Ammonia

Ammonia is an inorganic chemical compound of nitrogen and hydrogen with the formula NH
3. A stable binary hydride and the simplest pnictogen hydride, ammonia is a colourless gas with a distinctive pungent smell.[1] It is widely used in fertilizers, refrigerants, explosives, cleaning agents, and is a precursor for numerous chemicals.[1] Renewable ammonia is considered as an important energy carrier in future energy systems.[2][3] Biologically, it is a common nitrogenous waste, and it contributes significantly to the nutritional needs of terrestrial organisms by serving as a precursor to fertilisers.[4] Around 70% of ammonia produced industrially is used to make fertilisers[5] in various forms and composition, such as urea and diammonium phosphate. Ammonia in pure form is also applied directly into the soil.

Ammonia, either directly or indirectly, is also a building block for the synthesis of many chemicals. In many countries, it is classified as an extremely hazardous substance.[6] Ammonia is toxic, causing damage to cells and tissues. For this reason it is excreted by most animals in the urine, in the form of dissolved urea.

Ammonia is produced biologically in a process called nitrogen fixation, but even more is generated industrially by the Haber process. The process helped revolutionise agriculture by providing cheap fertilizers. The global industrial production of ammonia in 2021 was 235 million tonnes.[7][8] Industrial ammonia is transported by road in tankers, by rail in tank wagons, by sea in gas carriers, or in cylinders.[9] Ammonia occurs in nature and has been detected in the interstellar medium.

Ammonia boils at −33.34 °C (−28.012 °F) at a pressure of one atmosphere, but the liquid can often be handled in the laboratory without external cooling. Household ammonia or ammonium hydroxide is a solution of ammonia in water.

## Contents

* 1 Etymology
* 2 Natural occurrence (abiological)
* 2.1 Atmospheric occurrence
* 2.2 Reactions of atmospheric ammonia
* 3 Properties
* 3.1 Solid
* 3.2 Liquid
* 3.3 Solvent properties
* 3.3.1 Redox properties of liquid ammonia
* 3.4 Structure
* 3.5 Basicity
* 3.6 Self-dissociation
* 3.7 Combustion
* 3.8 Precursor to organonitrogen compounds
* 3.9 Precursor to inorganic nitrogenous compounds
* 3.10 Reactions relevant to ammonia detection
* 4 History
* 5 Applications
* 5.1 Fertilizer
* 5.2 Refrigeration–R717
* 5.3 Antimicrobial agent for food products
* 5.4 Fuel
* 5.4.1 Ships and maritime transport
* 5.4.2 Vehicles, aviation and space
* 5.4.3 Power stations
* 5.5 Other
* 5.5.1 Remediation of gaseous emissions
* 5.5.2 Stimulant
* 5.5.3 Textile
* 5.5.4 Lifting gas
* 5.5.5 Fuming
* 5.5.6 Cleaning agent
* 6 Safety
* 7 Toxicity
* 7.1 Coking wastewater
* 7.2 Aquaculture
* 7.3 Storage information
* 7.4 Laboratory
* 7.5 Laboratory use of anhydrous ammonia (gas or liquid)
* 8 Production
* 8.1 Haber–Bosch
* 8.2 Electrochemical
* 9 Biochemistry and medicine
* 9.1 Biosynthesis
* 9.2 Physiology
* 9.3 Excretion
* 10 Extraterrestrial occurrence
* 10.1 Interstellar space
* 10.1.1 Interstellar formation mechanisms
* 10.1.2 Interstellar destruction mechanisms
* 10.1.3 Single antenna detections
* 10.1.4 Interferometric studies
* 10.1.5 Infrared detections
* 10.1.6 Observations of nearby dark clouds
* 10.1.7 UC HII regions
* 10.1.8 Extragalactic detection
* 11 See also
* 12 References
* 12.1 Works cited
* 13 Further reading
* 14 External links

