1. What enables metals to conduct electricity?

a) The presence of weak intermolecular bonds
b) The presence of delocalised electrons
c) The presence of delocalised ions
d) The fact that metals have giant structures enables them to conduct electricity and heat

2. The high melting and boiling points for most metals suggests that they have:

a) A simple molecular structure
b) Strong intermolecular bonds
c) Strong ionic bonds between the metal ions
d) A giant structure with lots of strong bonds

3. Which word describes the ability of a metal to be drawn out into a wire?

a) Malleable
b) Conductive
c) Ductilite
d) Lustre

4. Metals can be hammered, rolled and beaten in different shapes, this means that they are .

5. The high density of metals can be attributed to:

a) The tightly packed arrangement of ions within the giant metallic structure
b) The attraction of the delocalised electrons for the metal ions
c) The presence of metallic bonds
d) The ability of the layers of metal ions to slide over each other

6. Metals consist of a giant structure of charged metals ions which are attracted to a "sea" of negatively charged electrons.

7. In a metallic bond there is attractions between:

a) Positively charged ions and negative ions.
b) Positively charged ions and delocalised electrons
c) Negative ions and delocalised electrons
d) Positive ions and neutral atoms

8. Which of the following best describes the "sea of electrons" model to describe the structure of a metal?

a) Electrons tightly held in fixed positions around each nucleus
b) The movement of delocalised electrons throughout the metallic structure
c) Electrons shared in pairs between adjacent metal atoms
d) Electrons that are constantly being gained and lost by metal atoms

9. A key feature of metallic bonds is that they are not but they are constantly breaking and reforming as the delocalised electrons move.

10. The ability of ions in a metal to slide over each other is explained by:

a) The strong fixed metallic bonds
b) The repulsion between the metal ions
c) The absence of any bonds between the layers of metal ions
d) The fact that metallic bonds are constantly breaking and reforming