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|style="background: #F8EABA; text-align: center;" colspan="2"||Hydroxylamine|
|Molar mass||33.0298 g/mol|
|style="background: #F8EABA; text-align: center;" colspan="2"|| Except where noted otherwise, data are given for|
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references
Hydroxylamine is a reactive chemical with formula NH2OH. It can be considered a hybrid of ammonia and water due to parallels it shares with each. At room temperature pure NH2OH is ordinarily a white, unstable crystalline, hygroscopic compound; however it is almost always encountered as an aqueous solution.
Hydroxylamine tends to be explosive, and the nature of the hazard is not entirely 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.
NH2OH can be synthesized via several routes:
Raschig synthesis: Aqueous ammonium nitrite is reduced by HSO4−/SO2 at 0°C to yield a hydroxylamido-N,N-disulfate anion, which can be hydrolyzed to give (NH3OH)2SO4.
- NH4NO2 + 2SO2 + NH3 + H2O → [NH4]2[N(OH)(OSO2)2]
- [NH4]+2[N(OH)(OSO2)2]2− + H2O → [NH4][NH(OH)(OSO2)] + [NH4][HSO4]
- 2[NH4]+[NH(OH)(OSO2)]− + 2H2O → [NH3(OH)]2[SO4] + [NH4]2[SO4]
Solid NH2OH can be collected by treatment with liquid ammonia. Ammonium sulfate is insoluble in liquid ammonia and is removed by filtration; the liquid ammonia is evaporated to give the desired product.
Another method of synthesis is to make hydroxylammonium salts which can then be converted to hydroxylamine.
- [NH3(OH)]Cl + NaOBu → NH2OH + NaCl + BuOH
- HNO2 + 2 HSO3− → [N(OH)(OSO2)2]2− + 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
NH2OH reacts with chlorosulfuric acid to give hydroxylamine-O-sulfonic acid, a useful reagent for the synthesis of caprolactam.
- HOSO2Cl + NH2OH → NH2OSO2OH + HCl
The hydroxylamine-O-sulfonic acid, which should be stored at 0 °C, can be checked by iodometric titration.
- NH2OH (Zn/HCl) → NH3
- R-NHOH (Zn/HCl) → R-NH2
Hydroxylamine and its salts are commonly used as reducing agents in a myriad of organic and inorganic reactions. They can also act as antioxidants for fatty acids. Some non-chemical uses include removal of hair from animal hides and photography developing solutions.
This has also been used in the past by biologists to introduce random mutations by switching base pairs from A to G, 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.
In the semiconductor industry, hydroxylamine is often a component in the "resist stripper" which removes photoresist after lithography.
Hydroxylamine may explode on heating. 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.
- ↑ Martel, B.; Cassidy, K. (2004). Chemical Risk Analysis: A Practical Handbook, 362, Butterworth–Heinemann.
- ↑ 2.0 2.1 2.2 Greenwood and Earnshaw. Chemistry of the Elements. 2nd Edition. Reed Educational and Professional Publishing Ltd. pp. 431-432. 1997.
- ↑ Japan Science and Technology Agency Failure Knowledge Database.
- ↑ Smith, Michael and Jerry March. March's advanced organic chemistry : reactions, mechanisms, and structure. New York. Wiley. p. 1554. 2001.
- ↑ Patnaik, Pradyot. Handbook of Inorganic Chemicals. McGraw Hill. pp. 385-386. 2003.
- ↑ 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).
- Calorimetric studies of hydroxylamine decomposition
- Chemical company BASF info
- Deadly detonation of hydroxylamine at Concept Sciences facility
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