## Etymology

The name ammonia is derived from the name of the Egyptian deity Amun (Ammon in Greek) since priests and travellers of those temples would burn soils rich in ammonium chloride, which came from animal dung and urine.[1] Pliny, in Book XXXI of his Natural History, refers to a salt named hammoniacum, so called because of the proximity of its source to the Temple of Jupiter Amun (Greek Ἄμμων Ammon) in the Roman province of Cyrenaica.[10] However, the description Pliny gives of the salt does not conform to the properties of ammonium chloride. According to Herbert Hoover's commentary in his English translation of Georgius Agricola's De re metallica, it is likely to have been common sea salt.[11] In any case, that salt ultimately gave ammonia and ammonium compounds their name.

Substances containing ammonia, or those that are similar to it, are called ammoniacal.[12]

## Natural occurrence (abiological)

Ammonia is found throughout the Solar System on Earth, Venus, Mars, Jupiter, Saturn, Uranus, Neptune, and Pluto, among other places: on smaller, icy bodies such as Pluto, ammonia can act as a geologically important antifreeze, as a mixture of water and ammonia can have a melting point as low as −100 °C (−148 °F; 173 K) if the ammonia concentration is high enough and thus allow such bodies to retain internal oceans and active geology at a far lower temperature than would be possible with water alone.[13][14]

### Atmospheric occurrence

Ammonia arises in the atmosphere from both anthropogenic and natural sources. The prevalent source is agriculture at around 80%.[15] This includes fertilizers, urea[15] produced by livestock, and manure in order of contribution. Biomass burning also contributes to atmospheric ammonia, with forest fires and agricultural waste burning emitting roughly the same amount of ammonia into the atmosphere. Ammonia can be emitted naturally from soils and plants when the concentration of ammonia in the soil or plant is higher than the concentration of ammonia in the air. This is known as one part of the bi-directional exchange model.[15]

The dominant sink for atmospheric ammonia is rain. In soil, ammonia-oxidizing archaea (AOA) and ammonia-oxidizing bacteria (AOB) convert ammonia into nitrite.[16] The atmospheric lifetime of ammonia through these processes vary from 12 to 48 hours.[17]

### Reactions of atmospheric ammonia

Atmospheric ammonia gives sulfate-nitrate aerosols through reactions with sulfuric acid and nitric acid, with ammonium sulfate being prominent in this process due to its low vapour pressure.[17][18] These aerosols affect the climate and can impact human health. Atmospheric ammonia can also be oxidised itself by the hydroxyl radical:[17]

NH3 \+ ·OH → ·NH2 \+ H2O

The lifetime of ammonia through oxidisation is much longer than through deposition, with it being as low as 30 days.[17] The amino radical then can be oxidised by multiple compounds to form greenhouse gases, such as nitrous oxide. The oxidation of ammonia may also result in the production of nitric oxide, increasing NOx levels significantly in rural areas where relative levels are typically lower compared to urban areas.[17]

## Properties

Liquid NH3

Solid NH3

Two visible states of NH3

Ammonia is a colourless gas with a characteristically pungent smell. It is lighter than air, its density being 0.589 times that of air. It is easily liquefied due to the strong hydrogen bonding between molecules. Gaseous ammonia turns to a colourless liquid, which boils at −33.1 °C (−27.58 °F), and freezes to colourless crystals[19] at −77.7 °C (−107.86 °F). Little data is available at very high temperatures and pressures, but the liquid-vapor critical point occurs at 405 K and 11.35 MPa.[20]

### Solid

The crystal symmetry is cubic, Pearson symbol cP16, space group P213 No.198, lattice constant 0.5125 nm.[21]

### Liquid

Liquid ammonia possesses strong ionising powers reflecting its high ε of 22 at −35 °C (−31 °F).[22] Liquid ammonia has a very high standard enthalpy change of vapourisation (23.5 kJ/mol;[23] for comparison, water's is 40.65 kJ/mol, methane 8.19 kJ/mol and phosphine 14.6 kJ/mol) and can be transported in pressurised or refrigerated vessels; however, at standard temperature and pressure liquid anhydrous ammonia will vaporise.[24]

