Examples of diamond in the following topics:
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- Diamond is probably the most well known carbon allotrope.
- Each carbon atom in a diamond is covalently bonded to four other carbons in a tetrahedron.
- As a result, diamond exhibits the highest hardness and thermal conductivity of any bulk material.
- Diamonds do not generally react with any chemical reagents, including strong acids and bases.
- Uses of diamond include cutting, drilling, and grinding; jewelry; and in the semi-conductor industry.
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- Diamond is also an allotrope of carbon.
- Diamond cannot be melted; above 1700 °C it is converted to graphite, the more stable form of carbon.
- The diamond unit cell is face-centered cubic and contains eight carbon atoms.
- Its structure is very much like that of diamond, with every other carbon replaced by silicon.
- Cubic boron nitride is the second-hardest material, after diamond.
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- Interestingly, carbon allotropes span a wide range of physical properties: diamond is the hardest naturally occurring substance, and graphite is one of the softest known substances.
- Diamond is transparent, the ultimate abrasive, and can be an electrical insulator and thermal conductor.
- Allotropes of carbon are not limited to diamond and graphite, but also include buckyballs (fullerenes), amorphous carbon, glassy carbon, carbon nanofoam, nanotubes, and others.
- Some allotropes of carbon: a) diamond, b) graphite, c) lonsdaleite, d–f) fullerenes (C60, C540, C70); g) amorphous carbon, h) carbon nanotube.
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- Turning graphite into diamond requires extremely high temperatures and pressures, and therefore is impractical in a laboratory setting.
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- Although both diamond and graphite are types of carbon, their entropies differ significantly.
- Graphite, which is built up of loosely-bound stacks of hexagonal sheets, soaks up thermal energy twice as well as diamond.
- The carbon atoms in diamond are tightly locked in a three-dimensional lattice, preventing them from vibrating around their equilibrium positions.
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- Another well-characterized carbon allotrope is diamond.
- Diamond is an extended array of sp3 hybridized carbon atoms; whereas, graphite consists of overlapping sheets of sp2 hybridized carbon atoms arranged in a hexagonal pattern.
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- Two experimental studies have proposed the existence of diamond-like and graphite-like B2O, as for boron nitride and carbon solids.
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- Some examples include sodium chloride, ice, metals, and diamonds.
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- How can soot and diamond be so different in appearance yet so chemically similar?
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- For example, pure carbon can exist as diamond, which has a very high melting point, or as graphite, whose melting point is still high but much lower than that of diamond.