Nitrite
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Systematic IUPAC name
dioxidonitrate(1−)
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| Other names
nitrite
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| Identifiers | |||
| 14797-65-0 | |||
| 3D model (Jmol) | Interactive image | ||
| ChEBI | CHEBI:16301 | ||
| ChemSpider | 921 | ||
| EC Number | 233-272-6 | ||
| PubChem | 946 | ||
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| Properties | |||
| NO− 2 |
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| Molar mass | 46.01 g·mol−1 | ||
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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| Infobox references | |||
The nitrite ion, which has the chemical formula NO−
2, is a symmetric anion with equal N–O bond lengths. Upon protonation, the unstable weak acid nitrous acid is produced. Nitrite can be oxidized or reduced, with the product somewhat dependent on the oxidizing/reducing agent and its strength. The nitrite ion is an ambidentate ligand, and is known to bond to metal centers in at least five different ways. Nitrite is also important in biochemistry as a source of the potent vasodilator nitric oxide. In organic chemistry the –NO2 group is present in nitrous acid esters and nitro compounds. Nitrites are also used in the food production industry for curing meat.
Nitrate or nitrite (ingested) under conditions that result in endogenous nitrosation has been classified as "Probably carcinogenic to humans" (Group 2A) by International Agency for Research on Cancer (IARC), the specialized cancer agency of the World Health Organization (WHO) of the United Nations.
Sodium nitrite is made industrially by passing "nitrous fumes" into aqueous sodium hydroxide or sodium carbonate solution:
The product is purified by recrystallization. Alkali metal nitrites are thermally stable up to and beyond their melting point (441 °C for KNO2). Ammonium nitrite can be made from dinitrogen trioxide, N2O3, which is formally the anhydride of nitrous acid:
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