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Oxidizing agent

Chemical compound used to oxidize another substance in a chemical reaction

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

thumb|right|100px|[[Tetracyanoquinodimethane]] is an organic electron-acceptor. 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 , 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.

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 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. Examples include (permanganate), (chromate), OsO4 (osmium tetroxide), and especially (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 to , ie permanganate to 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 such as potassium nitrate (KNO3), the oxidizer in black powder
Potassium chlorate (KClO3)
Xenon difluoride (XeF2)
Xenon tetrafluoride (XeF4)
Xenon hexafluoride (XeF6)
Krypton difluoride (KrF2)
Sulfur (S8)
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 (·)
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

The dangerous goods definition of an oxidizing agent is a substance that can cause or contribute to the combustion of other material. 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."

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−,
ClO− hypochlorite	Cl−, H2O
chlorate	Cl−, H2O
HNO3 nitric acid	NO nitric oxide (Dilute nitric acid)
NO2 nitrogen dioxide (Concentrated nitric acid)
H2SO4(l) Concentrated sulphuric acid	SO2 Sulphur dioxide (non-aqueous)
SO2 sulfur dioxide	S sulfur
(Claus process, ultramarine production, more commonly reducing agent)
Hexavalent chromium
CrO3 chromium trioxide
chromate
dichromate	Cr3+, H2O
permanganate
manganate	Mn2+ (acidic) or
MnO2 (basic)
Ag+ ion Silver ion	Ag (Metal)
SbF5 antimony pentafluoride	SbF6− hexafluoroantimonate or SbF3 antimony trifluoride
PtF6 platinum hexafluoride	PtF6− hexafluoroplatinate
ruthenium tetroxide
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

References

N. G. Connelly, W. E. Geiger. (1996). "Chemical Redox Agents for Organometallic Chemistry". [[Chemical Reviews]].
{{March6th
Australian Dangerous Goods Code, 6th Edition
49 CFR 172.127 General Requirements for Shipments and Packagings; Subpart D

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