### Solvent properties

Ammonia readily dissolves in water. In an aqueous solution, it can be expelled by boiling. The aqueous solution of ammonia is basic, and may be described as aqueous ammonia or ammonium hydroxide.[25] The maximum concentration of ammonia in water (a saturated solution) has a specific gravity of 0.880 and is often known as '.880 ammonia'.[26]

Thermal and physical properties of saturated liquid ammonia[27][28] Temperature
(°C)  | Density
(kg/m3)  | Specific heat
(kJ/(kg·K))  | Kinematic
viscosity
(m2/s)  | Thermal
conductivity
(W/(m·K))  | Thermal
diffusivity
(m2/s)  | Prandtl
Number  | Bulk modulus
(K−1)

|
|
|
|
|
|
|

−50  | 703.69  | 4.463  | 4.35×10−7 | 0.547  | 1.74×10−7 | 2.6  |
−40  | 691.68  | 4.467  | 4.06×10−7 | 0.547  | 1.78×10−7 | 2.28  |
−30  | 679.34  | 4.476  | 3.87×10−7 | 0.549  | 1.80×10−7 | 2.15  |
−20  | 666.69  | 4.509  | 3.81×10−7 | 0.547  | 1.82×10−7 | 2.09  |
−10  | 653.55  | 4.564  | 3.78×10−7 | 0.543  | 1.83×10−7 | 2.07  |
0  | 640.1  | 4.635  | 3.73×10−7 | 0.540  | 1.82×10−7 | 2.05  |
10  | 626.16  | 4.714  | 3.68×10−7 | 0.531  | 1.80×10−7 | 2.04  |
20  | 611.75  | 4.798  | 3.59×10−7 | 0.521  | 1.78×10−7 | 2.02  | 2.45×10−3
30  | 596.37  | 4.89  | 3.49×10−7 | 0.507  | 1.74×10−7 | 2.01  |
40  | 580.99  | 4.999  | 3.40×10−7 | 0.493  | 1.70×10−7 | 2  |
50  | 564.33  | 5.116  | 3.30×10−7 | 0.476  | 1.65×10−7 | 1.99  |
Thermal and physical properties of ammonia (NH
3) at atmospheric pressure[27][28] Temperature
(K)  | Temperature (°C)  | Density
(kg/m3)  | Specific heat
(kJ/(kg·K))  | Dynamic
viscosity
(kg/(m·s))  | Kinematic
viscosity
(m2/s)  | Thermal
conductivity
(W/(m·K))  | Thermal
diffusivity
(m2/s)  | Prandtl
Number

|
|
|
|
|
|
|
|

273  | −0.15  | 0.7929  | 2.177  | 9.35×10−6 | 1.18×10−5 | 0.0220  | 1.31×10−5 | 0.90
323  | 49.85  | 0.6487  | 2.177  | 1.10×10−5 | 1.70×10−5 | 0.0270  | 1.92×10−5 | 0.88
373  | 99.85  | 0.559  | 2.236  | 1.29×10−5 | 1.30×10−5 | 0.0327  | 2.62×10−5 | 0.87
423  | 149.85  | 0.4934  | 2.315  | 1.47×10−5 | 2.97×10−5 | 0.0391  | 3.43×10−5 | 0.87
473  | 199.85  | 0.4405  | 2.395  | 1.65×10−5 | 3.74×10−5 | 0.0467  | 4.42×10−5 | 0.84
480  | 206.85  | 0.4273  | 2.43  | 1.67×10−5 | 3.90×10−5 | 0.0492  | 4.74×10−5 | 0.822
500  | 226.85  | 0.4101  | 2.467  | 1.73×10−5 | 4.22×10−5 | 0.0525  | 5.19×10−5 | 0.813
520  | 246.85  | 0.3942  | 2.504  | 1.80×10−5 | 4.57×10−5 | 0.0545  | 5.52×10−5 | 0.827
540  | 266.85  | 0.3795  | 2.54  | 1.87×10−5 | 4.91×10−5 | 0.0575  | 5.97×10−5 | 0.824
560  | 286.85  | 0.3708  | 2.577  | 1.93×10−5 | 5.20×10−5 | 0.0606  | 6.34×10−5 | 0.827
580  | 306.85  | 0.3533  | 2.613  | 2.00×10−5 | 5.65×10−5 | 0.0638  | 6.91×10−5 | 0.817

