2006-12-04 03:58:55 · 9 answers · asked by sadiq h 1 in Science & Mathematics ➔ Chemistry
The carbon atoms in diamond form a tetrahedrally-bonded cubic crystal structure, which is extremely uniform and stable. Those of graphite are hexagonally-bonded in a planar structure. The planar structures themselves are strong and extremely stable, but the forces between the planes are the much weaker van der Waal forces. That's why the planes slip against each other so freely. See the references for diagrams and their respective properties.
2006-12-04 04:11:32 · answer #1 · answered by Frank N 7 · 0⤊ 0⤋
Their structure is different. In diamond, the carbon atoms are bonded covalently to each other. Each carbon atom is bonded to FOUR other carbon atoms in a tetrahedral structure. On the other hand, though in graphite the carbon atoms are also bonded covalently, each carbon atom is only bonded to THREE other carbon atoms in a network of hexagons, and one valence electron is not used in forming bonds.
This also explains why graphite can conduct electricity while diamonds cannot (2nd diff), as this unbonded electrons can move along the layers of hexagons and conduct electricity.
3rd diff. Diamond is abrasive while graphite is slippery. As u know from above their structure, its really very compact and the atoms are bonded strongly to each other. So a large amount of energy is needed to break these bonds. However, in graphite, the layers are held together by weak van der Waal's forces, hence they are easily broken.
Hope this helps=)
2006-12-04 12:08:19 · answer #2 · answered by luv_phy 3 · 0⤊ 0⤋
Graphite consists of layers of graphene which are carbon atoms arranged in a hexagonal lattice (i.e. each atom is covalently (strongly) bound to 3 other atoms). The layers are bound together more weakly than the bonds within each layer. The graphene layers actually "slide" around on each other. This is why graphite is used as a lubricant.
Diamond is a compound in which each each carbon atom is strongly bound to 4 other carbon atoms. It is not a 2D structure like graphene.
2006-12-04 12:06:20 · answer #3 · answered by csferrie 2 · 0⤊ 0⤋
The arrangement of the atoms. In graphite, they are in sheets, diamond is a matrix.
2006-12-04 12:01:39 · answer #4 · answered by Anonymous · 0⤊ 0⤋
the configuration of the carbon bonds. diamond is more rigid while graphite is layered in sheets
2006-12-04 12:01:36 · answer #5 · answered by shiara_blade 6 · 0⤊ 0⤋
Nothing. By the way, I have a graphite ring for sale if youre interested....
2006-12-04 12:00:26 · answer #6 · answered by Anonymous · 0⤊ 1⤋
#2 Graphite will answer questions on a scan-tron test.
A diamond will encourage her to say yes.
2006-12-04 12:03:27 · answer #7 · answered by 110% 2 · 0⤊ 0⤋
both are molecular network solids, just in different arrangements.
diamond is a 3D network, starting from one carbon atom and branching out in all directions like a sphere.
graphite exists in layers and sheets which are just bound to each other with weak bonds, therefore you can rub it off onto other surfaces easily (a pencil)
2006-12-04 12:05:25 · answer #8 · answered by recneps 2 · 0⤊ 0⤋
About 1,000,000 lbs of pressure over a very long time.
2006-12-04 12:07:11 · answer #9 · answered by Anonymous · 0⤊ 0⤋