Hydroxylamine

Hydroxylamine (also known as hydroxyammonia) is an inorganic compound with the chemical formula NH2OH. The compound is in a form of a white hygroscopic crystals. Hydroxylamine is almost always provided and used as an aqueous solution. It is consumed almost exclusively to produce Nylon-6. The oxidation of NH3 to hydroxylamine is a step in biological nitrification.

History
Hydroxylamine was first prepared as hydroxylammonium chloride 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). The coordination complex ZnCl2(NH2OH)2 (zinc dichloride di(hydroxylamine)), known as Crismer's salt, releases hydroxylamine upon heating.

Production
Hydroxylamine or its salts (salts containing hydroxylammonium cations [NH3OH]+) can be produced via several routes but only two are commercially viable. It is also produced naturally as discussed in a section on biochemistry.

From nitric oxide
NH2OH is mainly produced as its sulfuric acid salt, hydroxylammonium hydrogen sulfate ([NH3OH]+[HSO4]−), by the hydrogenation of nitric oxide over platinum catalysts in the presence of sulfuric acid.


 * 2 NO + 3 H2 + 2 H2SO4 → 2 [NH3OH]+[HSO4]−

Raschig process
Another route to NH2OH is the Raschig process: aqueous ammonium nitrite is reduced by HSO3− and SO2 at 0 °C to yield a hydroxylamido-N,N-disulfonate anion:
 * [NH4]+[NO2]− + 2 SO2 + NH3 + H2O → 2 [NH4]+ + N(OH)(SO3−)2

This anion is then hydrolyzed to give hydroxylammonium sulfate [NH3OH]2SO4:
 * N(OH)(SO3−)2 + H2O → NH(OH)(SO3−) + HSO4-
 * 2 NH(OH)(SO3−) + 2 H2O → [NH3OH]2SO4 + SO4(2-)

Solid NH2OH can be collected by treatment with liquid ammonia. Ammonium sulfate, [NH4]2SO4, 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 NO2- + 4 SO2 + 6 H2O + 6 NH3 → 4 SO4(2-) + 6 [NH4]+ + 2 NH2OH

A base then frees the hydroxylamine from the salt:
 * [NH3OH]Cl + NaO(CH2)3CH3 → NH2OH + NaCl + CH3(CH2)3OH

Other methods
Julius Tafel discovered that hydroxylamine hydrochloride or sulfate salts can be produced by electrolytic reduction of nitric acid with HCl or H2SO4 respectively:


 * HNO3 + 3 H2 → NH2OH + 2 H2O

Hydroxylamine can also be produced by the reduction of nitrous acid or potassium nitrite with bisulfite:
 * HNO2 + 2 HSO3− → N(OH)(OSO2−)2 + H2O → NH(OH)(OSO2−) + HSO4−
 * NH(OH)(OSO2−) + [H3O]+ → [NH3OH]+ + HSO4− (100 °C, 1 h)

Hydrochloric acid disproportionates nitromethane to hydroxylamine hydrochloride and carbon monoxide via the hydroxamic acid.

A direct production of hydroxylamine from molecular nitrogen is also possible in water plasma.

Reactions
Hydroxylamine reacts with electrophiles, such as alkylating agents, which can attach to either the oxygen or the nitrogen atoms:
 * R\sX + NH2OH → R\sO\sNH2 + HX
 * R\sX + NH2OH → R\sNH\sOH + HX

The reaction of NH2OH with an aldehyde or ketone produces an oxime.
 * R2C\dO + [NH3OH]Cl → R2C\dN\sOH + NaCl + H2O (in NaOH solution)

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.

Oximes such as dimethylglyoxime are also employed as ligands.

NH2OH reacts with chlorosulfonic acid to give hydroxylamine-O-sulfonic acid:
 * HO\sS(\dO)2\sCl + NH2OH → NH2\sO\sS(\dO)2\sOH + HCl

When heated, hydroxylamine explodes. A detonator can easily explode aqueous solutions concentrated above 80% by weight, and even 50% solution might prove detonable if tested in bulk. In air, the combustion is rapid and complete:
 * 4 NH2OH + O2 → 2 N2 + 6 H2O

Absent air, pure hydroxylamine requires stronger heating and the detonation does not complete combustion:
 * 3 NH2OH → N2 + NH3 + 3 H2O

Partial isomerisation to the amine oxide H3N+\sO− contributes to the high reactivity.

