2.3 Structure and Bonding of Carbon
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What are the properties of diamond and why?
Very hard Very high melting point Does not conduct electricity Each carbon atom is joined to 4 other carbon atoms, using up all of its bonds, so there are very strong forces of attraction Because all of the electrons are used up, there are no delocalised electrons to carry electrical charge
Draw out the structure of diamond
What are the properties of graphite?
Each carbon is bonded to 3 other carbons Forms hexagonal rings No covalent bonds between layers Conducts electricity
Why is graphite soft?
Each carbon has 3 bonds No bonds between layers Only weak intermolecular forces, this means layers can easily slide over each other
Why can graphite conduct electricity?
Only uses 3 of the 4 delocalised electrons for bonds Therefore each carbon atom has a delocalised electron which is able to conduct
What is graphene?
Single layer of graphite
What are the properties of graphene?
Very strong because atoms are tightly bonded Elastic, because planes of atoms can flex easily without breaking atoms apart
What is a fullerene?
Molecules of carbon atoms with hollow shapes Based on hexagonal rings, but can have 5 or 7 carbon atoms
What was the first fullerene discovered?
Buckminsterfullerene (C60)
What is a carbon nanotube?
Cylindrical fullerenes with very high length to diameter ratios
What are carbon nanotbues used for?
Lubricants - to deliver drugs in the body and catalysyts Reinforcing materials e.g. tennis rackets Electronics