Linked from

The 203 pages that link to Redox, each with the reason it gives.

• Metabolic pathwayRelated: Electron transfers power and balance many energy-producing metabolic pathways.

• Organic compoundRelated: Organic reactions often alter carbon’s oxidation state without transferring free electrons.

• OxideNarrower topic: Oxide formation and reduction are linked electron-transfer processes.

• PhotocatalysisRelated: Photogenerated electrons and holes commonly power reduction and oxidation steps.

• PolyphenolRelated: Some polyphenols donate electrons and are converted into oxidized products.

• SmeltingNarrower topic: Smelting reduces metal compounds by transferring oxygen or electrons to a reducing agent.

• Oxygenic photosynthesisNarrower topic: Water loses electrons while electron acceptors gain them in photosynthetic energy conversion.

• Phlogiston theoryNarrower topic: Modern redox chemistry accounts for the paired changes that phlogiston theory described separately.

• Potassium permanganateNarrower topic: Permanganate accepts electrons as it oxidizes other substances.

• Hexavalent chromiumNarrower topic: Electron transfer converts chromium(VI) into lower oxidation states in cells and treatment systems.

• Iron(III) oxideNarrower topic: Iron extraction and thermite both transform Fe₂O₃ through coupled oxidation and reduction.

• Manganese dioxideNarrower topic: MnO₂ functions as an oxidant by accepting electrons and being reduced.

• NADHNarrower topic: NADH’s defining role is to donate electrons in redox reactions.

• Reference electrodeNarrower topic: Reference potentials compare the tendency of redox couples to gain or lose electrons.

• Alessandro VoltaRelated: Electron-transfer reactions provide the chemical basis for current in electrochemical cells.

• DichromateNarrower topic: Dichromate oxidizes other substances by accepting electrons.

• Galvanic corrosionNarrower topic: Metal dissolution and cathodic reactions are paired redox processes.

• PeroxidesNarrower topic: Peroxides participate in oxidation and reduction through their O–O bond.

• Reducing sugarNarrower topic: Reducing sugars act as electron donors in these reactions.

• Sodium thiosulfateNarrower topic: Thiosulfate acts as a reducing agent in several of its practical reactions.

• SulfideNarrower topic: Sulfide’s reduced sulfur can donate electrons and become elemental sulfur or sulfate.

• Alcohol dehydrogenaseNarrower topic: Alcohol oxidation and cofactor reduction are coupled parts of the same redox reaction.

• BiogeochemistryRelated: Changes in oxidation state govern which chemical forms persist in soils, water, and sediments.

• ChemolithotrophyNarrower topic: Chemolithotrophy conserves energy through redox reactions involving inorganic donors.

• Qualitative inorganic analysisRelated: Redox tests identify ions through characteristic changes in oxidation state and color.

• CeriumNarrower topic: Cerium compounds switch between Ce(III) and Ce(IV) through electron-transfer reactions.

• Environmental chemistryRelated: Redox conditions shape the forms and mobility of metals and nutrients.

• IodideRelated: Iodide can lose an electron and become elemental iodine.

• Neil BartlettNarrower topic: The discovery depended on platinum hexafluoride oxidizing xenon.

• PermanganateNarrower topic: Permanganate accepts electrons as manganese is reduced from its +7 oxidation state.

• Xenon hexafluoroplatinateNarrower topic: The synthesis involves electron transfer from xenon to the platinum hexafluoride reagent.

• Albert Szent-GyörgyiNarrower topic: Biological combustion consists largely of controlled oxidation-reduction reactions.

• Alkaline batteryNarrower topic: The battery’s electrical output comes from coupled oxidation and reduction reactions.

• ChlorateNarrower topic: Chlorate’s reactions commonly pair its reduction with oxidation of another substance.

• HypochloriteNarrower topic: Hypochlorite oxidizes many substances while chlorine is reduced.

• Inorganic chemistryRelated: Electron transfer drives many inorganic reactions, from corrosion to metal-ion chemistry.

• Iron(II)Related: Iron(II) can lose an electron to become iron(III).

• Iron(III)Narrower topic: Iron(III) compounds gain or lose electrons through redox reactions.

• Methylene blueNarrower topic: Methylene blue changes between colored and colorless forms as it gains or loses electrons.

• Potassium chlorateNarrower topic: Chlorate’s oxygen-rich chlorine is reduced as other materials are oxidized.

• Pourbaix diagramRelated: Redox equilibria generate potential-dependent boundaries between oxidation states.

• Redox titrationNarrower topic: Electron transfer between titrant and analyte is the defining reaction.

• Reducing agentNarrower topic: A reducing agent is one half of this paired oxidation-and-reduction process.

• Sodium chlorateNarrower topic: Sodium chlorate’s oxidizing action is expressed through electron-transfer reactions.

• Standard hydrogen electrodeNarrower topic: The electrode's potential arises from a reversible redox process.

• Chromium trioxideNarrower topic: Chromium trioxide accepts electrons as it oxidizes other substances.

• Electrolytic cellNarrower topic: Electrolysis separates oxidation and reduction into reactions at different electrodes.

• LaccaseNarrower topic: Laccase oxidizes substrates by removing electrons and transfers them to oxygen.

• Oxalic acidRelated: Oxalic acid can act as a reducing agent and is oxidized to carbon dioxide.

• Permanganate titrationNarrower topic: Permanganate consumes reducing equivalents by accepting electrons from the analyte.