Diamond and graphite | Exit Quiz | Oak National Academy

What is an allotrope?

• a type of chemical bond

• a different structural form of an element

• a kind of molecular geometry

• a category of organic compounds

Answer explanation

An allotrope is a different structural form of an element, like graphite and diamond are allotropes of carbon.

What makes diamond so hard?

• intermolecular forces

• delocalised electrons

• hexagonal rings

• covalent bonds

Answer explanation

Diamond's hardness comes from its giant covalent structure, where each carbon atom is bonded strongly to four others.

Why can graphite be used as a lubricant?

• strong covalent bonds within atoms

• weak intermolecular forces between layers

• delocalised electrons

• high melting point

• ability to conduct electricity

Answer explanation

Graphite's layers can easily slide over each other due to the weak intermolecular forces between them, making it a good lubricant.

In diamond, each carbon atom forms ___ covalent bonds.

Answer explanation

In diamond, each carbon atom forms four covalent bonds, creating a very strong and rigid structure.

True or false? In graphite, each carbon atom is bonded to four other carbon atoms.

• True

• False

Answer explanation

In graphite, each carbon atom is covalently bonded to three others, forming layers of hexagonal rings.

Graphite conducts electricity because it has ___ which can move and carry charge/current.

Answer explanation

Graphite conducts electricity because it has delocalised electrons which can move and carry charge/current.