Liquid ammonia is a widely studied nonaqueous ionising solvent. Its most conspicuous property is its ability to dissolve alkali metals to form highly coloured, electrically conductive solutions containing solvated electrons. Apart from these remarkable solutions, much of the chemistry in liquid ammonia can be classified by analogy with related reactions in aqueous solutions. Comparison of the physical properties of NH
3 with those of water shows NH
3 has the lower melting point, boiling point, density, viscosity, dielectric constant and electrical conductivity. These differences are attributed at least in part to the weaker hydrogen bonding in NH
3. The ionic self-dissociation constant of liquid NH
3 at −50 °C is about 10−33.

A train carrying anhydrous ammonia | Solubility (g of salt per 100 g liquid NH

|

Ammonium acetate | 253.2
Ammonium nitrate | 389.6
Lithium nitrate | 243.7
Sodium nitrate | 97.6
Potassium nitrate | 10.4
Sodium fluoride | 0.35
Sodium chloride | 157.0
Sodium bromide | 138.0
Sodium iodide | 161.9
Sodium thiocyanate | 205.5

Liquid ammonia is an ionising solvent, although less so than water, and dissolves a range of ionic compounds, including many nitrates, nitrites, cyanides, thiocyanates, metal cyclopentadienyl complexes and metal bis(trimethylsilyl)amides.[27] Most ammonium salts are soluble and act as acids in liquid ammonia solutions. The solubility of halide salts increases from fluoride to iodide. A saturated solution of ammonium nitrate (Divers' solution, named after Edward Divers) contains 0.83 mol solute per mole of ammonia and has a vapour pressure of less than 1 bar even at 25 °C (77 °F). However, few oxyanion salts with other cations dissolve.[29]

Liquid ammonia will dissolve all of the alkali metals and other electropositive metals such as Ca,[30] Sr, Ba, Eu and Yb (also Mg using an electrolytic process[28]). At low concentrations (<0.06 mol/L), deep blue solutions are formed: these contain metal cations and solvated electrons, free electrons that are surrounded by a cage of ammonia molecules.

These solutions are strong reducing agents. At higher concentrations, the solutions are metallic in appearance and in electrical conductivity. At low temperatures, the two types of solution can coexist as immiscible phases.

#### Redox properties of liquid ammonia

Liquid ammonia bottle | E° (V, ammonia)  | E° (V, water)

|
|

Li+
\+ e−
⇌ Li | −2.24  | −3.04

\+ e−
⇌ K | −1.98  | −2.93
Na+
\+ e−
⇌ Na | −1.85  | −2.71
Zn2+ \+ 2 e−
⇌ Zn | −0.53  | −0.76
2 [NH
4]+
\+ 2 e−
⇌ H
2 \+ 2 NH
3 | 0.00  | —
Cu2+ \+ 2 e−
⇌ Cu | +0.43  | +0.34
Ag+
\+ e−
⇌ Ag | +0.83  | +0.80

In practice, both oxidation to dinitrogen and reduction to dihydrogen are slow, although ammonia in principle is labile under both conditions. The thermodynamic stability of liquid ammonia solutions is low because it is easily oxidised to dinitrogen:

