Module 5

Lesson 1.6 - Disproportionation



Key Concepts


A reaction in which the same species is both oxidized and reduced is called disproportionation. For example, consider what happens when two copper(I) ions in a solution collide.


\( \mathrm { Cu^+(aq) + 1e^- \rightarrow Cu(s) } \) reduction half-reaction
\( \mathrm { Cu^+(aq) \rightarrow Cu^{2+}(aq) + 1e^- } \) oxidation half-reaction
\( \mathrm { 2 Cu^+(aq) \rightarrow Cu(s) + Cu^{2+}(aq) } \)    redox reaction
Cu+ is the reducing agent and the oxidizing agent.

Watch



Read "Disproportionation" on pages 577 and 578 of the textbook.

Check Your Understanding


For the following reaction, write the reduction and oxidation half-reactions and identify the reducing agent and the oxidizing agent. Click on the link below to check your work.

  1. \( \mathrm { 2 H_{2}O_{2}(l) \rightarrow 2 H_{2}O(l) + O_{2}(g) } \)

  1. This is an example of disproportionation.
    Process Half-reaction
    Reduction \( \mathrm { O^{1-} + 1e^{-1} \rightarrow O^{-2}(l) } \)
    Oxidation \( \mathrm { 2O^{1-} \rightarrow O_{2}(g) + 2e^{-1} } \)
    Reducing Agent \( \mathrm { H_2O_2(l) } \)
    Oxidizing Agent \( \mathrm { H_2O_2(l) } \)