NITRITE

A resonance hybrid, showing the N-O bonds in the nitrite ion have a bond order of about 1.5, leaving most of the single negative charge shared between the terminal oxygen atoms

Space-filling model of NO2−

The 'nitrite' ion is NO2−. The anion is bent, being isoelectronic with O3.
A 'nitrite' is either a salt or an ester of nitrous acid.

Contents
Examples
Organic nitrites
External links
References

Examples



★ nitrous acid, HNO2

★ sodium nitrite, NaNO2

★ methyl nitrite, CH3NO2

★ alkyl nitrites, commonly known as poppers
See for a bigger list.
In inorganic chemistry, nitrites are salts of nitrous acid HNO2. They contain the nitrite ion NO2−. Nitrites of the alkali and alkaline earth metals can be synthesized by reacting a mixture of nitrogen monoxide NO and nitrogen dioxide NO2 with the corresponding metal hydroxide solution, as well as through the thermal decomposition of the corresponding nitrate. Other nitrites are available through the reduction of the corresponding nitrates.
The two canonical structures of NO2− which contribute to the resonance hybrid shown at the top of the article

Sodium nitrite is used for the curing meat because it prevents bacterial growth and, in a reaction with the meat's myoglobin, gives the product a desirable dark red color. Because of the toxicity of nitrite (lethal dose of nitrite for humans is about 22 mg per kg body weight), the maximum allowed nitrite concentration in meat products is 200 ppm. Under certain conditions, especially during cooking, nitrites in meat can react with degradation products of amino acids, forming nitrosamines, which are known carcinogens.
Nitrite is detected and analyzed by the '
Griess Reaction', involving the formation of a deep penetration red-color azo dye upon treatment of a NO2−-containing sample with sulfanilic acid and naphthyl-1-amine in the presence of acid.[1]
Nitrite can be reduced to nitric oxide or ammonia by many species of bacteria.

Organic nitrites


Structure of the nitrosooxy functional group

In organic chemistry, nitrites are esters of nitrous acid and contain the nitrosooxy functional group. They possess the general formula RONO, where R is an aryl or alkyl group. Amyl nitrite is used in medicine for the treatment of heart diseases.
Nitrites should not be confused with nitrates, the salts of nitric acid, or with nitro compounds, though they share the formula RNO2. The nitrite anion NO2− should not be confused with the nitronium cation NO2+.

External links



★ Case Studies in Environmental Medicine - Nitrate/Nitrite Toxicity

References


1. ''The 125th Anniversary of the Griess Reagent'' by V. M. Ivanov in Journal of Analytical Chemistry, Vol. 59, No. 10, 2004, pp. 1002 – 1005. Translated from Zhurnal Analiticheskoi Khimii, Vol. 59, No. 10, 2004, pp. 1109 – 1112.


This article provided by Wikipedia. To edit the contents of this article, click here for original source.

psst.. try this: add to faves
©2009 TripAtlas.com