Linked from

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

• OxygenNarrower topic: Oxygen often accepts electrons as other substances are oxidized.

• OxidationNarrower topic: It describes the complete electron-transfer process that oxidation alone cannot capture.

• CorrosionNarrower topic: Corrosion of metals commonly couples metal oxidation with reduction of another species.

• Oxidizing agentNarrower topic: Oxidizing agents participate in redox reactions by accepting electrons.

• Reactive oxygen speciesNarrower topic: Reactive oxygen species form and act through electron-transfer chemistry.

• ElectrolysisNarrower topic: Every electrolytic reaction couples oxidation at one electrode with reduction at the other.

• Oxidative stressNarrower topic: Oxidative stress arises from disrupted control of electron-transfer chemistry in cells.

• Oxidative phosphorylationNarrower topic: Electron transfers release energy that respiratory complexes harness for proton pumping.

• Electrochemical cellNarrower topic: Every electrochemical cell couples oxidation to reduction at separate or shared electrodes.

• Fuel cellNarrower topic: Fuel-cell electricity arises from separating the electron-transfer steps of a redox reaction.

• ElectroplatingNarrower topic: Metal ions are reduced to atoms as the plating reaction proceeds.

• Anaerobic respirationNarrower topic: Respiration conserves energy through a sequence of redox reactions.

• AntioxidantNarrower topic: Antioxidant activity is one outcome of electron-transfer chemistry.

• Alcoholic fermentationNarrower topic: Ethanol formation transfers reducing power from NADH to acetaldehyde.

• Galvanic cellNarrower topic: A spontaneous redox reaction supplies the chemical energy converted by the cell.

• Redox potentialNarrower topic: Redox potential quantifies the electron-transfer tendency that drives these reactions.

• Standard electrode potentialNarrower topic: Each electrode potential describes one side of an electron-transfer reaction.

• ElectrochemistryNarrower topic: Electron transfer is the shared chemical basis of electrochemical reactions.

• Electrode potentialNarrower topic: Electrode potential expresses the tendency of a redox half-reaction to proceed.

• Iron oxideNarrower topic: Iron oxidation and oxygen reduction drive the formation of many iron oxides.

• ChemosynthesisNarrower topic: Electron transfer in redox reactions releases the energy chemosynthetic metabolism captures.

• Electron transport chainNarrower topic: Each carrier passes electrons by alternating between oxidized and reduced states.

• Lactate dehydrogenaseNarrower topic: The enzyme catalyzes coupled oxidation and reduction of pyruvate, lactate, NADH, and NAD⁺.

• AnodeNarrower topic: Anodic oxidation is one half of a coupled redox reaction.

• Chemical oxygen demandNarrower topic: COD depends on electron transfer from oxidizable substances to a chemical oxidant.

• NADPHNarrower topic: NADPH's central role is to donate electrons in cellular redox reactions.

• ReductionNarrower topic: Reduction is one half of every redox reaction.

• CathodeNarrower topic: Cathodic reduction is one half of the coupled redox chemistry in a cell.

• Electrochemical seriesNarrower topic: Each entry represents the reduction direction of a redox reaction and its reverse oxidation.

• Flavin adenine dinucleotideNarrower topic: FAD’s coenzyme role is to accept or donate electrons in these reactions.

• Aerobic respirationNarrower topic: Respiration releases fuel energy through linked electron-transfer reactions.

• Ascorbic acidNarrower topic: Ascorbic acid acts as an electron donor in reactions that maintain cellular redox balance.

• BloomeryNarrower topic: Iron reduction and carbon oxidation are coupled reactions within the furnace.

• Chlorine dioxideNarrower topic: Its reactions with microbes and dyes are electron-transfer processes.

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

• 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.

• 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.