Giant Covallent Structures

Question 1

How are they bonded

Answer 1

All atoms are bonded together by strong covalent bonds

Question 2

What are their melting and boiling points like

Answer 2

They have very high melting and boiling points because a lot of energy is needed to break the covalent bonds

Question 3

Can they conduct

Answer 3

Generally dont conduct electricity because they dont contain charged particles

Question 4

Properties of Diamond

Answer 4

Forms 4 covalent bonds

High melting point

Covalent bonds hold it in a rigid lattice structure

Has no free electrons or ions

Question 5

Properties of graphene

Answer 5

Its a type of fullerene and is one layer of graphite

Its a sheet of carbon atoms joined together in hexagons

The sheet is one atom thick, making it a 2 dimensional compound

Question 6

Properties of graphite

Answer 6

Each carbon atom forms 3 covalent bonds, creating sheets of carbon atoms arranged in hexagons

There aren’t any covalent bonds between the layers, they’re held together weakly so are free to move over each other

Its soft and slippery, making it an ideal lubricating material

Got a high melting point

Only 3 out of each of carbons 4 outer electrons are used in bonds so each carbon atom has 1 delocalised electron that can move

It conducts electricity and is often used to make electrodes