Explain alltrops of carbon
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When an element exists in more than one crystalline form, those forms are called allotropes; the two most common allotropes of carbon are diamond and graphite. The distance between carbon atoms along the bond is 1.54 × 10−8 cm, and this is called the single-bond length.
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- Diamond: It is extremely hard, transparent crystal, with the carbon atoms arranged in a tetrahedral lattice. This allotrope of carbon is a poor electrical conductor and an excellent thermal conductor.
- Lonsdaleite: These are also called hexagonal diamond.
- Graphene: It is the basic structural element of other allotropes, nanotubes, charcoal, and fullerenes.
- Q-carbon: These carbon allotropes are ferromagnetic, tough, and brilliant crystal structure that is harder and brighter than diamonds.
- Graphite: It is a soft, black, flaky solid, a moderate electrical conductor. The C atoms are bonded in flat hexagonal lattices (graphene), which are then layered in sheets.
- Linear acetylenic carbon (Carbyne)
- Amorphous carbon
- Fullerenes, including Buckminsterfullerene, also known as “buckyballs”, such as C60.
- Carbon nanotubes: Allotropes of carbon with a cylindrical nanostructure.
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