2 \+ 6 [NH
4]+
\+ 6 e−
⇌ 8 NH
3 E° = +0.04 V

Although oxidation of liquid ammonia is usually slow, there is still a risk of explosion, particularly if transition metal ions are present as possible catalysts. The stability of ammonia under reducing conditions is evidenced by the slow (hours) decomposition of solutions containing alkali metals. That decomposition give metal amide and dihydrogen:

2 NH
3 \+ 2 M → 2 MNH
2 \+ H

### Structure

Molecular structure of ammonia and its three-dimensional shape. It has a net dipole moment of 1.484 D. Dot and cross structure of ammonia

The ammonia molecule has a trigonal pyramidal shape, as predicted by the valence shell electron pair repulsion theory (VSEPR theory) with an experimentally determined bond angle of 106.7°.[31] The central nitrogen atom has five outer electrons with an additional electron from each hydrogen atom. This gives a total of eight electrons, or four electron pairs that are arranged tetrahedrally. Three of these electron pairs are used as bond pairs, which leaves one lone pair of electrons. The lone pair repels more strongly than bond pairs; therefore, the bond angle is not 109.5°, as expected for a regular tetrahedral arrangement, but 106.7°.[31] This shape gives the molecule a dipole moment and makes it polar. The molecule's polarity, and especially its ability to form hydrogen bonds, makes ammonia highly miscible with water. The lone pair makes ammonia a base, a proton acceptor. Ammonia is moderately basic; a 1.0 M aqueous solution has a pH of 11.6, and if a strong acid is added to such a solution until the solution is neutral (pH = 7), 99.4% of the ammonia molecules are protonated. Temperature and salinity also affect the proportion of ammonium [NH
4]+
. The latter has the shape of a regular tetrahedron and is isoelectronic with methane.

The ammonia molecule readily undergoes nitrogen inversion at room temperature; a useful analogy is an umbrella turning itself inside out in a strong wind. The energy barrier to this inversion is 24.7 kJ/mol, and the resonance frequency is 23.79 GHz, corresponding to microwave radiation of a wavelength of 1.260 cm. The absorption at this frequency was the first microwave spectrum to be observed[32] and was used in the first maser.

### Basicity

One of the most characteristic properties of ammonia is its basicity. Ammonia is considered to be a weak base. It combines with acids to form ammonium salts. Thus, with hydrochloric acid it forms ammonium chloride, with nitric acid, ammonium nitrate, etc. Perfectly dry ammonia gas will not combine with perfectly dry hydrogen chloride gas; moisture is necessary to bring about the reaction.[33][34]

As a demonstration experiment under air with ambient moisture, opened bottles of concentrated ammonia and hydrochloric acid solutions produce a cloud of ammonium chloride, which seems to appear 'out of nothing' as the salt aerosol forms where the two diffusing clouds of reagents meet between the two bottles.

3 \+ HCl → [NH
4]Cl

Although ammonia is well known as a weak base, it can also act as an extremely weak acid. It is a protic substance and is capable of formation of amides (which contain the NH−
2 ion). For example, lithium dissolves in liquid ammonia to give a blue solution (solvated electron) of lithium amide:

2 Li + 2 NH
3 → 2 LiNH
2 \+ H

### Self-dissociation

Like water, liquid ammonia undergoes molecular autoionisation to form its acid and base conjugates:

2 NH
3 ⇌ NH+
4 \+ NH−

Ammonia often functions as a weak base, so it has some buffering ability. Shifts in pH will cause more or fewer ammonium cations (NH+
4) and amide anions (NH−
2) to be present in solution. At standard pressure and temperature,

K = [NH+
4] × [NH−
2] = 10−30.

### Combustion

File:86. Каталитичка оксидација на амонијак.oggHeated Cr2O3 catalyses the combustion of a flask of ammonia.

