22: Oxidation-Reduction Reactions

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22.1: Oxygen in Reactions
This page discusses teeth bleaching, a common procedure for discoloration typically done in dental offices with peroxide-based agents. It also notes that whitening toothpastes provide a more accessible, albeit less effective option. The page explains the chemical processes involved—oxidation and reduction—highlighting their interconnection and the role of oxidation in chemical reactions.
22.2: Redox Reactions and Ionic Compounds
This page explains the production of nitric acid from ammonia, emphasizing its use in fertilizers and explosives. It details redox reactions, highlighting the electron transfer, with oxidation as electron loss and reduction as electron gain. Examples include reactions between zinc and sulfur, and sodium and chlorine, with half-reactions illustrated. Key concepts of oxidation, reduction, and half-reactions are defined, while balancing equations will be discussed in subsequent sections.
22.3: Oxidizing and Reducing Agents
This page explains that life on Earth is intertwined with complex processes like photosynthesis, where plants produce oxygen through chlorophyll. It also describes chemical reactions, specifically redox reactions, highlighting the roles of oxidizing agents (which accept electrons) and reducing agents (which donate electrons).
22.4: Molecular Redox Reactions
This page discusses acetone's role as a solvent and its production process, emphasizing its use in plastics and products like nail polish remover. It details the oxidation process in acetone manufacturing and explains molecular redox reactions, highlighting how hydrogen atoms are oxidized and oxygen is reduced in the formation of water, illustrating the principles of oxidation and reduction in chemical reactions.
22.5: Corrosion
This page discusses the obsolescence of old tractors due to corrosion and scarce parts, detailing rust and corrosion as damaging redox processes costing the U.S. economy over $100 billion yearly. It also presents corrosion-resistant metals and prevention methods, including surface and cathodic protection, with zinc's application on steel ships as an example to enhance durability.
22.6: Assigning Oxidation Numbers
This page discusses oxidation numbers, detailing their historical background, including contributions from Lavoisier and Latimer. It outlines six rules for assigning oxidation numbers, such as that free elements have an oxidation number of zero and specific rules for hydrogen, oxygen, and halogens. Examples are included to illustrate the determination of oxidation numbers in compounds, highlighting that different elements can exhibit multiple oxidation states.
22.7: Changes in Oxidation Number in Redox Reactions
This page explains the process of obtaining zinc from zinc carbonate through roasting and subsequent carbon treatment. It describes redox reactions, focusing on the changes in oxidation numbers, highlighting that oxidation involves electron loss and reduction involves electron gain. The page also emphasizes the importance of identifying oxidizing and reducing agents by analyzing these changes in oxidation numbers, summarized with tables for clarity.
22.8: Identifying Reaction Types
This page discusses redox reactions, highlighting that they entail changes in oxidation numbers for two elements—one oxidized and the other reduced. It categorizes single-replacement and combustion reactions as redox reactions, along with most combination and decomposition reactions. In contrast, it notes that double-replacement and acid-base reactions do not qualify as redox reactions due to the absence of electron transfer or changes in oxidation states.
22.9: Balancing Redox Reactions- Oxidation Number Change Method
This page discusses the production and uses of sulfuric acid, emphasizing its role in fertilizers and lead-acid batteries. It covers the process of creating sulfuric acid through the oxidation of sulfur and provides an example of balancing redox reactions with iron (II) oxide and carbon monoxide, using the oxidation-number-change method. The setting for this balancing act is a blast furnace, highlighting the importance of adjusting coefficients to achieve a balanced reaction.
22.10: Balancing Redox Reactions- Half-Reaction Method
This page discusses the Thunder Dolphin amusement ride and explains the half-reaction method for balancing redox equations, using the oxidation of Fe²⁺ to Fe³⁺ by dichromate in acidic solution as an example.
22.11: Half-Reaction Method in Basic Solution
This page discusses cyanide, a toxic industrial byproduct that can cause significant harm. It explains a treatment method involving chlorine gas to convert cyanide into harmless nitrogen. Additionally, it covers the half-reaction method for balancing redox reactions in basic solutions, providing a specific example of iron oxidation by dichromate. The page emphasizes the versatility of this method for various aqueous reactions.

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