(40) GCSE Chemistry Revision "Graphite"

Graphite

A giant covalent molecule formed from carbon where each carbon atom forms covalent bonds to three other carbon atoms.

Covalent bonds in graphite

Carbon atoms in graphite form bonds to three other carbon atoms, creating hexagonal rings arranged in layers.

Properties of graphite

Graphite is soft, slippery, has a high melting and boiling point, and is a good conductor of electricity and heat.

Structure of graphite

Graphite consists of layers of hexagonal rings of carbon atoms with no covalent bonds between the layers, allowing them to slide over each other.

Delocalized electrons

Electrons in graphite that are not involved in covalent bonds and can move freely, allowing graphite to conduct electricity and heat.

Melting point of graphite

Graphite has a high melting and boiling point due to the strong covalent bonds that need to be broken.

Uses of graphite

Graphite is often used as a lubricant in machines to reduce friction between moving parts.

Comparison between graphite and metals

Both graphite and metals have delocalized electrons that can move, making them good conductors of heat and electricity, but graphite is not a metal.