Carbon allotropes

Graphene is a single layer of carbon atoms with unique properties, including high electrical conductivity and flexibility, making it ideal for flexible electronics and display screens.

Graphene is defined as a two-dimensional, single-layer sheet of carbon atoms arranged in a hexagonal (honeycomb) lattice structure.

Diamond is extremely hard because each carbon atom is covalently bonded to four other carbon atoms in a rigid, giant tetrahedral lattice structure, which requires significant energy to break.

In graphite, each carbon atom is bonded to three others, leaving one electron per atom delocalized. These free electrons are able to move throughout the structure and carry an electrical current.

Fullerenes are used in medicine for drug delivery, as lubricants, and as catalysts due to their cage-like structure. They are not used for manufacturing paper.

Graphite is used as a dry lubricant because its layers are held together by weak intermolecular forces, allowing them to slide over one another easily.

Graphene was first isolated in 2004 by Andre Geim and Konstantin Novoselov at the University of Manchester.

Fullerenes are molecules of carbon atoms with a hollow, spherical, or ellipsoidal shape, the most famous being Buckminsterfullerene (C60).

Graphite and diamond are giant covalent structures. To melt them, a massive amount of energy is required to break the many strong covalent bonds holding the atoms together.

Graphite is an allotrope of carbon, meaning it is composed entirely of carbon atoms arranged in a specific structure.