A different structural form of an element, e.g. graphite and diamond are allotropes of carbon.

An allotrope of carbon consisting of a sheet that is one-atom-thick. Each atom is covalently bonded to three others arranged in hexagonal rings.

A molecular allotrope of carbon. Each atom is covalently bonded to three others, forming nanoparticles with hollow spheres or tubes.

A spherical fullerene composed of 60 carbon atoms (held together by covalent bonds). It is a very stable structure.

A cylindrical fullerene, essentially a tube of graphene. A nanoparticle known for its strength and electrical conductivity.

Graphene and fullerenes

Chemistry

In the Organic chemistry unit, pupils will learn more about hydrocarbons and learning about other homologous series, along with their reactions.

In the Structure and bonding unit, pupils learned about metallic, ionic and covalent bonding and about giant ionic structures, as well as the structure of covalent molecules, beginning to form links to properties

Chemistry of carbon

Which property is **not** associated with graphene?

spherical fullerene composed of 60 carbon atoms

cylindrical fullerene known for its strength and conductivity

molecular allotrope of carbon forming nanoparticles with hollow shapes

Match the following terms with their correct descriptions.

All carbon allotropes are giant covalent substances.

Arrange the following carbon allotropes in order of their tensile strength, from weakest to strongest.

A Buckminsterfullerene is a spherical fullerene of {{}} carbon atoms.

a different physical form in which an element can exist

a compound formed from two or more elements

What does the term 'allotrope' mean in chemistry?

Match the carbon allotrope to its primary use.

Each atom forms four single bonds with other atoms.

Each atom forms double bonds with three other atoms.

Each atom forms three single bonds with other atoms and has one free electron.

Each carbon atom is bonded to four other atoms in a layered hexagonal structure.

Which statement correctly describes the bonding in graphite?

Graphite is used as a lubricant because it is ...

each carbon atom donates multiple electrons to a 'sea of electrons'

one electron from each carbon atom is delocalised across the structure

Graphite exists as a layered structure of hexagonal rings of carbon atoms, each bonded to three other atoms. Between the layers there are weak {{}} holding them together. 

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