Textbook Question
Do you expect a compound with vanadium in the +2 oxidation state to be an oxidizing or a reducing agent? Explain.
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Ch.21 - Transition Elements and Coordination Chemistry
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 21, Problem 56
Which is the stronger oxidizing agent, Cr2+ or Cu2+? Explain.
Verified step by step guidance1
Step 1: Understand the concept of an oxidizing agent. An oxidizing agent is a substance that gains electrons in a chemical reaction and is reduced in the process. The stronger the oxidizing agent, the more readily it gains electrons.
Step 2: Look up the standard reduction potentials (E°) for the half-reactions of Cr^{2+} and Cu^{2+}. The standard reduction potential indicates the tendency of a species to gain electrons and be reduced.
Step 3: Write the half-reactions for the reduction of Cr^{2+} and Cu^{2+}. For example, Cr^{2+} + 2e^- \(\rightarrow\) Cr and Cu^{2+} + 2e^- \(\rightarrow\) Cu.
Step 4: Compare the standard reduction potentials of the two half-reactions. The species with the higher (more positive) standard reduction potential is the stronger oxidizing agent because it has a greater tendency to gain electrons.
Step 5: Conclude which ion, Cr^{2+} or Cu^{2+}, is the stronger oxidizing agent based on their standard reduction potentials.
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, which is often reflected in its standard reduction potential. A higher reduction potential indicates a stronger oxidizing agent.
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01:01
Oxidizing and Reducing Agents
Standard Reduction Potentials
Standard reduction potentials are measured values that indicate the tendency of a species to be reduced, expressed in volts. These values are determined under standard conditions and can be found in tables. By comparing the standard reduction potentials of Cr<sup>2+</sup> and Cu<sup>2+</sup>, one can determine which ion is the stronger oxidizing agent.
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01:10Standard Reduction Potentials
Electrochemical Series
The electrochemical series is a list of standard reduction potentials for various half-reactions, arranged from strongest to weakest oxidizing agents. This series helps predict the direction of redox reactions and the relative strength of oxidizing and reducing agents. By consulting this series, one can easily compare Cr<sup>2+</sup> and Cu<sup>2+</sup> to identify the stronger oxidizing agent.