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Hydroxylamine is an inorganic compound with the formula NH₂OH. The pure material is a white, unstable crystalline, hygroscopic compound.^[4] 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).^[5]Hydroxylamine oxidoreductase (HAO) further oxidizes hydroxylamine to nitrite.^[6]

History

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.^[7] 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).^[8][9]

Functional group

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.

Production

NH₂OH can be produced via several routes. The main route is via the Raschig process: aqueous ammonium nitrite is reduced by HSO₃⁻ and SO₂ at 0 °C to yield a hydroxylamido-N,N-disulfonate anion:

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
₃OH)
₂SO
₄ + SO²⁻
₄

Solid NH₂OH can be collected by treatment with liquid ammonia. Ammonium sulfate, (NH
₄)
₂SO
₄, a side-product insoluble in liquid ammonia, is removed by filtration; the liquid ammonia is evaporated to give the desired product.^[4]

The net reaction is:

2NO⁻
₂ + 4SO
₂ + 6H
₂O + 6NH
₃ → 4SO²⁻
₄ + 6NH⁺
₄ + 2NH
₂OH

Hydroxylammonium salts can then be converted to hydroxylamine by neutralization:

(NH₃OH)Cl + NaOBu → NH₂OH + NaCl + BuOH^[4]

Julius Tafel discovered that hydroxylamine hydrochloride or sulfate salts can be produced by electrolytic reduction of nitric acid with HCl or H₂SO₄ respectively:^[10][11]

HNO₃ + 3H₂ → NH₂OH + 2H₂O

Hydroxylamine can also be produced by the reduction of nitrous acid or potassium nitrite with bisulfite:

HNO₂ + 2 HSO₃⁻ → N(OH)(OSO₂)₂²⁻ + H₂O → NH(OH)(OSO₂)⁻ + HSO₄⁻

NH(OH)(OSO₂)⁻ + H₃O⁺ (100 °C/1 h) → NH₃(OH)⁺ + HSO₄⁻

Reactions

Hydroxylamine reacts with electrophiles, such as alkylating agents, which can attach to either the oxygen or the nitrogen atoms:

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.^[12]

Oximes, e.g., dimethylglyoxime, are also employed as ligands.

NH₂OH reacts with chlorosulfonic 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 to prevent decomposition, can be checked by iodometric titration.^{[clarification needed]}

Hydroxylamine (NH₂OH), or hydroxylamines (R-NHOH) can be reduced to amines.^[13]

NH₂OH (Zn/HCl) → NH₃

R-NHOH (Zn/HCl) → R-NH₂

Hydroxylamine explodes with heat:

4 NH₂OH + O₂ → 2 N₂ + 6 H₂O

The high reactivity comes in part from the partial isomerisation of the NH₂OH structure to ammonia oxide (also known as azane oxide), with structure NH₃⁺O⁻.^[14]

Uses

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.

Conversion from cyclohexanone to caprolactam involving the Beckmann Rearrangement can be understood with this scheme.

In the synthesis of nylon 6, cyclohexanone (1) is first converted to its oxime (2); treatment of this oxime with acid induces the Beckmann rearrangement to give caprolactam (3):

The nitrate salt, hydroxylammonium nitrate, is being researched as a rocket propellant, both in water solution as a monopropellant and in its solid form as a solid propellant.

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.

This route also involves the Beckmann Rearrangement, like the conversion from cyclohexanone to caprolactam.

An alternative industrial synthesis of paracetamol developed by Hoechst–Celanese involves the conversion of ketone to a ketoxime with hydroxylamine.

Some non-chemical uses include removal of hair from animal hides and photography developing solutions.^[2] In the semiconductor industry, hydroxylamine is often a component in the "resist stripper", which removes photoresist after lithography.

Safety and Environmental Concerns

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.^[15] It is known, however, that ferrous and ferric iron salts accelerate the decomposition of 50% NH₂OH solutions.^[16] 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.^[17]

Cytochrome P460, an enzyme found in the ammonia-oxidizing bacteria Nitrosomonas europea, can convert hydroxylamine to nitrous oxide, a potent greenhouse gas.^[18]

See also

• Amine

References

Further reading

• Hydroxylamine


• 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).

External links

• Calorimetric studies of hydroxylamine decomposition


• Chemical company BASF info


• MSDS


• Deadly detonation of hydroxylamine at Concept Sciences facility

Hydroxylamine

Names
Preferred IUPAC name Hydroxylamine (only preselected[1])
Other names Azinous acid Aminol Azanol Hydroxyamine Hydroxyazane Hydroxylazane Nitrinous acid
Identifiers
CAS Number	7803-49-8 Y
3D model (JSmol)	Interactive image Interactive image
3DMet	B01184
ChEBI	CHEBI:15429 Y
ChEMBL	ChEMBL1191361 N
ChemSpider	766 Y
ECHA InfoCard	100.029.327
EC Number	232-259-2
Gmelin Reference	478
KEGG	C00192 Y
MeSH	Hydroxylamine
PubChem CID	787
RTECS number	NC2975000
UNII	2FP81O2L9Z Y
InChI InChI=1S/H3NO/c1-2/h2H,1H2 Y Key: AVXURJPOCDRRFD-UHFFFAOYSA-N Y InChI=1/H3NO/c1-2/h2H,1H2 Key: AVXURJPOCDRRFD-UHFFFAOYAD
SMILES NO ON
Properties
Chemical formula	H3NO
Molar mass	7001330300000000000♠33.030 g·mol−1
Appearance	Vivid white, opaque crystals
Density	1.21 g cm−3 (at 20 °C)[2]
Melting point	33 °C (91 °F; 306 K)
Boiling point	58 °C (136 °F; 331 K) /22 mm Hg (decomposes)
log P	−0.758
Acidity (pKa)	6.03 (NH3OH+)
Basicity (pKb)	7.97
Structure
Coordination geometry	Trigonal at N
Molecular shape	Tetrahedral at N
Dipole moment	0.67553 D
Thermochemistry
Heat capacity (C)	46.47 J K−1 mol−1
Std molar entropy (So298)	236.18 J K−1 mol−1
Std enthalpy of formation (ΔfHo298)	−39.9 kJ mol−1
Hazards
Safety data sheet	ICSC 0661
EU classification (DSD) (outdated)	E Xn Xi N
R-phrases (outdated)	R2, R21/22, R37/38, R40, R41, R43, R48/22, R50
S-phrases (outdated)	(S2), S26, S36/37/39, S61
NFPA 704
Flash point	129 °C (264 °F; 402 K)
Autoignition temperature	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)[3]
Related compounds
Related hydroxylammonium salts	Hydroxylammonium chloride Hydroxylammonium nitrate Hydroxylammonium sulfate
Related compounds	Ammonia Hydrazine
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references