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. 

JG
Answered by Jasmine G. Chemistry tutor

4105 Views

See similar Chemistry GCSE tutors

Related Chemistry GCSE answers

All answers ▸

Describe and explain the reactivity of group 1 metals


Explain why chlorine is more reactive than iodine.


25 cm^3 of a solution of known 0.2M HCl is neutralised by titration by 21.5cm^3 of NaOH solution. Calculate then concentration of the NaOH solution to 3dp.


Magnesium oxide contains magnesium ions (Mg2+) and oxide ions (O2–). Describe what happens when magnesium atoms react with oxygen atoms to produce magnesium oxide.


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