Redox

The most fundamental reactions in chemistry are the redox processes. The term redox process accounts for all processes in which atoms have their oxidation number (oxidation state) changed. This can be a simple redox process, such as the combustion of carbon by oxygen to yield carbon dioxide, it could be the reduction of carbon by hydrogen to yield methane, or it could be the oxidation of sugar in the human body, through a series of very complex electron transfer processes, to yield water and carbon dioxide. The term ''redox'' comes from the two concepts of reduction and oxidation. :''Reduction'' describes the ''uptake'' of an electron by a molecule or atom. :''Oxidation'' describes the ''loss'' of an electron by a molecule or atom. A simple way to remember this is the mnemonic "''LEO the lion goes GER''". LEO means "Lose Electrons, Oxidize" and GER means "Gain Electrons, Reduce". An alternative mnemonic is "''OIL RIG''", "Oxidation Is Loss", "Reduction Is Gain". These two terms go together, because in a chemical reaction, one cannot occur without the other; electrons lost by one compound must be gained by another. ==Oxidizing and Reducing agents== Substances that have the ability to oxidize (Commonwealth English ''oxidise'') other substances are said to be oxidative and are known as oxidizing agents/oxidants or oxidizers. Put in another way, the oxidant removes electrons from the substance. Oxidants are usually chemical substances in high oxidation numbers (e.g. hydrogen peroxide, MnO₄^-, CrO₃, OsO₄) or very electronegative substances that can gain one or two extra electrons by oxidizing a substance (Oxygen, ozone, Fluorine, Chlorine, Bromine). Substances that have the ability to reduce other substances are said to be reductive and are known as reductive agents/reductants or reducers. Put in another way, the reductant transfers electrons to the substance. Reductants in chemistry are very diverse. ''Metal reduction'' - electropositive elemental metals can be used (Li, Na, Mg, Fe, Zn, Al). These metals are very eager to give away electrons. Other kinds of reductants are ''hydride transfer reagents'' (NaBH₄, LiAlH₄), these reagents are widely used in organic chemistry, primarily in the reduction of carbonyl compounds to alcohols. Another useful method is reductions involving hydrogen gas (H₂) with a palladium, platinum or nickel catalyst. These ''catalytic reductions'' are primarily used in the reduction of carbon-carbon double or triple bonds. The chemical way to look at redox processes is that ''the reductant transfers electrons to the oxidant''. Thus, at the end of the reaction, the reductant will have been oxidized and the oxidant will have been reduced. This does not mean however, that the reverse process takes place (because that would lead to status quo), but it does often lead to equilibrium. Chemistry students sometimes remember the nature of oxidation and reduction using the simple mnemonic device "LEO says GER" - the Loss of Electrons is Oxidation, while the Gain of Electrons is Reduction. Another is "OIL RIG" - Oxidation Is Loss, Reduction Is Gain. ==Former meaning (Oxygen/Hydrogen)== Formerly, oxidation simply meant the addition of oxygen or the removing of hydrogen (hence the name oxidation), and reduction was removal of oxygen or the addition of hydrogen. Currently, however, the terms are normally used in the more general sense. ==Examples of redox reactions== A good example is the reaction between hydrogen and fluorine: :H₂ + F₂ → 2HF We can write this overall reaction as two half-reactions: an oxidation reaction: :H₂ → 2H⁺ + 2e^- and a reduction reaction: :F₂ + 2e^- → 2F^- Elements always have an oxidation number of zero. In the first half reaction hydrogen is oxidized from an oxidation number of zero to an oxidation number of +1. In the second half reaction fluorine is reduced from an oxidation number of zero to an oxidation number of −1. When adding the reactions together the electrons cancel: :H₂ → 2H⁺ + ~~2e^-~~ :+ ~~2e^-~~ + F₂ → 2F^- : --------------------- :H₂ + F₂ → 2H⁺ + 2F^- And the ions combine to form hydrogen fluoride: 2H⁺ + 2F^- → 2HF ===Other examples=== *iron(II) oxidizes to iron(III): :Fe²⁺ → Fe³⁺ + e^- *hydrogen peroxide reduces to hydroxide: :H₂O₂ + 2 e^- → 2 OH^- overall equation for the above: :2Fe²⁺ + H₂O₂ + 2H⁺ → 2Fe³⁺ + 2H₂O *denitrification, nitrate reduces to nitrogen: :2NO₃^- + 10e^- + 12 H⁺ → N₂ + 6H₂O *iron(II) oxidizes to iron(III) oxide and oxygen is reduced forming iron(III) oxide (commonly known as rusting or tarnishing): :4Fe + 3O₂ → 2 Fe₂O₃. *Burning of hydrocarbons to produce water, carbon dioxide, some partially oxidized forms, and heat energy. Complete oxidation of materials containing carbon produces carbon dioxide, which is linked to global warming because it absorbs certain wavelengths of infrared light. *In organic chemistry, stepwise oxidation of a hydrocarbon produces water and, successively, an alcohol, an aldehyde or a ketone, carboxylic acid, and then a peroxide. *In inorganic chemistry terms, incompletely oxidized carbon takes the form of carbonate, bicarbonate or carbon monoxide. ==Redox reactions in biology== Much biology energy is stored and released by means of redox reactions. Photosynthesis involves the reduction of carbon dioxide into sugars and the oxidation of water (molecule) into molecular oxygen. The reverse reaction, respiration, oxidizes sugars to produce carbon dioxide and water. As intermediate steps, the reduced carbon compounds are used to reduce Nicotinamide adenine dinucleotide (NAD⁺), which then contributes to the creation of a proton gradient, which drives the synthesis of Adenosine triphosphate (ATP) and is maintained by the reduction of oxygen. In animal cells, mitochondria perform similar functions. The term redox state is often used to describe the balance of NAD⁺/NADH and NADP⁺/NADPH in a biological system such as a cell or organ. The redox state is reflected in the balance of several sets of metabolites (e.g., lactate and pyruvate, beta-hydroxybutyrate and acetoacetate) whose interconversion is dependent on these ratios. An abnormal redox state can develop in a variety of deleterious situations, such as hypoxia, shock, and sepsis. ==See also== * Bioremediation * Calvin cycle * Citric acid cycle * Electrochemical cell * Electrochemistry * Galvanic cell ==External link== * [http://www.shodor.org/UNChem/advanced/redox/redoxcalc.html Redox Reactions Calculator] Electrochemistry

Redox

what are the reaction between a solution containing hydrated ethanedioic acid with sodium enthanedioate and hydroxyl ions? == Merge == Oxidation should be merged into this article!!! Reduction (chemistry) redirects to Oxidation. See Talk:Oxidation#Merge?. User:210.50.105.135 12:17, 5 Nov 2004 (UTC) Oxidation has been merged into this article. User:Brianjd 06:43, 2004 Nov 7 (UTC) == Add titration to this article! == I think this subject article would be better if the topic titration is added to it.

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