The Properties of Carbon: Diamonds, Graphite, Graphene, and Fullerenes

The video explores the unique properties of carbon, focusing on its ability to form covalent bonds. It discusses the structure and characteristics of diamonds, graphite, graphene, and fullerenes. Diamonds are hard and have a high melting point due to strong covalent bonds, while graphite is soft and conducts electricity because of its layered structure. Graphene, a single layer of graphite, is strong and conductive. Fullerenes, including nanotubes, have unique shapes and are useful in electronics.

What characteristic of diamond makes it a poor conductor of electricity?

• High melting point

• Presence of delocalized electrons

• Absence of delocalized electrons

• Weak covalent bonds

Why can the layers in graphite slide over each other?

• High melting point

• Presence of delocalized electrons

• Weak bonds between layers

• Strong bonds between layers

What makes graphene a strong material?

• Presence of pentagonal rings

• Weak bonds between layers

• Strong covalent bonds with three other carbon atoms

• Its single layer structure

What is a unique feature of fullerenes?

• They are poor conductors of electricity

• They have hollow shapes

• They are made of layers of hexagonal rings

• They have a high melting point

Why are nanotubes useful in electronic circuits?

• They have a high length-to-diameter ratio and can conduct electricity

• They are poor conductors of electricity

• They are made of layers of hexagonal rings

• They have a low length-to-diameter ratio