Displacement Reactions: KS3 Chemistry Explained

A displacement reaction occurs when a more reactive element takes the place of a less reactive element in a compound. In metals chemistry, a more reactive metal will push a less reactive metal out of its salt solution, forming a new compound and releasing the displaced metal.

What is reactivity and why does it matter?

Before we can understand displacement reactions, we need to picture what "reactivity" means at the particle level. Reactivity describes how readily a metal reacts with water, acids, or oxygen — in other words, how strongly a metal's atoms "want" to lose electrons and become positive ions.

The reactivity series ranks metals from most to least reactive:

potassium > sodium > calcium > magnesium > aluminium > zinc > iron > nickel > tin > lead > copper > silver > gold > platinum

Metals high in the series react vigorously — potassium ignites on contact with water, sodium fizzes energetically. Metals low in the series (copper, silver, gold) are largely unreactive, which is why gold objects remain shiny for thousands of years and why these metals occur naturally in a pure state rather than as ores.

The key principle: a metal higher in the reactivity series will always displace a metal that sits lower, because the higher metal has a stronger drive to form ions.

How does a displacement reaction work at the particle level?

Picture copper sulfate solution first. It contains Cu²⁺ ions and SO₄²⁻ ions dissolved in water — the characteristic blue colour comes from the hydrated Cu²⁺ ions.

Now add an iron nail. At the particle level:

Iron atoms (Fe) lose electrons more readily than copper ions need them: Fe → Fe²⁺ + 2e⁻ (iron is oxidised)

The free electrons are taken up by Cu²⁺ ions in solution: Cu²⁺ + 2e⁻ → Cu (copper is reduced)

Net result: iron enters solution as Fe²⁺ ions; copper deposits as solid pink/brown copper metal on the surface of the nail; the solution colour changes from blue to pale green (Fe²⁺ in solution is pale green; blue Cu²⁺ is removed)

This is simultaneously a redox reaction: one species is oxidised (iron loses electrons) and another is reduced (copper ions gain electrons). At KS3, knowing the observations and the word equation is the priority; the oxidation/reduction language deepens at GCSE.

What are some classic examples of displacement reactions?

Example 1: Iron + copper sulfate solution

Iron + copper sulfate → iron sulfate + copper

Fe + CuSO₄ → FeSO₄ + Cu

Observations: blue solution turns pale green; pink/brown copper metal deposits on the iron nail. Iron is above copper in the reactivity series, so iron displaces copper. ✓

Example 2: Zinc + copper sulfate solution

Zinc + copper sulfate → zinc sulfate + copper

Zn + CuSO₄ → ZnSO₄ + Cu

Observations: blue solution decolourises; the grey zinc surface becomes coated in copper. Zinc is above copper in the reactivity series. ✓

Example 3: Copper + silver nitrate solution

Copper + silver nitrate → copper nitrate + silver

Cu + 2AgNO₃ → Cu(NO₃)₂ + 2Ag

Observations: colourless solution turns blue (Cu²⁺ forms); silver crystals grow on the copper surface. Copper is above silver in the reactivity series. ✓

Non-reaction: Copper + zinc sulfate solution

No reaction occurs. Copper sits below zinc in the reactivity series, so copper atoms do not have sufficient drive to displace zinc ions from solution. No colour change, no new solid — nothing visible happens. This is just as important a result as a successful displacement — it confirms the rule.

What is competition for oxygen?

Displacement reactions also occur with metal oxides, not just salt solutions. A more reactive metal can "steal" oxygen from the oxide of a less reactive metal — this is sometimes described as competition for oxygen.

The most dramatic example taught at KS3 is the thermite reaction:

aluminium + iron(III) oxide → aluminium oxide + iron

2Al + Fe₂O₃ → Al₂O₃ + 2Fe

Aluminium (higher in the reactivity series) displaces iron from its oxide. The reaction releases an enormous amount of heat — temperatures can reach around 2500 °C — hot enough to produce molten iron. This makes thermite useful for welding railway tracks in the field, where a portable, self-sustaining heat source is needed.

