Graphite
Graphite has a giant covalent structure in which:
- each carbon atom forms three A covalent bond is formed by a shared pair of electrons. with other carbon atoms
- the carbon atoms form layers of hexagonal rings
- there are weak forces of attraction between the layers
- there is one, non-bonded – or delocalised – electron for each atom
Graphite’s properties include:
- high melting and boiling points. Graphite’s many covalent bonds are strong and substantial energy is needed to break them.
- good electrical conductivity. Each carbon atom has an unbonded electron. The unbonded electrons are delocalised electrons that are free to move and carry charge.
- softness. The weak forces between graphite’s layers allow them to slide.
Graphite is used as a Anything which reduces the friction between two surfaces. and in pencils.
The dotted lines represent the weak forces between the layers in graphite.
