GCSE Chemistry revision

The reactivity series

Reactivity of metals

AQA 4.4.1.2 Foundation & Higher

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Metals react by losing electrons from their outermost shell to form positive ions, and the easier a metal does this, the more reactive it is.
The reactivity series arranges metals in order of how readily they form positive ions, from most reactive to least reactive.
Carbon and hydrogen are included in the reactivity series as non-metal reference points to help compare metals against them.
Group 1 metals are the most reactive, followed by Group 2 metals, with transition metals generally being the least reactive.

1. Introduction AQA

Metals react by losing electrons from their outermost shell to form positive ions, and the easier a metal does this, the more reactive it is.
The reactivity series arranges metals in order of how readily they form positive ions, from most reactive to least reactive.
Carbon and hydrogen are included in the reactivity series as non-metal reference points to help compare metals against them.
Group 1 metals are the most reactive, followed by Group 2 metals, with transition metals generally being the least reactive.

When a metal reacts with an acid, it produces a salt and hydrogen gas.
For example, potassium reacting with hydrochloric acid produces potassium chloride and hydrogen gas, reacting explosively and possibly catching fire.
The violence of the reaction decreases as you go down the reactivity series — magnesium produces vigorous bubbling, zinc and iron produce fewer bubbles, and copper does not react at all.
To fairly compare the reactivity of metals with acids, each metal sample must have the same mass and surface area, and the same type and concentration of acid must be used each time.
As well as observing how violent the reaction is, the temperature change can be measured, since more reactive metals release more heat.

2. Metals Reacting with Acids AQA

When a metal reacts with an acid, it produces a salt and hydrogen gas.
For example, potassium reacting with hydrochloric acid produces potassium chloride and hydrogen gas, reacting explosively and possibly catching fire.
The violence of the reaction decreases as you go down the reactivity series — magnesium produces vigorous bubbling, zinc and iron produce fewer bubbles, and copper does not react at all.
To fairly compare the reactivity of metals with acids, each metal sample must have the same mass and surface area, and the same type and concentration of acid must be used each time.
As well as observing how violent the reaction is, the temperature change can be measured, since more reactive metals release more heat.

When reactive metals react with water, they produce a metal hydroxide and hydrogen gas.
For example, lithium reacts with water to form lithium hydroxide and hydrogen: 2Li + 2H₂O → 2LiOH + H₂.
Only the most reactive metals (such as Group 1 metals) react vigorously with cold water, whilst magnesium reacts only very slightly.
Zinc, iron, and copper are not reactive enough to react with cold water at all.

3. Metals Reacting with Water AQA

When reactive metals react with water, they produce a metal hydroxide and hydrogen gas.
For example, lithium reacts with water to form lithium hydroxide and hydrogen: 2Li + 2H₂O → 2LiOH + H₂.
Only the most reactive metals (such as Group 1 metals) react vigorously with cold water, whilst magnesium reacts only very slightly.
Zinc, iron, and copper are not reactive enough to react with cold water at all.

In a displacement reaction, a more reactive metal can displace (push out) a less reactive metal from its salt solution.
For example, magnesium added to iron sulfate solution displaces the iron, forming magnesium sulfate and iron metal, because magnesium is more reactive than iron.
If a less reactive metal is added to a salt solution of a more reactive metal, no reaction occurs — for example, copper added to iron sulfate solution produces no reaction.

4. Displacement Reactions AQA

In a displacement reaction, a more reactive metal can displace (push out) a less reactive metal from its salt solution.
For example, magnesium added to iron sulfate solution displaces the iron, forming magnesium sulfate and iron metal, because magnesium is more reactive than iron.
If a less reactive metal is added to a salt solution of a more reactive metal, no reaction occurs — for example, copper added to iron sulfate solution produces no reaction.