What is the Reactivity Series in the context of Cambridge IGCSE Coordinated Science?

The Reactivity Series is a list of metals arranged in order of decreasing reactivity. In the Cambridge IGCSE Coordinated Science curriculum, it helps students understand how different metals react with substances like water, acids, and oxygen. The series is crucial for predicting the outcomes of chemical reactions involving metals.

Why is the Reactivity Series important for understanding metal reactions?

The Reactivity Series is important because it allows students to predict how metals will react with other substances. For example, more reactive metals like potassium and sodium will react vigorously with water, while less reactive metals like gold and platinum do not react easily. This understanding is essential for explaining various chemical processes and reactions in the Cambridge IGCSE Coordinated Science syllabus.

How can the Reactivity Series be used to extract metals from their ores?

The Reactivity Series helps determine the method used to extract metals from their ores. Metals higher in the series, such as aluminum, require electrolysis for extraction due to their high reactivity. In contrast, metals lower in the series, like iron, can be extracted using reduction with carbon. This concept is a key part of the Cambridge IGCSE Coordinated Science curriculum.

What are some common reactions that demonstrate the Reactivity Series?

Common reactions include the reaction of metals with water, acids, and oxygen. For instance, when metals like calcium react with water, they form hydroxides and release hydrogen gas. Similarly, metals like zinc react with hydrochloric acid to produce zinc chloride and hydrogen gas. These reactions illustrate the principles of the Reactivity Series as taught in the Cambridge IGCSE Coordinated Science course.

How does the Reactivity Series explain displacement reactions?

The Reactivity Series explains displacement reactions by showing that a more reactive metal can displace a less reactive metal from its compound. For example, if you place a strip of zinc in a copper sulfate solution, zinc will displace copper because it is more reactive. This concept is fundamental in understanding chemical reactions in the Cambridge IGCSE Coordinated Science curriculum.

Why is "Predicting that silver reacts with copper sulfate to give copper" a common mistake in Reactivity Series ?

Why it happens: Students apply 'metal + metal salt → displacement' without checking the reactivity order. How to avoid it: Always check the reactivity series: silver is BELOW copper → no displacement. Only metals ABOVE the target metal can displace it.

Why is "Saying copper reacts with dilute hydrochloric acid" a common mistake in Reactivity Series ?

Why it happens: Students apply the 'metal + acid → salt + H₂' rule to all metals. How to avoid it: Copper is below hydrogen in the reactivity series; it does NOT react with dilute acids. Only metals above hydrogen in the series react with dilute HCl or H₂SO₄. Source: 0654 Examiner Report 2022

Why is "Writing unbalanced displacement equations" a common mistake in Reactivity Series ?

Why it happens: Students focus on the concept of displacement and forget to balance atoms/charges. How to avoid it: Always balance the equation after writing it. For Zn + CuSO₄: 1 Zn replaces 1 Cu²⁺ (both 2+ ions) → balanced as written. For Na + CuSO₄: 2 Na needed for 1 Cu²⁺.

MetalsCambridge IGCSE Coordinated Sciences 0654

Reactivity Series

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Reactivity Series — Cambridge IGCSE Coordinated Science 0654

The reactivity series ranks metals by their tendency to lose electrons. Cambridge tests displacement reactions (used to determine the series), reactions with water and acid, and the link to extraction methods.

What you’ll learn

Mapped to the Cambridge IGCSE 0654 syllabus (2025-2027).

C10.4 — State the reactivity series in order and explain reactions with water and dilute acids.
C10.5 — Use displacement reactions to determine relative reactivity.
C10.6 — Relate position in reactivity series to extraction method.

The Reactivity Series

The reactivity series orders metals by their tendency to lose electrons and form positive ions. More reactive metals displace less reactive ones.

Reactivity series (most reactive at top):

K > Na > Li > Ca > Mg > Al > C > Zn > Fe > H > Cu > Ag > Au

(C = carbon; H = hydrogen — included for comparison)

Reactions with cold water:

K, Na: vigorous (K catches fire; Na fizzes vigorously)
Ca: steady fizzing
Mg: very slow with cold water (fast with steam)
Zn, Fe, Cu: no reaction with cold water

Reactions with dilute acid (dilute HCl or H₂SO₄):

K, Na: explosively fast (dangerous — not done with dilute acid)
Ca, Mg: vigorously fast
Zn, Fe: moderate rate
Cu, Ag, Au: no reaction (below H in series)

Displacement reactions: A more reactive metal displaces a less reactive metal from a salt solution.

