Bonding in metals and their properties

How are the atoms in metals arranged?

• In isolated clusters

• In a regular pattern layer by layer

• In a gaseous state

• In a random pattern

What type of structure do metals have?

• Giant lattice structure

• Giant molecular structure

• Simple molecular structure

• Ionic structure

What are the metal ions in the structure described as?

• Non-existent

• Negatively charged

• Positively charged

• Neutral

What type of attraction bonds metal ions to each other?

• Magnetic attraction

• Chemical attraction

• Electrostatic attraction

• Gravitational attraction

What are the free-moving electrons in metals called?

• Localized electrons

• Delocalised electrons

• Protons

• Static electrons

Why do metals conduct electricity?

• Because of their high melting points

• Because of the static electrons

• Because of the ionic bonds

• Because of their delocalised electrons

What property allows metals to be good conductors of thermal energy?

• Their metallic bonding

• Their delocalised electrons

• Their crystalline structure

• Their high density

Why do metals have high melting and boiling points?

• Because they are in a gaseous state

• Because the metallic bonding is very strong

• Because they are made of small molecules

• Because of weak metallic bonding

What is needed to overcome the metallic bonds in melting and boiling metals?

• Low amounts of energy

• Water

• Magnetic fields

• Large amounts of energy

How are the metal ions arranged in the structure?

• In regular layers

• Isolated from each other

• In irregular patterns

• In a single layer