Diamond vs. Graphite


by arabianchick
Tags: diamond, graphite
arabianchick
arabianchick is offline
#1
May24-08, 10:45 PM
P: 2
Why is diamond a poor conductor of an electric current and graphite a good conductor?

all i can come up with is that diamond is a good insulator and that the fundamental difference between graphite and diamond being that graphite molecules are flat groupings of carbon atoms while diamond molecules are tetrahedral (pyramid-shaped) groupings of carbon atoms.

can someone tell me if this is anywhere close? and help me on a bit..
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Kushal
Kushal is offline
#2
May25-08, 02:14 AM
P: 440
look carefully at the structure of both diamond and graphite. find out how many covalent bonds are there for each carbon atom in both diamond and graphite.

what can you deduce?
The_ArtofScience
The_ArtofScience is offline
#3
May26-08, 03:30 PM
P: 83
hint: delocalized pi bonds

EvilSpanner
EvilSpanner is offline
#4
Feb10-10, 02:41 PM
P: 1

Diamond vs. Graphite


Quote Quote by arabianchick View Post
Why is diamond a poor conductor of an electric current and graphite a good conductor?

all i can come up with is that diamond is a good insulator and that the fundamental difference between graphite and diamond being that graphite molecules are flat groupings of carbon atoms while diamond molecules are tetrahedral (pyramid-shaped) groupings of carbon atoms.

can someone tell me if this is anywhere close? and help me on a bit..
Graphite and diamond are both made from carbon, which has 4 electrons in it's outer shell. Diamond has four bonds, meaning there are no free electrons. Graphite has three bonds giving it a free electron which alows the current of electricity to flow. Hope this helps.


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