Allotropes of carbon

Question 1

Explain why graphite is a good electrical conductor

Answer 1

has delocalised electrons
(so electrons) can move through the structure

Question 2

Explain why graphite is soft and slippery

Answer 2

no (covalent) bonds between layers
so the layers can slide over each other OR weak forces between the layers so layers can slide over each other

Question 3

Give ONE reason why diamond is used for tips of drill ( in terms of the properties of diamond)

Answer 3

diamond is Hard

Question 4

How many other carbon atoms are bonded to one atom in diamond?

Answer 4

each carbon atom is bonded to 4 other carbon atoms

Question 5

How many other carbon toms are bonded to one atoms in graphite?

Answer 5

each carbon atom is bonded to three other carbon atoms

Question 6

Explain why diamond is not a good conductor of electricity?

Answer 6

there are no free/delocalised electrons that can move throughout the structure

Question 7

give one example of what graphite is used for.

Answer 7

pencils or lubricant

Question 8

what type of bonding occurs within the carbon atom?

Answer 8

covalent bonding

Question 9

what type of structure does diamond have ?

Answer 9

Giant covalent structure

Question 10

what type of structure does graphite have?

Answer 10

Giant covalent structure

Question 11

why can carbon nanotubes conduct electricity?

Answer 11

because they have delocalized electrons that are free to move and carry a charge.