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The nitrite ion has the chemical formula NO − 2. Nitrite (mostly sodium nitrite) is widely used throughout chemical and pharmaceutical industries. [1] The nitrite anion is a pervasive intermediate in the nitrogen cycle in nature. The name nitrite also refers to organic compounds having the –ONO group, which are esters of nitrous acid.
Sodium nitrite is an inorganic compound with the chemical formula Na N O 2. It is a white to slightly yellowish crystalline powder that is very soluble in water and is hygroscopic . From an industrial perspective, it is the most important nitrite salt.
The term "amyl nitrite" encompasses several isomers.In older literature, the common non-systematic name amyl was often used for the pentyl group, where the amyl group is a linear or normal (n) alkyl group, and the resulting amyl nitrite would have the structural formula CH 3 (CH 2) 3 CH 2 ONO, also referred to as n-amyl nitrite.
Barium nitrite is a chemical compound, the nitrous acid salt of barium. It has the chemical formula Ba(NO 2) 2. It is a water-soluble yellow powder. It is used to prepare other metal nitrites, such as lithium nitrite.
Chloramphenicol is a rare example of a naturally occurring nitro compound. At least some naturally occurring nitro groups arose by the oxidation of amino groups. [17] 2-Nitrophenol is an aggregation pheromone of ticks. Examples of nitro compounds are rare in nature. 3-Nitropropionic acid found in fungi and plants .
Ammonium nitrite is a chemical compound with the chemical formula [NH 4]NO 2. It is the ammonium salt of nitrous acid. It is composed of ammonium cations [NH 4] + and nitrite anions NO − 2. It is not used in pure isolated form since it is highly unstable and decomposes into water and nitrogen, even at room temperature.
Nitrate is a polyatomic ion with the chemical formula NO − 3. Salts containing this ion are called nitrates. Nitrates are common components of fertilizers and explosives. [1] Almost all inorganic nitrates are soluble in water. An example of an insoluble nitrate is bismuth oxynitrate.
Alkyl nitrites are also used in the formation of oximes with the stronger carbon acids and acid or base catalysis for example in the reaction of 2-butanone, ethyl nitrite and hydrochloric acid forming the oxime, [7] the similar reaction with phenacyl chloride, [8] or the reaction of phenylacetonitrile with methyl nitrite and sodium hydroxide. [9]