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

17140 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

How would you expect the H-NMR spectrum of ethanol to differ from the H-NMR spectrum of ethane?


How do mass spectrometers work?


Giving the electronic configurations for each element, predict the trend in 1st ionisation energies going across period 2 from Lithium to Neon.


How do double bonds form?


We're here to help

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

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences