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Allotropes of Carbon (GRAPHITE (Special Properties (soft and slippery due…
Allotropes of Carbon
GRAPHITE
Structure
each C atom is Sp2 hybridized and covalently bonded to 3 others, forming hexagons in parallel layers with bond angles of 120. The layers are held only by weak, London dispersion forces so they can slide over each other
Electrical conductivity
Good electrical conductor; contains one non-bonded, delocalized electron per atom that gives electron mobility
Thermal Conductivity
not a good conductor, unless the heat can be forced to conduct in a direction parallel to the crystal layers
Appearance
Non-lustrous, grey crystalline solid
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DIAMOND
Structure
Each C atom is Sp3 hybridized and covalently bonded to 4 others tetrahedrally arranged in a regular repetitive pattern with bond angles of 109.5
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Thermal Conductivity
Very efficient thermal conductor, better than metals
Appearance
highly transparent, lustrous crystal
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FULLERENE C60
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Structure
Each C atom is Sp2 hybridized and bonded in a sphere of 60 carbon atoms, consisting of 12 pentagons and 20 hexagons. Structure is a closed spherical cage in which each carbon is bonded to 3 others. (it is not a giant molecule as it has a fixed formula)
Electrical Conductivity
A semiconductor at normal temperature and pressure due to some electron mobility; easily accepts electrons to form negative ions
Appearance
yellow crystalline solid, soluble in benzene
Uses
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related forms are used to make nanotubes and nanobuds used as capacitors in electronics industry and catalyst
GRAPHENE
Structure
Each C atom is covalently bonded to 3 others, as in graphite, forming hexagons with bond angles of 120. But it is a single layer, so exists as a two-dimensional material only. It is often described as a honeycomb or chicken wire structure
Electrical Conductivity
very good electrical conductor; one delocalized electron per atom gives electron mobility across the layers
Thermal Conductivity
best thermal conductivity known, even better than diamond
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