Carbon Allotropes: Diamond, Graphite, Graphene and Fullerenes Flashcards

1️⃣ Familiarise yourself with the flashcards:

  • Look through all the flashcards to see what's on both sides.
  • Make sure you understand the information on each card. If something's unclear, click the link to the revision notes at the bottom of the page for more details.

2️⃣ Test yourself:

  • Look at the question or prompt on each card and try to remember the answer before flipping it over.
  • Check the answer and make a note of any cards you find challenging and need to go over more.

3️⃣ Consistently Review and Practice:

  • Use spaced repetition: spend more time on the cards you struggle with and go over them more often.
  • Regularly review all the flashcards to help you better understand and retain the information over time.

Note: We may include questions that have multiple correct answers. It's useful to remember specific examples to understand these concepts better.

PERSONALISED 1-TO-1 TUTORING

Need more help on this topic? Get 1-to-1 support

Get support with clear explanations, practice and feedback (Ages 5 to 16).

  • DBS-checked tutors
  • Flexible times
  • Parents can be updated

Want an ad-free experience? Subscribe to remove ads

What is meant by an allotrope of carbon?

An allotrope of carbon is a different form of pure carbon, with the atoms arranged in a different structure.

What type of structure do diamond and graphite have?

Diamond and graphite both have giant covalent structures made only of carbon atoms.

How is each carbon atom bonded in diamond?

In diamond, each carbon atom is covalently bonded to four other carbon atoms in a 3D lattice.

Why is diamond very hard and has a very high melting point?

Diamond is very hard and has a high melting point because many strong covalent bonds join the atoms in a rigid 3D network.

How is each carbon atom bonded in graphite?

In graphite, each carbon atom is covalently bonded to three other carbon atoms in flat hexagon layers.

Why can graphite conduct electricity but diamond cannot?

Graphite can conduct electricity because each carbon has one delocalised electron that can move. In diamond, all electrons are in bonds, so it cannot conduct.

Why is graphite soft and slippery?

Graphite is soft and slippery because the layers are held together by weak forces, so they can slide over each other.

What is graphene?

Graphene is a single one-atom-thick layer of carbon atoms arranged in a hexagon lattice, like one sheet of graphite.

Give one reason why graphene is useful in electronics.

Graphene is useful in electronics because it is an excellent conductor of electricity and is very thin and strong.

What is a fullerene?

A fullerene is a molecule made only of carbon atoms arranged in hollow shapes, such as spheres, tubes or cages.

Give one use of fullerenes or carbon nanotubes.

Fullerenes or carbon nanotubes can be used to deliver drugs in the body, as catalysts, or to reinforce materials like sports equipment.