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These forms exist due to the different allotropes having different arrangements and bonding patterns of carbon atoms. Carbon is capable of forming many allotropes due to its valency and its ability to bond with other carbon atoms to form endless chains and rings. The most well-known and common allotrope of carbon is graphite, which is composed of stacked layers of carbon atoms arranged in a hexagonal lattice. Graphite is known for its softness and ability to conduct electricity due to the delocalized electrons in its structure. Another well-known allotrope is diamond, which is the hardest known natural material. Diamond is made up of carbon atoms arranged in a tetrahedral lattice, making it extremely dense and stable. Fullerene molecules, also known as buckyballs, are another form of carbon allotrope. These molecules consist of spherical or cylindrical cages of carbon atoms. One of the most famous fullerene molecules is C60, also known as Buckminsterfullerene or the "buckyball," which consists of 60 carbon atoms arranged in a soccer ball-like shape. Carbon nanotubes are cylindrical structures made up of carbon atoms arranged in hexagonal lattice patterns. These nanotubes possess unique properties that make them useful in various applications, such as nanotechnology, electronics, and materials science. Other carbon allotropes include amorphous carbon, which lacks a defined crystal lattice and can be found in substances like coal and soot, as well as glassy carbon, which is a non-graphitizing, or non-crystalline, form of carbon. Overall, the different allotropes of carbon exhibit diverse physical and chemical properties, ranging from electrical conductivity to hardness, making carbon a versatile element with various applications in industries such as electronics, materials science, and nanotechnology.