Ammonia does not burn readily or sustain combustion, except under narrow fuel-to-air mixtures of 15–28% ammonia by volume in air.[35] When mixed with oxygen, it burns with a pale yellowish-green flame. Ignition occurs when chlorine is passed into ammonia, forming nitrogen and hydrogen chloride; if chlorine is present in excess, then the highly explosive nitrogen trichloride (NCl
3) is also formed.

The combustion of ammonia to form nitrogen and water is exothermic:

4 NH
3 \+ 3 O
2 → 2 N
2 \+ 6 H
2O(g), ΔH°r = −1267.20 kJ (or −316.8 kJ/mol if expressed per mol of NH

The standard enthalpy change of combustion, ΔH°c, expressed per mole of ammonia and with condensation of the water formed, is −382.81 kJ/mol. Dinitrogen is the thermodynamic product of combustion: all nitrogen oxides are unstable with respect to N
2 and O
2, which is the principle behind the catalytic converter. Nitrogen oxides can be formed as kinetic products in the presence of appropriate catalysts, a reaction of great industrial importance in the production of nitric acid:

4 NH
3 \+ 5 O
2 → 4 NO + 6 H

A subsequent reaction leads to NO

2 NO + O
2 → 2 NO

The combustion of ammonia in air is very difficult in the absence of a catalyst (such as platinum gauze or warm chromium(III) oxide), due to the relatively low heat of combustion, a lower laminar burning velocity, high auto-ignition temperature, high heat of vapourisation, and a narrow flammability range. However, recent studies have shown that efficient and stable combustion of ammonia can be achieved using swirl combustors, thereby rekindling research interest in ammonia as a fuel for thermal power production.[36] The flammable range of ammonia in dry air is 15.15–27.35% and in 100% relative humidity air is 15.95–26.55%.[37][clarification needed] For studying the kinetics of ammonia combustion, knowledge of a detailed reliable reaction mechanism is required, but this has been challenging to obtain.[38]

### Precursor to organonitrogen compounds

Ammonia is a direct or indirect precursor to most manufactured nitrogen-containing compounds. It is the precursor to nitric acid, which is the source for most N-substituted aromatic compounds.

Amines can be formed by the reaction of ammonia with alkyl halides or, more commonly, with alcohols:

3OH + NH
3 → CH
3NH
2 \+ H

Its ring-opening reaction with ethylene oxide give ethanolamine, diethanolamine, and triethanolamine.

Amides can be prepared by the reaction of ammonia with carboxylic acid and their derivatives. For example, ammonia reacts with formic acid (HCOOH) to yield formamide (HCONH
2) when heated. Acyl chlorides are the most reactive, but the ammonia must be present in at least a twofold excess to neutralise the hydrogen chloride formed. Esters and anhydrides also react with ammonia to form amides. Ammonium salts of carboxylic acids can be dehydrated to amides by heating to 150–200 °C as long as no thermally sensitive groups are present.

* Amino acids, using Strecker amino-acid synthesis
* Acrylonitrile, in the Sohio process

Other organonitrogen compounds include alprazolam, ethanolamine, ethyl carbamate and hexamethylenetetramine.

### Precursor to inorganic nitrogenous compounds

Nitric acid is generated via the Ostwald process by oxidation of ammonia with air over a platinum catalyst at 700–850 °C (1,292–1,562 °F), ≈9 atm. Nitric oxide and nitrogen dioxide are intermediate in this conversion:[39]

3 \+ 2 O
2 → HNO
3 \+ H

Nitric acid is used for the production of fertilisers, explosives, and many organonitrogen compounds.

The hydrogen in ammonia is susceptible to replacement by a myriad substituents. With alkenes and with alcohols, ammonia gives alkylamines.

Ammonia gas reacts with metallic sodium to give sodamide, NaNH

With chlorine, monochloramine is formed.

