Giant covalent structures - Y9

What type of structure do diamond and graphite have?

• Giant covalent structure

• Ionic structure

• Simple molecular structure

• Metallic structure

How many covalent bonds does each carbon atom form in diamond?

• Six

• Four

• Two

• Three

What makes diamond very hard?

• Hexagonal layers

• Regular tetrahedral network structure

• Delocalised electrons

• Ionic bonding

Why does diamond not conduct electricity?

• Because it is a liquid at room temperature

• Because it has no free electrons

• Because it has a high melting point

• Because it has delocalised electrons

What is the shape of the carbon atoms' arrangement in graphite?

• Linear

• Cubic

• Tetrahedral

• Hexagonal rings

Why can graphite conduct electricity?

• Because it has a high melting point

• Because it has ionic bonds

• Because it has delocalised electrons

• Because it is a metal

What property makes graphite useful as a lubricant?

• Its hardness

• Its layers can slide over each other

• Its ability to conduct electricity

• Its high melting point

How many covalent bonds does each carbon atom form in graphite?

• Two

• Five

• Four

• Three

What is a common use for diamond due to its hardness?

• In batteries

• As a lubricant

• For conducting electricity

• For cutting tools

What is the main reason graphite is used in electrodes?

• Its high melting point

• Its hardness

• Its ability to conduct electricity

• Its slippery nature