Describe the differences in properties between diamond and graphite.

Diamond – The electrons are tightly bound between the atoms. Bonds are difficult to break as they are held firmly together hence diamond has a hard structure. Diamond does not have free electrons to carry the current therefore electricity cannot flow. It is an insulator. Graphite – The carbon atoms are arranged in layers. Not all the bonds between the atoms are strong. The electrons can move freely. Movement of electrons means that graphite is a conductor of electricity. Layers of atoms are not held together very strongly; the layers can slide over each other quite easily therefore is also a good lubricant. 

Answered by Jasmine G. Chemistry tutor

3114 Views

See similar Chemistry GCSE tutors

Related Chemistry GCSE answers

All answers ▸

Explain what an ionic bond is and how the charges and radii can affect the melting and boiling points of the ionic compounds


What is ionic bonding?


Explain the trends in electronegativity in the periodic table


Explain the process of fractional distillation of crude oil


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo
Cookie Preferences