Linked from

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

• Oxidation stateRelated: Changes in assigned oxidation states identify which species are oxidized and reduced.

• Nernst equationRelated: Its balanced electron stoichiometry sets the equation’s charge factor.

• MetabolismRelated: Electron transfers let metabolic pathways capture energy and move chemical power between molecules.

• Planetary habitabilityRelated: Redox gradients can supply usable energy to life even where sunlight is unavailable.

• IodineRelated: Iodine readily interconverts between elemental iodine, iodide, and other oxidation states.

• Disulfide bondRelated: Disulfide formation is an oxidation, while bond cleavage is a reduction.

• Faraday's laws of electrolysisRelated: Electrode products form through electron-transfer reactions whose stoichiometry sets the charge required.

• HemeRelated: Heme proteins can transfer electrons by changing the oxidation state of their iron.

• GeochemistryRelated: Redox conditions control the forms and mobility of many elements in Earth materials.

• HalogenRelated: Halogen reactions commonly involve gaining electrons while another substance is oxidized.

• Ore depositRelated: Changes in oxidation state can make dissolved metals precipitate as ore minerals.

• CysteineRelated: Forming a disulfide oxidizes cysteine thiols; breaking it reduces them.

• 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.

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

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

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

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

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

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

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

• 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).

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

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

• Water chemistryRelated: Redox conditions determine the forms of metals, nutrients, and contaminants.

• Etching (chemical machining)Related: Many metal etchants dissolve surfaces through coupled oxidation and reduction.

• Metal oxideRelated: Many oxide-forming and oxide-consuming reactions transfer oxygen through redox chemistry.

• Oxidation zoneRelated: Oxidation of sulfide minerals releases dissolved metals and sulfate.

• Primary cellRelated: Electron transfer at the cell’s electrodes generates its electrical current.

• Rechargeable batteryRelated: Electron transfer at the electrodes underlies both charging and discharging.

• Addition reactionRelated: Many additions change oxidation states, but addition describes connectivity rather than electron balance.

• Chloric acidRelated: Chloric acid’s oxidizing behavior consists of chlorine gaining electrons from reducing agents.

• Manganese noduleRelated: Redox reactions govern the changing forms and precipitation of manganese and iron.

• Microbial metabolismRelated: Electron transfer powers many microbial energy-conserving pathways.

• Oxygen fugacityRelated: Oxygen fugacity sets conditions that favor oxidation or reduction.

• Phosphorus oxidation stateRelated: A change in phosphorus oxidation state tracks its oxidation or reduction.

• VoltammetryRelated: Electrode-driven redox reactions produce the currents recorded in voltammetry.

• Copper(I) oxideRelated: Copper(I) oxide forms and reacts through changes in copper’s oxidation state.

• Gallic acidRelated: Gallic acid’s phenolic groups can donate electrons as they oxidize.

• Iron(III) sulfateRelated: Iron(III) can be reduced to iron(II) by suitable reducing agents.

• John B. GoodenoughRelated: Cathode voltage arises as transition-metal ions change oxidation state during lithium removal and return.

• Native element mineralRelated: Low oxygen availability or reducing conditions can favor elemental forms over oxidized compounds.

• PyrolusiteRelated: Pyrolusite acts as an oxidant when manganese(IV) is reduced.

• Arsenic pentoxideRelated: Arsenic pentoxide can participate in redox chemistry as arsenic changes from its +5 state.

• GlyoxalRelated: Glyoxal can be oxidized to oxalic acid or reduced to glycolaldehyde and related products.

• Hydrogen iodideRelated: Iodide derived from HI readily donates electrons in many reactions.

• Xenon trioxideRelated: XeO₃ can act as an oxidizing agent as xenon is reduced.

• Calcium nitrateRelated: Calcium nitrate’s industrial oxidizer role depends on nitrate participating in redox chemistry.

• Hydrogen selenideRelated: H₂Se can act as a reducing agent as selenium changes oxidation state.