2.3 Structure and Bonding of Carbon Flashcards
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
