2.3 Structure and bonding of carbon

Question 1

2.3.1 Diamond

Diamond

Answer 1

• 4 covalent bonds per carbon atom
• very strong covalent bonds - strong intermolecular forces
• high MP and BP - large amounts of energy needed to break bonds
• does not conduct electricity - no free electrons

Question 2

2.3.2 Graphite

Graphite

Answer 2

• 3 covalent bonds per carbon atom
• layers of hexagonal rings
• layers slide over each other (no bonds between layers) soft & slippery
• high MP to breaks bonds, strong intermolecular forces
• conducts electricity (has delocalised electrons per carbon atom)

Question 3

2.3.3 Graphene

Graphene

Answer 3

• one layer of graphite
• very strong, very light
• sheets of carbon atoms
• high MP, BP
• conducts electricity (has delocalised electrons)
• used to make composites

Question 4

2.3.3 Fullerenes

Fullerenes

Buckminsterfullerene and nanotubes

Answer 4

Buckminsterfullerene:
* weak intermolecular forces
* slippery
* low MP, BP

Nanotubes:
* cylindrical fullerenes
* high length to diameter ratio
* resistant to being stretched
* conducts electricity (delocalised electrons)
* useful for nanotechnology and electronics