carbon allotropes

Question 1

name 3 carbon allotropes

Answer 1

diamond, graphite, graphene

Question 2

Diamond is a giant covalent structure in where?

Answer 2

each carbon atom is joined to four other carbon atoms by strong covalent bonds

the carbon atoms form a regular tetrahedral network structure

there are no free electrons

Question 3

name property’s of diamond

Answer 3

diamond is very hard

diamond has a very high melting point

diamond does not conduct electricity because it has no free electrons

Question 4

Graphite has a giant covalent structure in which

Answer 4

each carbon atom forms three covalent bonds with other carbon atoms

the carbon atoms form layers of hexagonal rings

there are no covalent bonds between the layers

there is one non-bonded - or delocalised - electron from each atom

Question 5

what does delocalised mean

Answer 5

Electrons that are not associated with a particular atom, eg in a metal, outer electrons can be free to move through the solid

Question 6

what are the property’s of Graphite

Answer 6

graphite can conduct electricity This makes graphite useful for electrodes in batteries and for electrolysis.

The forces between the layers in graphite are weak. This means that the layers can slide over each other. This makes graphite slippery, so it is useful as a lubricant.

Question 7

Explain why diamond does not conduct electricity and why graphite does conduct electricity.

Answer 7

Diamond does not conduct electricity because it has no charged particles that are free to move. Graphite does conduct electricity because it has delocalised electrons which move between the layers.

Question 8

name uses of graphite

Answer 8

lubricant

batteries

electrolysis

Question 9

name uses of diamond

Answer 9

This makes it useful for cutting tools, such as diamond-tipped glass cutters and oil rig drills.