Physical chemistryLesson 2 of 5 in the course Electrochemistry

Galvanic Cells: Electron Flow, Cell Notation, and Redox Reactions

5 flashcards · 5 quiz questions · 5 match pairs · 5 fill-in sentences · English

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Summary

A galvanic cell converts the energy released by a spontaneous redox reaction into electrical energy. This lesson uses the reaction between copper and silver ions to show how separating oxidation and reduction allows electrons to travel through an external circuit.

When a copper wire is immersed directly in a solution containing silver ions, copper atoms are oxidized to copper(II) ions, and silver ions are reduced to solid silver. The solution becomes blue as copper(II) ions form, while silver deposits on the copper wire.

All flashcards

What is a galvanic cell?
An electrochemical cell in which a spontaneous redox reaction produces electrical energy.
What occurs at the anode?
Oxidation occurs at the anode; in a copper–silver cell, copper forms Cu²⁺ ions.
What occurs at the cathode?
Reduction occurs at the cathode; in a copper–silver cell, Ag⁺ ions form solid silver.
What does a salt bridge do in a galvanic cell?
It permits ion movement between half-cells to help maintain charge balance.
What is an inert electrode?
A conductive surface for electron transfer that is not consumed in the cell reaction.

Quiz questions

  1. What type of reaction drives a galvanic cell?Answer: A spontaneous redox reaction.
  2. Why can a platinum electrode be used with the Fe³⁺/Fe²⁺ redox couple in solution?Answer: It provides a conductive surface without being consumed.
  3. What does the double vertical line in cell notation represent?Answer: The salt bridge separating the half-cells.
  4. In cell notation, what do commas separate?Answer: Substances that share the same phase.
  5. In a galvanic cell, which way do electrons travel through the external circuit?Answer: From the anode to the cathode.

Based on Chemistry 2e by Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson, PhD (OpenStax), licensed CC BY 4.0. Adapted into a summary, flashcards and quizzes.

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