Oxidizing agent
An oxidizing agent (also known as an oxidant, oxidizer, electron recipient, or electron acceptor) is a substance in a redox chemical reaction that gains or "accepts"/"receives" an electron from a reducing agent (called the reductant, reducer, or electron donor). In other words, an oxidizer is any substance that oxidizes another substance. The oxidation state, which describes the degree of loss of electrons, of the oxidizer decreases while that of the reductant increases; this is expressed by saying that oxidizers "undergo reduction" and "are reduced" while reducers "undergo oxidation" and "are oxidized". Common oxidizing agents are oxygen, hydrogen peroxide, and the halogens.
In one sense, an oxidizing agent is a chemical species that undergoes a chemical reaction in which it gains one or more electrons. In that sense, it is one component in an oxidation–reduction (redox) reaction. In the second sense, an oxidizing agent is a chemical species that transfers electronegative atoms, usually oxygen, to a substrate. Combustion, many explosives, and organic redox reactions involve atom-transfer reactions.
Electron acceptors
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Electron acceptors participate in electron-transfer reactions. In this context, the oxidizing agent is called an electron acceptor and the reducing agent is called an electron donor. A classic oxidizing agent is the ferrocenium ion Fe(C
5H
5)+
2, which accepts an electron to form Fe(C5H5)2. One of the strongest acceptors commercially available is "Magic blue", the radical cation derived from N(C6H4-4-Br)3.[2]
Extensive tabulations of ranking the electron accepting properties of various reagents (redox potentials) are available, see Standard electrode potential (data page).
Atom-transfer reagents
[edit]In more common usage, an oxidizing agent transfers oxygen atoms to a substrate. In this context, the oxidizing agent can be called an oxygenation reagent or oxygen-atom transfer (OAT) agent.[3] Examples include MnO−
4 (permanganate), CrO2−
4 (chromate), OsO4 (osmium tetroxide), and especially ClO−
4 (perchlorate). Notice that these species are all oxides.
In some cases, these oxides can also serve as electron acceptors, as illustrated by the conversion of MnO−
4 to MnO2−
4,ie permanganate to manganate.
Common oxidizing agents
[edit]- Oxygen (O2)
- Ozone (O3)
- Hydrogen peroxide (H2O2) and other inorganic peroxides, Fenton's reagent
- Fluorine (F2), chlorine (Cl2), and other halogens
- Nitric acid (HNO3) and nitrate compounds such as potassium nitrate (KNO3), the oxidizer in black powder
- Potassium chlorate (KClO3)
- Peroxydisulfuric acid (H2S2O8)
- Peroxymonosulfuric acid (H2SO5)
- Hypochlorite, chlorite, chlorate, perchlorate, and other analogous halogen oxyanions
- Fluorides of chlorine, bromine, and iodine
- Hexavalent chromium compounds such as chromic and dichromic acids and chromium trioxide, pyridinium chlorochromate (PCC), and chromate/dichromate compounds such as Sodium dichromate (Na2Cr2O7)
- Permanganate compounds such as potassium permanganate (KMnO4)
- Sodium perborate ([Na+
]
2·[B
2O
4(OH)
4]2−
) - Nitrous oxide (N2O), Nitrogen dioxide/Dinitrogen tetroxide (NO2 / N2O4)
- Sodium bismuthate (NaBiO3)
- Cerium (IV) compounds such as ceric ammonium nitrate and ceric sulfate
- Lead dioxide (PbO2)
Dangerous materials definition
[edit]The dangerous goods definition of an oxidizing agent is a substance that can cause or contribute to the combustion of other material.[4] 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.
The U.S. Department of Transportation defines oxidizing agents specifically. There are two definitions for oxidizing agents governed under DOT regulations. These two are Class 5; Division 5.1(a)1 and Class 5; Division 5.1(a)2. Division 5.1 "means a material that may, generally by yielding oxygen, cause or enhance the combustion of other materials." Division 5.(a)1 of the DOT code applies to solid oxidizers "if, when tested in accordance with the UN Manual of Tests and Criteria (IBR, see § 171.7 of this subchapter), its mean burning time is less than or equal to the burning time of a 3:7 potassium bromate/cellulose mixture." 5.1(a)2 of the DOT code applies to liquid oxidizers "if, when tested in accordance with the UN Manual of Tests and Criteria, it spontaneously ignites or its mean time for a pressure rise from 690 kPa to 2070 kPa gauge is less than the time of a 1:1 nitric acid (65 percent)/cellulose mixture."[5]
Common oxidizing agents and their products
[edit]| 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−, I− 3 |
| ClO− hypochlorite | Cl−, H2O |
| ClO− 3 chlorate |
Cl−, H2O |
| HNO3 nitric acid | NO nitric oxide NO2 nitrogen dioxide |
| SO2 sulfur dioxide | S sulfur (Claus process, ultramarine production, more commonly reducing agent) |
| Hexavalent chromium CrO3 chromium trioxide CrO2− 4 chromate Cr 2O2− 7 dichromate |
Cr3+, H2O |
| MnO− 4 permanganate MnO2− 4 manganate |
Mn2+ (acidic) or MnO2 (basic) |
| SbF5 antimony pentafluoride | SbF6- hexafluoroantimonate or SbF3 antimony trifluoride |
| PtF6 platinum hexafluoride | PtF6- hexafluoroplatinate |
| RuO 4 ruthenium tetroxide OsO 4 osmium tetroxide |
in organic lab scale synthesis |
| H2O2, other peroxides | Various, including oxides and H2O |
| Tl(III) thallic compounds | Tl(I) thallous compounds, in organic lab scale synthesis |
See also
[edit]- Combustion – Chemical reaction between a fuel and oxygen
- Electron acceptor – Chemical entity capable of accepting electrons
- Electron donor – Chemical entity capable of donating electrons to another entity
- Electrosynthesis – Synthesis of chemical compounds in an electrochemical cell
- Organic oxidation – Redox reaction that takes place with organic compounds
- Organic redox reaction – Redox reaction that takes place with organic compounds
- Reducing agent – Chemical species that donates an electron to another species in a redox reaction
- Solvated electron – Free electron in a solution, often liquid ammonia
References
[edit]- ^ "Metals". Bitesize. BBC. Archived from the original on November 3, 2022.
- ^ N. G. Connelly, W. E. Geiger (1996). "Chemical Redox Agents for Organometallic Chemistry". Chemical Reviews. 96 (2): 877–910. doi:10.1021/cr940053x. PMID 11848774.
- ^ Smith, Michael B.; March, Jerry (2007), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (6th ed.), New York: Wiley-Interscience, ISBN 978-0-471-72091-1
- ^ Australian Dangerous Goods Code, 6th Edition
- ^ 49 CFR 172.127 General Requirements for Shipments and Packagings; Subpart D
External links
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Media related to Oxidizing agents at Wikimedia Commons
