Summary
Metals are solid materials known for their high melting and boiling points, malleability, and excellent conductivity of heat and electricity. Metallic Bonding — a lattice of positive ions in a sea of electrons. Example: Explains why metals are good conductors and malleable.
- Alloys — mixtures of a metal with other elements. Example: Brass is an alloy of copper and zinc.
- Reactivity Series — order of metals based on their reactions with water, acids, and oxygen. Example: Potassium is more reactive than copper.
Exam Tips
Key Definitions to Remember
- Metallic bonding: A lattice of positive ions in a sea of delocalised electrons.
- Alloy: A mixture of a metal with other elements.
Common Confusions
- Alloys are not compounds; they are mixtures.
- Rusting is specific to iron and its alloys, not all metals.
Typical Exam Questions
- What is metallic bonding? A lattice of positive ions in a sea of electrons.
- Why are alloys used instead of pure metals? Alloys are harder and more durable due to the distorted layers of atoms.
- How does reactivity change across the reactivity series? Reactivity decreases from potassium to copper.
What Examiners Usually Test
- Understanding of metallic bonding and its properties.
- Differences between pure metals and alloys.
- Order and reasoning of the reactivity series.