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Understanding Redox Reactions and the Activity Series of Metals

This activity focuses on the activity series of metals, highlighting their ability to oxidize and reduce. Metals are ranked in order of reactivity, where those at the top easily lose electrons (oxidize), and those at the bottom tend to gain electrons (reduce). Practice problems help students arrange metals such as Zn, Cu, and Fe based on their oxidation potential and to determine the spontaneity of various redox reactions. Understanding this series is crucial for predicting the behavior of metals in reactions, particularly in acid solutions.

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Understanding Redox Reactions and the Activity Series of Metals

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  1. Unit Fourteen: Redox Reactions Day Four

  2. Activity Series

  3. Activity Series • Alisting of metals (and hydrogen) in order of decreasing activity, decreasing ability to oxidize, and decreasing tendency to lose electrons • The metals at the top of the series have the greatest tendency to lose electrons, more easily oxidized, and are more reactive. • The metals at the bottom of the series have the greatest tendency to accept electrons, more easily reduced, and are less reactive.

  4. Practice Problems • Arrange Zn, Cu, and Fe in order of decreasing ease to oxidize and write their oxidation half reactions • Zn > Fe > Cu • Zn(s) → • Fe(s) → • Cu(s) → Zn2+(aq) + 2e- Fe2+(aq) + 2e- Cu2+(aq) + 2e-

  5. Sometimes it is more convenient to think in terms of reduction. Write the reduction half reactions in order of best reducer to worst reducer. • → Cu(s) • → Fe(s) • → Zn(s) Cu2+(aq) + 2e- Fe2+(aq) + 2e- Zn2+(aq) + 2e-

  6. Activity Series • Each reaction in the Activity Series is an oxidation half reaction. • The half reactions at the top are most likely to occur in the forward direction. • The half reactions at the bottom are most likely to occur in the reverse direction. • Any half reaction on the list will be spontaneous when paired with the reverse of any half reaction below it. (Like the picture above to the left)

  7. Will the following redox reactions be spontaneous? • Mn(s) + Ni2+(aq) → Mn2+(aq) + Ni(s) • YES • Fe(s) + Mg2+(aq) → Fe2+(aq) + Mg(s) • NO • Fe(s) + Pb2+(aq) → Fe2+(aq) + Pb(s) • YES • Zn(s) + Ni2+(aq) → Zn2+(aq) + Ni(s) • YES • Zn(s) + Ca2+(aq) → Zn2+(aq) + Ca(s) • NO

  8. Metals above H2 on the activity series will dissolve in acids, while metals below H2 will not dissolve in acids.Practice Problems: Will the following metals dissolve in an acid? • Zinc • YES • Silver • NO • Gold • NO • Lead • YES • Copper • NO

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