Structure and bonding of carbon

Question 1

Diamond:

Answer 1

• each carbon is joined to 4 other carbons covalently
• very hard
• very high melting point
  -does not conduct electricity

Question 2

Graphite:

Answer 2

• each carbon is covalently bonded to 3 other carbons, forming layers of hexagonal rings
• layers can slide over each other due to no covalent bonds between the layers, but weak intermolecular forces. Meaning that graphite is soft and slippery
• one electron from each carbon atom is delocalised which makes it similar to metals
• can conduct electricity because the delocalised electrons can move

Question 3

Graphene:

Answer 3

• single layer of graphite
• has properties that make it useful in electronics and composites
• very strong because atoms within its layers are very tightly bonded
• elastic because the planes of atoms can flex relatively easily without the atoms breaking apart

Question 4

Fullerenes:

Answer 4

• molecules of carbon atoms with hollow shapes
• based on hexagonal rings of carbon atoms, but also may contain rings with 5 or 7 carbon atoms.
• first fullerene discovered was Buckminsterfullerene, which has a spherical shape

Question 5

Carbon nanotubes:

Answer 5

• cylinder fullerenes with very high length to diameter ratio
• properties make them useful for nanotechnology, electronics and materials
• can be used as lubricants, to deliver durgs in the body and catalysts
• can be used for reinforcing materials