Carbon fits into the reactivity series between aluminium and zinc, and it too can displace metals less reactive than itself from their oxides. This is industrially vital: carbon (as coke) is used in blast furnaces to displace iron from iron ore, and historically to extract zinc, tin, and lead from their ores.

How do we predict whether a displacement reaction will occur?

The rule is straightforward: if the metal being added is higher in the reactivity series than the metal in the compound, a displacement reaction occurs. If it is lower, no reaction takes place.

Metal being added | Metal in compound | Reaction? | Reasoning
Magnesium | Copper sulfate | Yes | Mg is above Cu in the reactivity series
Zinc | Iron sulfate | Yes | Zn is above Fe
Iron | Copper sulfate | Yes | Fe is above Cu
Copper | Iron sulfate | No | Cu is below Fe
Silver | Copper nitrate | No | Ag is below Cu
Magnesium | Zinc sulfate | Yes | Mg is above Zn

Use this table as a prediction tool: locate both metals in the reactivity series, then apply the rule.

Why are displacement reactions important in industry?

Understanding displacement reactions is not merely a classroom exercise — it underpins much of how humans extract and use metals:

Metal extraction from ores: the blast furnace uses carbon (coke) to displace iron from iron(III) oxide at high temperatures. Without this displacement reaction, iron and steel — the backbone of construction and engineering — would be unobtainable at scale.

Thermite welding: molten iron produced by the aluminium/iron oxide displacement reaction fuses railway track joints in remote locations where electrical welding equipment cannot easily be used.

Understanding corrosion: metals high in the reactivity series corrode fastest because they react most readily with oxygen and water. Iron rusts; gold does not. Zinc is used to galvanise (coat) steel because zinc is above iron — it reacts preferentially with any oxygen or water, protecting the iron beneath (sacrificial protection).

Electroplating: related electrochemical principles allow thin layers of one metal (e.g. silver or chrome) to be deposited on another, improving appearance or resistance to wear.

Frequently asked questions

How do you predict whether a displacement reaction will happen?

Look up both metals in the reactivity series. If the metal you are adding is positioned higher than the metal in the compound, it will displace that metal and a reaction occurs — you will observe colour changes, a new solid forming, and often a temperature rise. If the metal you are adding is lower in the series than the metal in the compound, no displacement takes place and the solution remains unchanged. For example, magnesium is near the top of the series and copper is near the bottom, so magnesium readily displaces copper from copper sulfate. Copper cannot displace magnesium from magnesium sulfate because copper is far less reactive.

What observations tell you a displacement reaction has happened?

Several visible changes confirm that displacement has occurred: a colour change in the solution (for example, blue copper sulfate turns pale green when iron displaces copper, because Fe²⁺ ions form and Cu²⁺ ions are removed); the appearance of a new solid on the surface of the added metal (copper deposits on zinc or iron); and a temperature rise (most metal displacement reactions are exothermic — energy is released). If none of these changes occur after a few minutes, it is safe to conclude no displacement reaction has taken place.

Is a displacement reaction a physical or chemical change?

A displacement reaction is definitely a chemical change. New substances are formed — the iron becomes iron sulfate in solution, and copper ions become solid copper metal. The chemical identities of the reactants change: iron atoms are converted to iron ions in solution; copper ions are converted to copper atoms. These new substances have different properties from the starting materials. The colour change, new solid, and energy release are all evidence that a permanent chemical transformation has occurred — it cannot be reversed by simple physical means such as filtering or evaporating.

Why does the thermite reaction produce so much heat?

In the thermite reaction, aluminium displaces iron from iron(III) oxide. Aluminium has a very high affinity for oxygen — the bonds in aluminium oxide (Al–O bonds) are significantly stronger, and therefore release more energy when formed, than the bonds in iron(III) oxide (Fe–O bonds) that are broken. The large difference in bond energies is released entirely as heat, producing temperatures of around 2500 °C — sufficient to melt the iron produced. This makes thermite uniquely useful for portable, electricity-free welding of railway tracks and other heavy metalwork, though the extremely high temperature and difficulty of controlling the reaction mean it is handled only by specialists.

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