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Redox (shorthand for reduction-oxidation reaction) describes all chemical reactions in which atoms have their oxidation number (oxidation state) changed. This can be either a simple redox process such as the oxidation of carbon to yield carbon dioxide or the reduction of carbon by hydrogen to yield methane (CH4), or it can be a complex process such as the oxidation of sugar in the human body through a series of complex electron transfer processes. The term redox comes from the two concepts of reduction and oxidation. It can be explained in simple terms:
Though sufficient for many purposes, these descriptions are not precisely correct. Oxidation and reduction properly refer to a change in oxidation number — the actual transfer of electrons may never occur. Thus, oxidation is better defined as an increase in oxidation number, and reduction as a decrease in oxidation number. In practice, the transfer of electrons will always cause a change in oxidation number, but there are many reactions that are classed as "redox" even though no electron transfer occurs (such as those involving covalent bonds). Non-redox reactions, which do not involve changes in formal charge, are known as metathesis reactions. The two parts of a redox reaction Rusting iron A bonfire. Combustion consists of redox reactions involving free radicals.From Wikipedia under the
GNU Free Documentation License Reduction-oxidation question? Q. In the reaction MnO4 --> MnO2 (unbalanced) it says that the species in undergoing reduction. What I don't understand is, how can it be said that the "species" is undergoing reduction? Isn't just Mn? Asked by Summer - Sat Jun 13 21:34:12 2009 - - 1 Answers - 0 Comments A. species is just a random posh word for it dont worry reduction is the loss of electrons, oxygen is a 2- ion so it can be seen as an electron, since it is loosing oxygen it means that it is been reduced Answered by Mr_Aplusplus - Sun Jun 14 01:52:44 2009 I have a basic chemistry question? Q. Hi I have a chem quiz tomorrow and currently, we are learning basic redox equations (reduction/oxidation). I am in first year chemistry in high school so these equations aren't too difficult but in my case, my chemistry teacher didn't teach us much so I'm still a bit shaky on calculating oxidation numbers. Can anyone give me a step my step instruction? If you need some problems to exemplify, here: KBr NH4+ [4 is a subscript] If anyone can help me, I'd greatly appreciate it :] Asked by New York - Fri May 18 00:57:55 2007 - - 2 Answers - 0 Comments A. There are a bunch of different rules for calculating the oxidation number. 1) Any species in its natural state (C(s), N(g), Hg (l) etc) will have an oxidation number of 0. 2) Any ion with only one atom (Mg++, H+ etc) will have an oxidation number equal to their charge. For example Mg will have an oxidation number of +2 and H +1) 3) H will (almost) always have a oxidation number of +1 there is a lone exception with metal hydrides but you will not have to worry about these in intro chemistry. 4) F will always have a oxidation number of -1. 5) (Almost) All combined O will have a oxidation number of -2. There are two exceptions to this rule, in peroxides it will be -1 and when with F it can be +. 6) Group 1 atoms will always have an… [cont.] Answered by Bob - Fri May 18 01:23:13 2007 multiple choice: What is the name of the type of chemical reaction batteries employ to produce electricity?
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