Redox Reactions — Electron Transfer Chemistry
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41件の反応
Redox (reduction-oxidation) reactions involve the transfer of electrons between chemical species. Oxidation is the loss of electrons; reduction is the gain of electrons — remembered by the mnemonic OIL RIG (Oxidation Is Loss, Reduction Is Gain). These reactions are among the most important in chemistry, encompassing corrosion, batteries, photosynthesis, respiration, and most metabolic processes. Every reaction where oxidation states change is a redox reaction.
Reaction Mechanism
Electron transfer can be direct (as in a displacement reaction) or indirect (through an external circuit, as in electrochemical cells). Oxidation numbers track electron distribution — an increase indicates oxidation, a decrease indicates reduction. Balancing redox equations requires conserving both mass and charge using the half-reaction method. In acidic solution, H+ and H2O balance oxygen and hydrogen; in basic solution, OH- ions are used. The electrochemical series quantifies the tendency of species to gain or lose electrons, measured as standard electrode potential (E0).
Everyday Examples
Rusting of iron (4Fe + 3O2 + 6H2O -> 4Fe(OH)3) is slow atmospheric redox. Batteries convert chemical energy to electrical energy through controlled redox — lithium-ion batteries power most modern electronics. Bleach (sodium hypochlorite) whitens fabrics by oxidizing chromophore molecules. Breathing is redox: we inhale O2 (the oxidant) and exhale CO2 after glucose is oxidized in our cells.
産業上の重要性
Electroplating uses redox to deposit thin metal coatings — chrome plating on car bumpers, gold plating on electronics connectors. Aluminum production via the Hall-Heroult process is electrolytic reduction of alumina, consuming roughly 3 percent of global electricity. Fuel cells generate electricity by the redox reaction of hydrogen and oxygen, promising cleaner energy for vehicles and power generation.
Safety Note
Strong oxidizing agents (permanganate, dichromate, peroxides) can cause fires when in contact with organic materials. Never mix oxidizers with reducing agents without proper safety controls. Store oxidizing chemicals separately from flammable materials.
Displacement of Hydrogen from Acid by Magnesium
Mg + 2HCl → MgCl₂ + H₂
Magnesium is oxidized from Mg⁰ to Mg²⁺ while hydrogen ions are reduced from H⁺ to H₂. This vigorous redox reaction …
Iron(II) to Iron(III) Oxidation by Oxygen
4Fe²⁺ + O₂ + 4H⁺ → 4Fe³⁺ + 2H₂O
Ferrous ions (Fe²⁺) are oxidized to ferric ions (Fe³⁺) by dissolved oxygen in acidic solution. This reaction is responsible for …
Bleaching with Sodium Hypochlorite
NaClO + dye → NaCl + oxidized dye
Sodium hypochlorite (bleach) oxidizes colored organic molecules by breaking the conjugated double bond systems (chromophores) that absorb visible light. The …
Copper Reduction of Silver Ion
Cu + 2Ag⁺ → Cu²⁺ + 2Ag
Copper metal reduces silver ions to metallic silver while being oxidized to Cu²⁺. Silver deposits on the copper surface in …
Aqua Regia Dissolving Gold
Au + 3HCl + HNO₃ → HAuCl₄ + NO + 2H₂O
Aqua regia (3:1 mixture of HCl and HNO₃) dissolves gold, which is inert to either acid alone. Nitric acid oxidizes …
Cerium(IV) Reduction by Iron(II)
Ce⁴⁺ + Fe²⁺ → Ce³⁺ + Fe³⁺
Cerium(IV) is a strong oxidizing agent that oxidizes iron(II) to iron(III) in a one-electron transfer. This reaction has a 1:1 …
Chlorine Oxidation of Bromide
