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Topic 2a - Allotropes of Carbon (Graphite (Each carbon only forms three…
Topic 2a - Allotropes of Carbon
Diamond
Each carbon atom forms four covalent bonds with other carbon atoms
Very rigid structure
Very high melting and boiling point because the strong covalent bonds take a lot of energy to overcome
Doesn't conduct electricity because no free electrons or ions
Graphite
Each carbon only forms three covalent bonds
Creates sheets of carbon atoms arranged in hexagons
Aren't any covalent bonds between layers so only held together by weak intermolecular forces so they are free to move over each other
Makes graphite soft and slippery ideal as a lubricating material
High melting and boiling point because the covalent bonds need a lot of energy to break
Conducts electricity because of free electron
Graphene
Basically a single layer of graphite
Very strong and incredibly light so can be added to composite materials
Delocalised electrons so can conduct electricity
Fullerenes
Hollow molecules of carbon, shaped like tubes or balls
Mainly made up of carbon atoms arranged in hexagons, but can contain pentagons or heptagons
Buckminsterfullerene - C60
Nanotubes - good conductors of electricity and heat
Uses of fullerenes
In medicine - cage other molecules, could be used to deliver a drug safely
As catalysts - huge surface area to volume ratio
As lubricants
Strengthen materials - nanotubes have high tensile strength
In electronics - nanotubes can conduct electricity and very small