Allotropes Of Carbon

The different forms or allotropes of carbon (see below) include the hardest naturally occurring substance, diamond, and also one of the softest known substances, graphite. Moreover, it has an affinity for bonding with other small atoms, including other carbon atoms, and is capable of forming multiple stable covalent bonds with such atoms. As a result, carbon is known to form almost ten million different compounds; the large majority of all chemical compounds. Carbon also has the highest melting and sublimation point of all elements. At atmospheric pressure it has no melting point as its triple point is at 10.8 ± 0.2 MPa and 4600 ± 300 K, so it sublimates at about 3900 K
Carbon sublimes in a carbon arc which has a temperature of about 5800 K. Thus, irrespective of its allotropic form, carbon remains solid at higher temperatures than the highest melting point metals such as tungsten or rhenium. Although thermodynamically prone to oxidation, carbon resists oxidation more effectively than elements such as iron and copper that are weaker reducing agents at room temperature.
Carbon compounds form the basis of all known life on Earth, and the carbon-nitrogen cycle provides some of the energy produced by the Sun and other stars. Although it forms an extraordinary variety of compounds, most forms of carbon are comparatively unreactive under normal conditions. At standard temperature and pressure, it resists all but the strongest oxidizers. It does not react with sulfuric acid, hydrochloric acid, chlorine or any alkalis. At elevated temperatures carbon reacts with oxygen to form carbon oxides, and will reduce such metal oxides as iron oxide to the metal. This exothermic reaction is used in the iron and steel industry to control the carbon content of steel:
Fe3O4 + 4 C(s) → 3 Fe(s) + 4 CO(g)
with sulfur to form carbon disulfide and with steam in the coal-gas reaction:
C(s) + H2O(g) → CO(g) + H2(g).
Carbon combines with some metals at high temperatures to form metallic carbides, such as the iron carbide cementite in steel, and tungsten carbide, widely used as an abrasive and for making hard tips for cutting tools.
As of 2009, graphene appears to be the strongest material ever tested. However, the process of separating it from graphite will require some technological development before it is economical enough to be used in industrial processes.
The system of carbon allotropes spans a range of extremes:
Synthetic nanocrystalline diamond is the hardest material known.Graphite is one of the softest materials known.
Diamond is the ultimate abrasive.
Graphite is a very good lubricant.

Diamond is an excellent electrical insulator.
Graphite is a conductor of electricity.

Diamond is the best known naturally occurring thermal conductor
Some forms of graphite are used for thermal insulation (i.e. firebreaks and heat shields)

Diamond is highly transparent.Graphite is opaque.

Diamond crystallizes in the cubic system.
Graphite crystallizes in the hexagonal system.

Amorphous carbon is completely isotropic.
Carbon nanotubes are among the most anisotropic materials ever produced.

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[hguner1]

It's worth to see electrochromism in graphene:

?v=IcKSZM39F6c

[Peshookhan1]

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