Domanda del libro di testo
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (b) Pt2+ (aq) → Pt(s)
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Ch.19 - Electrochemistry
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 19, Problema 43a
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (a) O2(g) → OH-(aq)
Guida verificata passo dopo passo1
Identify the oxidation states of the elements in the reactants and products. For O2(g), the oxidation state of oxygen is 0. In OH-(aq), the oxidation state of oxygen is -2.
Determine the change in oxidation state for oxygen. The oxidation state changes from 0 in O2(g) to -2 in OH-(aq).
Recognize that a decrease in oxidation state indicates a gain of electrons, which is characteristic of a reduction process.
Conclude that the half-reaction O2(g) → OH-(aq) is a reduction because oxygen is gaining electrons.
Remember that in a reduction half-reaction, the species undergoing reduction is the one that gains electrons.
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Oxidation and Reduction
Oxidation and reduction are chemical processes that involve the transfer of electrons between species. Oxidation refers to the loss of electrons, resulting in an increase in oxidation state, while reduction involves the gain of electrons, leading to a decrease in oxidation state. These processes are always coupled, meaning that when one species is oxidized, another must be reduced.
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01:53
Oxidation and Reduction Reactions
Half-Reactions
Half-reactions are equations that show either the oxidation or reduction process separately, allowing for a clearer understanding of electron transfer. In a half-reaction, the species being oxidized or reduced is explicitly shown along with the electrons involved. This method is particularly useful in balancing redox reactions and identifying the roles of different reactants.
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01:49First-Order Half-Life
Oxidation States
Oxidation states (or numbers) are a way to keep track of electrons in chemical reactions, particularly in redox processes. Each element in a compound is assigned an oxidation state based on its electron configuration and bonding. Changes in oxidation states during a reaction help determine which species is oxidized and which is reduced, providing insight into the overall reaction mechanism.
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02:42Oxidation Numbers
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