Oxidizing agent

An oxidizing agent or oxidising agent (also called an oxidant, oxidizer or oxidiser) can be defined as either:

1. a chemical compound that readily transfers oxygen atoms, or
2. a substance that gains electrons in a redox chemical reaction

In both cases, the oxidizing agent becomes reduced in the process.

In simple terms:

• The oxidizing agent is reduced.
• The reducing agent is oxidized.
• All atoms in a molecule can be assigned an oxidation number. This number changes when an oxidant acts on a substrate.
• Redox reactions occur when oxidation states of the reactants change.

A mnemonic for differentiating the reactions is "OIL RIG": Oxidation Is Loss, Reduction Is Gain (of electrons) or "LEO the lion says GER" (Lose Electrons: Oxidation, Gain Electrons: Reduction)

Contents 1 Definition 2 Example of oxidation 3 Alternate meanings 4 Common oxidizing agents 5 Common oxidizing agents and their products 6 See also 7 References

Definition

Oxidizing, literally, means converting to oxide. This goes under various names, and can apply to metals (iron convert to iron oxide), nonmetals (sulfur convert to sulfur oxide), and organic matter (mainly carbon and hydrogen convert to carbon oxide and hydrogen oxide). An obvious oxidizer is oxygen, which forms about 20% of air (due to photosynthetic organisms giving off oxygen to the atmosphere).

Later, this was greatly widened to include any time where formal charge is increased (losing electrons), and applies to substances which contain no oxygen (typically halogens and substances rich in these elements, and less commonly sulfur). Paradoxically the action of fluorine upon many oxides is an oxidation even if the reaction results in the removal of the oxygen from a substance. It is thus the generic opposite of reduction, where formal charge is decreased (gaining electrons). With this definition, the "oxide" part of the term is misleading, since oxygen might have no presence in the reaction; no alternative term has yet gained favor.

Many common oxidizers contain oxygen (KClO₄ is KCl "plus" 2 O₂)and can be considered compact storage of oxygen; a given volume of potassium perchlorate contains much more oxygen than the same volume of air. The fuel and oxidizer can be comminuted, which allows the reaction to proceed much faster than if oxygen is brought in from air. Gunpowder is one historically important application.

Example of oxidation

The formation of iron(III) oxide;

4Fe + 3O₂ → 2Fe₂O₃

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:

1. Oxidation Half Reaction: Fe⁰ → Fe³⁺ + 3e⁻
2. Reduction Half Reaction: O₂ + 4e⁻ → 2 O²⁻

Iron III (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)

Alternate meanings

Because the process of oxidation is so widespread (explosives, chemical synthesis, corrosion), the term oxidizing agent has acquired multiple meanings.

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 another 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 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 strict dangerous goods definition of an oxidizing agent are substances that, while in themselves not necessarily combustible, 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 goods sense. An example is potassium dichromate which does not pass the dangerous goods test of an oxidizing agent.

Common oxidizing agents

• Hypochlorite and other hypohalite compounds such as Bleach
• Iodine and other halogens
• Chlorite, chlorate, perchlorate, and other analogous halogen compounds
• Permanganate salts
• Ammonium cerium(IV) nitrate and probably related Cerium(IV) compounds
• Hexavalent chromium compounds such as chromic and dichromic acids and chromium trioxide, Pyridinium chlorochromate (PCC), and chromate/dichromate compounds
• Peroxide compounds
• Tollen's Reagent
• Sulfoxides
• Persulfuric acid
• Ozone
• Osmium tetroxide (OsO₄)
• Nitric acid
• Nitrous oxide (N₂O)

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−, 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

See also

• Reducing agent
• Organic oxidation

References