Can someone give me three points why Graphite can conduct electricity but Diamond can't?

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I've already got that graphite has a sea of delocalised electrons.

Please could anyone tell me the other two

Thanks :)

Posted Sun 4th November, 2012 @ 14:40 by :) PurpleJaguar (: - Team GR

7 Answers

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I think it's because it's in layers too so the electrons can travel throughout. 

Answered Sun 4th November, 2012 @ 14:46 by Joanne
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Thanks Joanne :)

I need only one more point now :P

Answered Sun 4th November, 2012 @ 14:51 by :) PurpleJaguar (: - Team GR
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Its not so much a sea of delocalised electrons as the outer electrons of graphite are delocalised and can carry a charge between planes

Answered Sun 4th November, 2012 @ 15:22 by cameron colluney
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Okay Thanks :)

we were taught that metals have a sea of delocalised electrons :S ...

Answered Sun 4th November, 2012 @ 15:25 by :) PurpleJaguar (: - Team GR
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Graphite is not a metal it is a convalent compound that is an alatrope of carbon (consists of only carbon with a diffrent structure)

Answered Sun 4th November, 2012 @ 15:49 by cameron colluney
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Graphite's carbon atoms only forms 3 bonds (that's why there are free electrons), whereas diamond's carbon atoms form 4 bonds, which is why it cannot conduct electricity.

Answered Sun 4th November, 2012 @ 16:10 by Former Member
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Diamond and Graphite are the allotropes of carbon

The valency of carbon is 4

In diamond each carbon atom is bonded to four other carbon atoms at the sides of a tetrahedron in a 3d shape satisfying all the 4 valencies.

In Graphite each carbon atom is bonded to 3 other carbon atom in hexagonal planar structure leaving a free electron. 

Thus due to the flow of this free electron graphite is a good conductor of electricity

Answered Thu 15th November, 2012 @ 06:27 by dhairya