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Metal Displacement Reactions.

Metal Displacement Reactions. A metal will displace(take the place of) a less reactive metal in a metal salt solution. For example, iron + copper(II) sulfate  iron sulfate +copper . If a less reactive metal is added to a metal salt solution there will be no reaction

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Metal Displacement Reactions.

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  1. Metal Displacement Reactions. • A metal will displace(take the place of) a less reactive metal in a metal salt solution. • For example,iron + copper(II)sulfateiron sulfate +copper. If a less reactive metal is added to a metal salt solution there will be no reaction • 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 -SO42-.

  2. The order of the metals in the reactivity seriescan be worked out by using displacement reactions. • For example,tin would be seen to displace lead from lead chloridebut 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 nitratebut 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.

  3. Reactivity series • The reactivity series of metals is a tool used to predict products in displacement reactions • The reactivity series is a chart of metals listed in order of declining relative reactivity.

  4. The reactivity series of metals is as follows.

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