GCSE SCIENCE CHEMISTRY HIGH SCHOOL - The Reactivity Series - Metal Displacement Reactions

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Metal Displacement Reactions.

A metal will displace (take the place of) a less reactive metal
in a metal salt solution.
This is similar to the non-metal displacement reactions
seen on page 23 of the periodic table.

For example,
iron + copper(II) sulfate iron sulfate + copper.
Fe_(s) + CuSO₄_(aq) FeSO₄_(aq) + Cu_(s)

Copper(II) sulfate is blue, iron sulfate is colourless.
During the reaction the blue solution loses its colour
and the iron metal is seen to turn pink-brown
as the displaced copper becomes deposited on it.

If a less reactive metal is added to a metal salt solution
there will be no reaction - nothing will happen!
For example, iron is less reactive than magnesium.
iron + magnesium sulfate no reaction.

In these displacement reactions
the metals are competing for the non-metal anion.
In the above examples the non-metal anion is sulfate - SO₄^2-.
Reactions using chlorides or nitrates can also be used.
The order of the metals in the reactivity series
can be worked out by using these type of reactions.

For example,
tin would be seen to displace lead from lead chloride
but would not react with iron(II) chloride.

tin + lead chloride tin chloride + lead.
Sn_(s) + PbCl₂_(aq) SnCl₂_(aq) + Pb_(s)

tin + iron(II) chloride no reaction.
Sn_(s) + FeCl₂_(aq)
Therefore tin must be above lead but below iron in the reactivity series.

Copper would be seen to displace silver from silver nitrate
but would not react with lead nitrate.

copper + silver nitrate copper nitrate + silver.
Cu_(s) + 2AgNO₃_(aq) Cu(NO₃)₂_(aq) + 2Ag_(s)

copper + lead nitrate no reaction.
Cu_(s) + Pb(NO₃)₂_(aq)
Therefore copper must be above silver but below lead in the reactivity series.

These reactions can be written as ionic equations.

Headings Reactivity Series Search Questions

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