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Assuming a perfect diamond with no impurities. Would this diamond considered to be a single large molecule? Browsing the interweb I found several opinions about this but did not find a clear Yes or No.

From what if gathered so far I'm pretty sure a diamond is a monocrystalline solid. Since all its parts are connected with covalent bonds I would assume that it should be considered a molecule even though it has no fixed number of atoms in its molecule formula.

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    $\begingroup$ "[...] even though it has no fixed number of atoms in its molecule formula" That exactly would be my argument against it. $\endgroup$ – Klaus-Dieter Warzecha Jan 26 '14 at 10:02
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Diamond is a covalent network solid, like a number of other common materials (quartz, graphite, glass, and a whole bunch of stuff).

Because they are not discrete molecules - there is no 'diamond' molecule the same way there are molecules of caffeine, benzoic acid, citric acid, N,N-dimethylaminopyridine, etc. - network solids form one of the two main classes of macromolecules, the other being polymers. You'll note that the Wikipedia article on macromolecules seems to imply that 'macromolecule' and 'polymer' are synonymous. They are not, at least not to those chemists working in the field.

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    $\begingroup$ The Wikipedia Article about network solids contains a key phrase: "In a network solid there are no individual molecules and the entire crystal may be considered a macromolecule." For me this means: Diamonds are macromolecules. Thanks! $\endgroup$ – Christoph Grimmer-Dietrich Jan 26 '14 at 12:01
  • $\begingroup$ @ChristophGrimmer-Dietrich Giant molecule is another term used often. $\endgroup$ – juanrga Feb 24 '18 at 4:20
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Single crystal diamond is literally a single molecule. Every carbon is covalently bonded to the whole. A modest level of impurities makes no difference. Consider epoxy. A well compounded, well measured, well mixed sample will crosslink into a single molecule with every atom bonded to the whole body. Ionic crystals are collections of interacting formula units.

Diamond, graphite, and buckeyballs are not organic compounds, for they are not compounds.

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    $\begingroup$ Buckyballs are discrete molecules and therefore, by any definition, molecules. Diamond and graphite are better called covalent network solids. $\endgroup$ – matt_black Mar 15 '17 at 23:55
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It isn't helpful to describe network solids as molecules, so we probably shouldn't

The problem here is that there in't a strict definition of molecule in chemistry. So we have to decide whether particular uses of the term are helpful or not.

We could argue that any entity where all the bonds are covalent is a "molecule". This would include diamond and polymers. But this is not helpful in practice. polymer scientists don't, for example, find it helpful to describe the components of a polymer as a molecule (they might use the more specific term macro-molecule). Most non-crosslinked polymers don't consist of single "molecules" but a mixture of many entities with different chain lengths. Talking about "molecules" isn't much use in describing or characterising the overall polymer. Many properties depend on the statistical distribution of chain length and thinking individually about each specific chain is unhelpful and irrelevant.

For many substances it is helpful to talk about the molecules making up the substance. Usually this is because the molecules that make up the substance are well defined. We can exactly describe the atomic makeup of each molecule making up the substance. Every molecule of aspirin is $$\ce{C9H8O4}$$ and no matter how much we have that describes the substance in a useful way. Where a substance is made up from more than one molecule, this is still true.

The problem with network solids is that there is no unique molecule. Every single crystal contains a different number of atoms; every diamond is different. So the idea of being able to describe the common feature of the substance as being the properties of the components (molecules) making it up goes out the window. It is better to call them network solids and think about the properties as a product of how the atomic components are connected. In mineralogy, for example, there are a lot of network solids. Silicate minerals, for example, can contain silica 3D networks (like diamond, in fact), flat silica sheets, linear silica chains and small silica units. Describing these components as "molecules" adds nothing useful; recognising the structures as components of a network is clearer and more useful.

In conclusion describing the components of network solids as "molecules" doesn't help so it isn't a useful use of the term.

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A diamond is not considered as a molecule because each carbon atom is covalently bonded with four other carbon atoms. This is what makes diamond a network solid. Since it's a whole network of covalently bonded atoms(carbons), diamond is not considered to be one molecule.

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