Reactivity Series Flashcards
(14 cards)
Reactivity Series
- Potassium
- Sodium
- Lithium
- Calcium
- Magnesium
- Zinc
- Iron
- Copper
What metals will react with dilute acids?
Only metals above hydrogen in the reactivity series will react with dilute acids.
Metals and acids general formula
metal + acid ⟶ salt + hydrogen
Magnesium and sulphuric acid and hydrochloric acid
- Mg (s) + H2SO4 (aq) → MgSO4 (aq) + H2 (g)
- Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g)
How do zinc and iron react with water?
They only react slowly with steam.
Does copper react with water or steam?
No it doesn’t, it is highly unreactive.
What is a displacement reaction?
This means that a more reactive metal will displace a less reactive metal from its compounds.
What are the conditions needed for iron rust?
Oxygen and water must be present for rust to occur.
What are the three method of preventing iron from rusting?
- Barrier methods
- Sacrificial protection
- Galvanising
Explain the process of barrier methods
- Rust is prevented by coating iron with barriers (like paint, oil, grease, or electroplating) to block water and oxygen.
- If coatings are damaged, iron is exposed and begins to rust.
- Rust is porous, allowing air and water through, causing continuous internal corrosion even beneath broken barriers.
Explain the process of sacrificial protection
- A more reactive metal (like zinc) can be attached to iron.
- The more reactive metal oxidises and corrodes first, protecting the iron.
- Zinc loses electrons more easily than iron.
- To keep protection, zinc bars must be replaced before they fully corrode.
Explain the process of galvanising
- Galvanising coats iron with zinc (by electroplating or dipping in molten zinc).
- Zinc reacts with air to form ZnCO₃, acting as a barrier.
- If scratched, zinc still protects iron through sacrificial protection by corroding first.
Oxidising Agent
If you have been reduced, you are the oxidising agent.
Reducing Agent
If you have been oxidised, you are the reducing agent.
