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Chapter 20: Problem 1

In the half-cell \(\mathrm{Zn}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Zn}(s),\) what is the electrode and is this half-reaction an anodic reaction or a cathodic reaction?

Short Answer

Expert verified
The electrode is zinc, and the half-reaction is a cathodic reaction.

Step by step solution

01

Identify the Half-Cell Reaction Components

The given half-cell reaction is \(\mathrm{Zn}^{2+}(aq) + 2e^{-} \longrightarrow \mathrm{Zn}(s)\). The components involved are the zinc ion (\(\mathrm{Zn}^{2+}\)) and solid zinc (\(\mathrm{Zn}(s)\)).
02

Determine the Electrode Material

In this half-cell, the reaction shows \(\mathrm{Zn}(s)\) being produced from \(\mathrm{Zn}^{2+}(aq)\). Solid zinc (\(\mathrm{Zn}(s)\)) is the electrode material.
03

Classify the Reaction Type

Determine if the half-cell reaction involves reduction or oxidation. The reaction involves gaining electrons, \(\mathrm{Zn}^{2+}(aq) + 2e^{-} \longrightarrow \mathrm{Zn}(s)\), which is a reduction process. Hence, it is a cathodic reaction.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Electrode Materials
In electrochemistry, the electrode is the material where the half-cell reaction occurs. It serves as a surface for the transfer of electrons. This material can vary based on the reaction it facilitates.

Some common electrode materials include:
  • Metals like zinc, copper, or platinum
  • Graphite (carbon)
  • Mercury
In the given reaction \( \mathrm{Zn}^{2+}(aq) + 2e^{-} \rightarrow \mathrm{Zn}(s) \), the electrode material is solid zinc, \mathrm{Zn}(s)\. This means the surface on which the reaction occurs is composed of zinc metal. Electrode materials must be good conductors of electricity and chemically stable to provide accurate results.
Oxidation and Reduction
Oxidation and reduction are fundamental concepts in electrochemical reactions. Oxidation refers to the loss of electrons, while reduction means the gain of electrons. These reactions always occur together, known as redox reactions.

The mnemonic 'OIL RIG' helps remember:
  • Oxidation Is Loss (of electrons)
  • Reduction Is Gain (of electrons)
In the given half-cell reaction \( \mathrm{Zn}^{2+}(aq) + 2e^{-} \rightarrow \mathrm{Zn}(s) \), the zinc ion (Zn^2+) gains electrons, signifying a reduction process. Therefore, zinc ions are being reduced to solid zinc.
Cathodic Reactions
A cathodic reaction is one where reduction occurs. In an electrochemical cell, the cathode is the electrode where reduction takes place. It attracts cations (positively charged ions) from the electrolyte.

Key features of cathodic reactions include:
  • Gain of electrons
  • Occurs at the cathode
  • Cations move towards the cathode
Analyzing the provided half-cell reaction \( \mathrm{Zn}^{2+}(aq) + 2e^{-} \rightarrow \mathrm{Zn}(s) \), zinc ions (Zn^2+) gain electrons to form solid zinc. Since this process involves the gain of electrons, it classifies as a cathodic reaction.

Understanding these core concepts ensures a solid grasp of electrochemical reactions and the functioning of electrochemical cells.

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Most popular questions from this chapter

In our portable society, batteries have become a necessary power supply. As consumers, we want to purchase batteries that will last as long as possible. Advertisements tell us that some batteries last longer than others, but do they really? Design an investigation to answer the question. Is there a difference in longevity between the major brands of AA batteries? Add a cost- effectiveness component to your design.

Applying Ideas In lead-acid batteries, the battery cannot be recharged indefinitely. Explain why not.

a. What information is provided by the standard reduction potential of a given half-cell? b. What does the relative value of the reduction potential of a given half- reaction indicate about its oxidation-reduction tendency?

Which half reaction would more likely be an oxidation reaction: one with a standard reduction potential of \(-0.42 \mathrm{V},\) or one with a standard reduction potential of \(+0.42 \mathrm{V}\) ?

Distinguish between a voltaic cell and an electrolytic cell in terms of the nature of the reaction involved.
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