2 3 structure and bonding of carbon

Diamond does not conduct electricity because all of the outer shell electrons are held in the covalent bonds, and there are no freely moving delocalised electrons to carry the current.

Properties of diamond include:

Diamond is hard because each carbon atom is bonded to four other carbon atoms via strong covalent bonds.

Covalent bonds occur between the carbon atoms in diamond.

Each carbon atom forms four bonds.

False. Graphite is used in pencils, as an industrial lubricant, in inert electrodes, and in locks. Diamond is used in cutting tools.

In graphite:

False. Diamond is harder than graphite.

Properties of graphite include:

Graphite conducts electricity because it has delocalised electrons that can move and carry a charge throughout the structure.

Graphite is soft because there are weak intermolecular forces betwen the layers, which allows the layers to slide over each other.

Graphite suitable to be used as electrodes in an electrolytic cell because it conducts electricity, is inert and has a high melting point.

In graphite each carbon atom forms three bonds.

False. Graphene is essentially a 2D molecule since it is only one atom thick.

Four properties of graphene are:

Graphene is an excellent conductor of electricity because it has delocalised electrons which can move and carry a charge.

Fullerenes are molecules of carbon atoms with hollow shapes.

Carbon nanotubes are a type of fullerene produced by rolling graphene into a cylinder.

Two properties of carbon nanotubes are:

Since fullerenes are hollow they can be used to trap drug molecules and deliver them where needed.

Carbon nanotubes can conduct electricity because there are delocalised electrons which are free to move and carry a charge.

The formula of buckminsterfullerene is C60.

Graphene can be useful in electronics and composites.