Network Solids Quiz

What is the main difference between diamond and graphite?

• Diamond is harder than graphite

• Diamond is a conductor of electricity while graphite is not

• Diamond is more valuable than graphite

• Diamond is made up of carbon atoms arranged in a 3D network, while graphite is made up of carbon atoms arranged in a 2D sheet structure

Why is diamond so hard?

• Because it has strong covalent bonds in a 3D network

• Because it has a hexagonal structure

• Because it is made up of carbon atoms

• Because it conducts electricity

Why is graphite soft?

• Because it has weak van der Waals forces between sheets

• Because it conducts electricity

• Because it has a hexagonal structure

• Because it is made up of carbon atoms

Which type of bond is present in diamond?

• Metallic bonds

• Pi bonds

• Sigma bonds

• Ionic bonds

Which type of bond is present in graphite?

• Metallic bonds

• Ionic bonds

• Pi bonds

• Sigma bonds

Why is graphite a good lubricant?

• Because it has weak van der Waals forces between sheets

• Because it has a hexagonal structure

• Because it can break down into slippery platelets

• Because it conducts electricity

Why is diamond a poor conductor of electricity?

• Because it has a hexagonal structure

• Because it has strong covalent bonds in a 3D network

• Because it can break down into slippery platelets

• Because it has weak van der Waals forces between sheets

Which type of network structure does diamond have?

• 2D sheet structure

• Random structure

• Chain structure

• 3D network structure

Which type of network structure does graphite have?

• 3D network structure

• Random structure

• Chain structure

• 2D sheet structure

Why is diamond brittle?

• Because it has a hexagonal structure

• Because it has strong covalent bonds in a 3D network

• Because it has weak van der Waals forces between sheets

• Because it can break down into slippery platelets