|Systematic IUPAC name
|Jmol 3D model||Interactive image
|Molar mass||33.03 g·mol−1|
|Appearance||Vivid white, opaque crystals|
|Density||1.21 g cm−3 (at 20 °C)|
|Melting point||33 °C (91 °F; 306 K)|
|Boiling point||58 °C (136 °F; 331 K) /22 mm Hg (decomposes)|
|Trigonal at N|
|Tetrahedral at N|
|46.47 J K−1 mol−1|
|236.18 J K−1 mol−1|
Std enthalpy of
|−39.9 kJ mol−1|
|Safety data sheet||ICSC 0661|
EU classification (DSD)
|E Xn Xi N|
|R-phrases||R2, R21/22, R37/38, R40, R41, R43, R48/22, R50|
|S-phrases||(S2), S26, S36/37/39, S61|
|Flash point||129 °C (264 °F; 402 K)|
|265 °C (509 °F; 538 K)|
|Lethal dose or concentration (LD, LC):|
LD50 (median dose)
|408 mg/kg (oral, mouse); 59–70 mg/kg (intraperitoneal mouse, rat); 29 mg/kg (subcutaneous, rat)|
Related hydroxylammonium salts
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Hydroxylamine is an inorganic compound with the formula NH2OH. The pure material is a white, unstable crystalline, hygroscopic compound. However, hydroxylamine is almost always provided and used as an aqueous solution. It is used to prepare oximes, an important functional group. It is also an intermediate in biological nitrification. In biological nitrification, the oxidation of NH3 to hydroxylamine is mediated by the enzyme ammonia monooxygenase (AMO). Hydroxylamine oxidoreductase (HAO) further oxidizes hydroxylamine to nitrite.
Hydroxylamine was first prepared as hydroxylamine hydrochloride in 1865 by the German chemist Wilhelm Clemens Lossen (1838-1906); he reacted tin and hydrochloric acid in the presence of ethyl nitrate. It was first prepared in pure form in 1891 by the Dutch chemist Lobry de Bruyn and by the French chemist Léon Maurice Crismer (1858-1944).
Substituted derivatives of hydroxylamine are known. If the hydroxyl hydrogen is substituted, this is called an O-hydroxylamine, if one of the amine hydrogens is substituted, this is called an N-hydroxylamine. Similarly to ordinary amines, one can distinguish primary, secondary and tertiary hydroxylamines, the latter two referring to compounds where two or three hydrogens are substituted, respectively. Examples of compounds containing a hydroxylamine functional group are N-tert-butyl-hydroxylamine or the glycosidic bond in calicheamicin. N,O-Dimethylhydroxylamine is a coupling agent, used to synthesize Weinreb amides.
- NH4NO2 + 2 SO2 + NH3 + H2O → 2 NH4+ + N(OH)(OSO2)22−
This anion is then hydrolyzed to give (NH3OH)2SO4:
- N(OH)(OSO2)22− + H2O → NH(OH)(OSO2)− + HSO4−
- 2 NH(OH)(OSO2)− + 2 H2O → (NH
4 + SO2−
Solid NH2OH can be collected by treatment with liquid ammonia. Ammonium sulfate, (NH
4, a side-product insoluble in liquid ammonia, is removed by filtration; the liquid ammonia is evaporated to give the desired product.
The net reaction is:
2 + 4SO
2 + 6H
2O + 6NH
3 → 4SO2−
4 + 6NH+
4 + 2NH
Hydroxylammonium salts can then be converted to hydroxylamine by neutralization:
- (NH3OH)Cl + NaOBu → NH2OH + NaCl + BuOH
- HNO3 + 3H2 → NH2OH + 2H2O
- HNO2 + 2 HSO3− → N(OH)(OSO2)22− + H2O → NH(OH)(OSO2)− + HSO4−
- NH(OH)(OSO2)− + H3O+ (100 °C/1 h) → NH3(OH)+ + HSO4−
- R-X + NH2OH → R-ONH2 + HX
- R-X + NH2OH → R-NHOH + HX
The reaction of NH2OH with an aldehyde or ketone produces an oxime.
- R2C=O + NH2OH∙HCl , NaOH → R2C=NOH + NaCl + H2O
This reaction is useful in the purification of ketones and aldehydes: if hydroxylamine is added to an aldehyde or ketone in solution, an oxime forms, which generally precipitates from solution; heating the precipitate with an inorganic acid then restores the original aldehyde or ketone.
- HOSO2Cl + NH2OH → NH2OSO2OH + HCl
The hydroxylamine-O-sulfonic acid, which should be stored at 0 °C to prevent decomposition, can be checked by iodometric titration.[clarification needed]
- NH2OH (Zn/HCl) → NH3
- R-NHOH (Zn/HCl) → R-NH2
Hydroxylamine explodes with heat:
- 4 NH2OH + O2 → 2 N2 + 6 H2O
Hydroxylamine and its salts are commonly used as reducing agents in myriad organic and inorganic reactions. They can also act as antioxidants for fatty acids.
This has also been used in the past by biologists to introduce random mutations by switching base pairs from G to A, or from C to T. This is to probe functional areas of genes to elucidate what happens if their functions are broken. Nowadays other mutagens are used. Hydroxylamine can also be used to highly selectively cleave asparaginyl-glycine peptide bonds in peptides and proteins. It also bonds to and permanently disables (poisons) heme-containing enzymes. It is used as an irreversible inhibitor of the oxygen-evolving complex of photosynthesis on account of its similar structure to water.
Some non-chemical uses include removal of hair from animal hides and photography developing solutions. In the semiconductor industry, hydroxylamine is often a component in the "resist stripper", which removes photoresist after lithography.
Hydroxylamine may explode on heating. The nature of the explosive hazard is not well understood. At least two factories dealing in hydroxylamine have been destroyed since 1999 with loss of life. It is known, however, that ferrous and ferric iron salts accelerate the decomposition of 50% NH2OH solutions. Hydroxylamine and its derivatives are more safely handled in the form of salts.
It is an irritant to the respiratory tract, skin, eyes, and other mucous membranes. It may be absorbed through the skin, is harmful if swallowed, and is a possible mutagen.
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- L. Crismer (1891) "Préparation de l'hydroxylamine cristallisée" (Preparation of crystalized hydroxylamine), Bulletin de la Société chimique de Paris, series 3, 6 : 793-795.
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- Japan Science and Technology Agency Failure Knowledge Database.
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- MSDS Sigma-Aldrich
- Walters, Michael A. and Andrew B. Hoem. "Hydroxylamine." e-Encyclopedia of Reagents for Organic Synthesis. 2001.
- Schupf Computational Chemistry Lab
- M. W. Rathke A. A. Millard "Boranes in Functionalization of Olefins to Amines: 3-Pinanamine" Organic Syntheses, Coll. Vol. 6, p. 943; Vol. 58, p. 32. (preparation of hydroxylamine-O-sulfonic acid).