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Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.20 - ElectrochemistryProblema 13b
Capitolo 20, Problema 13b

(b) On which side of an oxidation half-reaction do the electrons appear?

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Understand that an oxidation half-reaction involves the loss of electrons from a species.
Recall that in a chemical equation, reactants are written on the left side and products on the right side.
In an oxidation half-reaction, the species losing electrons is the reactant.
Electrons are considered products in an oxidation half-reaction because they are released by the reactant.
Therefore, in an oxidation half-reaction, electrons appear on the right side of the equation.

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Oxidation and Reduction

Oxidation and reduction are chemical processes that involve the transfer of electrons between substances. Oxidation refers to the loss of electrons, while reduction involves the gain of electrons. These processes are coupled, meaning that when one substance is oxidized, another is reduced. Understanding these concepts is essential for identifying the roles of reactants in redox reactions.
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Oxidation and Reduction Reactions

Half-Reactions

Half-reactions are a way to represent oxidation and reduction processes separately. In a half-reaction, the species undergoing oxidation or reduction is shown along with the electrons involved in the process. This method simplifies the analysis of redox reactions by allowing chemists to focus on the electron transfer without the complexity of the entire reaction. Each half-reaction can be balanced independently.
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First-Order Half-Life

Electron Placement in Half-Reactions

In an oxidation half-reaction, electrons are shown on the right side of the equation, indicating that they are being produced or released as a result of the oxidation process. This placement reflects the loss of electrons by the oxidized species. Conversely, in a reduction half-reaction, electrons appear on the left side, signifying their gain by the reduced species. Understanding this placement is crucial for correctly interpreting redox reactions.
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Redox Half Reactions Example
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Domanda del libro di testo

Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (b) Chlorine gas is evolved as voltage is applied in the cell. Knowing this, identify the electrolyte.

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Domanda del libro di testo

Indicate whether each of the following statements is true or false: (a) If something is oxidized, it is formally losing electrons.

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Domanda del libro di testo

Indicate whether each of the following statements is true or false: (c) If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction.

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Domanda del libro di testo

Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (a) What is the most common oxidation number for Mg when it is part of a salt?

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Domanda del libro di testo

Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (c) Recall that in an electrolytic cell the anode is given the + sign and the cathode is given the – sign, which is the opposite of what we see in batteries. What half-reaction occurs at the anode in this electrolytic cell?

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