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Single Replacement Reactions

Sophie Calle, 

Take Care of Yourself (2007)

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AP Topic

Topic 4.7 Types of Chemical Reactions

Identify a reaction as acid-base, oxidation-reduction, or precipitation.

    • Oxidation-reduction (redox) reactions involve transfer of one or more electrons between chemical species, as indicated by changes in oxidation numbers of the involved species. Combustion is an important subclass of oxidation-reduction reactions, in which a species reacts with oxygen gas. In the case of hydrocarbons, carbon dioxide and water are products of complete combustion.

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Single Replacement Reactions

Single replacement reactions follow this general equation:

A + BC 🡪 AC + B

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🡪

+

+

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Single Replacement Reactions

In single-replacement reactions, one metal can replace another metal or hydrogen.

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Single Replacement Reactions

Due to differing reactivities, not all metals will replace a metal in a compound.

    • An activity series can be used to predict if reactions will occur.

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This chart (called an

Activity Series) is on

the back of your periodic table.

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Notice that if the above reaction occurs, silver would replace copper. But according to the activity series, silver is less reactive than copper. This means that silver is not reactive enough to replace copper and there is no reaction.

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Predicting Products

  • Identify which two elements would be likely to swap.
  • Consult the activity series to see which element is more reactive.
    • If the free element is more reactive, it will trade places with the element in the compound.
    • If the free element is less reactive, no reaction will take place.

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Single replacement Reactions

Halogens frequently replace other halogens in replacement reactions. See your activity series.

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Practice

Predict whether the following single replacement reactions will occur. If a reaction occurs, write a balanced equation for the reaction.

K + ZnCl2 🡪

This reaction will occur because K is more reactive than Zn.

So, 2 K + ZnCl2 🡪 Zn + 2 KCl

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Practice

1) Cl2(g) + HF(aq) 🡪

Yes, reaction!

Cl2(g) + 2 HF(aq) 🡪 2 HCl(aq) + F2(g)

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2) Fe(s) + Na3PO4(aq) 🡪

No reaction!

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3) Al(s) + Pb(NO3)2(aq) 🡪

Yes, reaction!

3 Al(s) + 2 Pb(NO3)2(aq) 🡪 2 Pb(s) + 3 Al(NO3)3(aq)