Consider the following substances: I2(s), Fe2+(aq), Cr2O72-(aq). Which is the strongest oxidizing agent? Which is the weakest oxidizing agent?

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insert step 1> Identify the oxidation states of the elements in each substance: I2(s), Fe2+(aq), and Cr2O72-(aq).

insert step 2> Recall that an oxidizing agent is a substance that gains electrons and is reduced in a chemical reaction.

insert step 3> Compare the standard reduction potentials (E°) for each substance to determine their ability to act as oxidizing agents.

insert step 4> The substance with the highest standard reduction potential is the strongest oxidizing agent, while the one with the lowest is the weakest.

insert step 5> Rank the substances based on their standard reduction potentials to identify the strongest and weakest oxidizing agents.

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Key Concepts

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

Oxidizing Agents

An oxidizing agent is a substance that gains electrons in a chemical reaction, causing another substance to be oxidized. The strength of an oxidizing agent is determined by its ability to accept electrons; stronger oxidizers have a higher reduction potential. Understanding the relative strengths of different oxidizing agents is crucial for predicting the outcomes of redox reactions.

Standard Reduction Potentials

Standard reduction potentials (E°) are measured values that indicate the tendency of a species to be reduced. These values are typically listed in tables, allowing for easy comparison between different oxidizing agents. A higher E° value corresponds to a stronger oxidizing agent, as it indicates a greater likelihood of gaining electrons.

Half-Reaction Method

The half-reaction method involves separating oxidation and reduction processes to analyze redox reactions. By writing the half-reactions for each species involved, one can determine which species is oxidized and which is reduced. This method is essential for identifying the strongest and weakest oxidizing agents among the given substances.

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Textbook Question

What conditions must be met for a cell potential E to qualify as a standard cell potential E°?

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Textbook Question

Arrange the following oxidizing agents in order of increasing strength under standard-state conditions: Br2(aq), MnO4+(aq), Sn4+(aq).

Textbook Question

Consider the following substances: Fe2+(aq), Sn2+(aq), I-(aq). Identify the strongest reducing agent and the weakest reducing agent.

Textbook Question

Consider the following substances: Fe(s), PbO2(s), H+(aq), Al(s), Ag(s), Cr2O72-(aq).(d) Which substances can be oxidized by Cu2+(aq)? Which can be reduced by H2O2(aq)?

Textbook Question

Consider the following substances: Fe(s), PbO2(s), H+(aq), Al(s), Ag(s), Cr2O72-(aq). (a) Look at the E° values in Appendix D, and classify each substance as an oxidizing agent or a reducing agent.