The international pictogram for oxidizing chemicals.
Dangerous goods label for oxidizing agents
In chemistry, an oxidizing agent (oxidant, oxidizer) is a substance that has the ability to oxidize other substances — in other words to cause them to lose electrons. 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 that removes one or more electrons from another atom. 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.
Contents
1Electron acceptors
2Atom-transfer reagents
2.1Common oxidizing agents
3Dangerous materials definition
4Common oxidizing agents and their products
5See also
6References
7External links
Electron acceptors
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.[1]
Tetracyanoquinodimethane is an organic electron-acceptor.
Extensive tabulations of ranking the electron accepting properties of various reagents (redox potentials) are available, see Standard electrode potential (data page).
Atom-transfer reagents
In more common usage, an oxidising agent transfers oxygen atoms to a substrate. In this context, the oxidising agent can be called an oxygenation reagent or oxygen-atom transfer (OAT) agent.[2] 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, manganate.
Common oxidizing agents
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
Sulfuric acid (H2SO4)
Peroxydisulfuric acid (H2S2O8)
Peroxymonosulfuric acid (H2SO5)
Chlorite, chlorate, perchlorate, and other analogous halogen compounds
Hypochlorite and other hypohalite compounds, including household bleach (NaClO)
Hexavalent chromium compounds such as chromic and dichromic acids and chromium trioxide, pyridinium chlorochromate (PCC), and chromate/dichromate compounds
Permanganate compounds such as potassium permanganate
Potassium nitrate (KNO3), the oxidizer in black powder
Sodium bismuthate
Dangerous materials definition
The dangerous materials definition of an oxidizing agent is a substance that can cause or contribute to the combustion of other material.[3] By this definition some materials that are classified as oxidising agents by analytical chemists are not classified as oxidising agents in a dangerous materials sense. An example is potassium dichromate, which does not pass the dangerous goods test of an oxidising 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 and Class 5; Division 5.2. Division 5.1 "means a material that may, generally by yielding oxygen, cause or enhance the combustion of other materials." Division 5.1 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 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."[4]
Common oxidizing agents and their products
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 sulphur dioxide
S sulphur (Claus process, ultramarine production, more commonly reducing agent)
Tl(I) thallous compounds, in organic lab scale synthesis
See also
Combustion
Dye
Electrosynthesis
Organic oxidation
Organic redox reaction
Reducing agent
References
^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 0-471-72091-7
^Australian Dangerous Goods Code, 6th Edition
^49 CFR 172.127 General Requirements for Shipments and Packagings; Subpart D
External links
Media related to Oxidizing agents at Wikimedia Commons
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NARA: 10647674
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Fullerton H1, Rogers R, Freedman DL, Zinder SH.
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