Cl₂ + 2Br⁻ → 2Cl⁻ + Br₂
Chlorine oxidizes bromide ions to bromine while being reduced to chloride. This halogen displacement demonstrates the trend in oxidizing power: …
Copper Oxidation by Nitric Acid
3Cu + 8HNO₃(dilute) → 3Cu(NO₃)₂ + 2NO + 4H₂O
Dilute nitric acid oxidizes copper to Cu²⁺ while the nitrate ion is reduced to nitric oxide (NO) gas. Unlike HCl …
Hypochlorite Oxidation of Hydrogen Peroxide
NaClO + H₂O₂ → NaCl + H₂O + O₂
Sodium hypochlorite oxidizes hydrogen peroxide to oxygen gas while being reduced to chloride. This vigorous reaction produces rapid oxygen evolution …
Hydrogen Peroxide as Oxidizing Agent (Acidic)
H₂O₂ + 2H⁺ + 2I⁻ → I₂ + 2H₂O
Hydrogen peroxide oxidizes iodide ions to iodine in acidic solution. H₂O₂ acts as the oxidizing agent, being reduced to water. …
Zinc Reduction of Silver Ion
Zn + 2Ag⁺ → Zn²⁺ + 2Ag
Zinc reduces silver ions to metallic silver with a large cell potential of +1.56 V. Zinc is oxidized from 0 …
Reduction of Manganese Dioxide by HCl
MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O
Manganese dioxide oxidizes hydrochloric acid to produce chlorine gas, with Mn(IV) being reduced to Mn(II). Two of the four HCl …
Sulfur Dioxide Reduction of Dichromate
Cr₂O₇²⁻ + 3SO₂ + 2H⁺ → 2Cr³⁺ + 3SO₄²⁻ + H₂O
Sulfur dioxide reduces orange dichromate to green chromium(III) while being oxidized to sulfate. This reaction changes the solution color from …
Reduction of Iron(III) Oxide by Carbon Monoxide
Fe₂O₃ + 3CO → 2Fe + 3CO₂
Carbon monoxide reduces iron(III) oxide to metallic iron in the blast furnace. CO is oxidized to CO₂ while Fe³⁺ is …
Zinc and Copper Sulfate Displacement
Zn + CuSO₄ → ZnSO₄ + Cu
Zinc is oxidized from Zn⁰ to Zn²⁺ while copper is reduced from Cu²⁺ to Cu⁰ in this classic redox displacement …
Copper Displaced by Iron
Fe + Cu²⁺ → Fe²⁺ + Cu
Iron reduces copper(II) ions to metallic copper while being oxidized to iron(II). This reaction proceeds because iron has a more …
Hydrogen Peroxide Disproportionation
2H₂O₂ → 2H₂O + O₂
Hydrogen peroxide simultaneously acts as both oxidizing and reducing agent in this disproportionation reaction. One molecule is reduced to water …
Tin(II) Reduction to Tin(IV)
Sn²⁺ + 2Fe³⁺ → Sn⁴⁺ + 2Fe²⁺
Tin(II) ions reduce iron(III) to iron(II) while being oxidized to tin(IV). Stannous chloride (SnCl₂) is a widely used reducing agent …
Iodine and Sodium Thiosulfate Titration
I₂ + 2Na₂S₂O₃ → Na₂S₄O₆ + 2NaI
Iodine oxidizes thiosulfate to tetrathionate while being reduced to iodide. This is the basis of iodometric titration, one of the …
Thermite Reaction
2Al + Fe₂O₃ → Al₂O₃ + 2Fe
Aluminum reduces iron(III) oxide in this extremely exothermic redox reaction, reaching temperatures above 2500 C. Aluminum is oxidized from Al⁰ …
Fenton's Reaction
Fe²⁺ + H₂O₂ → Fe³⁺ + OH⁻ + OH·
Fenton's reagent generates highly reactive hydroxyl radicals (OH·) from iron(II) and hydrogen peroxide. The hydroxyl radical is one of the …
Chromate-Dichromate Equilibrium
2CrO₄²⁻ + 2H⁺ ⇌ Cr₂O₇²⁻ + H₂O
Chromate (yellow, CrO₄²⁻) converts to dichromate (orange, Cr₂O₇²⁻) in acidic solution and vice versa in basic solution. This pH-dependent equilibrium …
Rusting Prevention by Oil Coating
4Fe + 3O₂ → 2Fe₂O₃ (prevented)
Oil or grease coating prevents iron oxidation by creating a physical barrier that excludes water and oxygen from the iron …
Permanganate Reduction in Basic Solution
2MnO₄⁻ + H₂O + 3e⁻ → 2MnO₂ + 4OH⁻
