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Ch.20 - Electrochemistry
All textbooksBrown 14th EditionCh.20 - ElectrochemistryProblem 3b
Chapter 20, Problem 3b

The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.
Molecular view of a process at an electrode in a voltaic cell, showing electron movement.


(b) Is the electrode the anode or cathode?
Close-up of molecular interactions at an electrode in a voltaic cell, illustrating electron transfer.

Verified step by step guidance
1
Identify the process occurring at the electrode by analyzing the molecular view. Notice that atoms are leaving the electrode surface, indicating a loss of material.
Recognize that the loss of atoms from the electrode surface suggests oxidation, as atoms are losing electrons and becoming ions.
Recall that in a voltaic cell, oxidation occurs at the anode. Therefore, the electrode where atoms are leaving must be the anode.
Confirm that the electrode is the anode by noting that oxidation (loss of electrons) is taking place, which is consistent with the behavior of an anode in a voltaic cell.
Conclude that the electrode depicted in the molecular view is the anode, as it is the site of oxidation where atoms are losing electrons and becoming ions.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Voltaic Cell

A voltaic cell, also known as a galvanic cell, is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two electrodes, an anode and a cathode, immersed in an electrolyte solution. The flow of electrons from the anode to the cathode generates an electric current, which can be harnessed for external use.
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The Electrolytic Cell

Anode and Cathode

In a voltaic cell, the anode is the electrode where oxidation occurs, meaning it loses electrons, while the cathode is where reduction takes place, gaining electrons. The anode is typically negative in a voltaic cell, as it donates electrons to the external circuit, while the cathode is positive, attracting electrons. Understanding the roles of these electrodes is crucial for analyzing the cell's operation.
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Electrolytic Cell Components Example

Electron Transfer

Electron transfer is a fundamental process in electrochemistry, where electrons move from one species to another during redox reactions. In the context of a voltaic cell, this transfer occurs between the anode and cathode, facilitating the flow of electric current. The diagram illustrates this movement, highlighting the importance of electron flow in generating electrical energy from chemical reactions.
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Related Practice
Textbook Question

In the Brønsted–Lowry concept of acids and bases, acid– base reactions are viewed as proton-transfer reactions. The stronger the acid, the weaker is its conjugate base. If we were to think of redox reactions in a similar way, what particle would be analogous to the proton? Would strong oxidizing agents be analogous to strong acids or strong bases? [Sections 20.1 and 20.2]

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Textbook Question

The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.

(a) Does the process represent oxidation or reduction?

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Textbook Question

The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.

(c) Why are the atoms in the electrode represented by larger spheres than those in the solution? [Section 20.3]

Textbook Question

Assume that you want to construct a voltaic cell that uses the following half-reactions: A2+1aq2 + 2 e- ¡ A1s2 Ered ° = -0.10 V B2+1aq2 + 2 e- ¡ B1s2 E°red = -1.10 V You begin with the incomplete cell pictured here in which the electrodes are immersed in water.

(a) What additions must you make to the cell for it to generate a standard emf?

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