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Chapter 17: Problem 16

Identify each of the following half-reactions as oxidation or reduction reactions. \begin{equation} \begin{array}{l}{\text { a. } \mathrm{K}(s) \rightarrow e^{-}+\mathrm{K}^{+}(a q)} \\ {\text { b. } \mathrm{Cu}^{2+}(a q)+e^{-} \longrightarrow \mathrm{Cu}^{+}(a q)} \\ {\text { c. } \mathrm{Br}_{2}(l)+2 e^{-} \rightarrow 2 \mathrm{Br}^{-}(a q)}\end{array} \end{equation}

Short Answer

Expert verified
Reaction a (Potassium) is an oxidation reaction; Reaction b (Copper) and Reaction c (Bromine) are both reduction reactions.

Step by step solution

01

Analyzing Reaction a

In this reaction, Potassium (\(K\)) is losing an electron to become \(K^{+}\). This is an oxidation reaction because an electron is being lost.
02

Analyzing Reaction b

In this reaction, Copper (\(Cu^{2+}\)) is gaining an electron to become \(Cu^{+}\). This is a reduction reaction because an electron is being gained.
03

Analyzing Reaction c

In this reaction, Bromine (\(Br_2\)) is gaining two electrons to become \(2Br^{-}\). This is a reduction reaction because electrons are being gained.

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