Summary
The Reactivity Series is a list of metals arranged in order of their reactivity with other substances. Metals react with oxygen to form metal oxides, and their reactivity determines how they interact with water and acids.
- Oxidation — a reaction where oxygen is added to an element or compound. Example: Copper reacts with oxygen to form copper oxide.
- Reduction — a reaction where oxygen is removed from an element or compound. Example: Zinc oxide reacts with carbon to form zinc and carbon monoxide.
- Reactivity Series — a ranking of metals based on their reactivity. Example: Potassium is more reactive than iron.
- Displacement Reaction — a more reactive metal displaces a less reactive metal from its compound. Example: Magnesium displaces copper from copper sulfate.
- Sacrificial Protection — using a more reactive metal to prevent corrosion of a less reactive metal. Example: Zinc is used to protect iron in steel boats.
Exam Tips
Key Definitions to Remember
- Oxidation: Addition of oxygen to a substance.
- Reduction: Removal of oxygen from a substance.
- Reactivity Series: Order of metals based on their reactivity.
- Displacement Reaction: A reaction where a more reactive metal displaces a less reactive one.
Common Confusions
- Confusing oxidation with reduction.
- Misunderstanding which metals can displace others in reactions.
Typical Exam Questions
- What is formed when magnesium burns in air? Magnesium oxide is formed.
- Can copper displace magnesium from magnesium chloride? No, copper cannot displace magnesium.
- What happens when potassium reacts with water? Potassium hydroxide and hydrogen gas are formed.
What Examiners Usually Test
- Understanding of oxidation and reduction processes.
- Ability to use the reactivity series to predict reactions.
- Knowledge of displacement reactions and their outcomes.