Fe + CuSO₄ → FeSO₄ + Cu (iron is above copper → displaces it) Cu + FeSO₄ → no reaction (copper is below iron)

Evidence: colour change in solution, coating of metal on surface

Explaining reactivity: The higher in the series, the easier the metal loses electrons (ionisation energy decreasing down real trends). K⁺ formation most favourable; Au⁺ formation very unfavourable.

Metals at the top lose electrons easily and react with water; metals below hydrogen are too unreactive to displace it.

K > Na > Li > Ca > Mg > Al > Zn > Fe > Cu > Ag > Au.
Above H: react with acids → H₂. K/Na/Ca react with water.
Displacement: more reactive metal from salt solution of less reactive metal.

Reactivity and Metal Extraction

The position of a metal in the reactivity series determines how it is extracted from its ore.

The more reactive a metal, the more stable its compounds → more energy needed to extract it.

Position in series	Extraction method
Very reactive (K, Na, Li, Ca, Al, Mg)	Electrolysis of molten ore — very high energy cost
Moderately reactive (Zn, Fe, Pb)	Reduction with carbon (coke) in a blast furnace
Below carbon (Cu, Ag, Au, Pt)	Thermal decomposition or found native (as pure metal); some by reduction

Blast furnace — extraction of iron:

Fe₂O₃ + 3CO → 2Fe + 3CO₂ (reduction of iron(III) oxide with carbon monoxide) C + CO₂ → 2CO (carbon dioxide reduced by more carbon)

Aluminium extraction (despite Al being less reactive than Na, it needs electrolysis because its oxide has too high a melting point to be reduced cheaply by carbon — electrolysis of molten Al₂O₃ in cryolite).

High reactivity → electrolysis needed (K, Na, Mg, Al, Ca).
Moderate reactivity → carbon reduction in blast furnace (Fe, Zn, Pb).
Low reactivity → thermal decomposition or found as native metal.

How it’s examined

Paper 4: 'Zinc is added to copper sulfate solution. State two observations and write an equation' (3 marks — blue colour fades, pink/copper solid forms, Zn + CuSO₄ → ZnSO₄ + Cu). 'Explain why aluminium is extracted by electrolysis but iron is extracted by reduction with carbon' (3 marks — Al more reactive, Al₂O₃ has very high MP; Fe less reactive, can be reduced by C at feasible temperatures). Reactivity series questions are in virtually every Paper 4.

Sources: Cambridge IGCSE Coordinated Sciences 0654 syllabus 2025-2027 (C10); 0654 Examiner Reports 2022-2024. Last reviewed 2026-05-14.

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Step-by-step worked examples — Reactivity Series

Step-by-step solutions to past-paper-style questions on reactivity series , written exactly the way a tutor would explain them at the board.

1Zinc displacing copper from solution
Extended
Question
A piece of zinc is added to copper sulfate solution. Describe what is observed and write a balanced equation.
Step-by-step solution
1. Step 1
  Zinc is more reactive than copper; zinc displaces copper from the copper sulfate solution.
  $\text{Zn} + \text{CuSO}_4 \rightarrow \text{ZnSO}_4 + \text{Cu}$
2. Step 2
  Observations: the blue colour of the copper sulfate solution fades/becomes colourless (Cu²⁺ removed); a reddish-brown/copper-coloured solid deposits on the zinc.
3. Step 3
  Zinc dissolves (the zinc surface corrodes); the solution becomes zinc sulfate (colourless).
Answer
Blue solution fades; copper deposits on zinc; $\text{Zn} + \text{CuSO}_4 \rightarrow \text{ZnSO}_4 + \text{Cu}$ .
Examiner tip
Both the observation (blue → colourless; copper deposit) and the equation are needed for full marks.
2Deducing reactivity order from observations
Core
Question
Use the following observations to arrange Mg, Fe, and Cu in order of decreasing reactivity: Mg reacts vigorously with dilute HCl; Fe reacts slowly; Cu does not react.
Step-by-step solution
1. Step 1
  Vigorous reaction with dilute acid → high reactivity → Mg is the most reactive.
2. Step 2
  Slow reaction → intermediate reactivity → Fe is less reactive than Mg.
3. Step 3
  No reaction with dilute acid → Cu is below H in reactivity series → least reactive of the three.
Answer
Decreasing reactivity: Mg > Fe > Cu.
3Why silver cannot displace copper
Extended
Question
Explain why adding silver metal to copper sulfate solution does not produce a reaction.
Step-by-step solution
1. Step 1
  In a displacement reaction, only a MORE reactive metal can displace a less reactive metal from its salt solution.
2. Step 2
  Silver (Ag) is BELOW copper in the reactivity series: K > Na > ... > Cu > Ag > Au.
3. Step 3
  Since Ag is less reactive than Cu, Ag cannot displace Cu²⁺ from the solution; no reaction occurs.
Answer
Silver is less reactive than copper (lower in the reactivity series); a less reactive metal cannot displace a more reactive one → no reaction.
4Reactions of metals with water
Core
Question
Describe the reactions of potassium, calcium, and iron with water or steam.
Step-by-step solution
1. Step 1
  Potassium (very reactive): reacts vigorously with cold water → KOH + H₂; lilac flame observed.
  $2\text{K} + 2\text{H}_2\text{O} \rightarrow 2\text{KOH} + \text{H}_2$
2. Step 2
  Calcium (reactive): reacts steadily with cold water → Ca(OH)₂ + H₂; bubbles form, white cloudy solution.
  $\text{Ca} + 2\text{H}_2\text{O} \rightarrow \text{Ca(OH)}_2 + \text{H}_2$
3. Step 3
  Iron (less reactive): does not react with cold water or steam under normal conditions; reacts very slowly with steam to form iron oxide + H₂.
  $3\text{Fe} + 4\text{H}_2\text{O} \rightarrow \text{Fe}_3\text{O}_4 + 4\text{H}_2$
Answer
K: vigorous cold water reaction, lilac flame. Ca: steady cold water reaction, cloudy solution. Fe: no cold water reaction; slow reaction with steam.

