Always run simultaneously. They are the reaction which changes hydrochloride the oxidation hydrochloride number of an element or ion. These processes are subject to surrender and accept electrons between the participating agents. Particles releasing electrons increase their oxidation number and called the reducer, while receiving particles hydrochloride electrons reduce their oxidation number and are called oxidizing agents. Schematically redox action can be expressed as follows: Reduction reduce oxidation number oxidant + electron reducer, an increase in oxidation number oxidation Since the electron is capable of independent existence, it must be both donor and recipient is present simultaneously in the same reaction system. Therefore, the oxidizing and reducing hydrochloride processes mutually conditional and occur simultaneously. An example would be the reduction of Fe3 + to Fe2 + iodide, is simultaneously oxidized to iodine: hydrochloride 2Fe3 + + 2I- = I2 + Fe2 + redox processes are carried out between jednoatomovými ions. Often, however, there are also cases where these reactions take part in polyatomic ions, or the entire molecule. Examples víceatomového ion which is an anion containing hydrochloride oxygen, permanganate, reducing in an acid medium a manganese salt. MnO4- 8H + + + = 5e- Mn2 + + 4H2O The reactions that can take place in both directions, we say that they are reversible, which is expressed hydrochloride by double arrows. Direction of course depends on what the two redox systems meet. Each redox system is characterized by various efforts electrons check in, or receive, hydrochloride which is quantified so. Redox potential.
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