Giant Covalent Structures

Question 1

Explain why graphite conducts electricity.

Answer 1

Has 3 covalent bonds

One delocalised electron

Can carry charge

Moves through structure

Question 2

Why is graphite soft?

Answer 2

There are no covalent bonds between layers of atoms

Question 3

Explain why graphite is good electrical conductor and is soft and slippery

Answer 3

Graphite 3 carbon atoms
Through covalent bonding
Has delocalised electrons
Electron carry charge and conduct electricity

Arranged in layers
Layers slide over each other
Due to weak intermolecular forces

Question 4

Explain why diamond has a high melting point.

Answer 4

Strong covalent bonds

Requires high amounts of energy

To break bonds

Question 5

Suggest one property fullerenes useful in nanotechnology

Answer 5

Conducts electricity

Question 6

Compare silicon dioxide, co2 and graphite (structure and bonding)

Answer 6

All non metals
All covalent bonds

Silicon dioxide and graphite are giant covalent whereas c02 is simple covalent

Silicon dioxide is lattice structure whereas graphite arranged in layers with weak intermolecular forces

Graphite has delocalised electrons