1.3 Structure and bonding of carbon

Question 1

Diamond

Answer 1

• Forms giant covalent lattice/structure.
• Every carbon atom forms 4 covalent bonds with other carbon atoms.
• High MP (lots of energy required to overtake covalent bonds).
• Very hard (strong covalent bonds in giant covalent structure).
• Doesn’t conduct electricity (every atom is bonded so no delocalised electrons).

Question 2

Graphite

Answer 2

• Forms layers of hexagonal rings which have no covalent bonds between the layers.
• Weak intermolecular forces between layers.
• Each carbon atom forms 3 covalent bonds with 3 other carbon atoms.
• One electron from each carbon atom is delocalised.

Question 3

Graphene

Answer 3

• Single layer of graphite
• Conducts electricity
• Thin and and be bent
• Useful in electronics and composites.

Question 4

Silica

Answer 4

• Forms giant covalent lattice/structure.
• Like diamond but with silicon and oxygen instead of carbon.
• Useful in linings of furnaces.

Question 5

Fullerenes

Answer 5

• Hollow shapes of molecules made of carbon atoms.
• Based on hexagonal (or pent-/hep-) rings of carbon atoms.
• Carbon nanotubes are cylindrical fullerenes - have

Question 6

Buckminsterfullerene.

Answer 6

• First fullerene discovered.
• C₆₀
• Spherical shape.
• Useful for drug delivery, lubricant and catalyst.

Question 7

Carbon nanotubes.

Answer 7

• Cylindrical fullerenes
• Very high length to diameter ratio.
• Very high strength to weight ratio.
• Useful for nanotechnology, electronics and materials.