Structures of Carbon

9. What are fullerenes used to make?

• 9. Spheres and tubes

• 9. Hexagonal layers

• 9. Regular 3D patterns

• 9. Tetrahedral structures

1. What are allotropes?

• 1. Different elements in the same physical state

• Different structural forms of the same element in the same physical state

• 1. Different compounds in the same physical state

• Different mixtures in the same physical state

1. Which of the following is NOT an allotrope of carbon?

• 1. Diamond

• 1. Graphite

• 1. Fullerenes

• 1. Quartz

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

• Two

• Three

• Four

• Five

1. Why does graphite conduct electricity?

• 1. Because it has free ions

• 1. Because it has delocalised electrons

• 1. Because it has a high melting point

• 1. Because it has a regular lattice structure

1. Why does diamond have a high melting point?

• 1. Because it has free electrons

• 2. Because it has a regular 3D pattern

• 1. Because it has strong covalent bonds

• 1. Because it has weak intermolecular forces

9. Which property of diamond prevents it from conducting electricity?

• 9. High melting point

• 9. Regular 3D pattern

• 9. Strong covalent bonds

• 9. Lack of free electrons or ions

9. What is the arrangement of carbon atoms in graphite?

• 9. Hexagonal layers

• 9. Tetrahedral structure

• 9. Linear chains

• 9. Cubic lattice

1. What is the structure of graphite?

• 1. Carbon atoms bonded to four other carbon atoms in a 3D pattern

• 1. Carbon atoms bonded to three other carbon atoms in hexagonal layers

• 1. Carbon atoms bonded to two other carbon atoms in a linear chain

• 1. Carbon atoms bonded to five other carbon atoms in a pentagonal structure

1. Why is graphite softer than diamond?

• 1. Because it has weaker covalent bonds

• 1. Because its layers are held together weakly and can slide over each other

• 1. Because it has fewer carbon atoms

• 1. Because it has a lower melting point