Van der Waals forces between molecules.
Covalent bonds are much stronger than Van der Waals forces and so require much more energy to overcome, and this leads to the higher melting point observed in silicon dioxide as melting requires the overcoming of forces between atoms/molecules.

HT
Answered by Holly T. Chemistry tutor

16512 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Write a balanced equation for the reaction between NaOH and sulfuric acid. A conical flask contains 25cm^3 of 0.124M NaOH, a burette contains 0.0625M sulfuric acid. Find the minimum amount of acid required to completely react with the NaOH in the flask.


How does radiocarbon dating work?


What is a disproportionation reaction?


Describe chemical test/s you could use to determine the identity of a carbonyl compound.


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