What happens at the edge of a diamond?
In a diamond, there is a regular 3D lattice of carbon atoms, right? In graphite, the atoms are arranged in rings. So far so good. At the edge of a piece of graphite, you just have one last ring. At the edge of a diamond, what do the last atoms of carbon bond to? Each other? Oxygen? What ever it is, it's this compound (not diamond) that is used for etching, cutting glass etc, 'cos it's on the outside edge. So do diamonds have a harder-than-diamond coating?
Answers:
there are different types of diamonds that have different compositions, but generally, the usual suspects will be on the surface-carbonyl, hydroxyl, and hydrogen groups
ok. if you say so
No. same strength all way through. Held by covalent bonds.
Etching is done by property of the geometry (modulus) not strength. Diamonds do go 'blunt' after constant usage.
The only explanation I can imagine would be that they are unbonded carbon atoms.
Great question.
For the most part they are hydrogenated (C-H), though there is some chance of oxidation to produce hydroxyl groups(C-OH). I think carbonyl groups (C=O) are highly unlikely, nay impossible, as this requires sp2 hybridised carbon centres which form trigonal planar bond angles. Diamond is made of purely sp3 carbons. Any sp2 carbons would disrupt the tetrahedral lattice structure of he sp3 carbons.
Diamonds are PURE carbon. every carbon atom is bonded to four other carbons, no hydrogens, no oxygens.
Any diamond formed on earth is not "pure" carbon and will have some impurities. In addition - the edge bonds have to find something to bond to and will usually attach to hydrogen. It's not really a coating but is part of what we call "a diamond" (no stronger than the rest - and diamonds do wear down). "Pure" carbon can not form diamond (or graphite, which is the second form of carbon) and is believed to form "bucky balls" of 60 or more carbon atoms with no other elements.
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Answers:
there are different types of diamonds that have different compositions, but generally, the usual suspects will be on the surface-carbonyl, hydroxyl, and hydrogen groups
ok. if you say so
No. same strength all way through. Held by covalent bonds.
Etching is done by property of the geometry (modulus) not strength. Diamonds do go 'blunt' after constant usage.
The only explanation I can imagine would be that they are unbonded carbon atoms.
Great question.
For the most part they are hydrogenated (C-H), though there is some chance of oxidation to produce hydroxyl groups(C-OH). I think carbonyl groups (C=O) are highly unlikely, nay impossible, as this requires sp2 hybridised carbon centres which form trigonal planar bond angles. Diamond is made of purely sp3 carbons. Any sp2 carbons would disrupt the tetrahedral lattice structure of he sp3 carbons.
Diamonds are PURE carbon. every carbon atom is bonded to four other carbons, no hydrogens, no oxygens.
Any diamond formed on earth is not "pure" carbon and will have some impurities. In addition - the edge bonds have to find something to bond to and will usually attach to hydrogen. It's not really a coating but is part of what we call "a diamond" (no stronger than the rest - and diamonds do wear down). "Pure" carbon can not form diamond (or graphite, which is the second form of carbon) and is believed to form "bucky balls" of 60 or more carbon atoms with no other elements.
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