Functional group


Hydroxylamine derivatives substituted in place of the hydroxyl or amine hydrogen are (respectively) called O- or Nhydroxyl&shy;amines. In general Nhydroxyl&shy;amines are more common. Examples are Ntertbutyl&shy;hydroxyl&shy;amine or the glycosidic bond in calicheamicin. N,ODimethyl&shy;hydroxylamine is a precursor to Weinreb amides.

Similarly to amines, one can distinguish hydroxylamines by their degree of substitution: primary, secondary and tertiary. When stored exposed to air for weeks, secondary hydroxylamines degrade to nitrones.

Norganyl&shy;hydroxyl&shy;amines, R\sNH\sOH, where R is an organyl group, can be reduced to amines R\sNH2:
 * R\sNH\sOH (Zn, HCl) → R\sNH2 + ZnO

Synthesis
Amine oxidation with benzoyl peroxide is the most common method to synthesize hydroxylamines. Care must be taken to prevent over-oxidation to a nitrone. Other methods include:
 * Hydrogenation of an oxime
 * Alkylating a precursor hydroxylamine
 * Amine oxide pyrolysis (the Cope reaction)

Uses

 * [[Image:Beckmann-rearangement.png|400px|thumb|left|Conversion of cyclohexanone to caprolactam involving the [[Beckmann rearrangement]].]]

Approximately 95% of hydroxylamine is used in the synthesis of cyclohexanone oxime, a precursor to Nylon 6. The treatment of this oxime with acid induces the Beckmann rearrangement to give caprolactam (3). The latter can then undergo a ring-opening polymerization to yield Nylon 6.

Laboratory 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.

High concentrations of hydroxylamine are used by biologists to introduce mutations by acting as a DNA nucleobase amine-hydroxylating agent. In is thought to mainly act via hydroxylation of cytidine to hydroxyaminocytidine, which is misread as thymidine, thereby inducing C:G to T:A transition mutations. But high concentrations or over-reaction of hydroxylamine in vitro are seemingly able to modify other regions of the DNA & lead to other types of mutations. This may be due to the ability of hydroxylamine to undergo uncontrolled free radical chemistry in the presence of trace metals and oxygen, in fact in the absence of its free radical affects Ernst Freese noted hydroxylamine was unable to induce reversion mutations of its C:G to T:A transition effect & even considered hydroxylamine to be the most specific mutagen known. Practically, it has been largely surpassed by more potent mutagens such as EMS, ENU, or nitrosoguanidine, but being a very small mutagenic compound with high specificity, it found some specialized uses such as mutation of DNA packed within bacteriophage capsids, & mutation of purified DNA in vitro.


 * Celanese synthesis of paracetamol.svg

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 photographic developing solutions. In the semiconductor industry, hydroxylamine is often a component in the "resist stripper", which removes photoresist after lithography.

Hydroxylamine can also be used to better characterize the nature of a post-translational modification onto proteins. For example, poly(ADP-Ribose) chains are sensitive to hydroxylamine when attached to glutamic or aspartic acids but not sensitive when attached to serines. Similarly, Ubiquitin molecules bound to serines or threonines residues are sensitive to hydroxylamine, but those bound to lysine (isopeptide bond) are resistant.

Biochemistry
In biological nitrification, the oxidation of NH3 to hydroxylamine is mediated by the ammonia monooxygenase (AMO). Hydroxylamine oxidoreductase (HAO) further oxidizes hydroxylamine to nitrite.

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

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.

Safety and environmental concerns
Hydroxylamine can be an explosive, with a theoretical decomposition energy of about 5 kJ/g, and aqueous solutions above 80% can be easily detonated by detonator or strong heating under confinement. 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.