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

17168 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Describe a simple way to distinguish between aqueous solutions of potassium nitrate (KNO3) and potassium sulfate (K2SO4) using one test tube reaction


When propanal is reacted with potassium cyanide under weakly acidic conditions the resulting mixture does not rotate plane polarised light. Explain this observation.


What is the difference between 'Electrospray Ionisation' and 'Electron Impact' during the ionisation stage in a mass spectrometer?


Name and explain briefly the main stages of mass spectroscopy.


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