Giant covalent substances contain atoms joined together covalent by bonds. Diamond, graphite and graphene are forms of carbon and have different properties because they have different structures.
Which of the following has a giant covalent structure?
What structure is shown in the diagram?
Why does silicon dioxide have such a high melting point?
Because the silicon and oxygen atoms are held by strong intermolecular forces
Because the silicon and oxygen atoms are held by many strong covalent bonds
Because there are strong electrostatic forces between the silicon and oxygen atoms
Why is graphite useful for pencil leads?
It is hard with a high melting point
It is black and slippery
It is shiny and melts easily
What type of structure do both diamond and graphite have?
A giant covalent structure
A giant ionic lattice structure
A simple molecular structure
Why is diamond used to coat metal drill bits?
It is a good conductor of electricity
It is slippery and cheap
It is very hard with a high melting point
Which of these is a covalent molecular structure?
Why does graphite conduct electricity?
It has delocalised electrons
It has a giant covalent structure
It forms a tetrahedral arrangement
Which of the following could have a molecular formula of C60?
Approximately how many carbon atoms might be linked together in a polymer molecule?