Carbon structures

Question 1

Covalent bonds (diamond)

Answer 1

Each carbon atom in diamond is bonded to four other carbon atoms by strong covalent bonds.

This creates a giant covalent structure.

Question 2

hard ( diamond)

Answer 2

There are lots of strong covalent bonds in diamond. This makes it very hard.

Question 3

conduct electricity (diamond)

Answer 3

Diamond does NOT conduct electricity because there are no delocalised electrons in the diamond structure.

Question 4

High melting point (diamond)

Answer 4

A lot of energy is needed to break strong covalent bonds.

Diamond has lots of strong covalent bonds. This means that it has a high melting point.

Question 5

thermal conductivity (diamond)

Answer 5

Diamond has a very rigid structure.

This means that vibrations can easily carry heat throughout the structure.

Diamond is an excellent thermal conductor.

Question 6

Covalent bonds (graphite)

Answer 6

Each carbon atom in graphite is bonded to 3 other carbon atoms by strong covalent bonds.

This creates a giant covalent structure

Question 7

Strong covalent bonds (graphite)

Answer 7

Due to the strong covalent bonds within the sheets, graphite:
Has a high melting point.
Is insoluble in solvents.

Question 8

Soft (graphite)

Answer 8

The carbon atoms form layers of hexagonal (6-sided) rings, with each layer held together by weak intermolecular forces.

The layers can slide over one another easily, so graphite is very soft.

This makes it useful as a lubricant and as pencil ‘lead

Question 9

Conducts electricity (graphite)

Answer 9

Each carbon atom forms 3 covalent bonds.

1 electron from every carbon atom in graphite is delocalised.

This electron can move freely, so graphite can conduct electricity.