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Given that both diamond and graphene are both just carbon, what's the difference between the two approaches?
by DasIch 10y ago
Given that both diamond and graphene are both just carbon, what's the difference between the two approaches?
- gilleain 10y agoWhat does sharing a common element have to do with anything? They are allotropes (https://en.wikipedia.org/wiki/Allotropes_of_carbon https://en.wikipedia.org/wiki/Allotropes_of_carbon) - diamond, graphite, fullerenes, SWNT, etc all have very different properties.
- DasIch 10y agoWell, I'm not a chemist or anything but I, maybe naively, thought that the properties would be similiar. More similar to each other than to silicon anyway. I mean it's similiarity that makes you think of carbon as an alternative to silicon rather than some other element, no?
- marcosdumay 10y agoThey have a similar resistance from electromigration, but nothing more. The atoms configuration dictate everything in organic chemistry. (And in inorganic too, but you rarely have alternative configurations there.)
- scentoni 10y agoDiamond's electronic and optical properties are far more similar to those of silicon than they are to graphite, graphene, or other forms of carbon. Diamond and silicon are diamond cubic lattices with sp3 hybridization (tetrahedral), graphite and related planar allotropes have sp2 hybridization (triangular).
- arxpoetica 10y agoThe article also mentions graphene. Carbon in different forms has different properties, so, in theory there could be something valuable about using synthetic diamond.