Chemistry · Both
Metals & the Reactivity Series
The reactivity series, displacement reactions, extraction of metals and preventing corrosion.
Metals differ in how readily they react. The reactivity series ranks metals and helps predict displacement reactions and how metals are extracted.
Reactivity series (common metals)
Most reactive → least reactive (simplified):
Potassium, sodium, lithium, calcium, magnesium, aluminium, (carbon), zinc, iron, (hydrogen), copper, silver, gold
• Metals above hydrogen react with acids to make salt + hydrogen
• More reactive metals displace less reactive metals from compounds
Worked example
Will zinc displace copper from copper sulfate solution?
Solution
**Yes** – zinc is more reactive than copper, so zinc + copper sulfate → zinc sulfate + copper.
Extraction of metals
• Metals **less reactive than carbon** can be extracted by heating the ore with carbon (reduction)
• Metals **more reactive than carbon** need electrolysis (e.g. aluminium)
Example: iron oxide + carbon → iron + carbon dioxide (in a blast furnace)
Rusting
Iron rusts when exposed to **oxygen and water**.
Rust is hydrated iron(III) oxide.
Prevention: painting, oiling, galvanising (coating with zinc), sacrificial protection, alloying (e.g. stainless steel).
Practice questions
Try these without looking at the answers first.
Q1.Which is more reactive: zinc or copper?
Show answer
Zinc
Q2.How is aluminium extracted?
Show answer
Electrolysis
Q3.What two things are needed for iron to rust?
Show answer
Oxygen and water