Carbon Allotropes Research Paper
Allotropes of carbon
Allotropes are different forms of an element in the same physical state. Examples of allotropes are i.e., the allotropes of carbon. They include; Diamond, where carbon atoms are found in a tetrahedral lattice arrangement. Graphite, where the carbon atoms are bonded together in sheets of a hexagonal lattice. Graphene, single sheets of graphite and Fullerene, where the carbon atoms are bonded together in a spherical cage. Different bonding within the structures gives rise to distinct forms with different properties.
Structure of carbon allotropes
Graphite Diamond Fullerene Graphene GRAPHITE: Each atom of carbon is sp2 hybridized oriented at 120 degrees, and is therefore covalently bonded 3 other carbon atoms forming hexagons in parallel layers. The weakest form of intermolecular forces, London Dispersion Forces, holds the layers together. This allows them to slide over each other.
DIAMOND:
Each carbon atom is sp3 hybridized producing four equal orbitals oriented at 109.5 degrees.
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Its hardness makes it suitable for tools for purposes such as cutting glass.
FULLERENE
Fullerene is used for binding specific molecules as well as it is a good catalyst.
GRAPHENE
Graphene is used in transmission electron microscopy (TEM), touch screens and high performance electronic devices. Extensive research is being done on use of graphene.
Structures of silicon and silicon dioxide
Silicon
Like carbon, whom allotropes are described in the last section, silicon is also found in group 14 of the periodic table. It therefore has four valence electrons. In its elemental state, each silicon atom is bonded to others covalently in a tetrahedral shape. As it is tetrahedrally arranged and has 3 charge centers it is sp3 hybridized. This results in silicon forming giant lattice structures that can be similar to diamond’s arrangement. This is shown in the picture below.
Silicon
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