Chemical hazard symbol for oxidizing agents]] label for oxidizing agents]]
An oxidizing agent (also called an oxidant, oxidizer or oxidiser) can be defined as either:
In both cases, the oxidizing agent becomes reduced in the process.
In simple terms:
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The formation of iron(III) oxide;
In the above equation, the iron (Fe) has an oxidation number of 0 before and 3+ after the reaction. For oxygen (O) the oxidation number began as 0 and decreased to 2−. These changes can be viewed as two "half-reactions" that occur concurrently:
Iron (Fe) has been oxidized because the oxidation number increased and is the reducing agent because it gave electrons to the oxygen (O). Oxygen (O) has been reduced because the oxidation number has decreased and is the oxidizing agent because it took electrons from iron (Fe).
Because the process of oxidation is so widespread (explosives, chemical synthesis, corrosion), the term oxidizing agent has acquired multiple meanings.
In one definition, an oxidizing agent receives - or accepts - electrons from a reagent. In this context, the oxidizing agent is called an electron acceptor. A classic oxidizing agent is the ferrocenium ion [Fe(C5H5)2]+ which accepts an electron to form Fe(C5H5)2. Of great interest to chemists are the details of the electron transfer event, which can be described as inner sphere or outer sphere.
In more colloquial usage, an oxidizing agent transfers oxygen atoms to the substrate. In this context, the oxidizing agent can be called an oxygenation reagent or oxygen-atom transfer agent. Examples include [MnO4]− permanganate, [CrO4]2− chromate, OsO4 osmium tetroxide, and especially [ClO4]− perchlorate. Notice that these species are all oxides, and are in fact polyoxides. In some cases, these oxides can also serve as electron acceptors, as illustrated by the conversion of [MnO4]− to [MnO4]2−, manganate.
The dangerous materials definition of an oxidizing agent is a substance that is not necessarily combustible, but may, generally by yielding oxygen, cause or contribute to the combustion of other material (Australian Dangerous Goods Code, 6th Edition). By this definition some materials that are classified as oxidizing agents by analytical chemists are not classified as oxidizing agents in a dangerous materials sense. An example is potassium dichromate, which does not pass the dangerous goods test of an oxidizing agent.
| Agent | Product(s) |
|---|---|
| O2 oxygen | Various, including the oxides H2O and CO2 |
| O3 ozone | Various, including ketones, aldehydes, and H2O; see ozonolysis |
| F2 fluorine | F− |
| Cl2 chlorine | Cl− |
| Br2 bromine | Br− |
| I2 iodine | I−, I3− |
| OCl− hypochlorite | Cl−, H2O |
| ClO3− chlorate | Cl−, H2O |
| HNO3 nitric acid | NO nitric oxide NO2 nitrogen dioxide |
| Hexavalent chromium CrO3 chromium trioxide CrO42− chromate Cr2O72− dichromate | Cr3+, H2O |
| MnO4− permanganate MnO42− manganate | Mn2+ (acidic) or MnO2 (basic) |
| H2O2, other peroxides | Various, including oxides and H2O |
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Plural |
oxidizing agent (plural oxidizing agents)
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Oxidizing agent can have two meanings. In a more specific sense, it can be a chemical that releases oxygen atoms. For example, potassium chlorate has a chemical formula of KClO3. When it oxidizes a reducing agent, such as powdered aluminum metal, it loses its oxygen to the aluminum and becomes potassium chloride, KCl. Another definition would be: a chemical that accepts electrons from a reducing agent. For example, potassium permanganate has an oxidation state of +7. In acid solution, it gains 5 electrons (e-), becoming a manganese compound with an oxidation state of +2. Most oxidizing agents of the second (electron-accepting) definition have oxygen, but not all. For example, fluorine (F2), the most powerful oxidizing agent, does not have any oxygen in it. When it acts as an oxidizing agent, it gains an electron to transfer from an oxidation state of 0 to an oxidation state of -1.
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