Describe the structure and properties of graphite

Graphite is made from layers of carbon which contain many 6-membered carbon rings (hexagonal). Each layer is held together by each carbon being covalently bonded to 3 other carbon atoms and this leaves a delocalised electron to move freely through the structure. Between layers are weak intermolecular forces which allows sliding of the layers on top of each other and so graphite is very slippery and used as a lubricant. The delocalisation of the electron in the layers also means that it is a good conductor of electricity as the free electrons can carry a charge.

LS
Answered by Lucy S. Chemistry tutor

5521 Views

See similar Chemistry GCSE tutors

Related Chemistry GCSE answers

All answers ▸

A student needs 0.2 moles of hydrochloric acid to conduct a reaction. How many milliliters of a 0.5 M HCl solution does the student need?


Explain why chlorine (Cl2) is a gas at room temperature, but sodium chloride (NaCl) is a solid at room temperature.


Graphite and diamond are both made from carbon atoms. Why can graphite conduct electricity while diamond cannot?


Describe and explain the changes between sulphuric acid with copper carbonate, connected to a test tube with limewater.


We're here to help

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

MyTutor is part of the IXL family of brands:

© 2025 by IXL Learning