Given \(E_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{0}=+0.80 \mathrm{~V} ; \quad E_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\circ}=+0.34 \mathrm{~V}\) \(E_{\mathrm{Ft}^{3}+i \mathrm{Fe}^{2}}=+0.76 \mathrm{~V} ; E^{\circ} \mathrm{Ce}^{4+} / \mathrm{Ce}^{3+}=+1.60 \mathrm{~V}\) Which of the following statements is not correct? (a) \(\mathrm{Fe}^{3+}\) does not oxidise \(\mathrm{Ce}^{3+}\). (b) Cu reduces \(\mathrm{Ag}^{+}\)to \(\mathrm{Ag}\). (c) Ag will reduce \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\). (d) \(\mathrm{Fe}^{3+}\) reduces \(\mathrm{Cu}^{2+}\) to \(\mathrm{Cu}\).

The electrochemical series, also known as the activity series, is a list that ranks chemical elements or ions based on their standard reduction potentials. This list is fundamentally important in the study of electrochemistry, as it helps predict the outcome of redox reactions.

Elements with higher reduction potentials are placed higher in the series and are more likely to be reduced, that is, to gain electrons. Conversely, those with lower reduction potentials appear lower in the series and are more likely to lose electrons and be oxidized. The electrochemical series serves as a guide to determine the direction of electron flow, and thus which substance will act as an oxidizing agent and which will act as a reducing agent.
Electrochemical series can:

Help determine which metals will corrode first in a given environment

Assist in constructing galvanic cells where two different metals can produce electric current

Predict how a metal will behave in electroplating processes

In the given exercise, comparing the standard reduction potentials was essential to predict reactions between different ions, aligning seamlessly with the electrochemical series.

Redox reactions, short for reduction-oxidation reactions, are processes that involve the transfer of electrons between two substances. During these reactions, the oxidation state of molecules, atoms, or ions changes. In every redox reaction, two concurrent processes occur: oxidation (loss of electrons) and reduction (gain of electrons).

Understanding these two processes is critical:

• Oxidation involves an increase in oxidation state and is accompanied by a loss of electrons.
• Reduction involves a decrease in oxidation state and is accompanied by a gain of electrons.

The substances that donate electrons are called reducing agents or reductants, and the substances that accept electrons are known as oxidizing agents or oxidants. An easy way to remember this is by the mnemonic 'LEO says GER' (Lose Electrons Oxidation, Gain Electrons Reduction).

In the textbook problem, identifying the correct redox behavior of ions based on their standard reduction potentials allowed for the correct evaluation of the given statements.

Electron transfer is the heart of all redox reactions. It is this movement of electrons from one species to another that defines whether a substance is being oxidized or reduced. To predict the direction of electron transfer, one must consider the relative standard reduction potentials of the reactants involved.

A species with a higher reduction potential will have a greater tendency to gain electrons and be reduced.

A species with a lower reduction potential will be more inclined to lose electrons and be oxidized.

For instance, in our textbook problem, the direction of electron transfer between ions was inferred based on their standard reduction potentials. This understanding is crucial for mastering redox reactions and is applicable in designing batteries, understanding corrosion, and many other applications in chemistry and industry.