Key Definitions and Keywords — Reactivity Series

Definitions to memorise and the exact keywords mark schemes credit for reactivity series answers — sharpened from recent examiner reports for the 2026 0654 sitting.

Reactivity series
Examiner keyword
An ordered list of metals (and carbon and hydrogen) from most to least reactive, based on their tendency to lose electrons. Order: K > Na > Li > Ca > Mg > Al > C > Zn > Fe > H > Cu > Ag > Au.
Displacement reaction
Examiner keyword
A reaction in which a more reactive element displaces a less reactive element from its compound. e.g. $\text{Zn} + \text{CuSO}_4 \rightarrow \text{ZnSO}_4 + \text{Cu}$
Reactivity and oxidation
More reactive metals are more easily oxidised (lose electrons more readily). The reactivity series reflects the ease of losing electrons to form positive ions.
Position of hydrogen
Hydrogen is included in the reactivity series between Al and Cu; metals above hydrogen react with dilute acids to produce H₂; metals below hydrogen (Cu, Ag, Au) do not.

Common Mistakes and Misconceptions — Reactivity Series

The traps other students keep falling into on reactivity series questions — taken from recent Cambridge IGCSE 0654 examiner reports and mark schemes — and how to avoid them.

✕Predicting that silver reacts with copper sulfate to give copper
Why it happens
Students apply 'metal + metal salt → displacement' without checking the reactivity order.
How to avoid it
Always check the reactivity series: silver is BELOW copper → no displacement. Only metals ABOVE the target metal can displace it.
✕Saying copper reacts with dilute hydrochloric acid
0654 Examiner Report 2022
Why it happens
Students apply the 'metal + acid → salt + H₂' rule to all metals.
How to avoid it
Copper is below hydrogen in the reactivity series; it does NOT react with dilute acids. Only metals above hydrogen in the series react with dilute HCl or H₂SO₄.
✕Writing unbalanced displacement equations
Why it happens
Students focus on the concept of displacement and forget to balance atoms/charges.
How to avoid it
Always balance the equation after writing it. For Zn + CuSO₄: 1 Zn replaces 1 Cu²⁺ (both 2+ ions) → balanced as written. For Na + CuSO₄: 2 Na needed for 1 Cu²⁺.

Practice questions

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Reactivity Series — frequently asked questions

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Reactivity Series

Short Study Notes in the form of Slides

Short Study Notes — Reactivity Series

Detailed Notes

What you’ll learn

How it’s examined

1Zinc displacing copper from solution

2Deducing reactivity order from observations

3Why silver cannot displace copper

4Reactions of metals with water

Reactivity series

Displacement reaction

Reactivity and oxidation

Position of hydrogen

✕Predicting that silver reacts with copper sulfate to give copper

✕Saying copper reacts with dilute hydrochloric acid

✕Writing unbalanced displacement equations

Practice questions

Past paper style quiz

Assess your understanding

Reactivity Series — frequently asked questions