Diamond, graphite and fullerenes (substances that include nanotubes and 'buckyballs' , such as buckminsterfullerene) are three allotropes of pure carbon. In all three allotropes, the carbon atoms are joined by strong covalent bonds, but in such different arrangements that the properties of the allotropes are very different.
Because of their distinctive structural makeup, graphite and diamond are distinct materials. Both have extremely high melting points due to their giant covalent structures. Diamond is incredibly strong and hard due to the four covalent links that each carbon atom in the mineral has with other carbon atoms. However, because each carbon in graphite is connected to three other carbons, it forms in layers.
Even though graphite is used to make pencils, despite the fact that each carbon atom only has three bonds, the layers are actually highly strong and have delocalized "free" electrons between them. Graphite appears soft because these electrons act as a lubricant between layers, allowing them to slide over one another. Graphite conducts electricity due to the free electrons. Diamond does not carry electricity because it lacks these free electrons.
There are more than three allotropes of carbon. These include diamond, graphite, graphene, carbon nanotubes, fullerenes, and carbon nanobuds.
Diamond
In a three-dimensional array, four additional carbon atoms are covalently attached to each carbon atom in a diamond. In essence, a diamond is one enormous molecule.
Graphite
The carbon atoms in graphite are bonded together in sheets of connected hexagons that resemble chicken wire. In essence, each sheet is a single molecule.
Each carbon atom in a sheet establishes solid covalent bonds with three other carbon atoms. The only forces keeping the sheets packed together are the modest intramolecular forces.
Graphene
In the form of a single sheet of graphite that is only one atom thick, graphene is made up entirely of carbon.
Nanocarbon tubes
Graphene sheet wrapped into a cylindrical tube of carbon atoms is how a carbon nanotube looks. Each atom connected to three other atoms, and the tube is one atom thick.
C60 and buckminsterfullerene
A single sheet of carbon atoms that has been folded into a spherical is what makes up buckminsterfullerene. Three additional atoms are connected to each carbon atom. With a carbon atom at each of the 20 hexagonal and 12 pentagonal corners, sixty carbon atoms are arranged in the shape of a ball.
There are numerous other known carbon balls, such as C70, C76, C84, and C540. They are collectively referred to as "buckyballs" or "fullerenes" and have varying amounts of pentagons and hexagons.
Nanocarbon buds
An allotrope of carbon called carbon nanobuds has fullerene-like "buds" that are covalently bonded to the sidewalls of carbon nanotubes.
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