Which metal cation is the best oxidizing agent? a. Pb 2+ b. Cr 3+ c. Fe 2+ d. Sn 2+

hey everyone in this example, we need to consider the following metal cat ions and identify which of the following is the best oxidizing agent. So we should recall that the strongest oxidizing agent is going to have the least negative reduction potential. So we're going to refer to our standard table of reduction potentials and we would find that in our textbooks or online. So beginning with the iron three plus carry on, we would see that we have a reduction potential value equal to positive 0.77V. And so we're going to actually write this down below. So we would have four iron three plus a reduction potential value according to our textbook equal to positive 0.77 volts. So moving on to our next pattern, we have nickel two plus, which has a reduction potential value equal to negative 0.23 volts. So we would already rule out nickel because it has a negative reduction potential and we want the least negative reduction potential for our best oxidizing agent. Moving on, we have cobalt two plus as a caravan which has a reduction potential value equal to negative 0.53 volts. Which we can already also rule out because it has a negative reduction potential value. And then lastly we have the reduction potential value for calcium two plus, which according to our textbooks has a value equal to negative two, sorry, equal to negative 2.76 volts. So we would also rule out calcium two plus. And this means that we can say therefore, since 0.77 volts was the most positive reduction potential value for the iron three plus catalon. We would say that the iron three plus Catalan is the best oxidizing agent, and this would be our final answer to complete this example. So I hope that everything I reviewed was clear. If you have any questions, please leave them down below, and I will see everyone in the next practice video.

Ch.20 - Electrochemistry

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Tro 5th Edition

Ch.20 - Electrochemistry

Problem 63

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Chapter 20, Problem 63

Which metal cation is the best oxidizing agent? a. Pb²⁺ b. Cr³⁺ c. Fe²⁺ d. Sn²⁺

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Identify the definition of an oxidizing agent: An oxidizing agent is a substance that gains electrons in a redox reaction, thereby causing another substance to be oxidized.

Understand that the strength of an oxidizing agent is determined by its ability to gain electrons. The more readily a cation gains electrons, the stronger the oxidizing agent it is.

Review the standard reduction potentials for each metal cation given. The cation with the highest positive standard reduction potential is the strongest oxidizing agent because it has the greatest tendency to gain electrons.

Locate the standard reduction potentials for Pb2+, Cr3+, Fe2+, and Sn2+ in a table of standard reduction potentials.

Compare the standard reduction potentials of the cations. The cation with the highest value is the best oxidizing agent among the choices provided.

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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 often determined by its reduction potential; the higher the reduction potential, the stronger the oxidizing agent. In this context, we need to compare the reduction potentials of the given metal cations to identify which one is the best oxidizing agent.

Reduction Potential

Reduction potential is a measure of the tendency of a chemical species to acquire electrons and be reduced. It is typically expressed in volts (V) and can be found in standard reduction potential tables. A more positive reduction potential indicates a greater ability to act as an oxidizing agent. Understanding these values is crucial for determining which cation is the best oxidizer among the options provided.

Metal Cations and Their Oxidation States

Metal cations can exist in various oxidation states, which influence their chemical behavior, including their ability to act as oxidizing or reducing agents. For example, Pb2+, Cr3+, Fe2+, and Sn2+ each have different oxidation states that affect their electron affinity and reactivity. Recognizing the oxidation states and their implications helps in predicting the relative strength of these cations as oxidizing agents.

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Calculate E°_cell for each balanced redox reaction and determine if the reaction is spontaneous as written. b. MnO₂(aq) + 4 H⁺(aq) + Zn(s) → Mn²⁺(aq) + 2H₂O(l) + Zn²⁺(aq) c. Cl₂(g) + 2 F^–(aq) → F₂(g) + 2 Cl^–(aq)

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Calculate E°_cell for each balanced redox reaction and determine if the reaction is spontaneous as written. c. PbO₂(s) + 4 H⁺(aq) + Sn(s) → Pb²⁺(aq) + 2 H₂O(l) + Sn²⁺(aq)

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Calculate the equilibrium constant for each of the reactions in Problem 65.

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Which metal cation is the best oxidizing agent? a. Pb2+ b. Cr3+ c. Fe2+ d. Sn2+

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Key Concepts

Oxidizing Agents

Reduction Potential

Metal Cations and Their Oxidation States

Which metal cation is the best oxidizing agent? a. Pb²⁺ b. Cr³⁺ c. Fe²⁺ d. Sn²⁺