In basic or neutral solution, permanganate is reduced to manganese dioxide (MnO₂) rather than Mn²⁺. The purple solution produces a …
Oxidation of Ethanol to Acetaldehyde
C₂H₅OH + [O] → CH₃CHO + H₂O
Ethanol is oxidized to acetaldehyde, with the carbon bearing the OH group changing oxidation state from -1 to +1. In …
Vanadium Redox Flow Battery
V²⁺ + VO₂⁺ + 2H⁺ ⇌ V³⁺ + VO²⁺ + H₂O
The vanadium redox flow battery (VRFB) uses four oxidation states of vanadium (V²⁺/V³⁺ and VO²⁺/VO₂⁺) in two electrolyte tanks. During …
Vitamin C as Reducing Agent
C₆H₈O₆ + I₂ → C₆H₆O₆ + 2HI
Ascorbic acid (vitamin C) reduces iodine to iodide while being oxidized to dehydroascorbic acid. The enediol group on ascorbic acid …
Copper Patina Formation (Verdigris)
2Cu + O₂ + H₂O + CO₂ → Cu₂(OH)₂CO₃
Copper slowly oxidizes in moist air containing CO₂ to form basic copper carbonate, the green patina known as verdigris. Copper …
Lead Dioxide and Sulfuric Acid (Lead-Acid Battery Discharge)
PbO₂ + Pb + 2H₂SO₄ → 2PbSO₄ + 2H₂O
During discharge, lead dioxide (cathode, Pb⁴⁺) is reduced to lead sulfate while lead metal (anode, Pb⁰) is oxidized to lead …
Hydrogen Sulfide Oxidation by Chlorine
H₂S + Cl₂ → 2HCl + S
Chlorine oxidizes hydrogen sulfide to elemental sulfur while being reduced to hydrochloric acid. Sulfur is oxidized from -2 to 0. …
Ostwald Process NO Oxidation
4NH₃ + 5O₂ → 4NO + 6H₂O
Ammonia is catalytically oxidized to nitric oxide over a platinum-rhodium gauze catalyst at about 850 C in the Ostwald process. …
Dichromate Oxidation of Ethanol
2Cr₂O₇²⁻ + 3C₂H₅OH + 16H⁺ → 4Cr³⁺ + 3CH₃COOH + 11H₂O
Potassium dichromate oxidizes ethanol to acetic acid in acidic solution. Chromium(VI) is reduced to chromium(III), changing color from orange to …
Permanganate Oxidation of Iron(II)
MnO₄⁻ + 5Fe²⁺ + 8H⁺ → Mn²⁺ + 5Fe³⁺ + 4H₂O
Permanganate ion is a powerful oxidizing agent that oxidizes iron(II) to iron(III) while being reduced from Mn(VII) to Mn(II) in …
Permanganate Oxidation of Oxalic Acid
2MnO₄⁻ + 5C₂O₄²⁻ + 16H⁺ → 2Mn²⁺ + 10CO₂ + 8H₂O
Permanganate oxidizes oxalate to CO₂ while Mn(VII) is reduced to Mn(II). This reaction is autocatalytic: the Mn²⁺ product catalyzes the …
Iron Corrosion (Rusting)
4Fe + 3O₂ + 6H₂O → 4Fe(OH)₃
Iron corrosion is an electrochemical process where iron is oxidized to Fe²⁺/Fe³⁺ at anodic sites while oxygen is reduced at …
Methanol Oxidation to Formaldehyde
2CH₃OH + O₂ → 2HCHO + 2H₂O
Methanol is oxidized to formaldehyde by oxygen over a metal oxide catalyst. The carbon oxidation state changes from -2 in …
Nitric Acid Oxidation of Silver
3Ag + 4HNO₃(dilute) → 3AgNO₃ + NO + 2H₂O
Dilute nitric acid dissolves silver metal, oxidizing it to Ag⁺ while the nitrate is reduced to NO gas. Silver does …
Galvanic Corrosion of Zinc (Sacrificial Anode)
Zn → Zn²⁺ + 2e⁻
Zinc acts as a sacrificial anode when electrically connected to iron or steel, preferentially oxidizing to protect the less reactive …
Contact Process SO₂ Oxidation
2SO₂ + O₂ ⇌ 2SO₃
Sulfur dioxide is oxidized to sulfur trioxide over a vanadium pentoxide catalyst in the contact process for sulfuric acid manufacture. …
Methane Partial Oxidation (Steam Reforming)
CH₄ + H₂O → CO + 3H₂
Methane reacts with steam over a nickel catalyst to produce synthesis gas (syngas), a mixture of carbon monoxide and hydrogen. …
Tollen's Test (Silver Mirror)
RCHO + 2Ag(NH₃)₂⁺ + 2OH⁻ → RCOO⁻ + 2Ag + 4NH₃ + H₂O
Tollens' reagent (silver-ammonia complex) is reduced to metallic silver by aldehydes, producing a silver mirror on the test tube walls. …