Pentavalent ammonia is known as λ5-amine, nitrogen pentahydride decomposes spontaneously into trivalent ammonia (λ3-amine) and hydrogen gas at normal conditions. This substance was once investigated as a possible solid rocket fuel in 1966.[40]

Ammonia is also used to make the following compounds:

* Hydrazine, in the Olin Raschig process and the peroxide process
* Hydrogen cyanide, in the BMA process and the Andrussow process
* Hydroxylamine and ammonium carbonate, in the Raschig process
* Urea, in the Bosch–Meiser urea process and in Wöhler synthesis
* ammonium perchlorate, ammonium nitrate, and ammonium bicarbonate

Cisplatin ([Pt(NH

2Cl
2) is a widely used anticancer drug.

Ammonia is a ligand forming metal ammine complexes. For historical reasons, ammonia is named ammine in the nomenclature of coordination compounds. One notable ammine complex is cisplatin (Pt(NH

2Cl
2, a widely used anticancer drug. Ammine complexes of chromium(III) formed the basis of Alfred Werner's revolutionary theory on the structure of coordination compounds. Werner noted only two isomers (fac\- and mer-) of the complex [CrCl
3(NH

3] could be formed, and concluded the ligands must be arranged around the metal ion at the vertices of an octahedron.

Ammonia forms 1:1 adducts with a variety of Lewis acids such as I
2, phenol, and Al(CH

3. Ammonia is a hard base (HSAB theory) and its E & C parameters are EB = 2.31 and CB = 2.04. Its relative donor strength toward a series of acids, versus other Lewis bases, can be illustrated by C-B plots.

### Reactions relevant to ammonia detection

Sulfur sticks are burnt to detect small leaks in industrial ammonia refrigeration systems. In a laboratorial setting, gaseous ammonia can be detected by using concentrated hydrochloric acid or gaseous hydrogen chloride. A dense white fume (which is ammonium chloride vapour) arises from the reaction between ammonia and HCl.[41]

## History

Jabir ibn Hayyan wrote about ammonia in the 9th century This high-pressure ammonia reactor was built in 1921 by BASF in Ludwigshafen and was re-erected on the premises of the University of Karlsruhe in Germany.

The ancient Greek historian Herodotus mentioned that there were outcrops of salt in an area of Libya that was inhabited by a people called the 'Ammonians' (now the Siwa oasis in northwestern Egypt, where salt lakes still exist).[42][43] The Greek geographer Strabo also mentioned the salt from this region. However, the ancient authors Dioscorides, Apicius, Arrian, Synesius, and Aëtius of Amida described this salt as forming clear crystals that could be used for cooking and that were essentially rock salt.[44] Hammoniacus sal appears in the writings of Pliny,[45] although it is not known whether the term is equivalent to the more modern sal ammoniac (ammonium chloride).[19][46][47]

The fermentation of urine by bacteria produces a solution of ammonia; hence fermented urine was used in Classical Antiquity to wash cloth and clothing, to remove hair from hides in preparation for tanning, to serve as a mordant in dyeing cloth, and to remove rust from iron.[48] It was also used by ancient dentists to wash teeth.[49][50][51]

In the form of sal ammoniac (نشادر, nushadir), ammonia was important to the Muslim alchemists. It was mentioned in the Book of Stones, likely written in the 9th century and attributed to Jābir ibn Hayyān.[52] It was also important to the European alchemists of the 13th century, being mentioned by Albertus Magnus.[19] It was also used by dyers in the Middle Ages in the form of fermented urine to alter the colour of vegetable dyes. In the 15th century, Basilius Valentinus showed that ammonia could be obtained by the action of alkalis on sal ammoniac.[53] At a later period, when sal ammoniac was obtained by distilling the hooves and horns of oxen and neutralising the resulting carbonate with hydrochloric acid, the name 'spirit of hartshorn' was applied to ammonia.[19][54]

Gaseous ammonia was first isolated by Joseph Black in 1756 by reacting sal ammoniac (ammonium chloride) with calcined magnesia (magnesium oxide).[55][56] It was isolated again by Peter Woulfe in 1767,[57][58] by Carl Wilhelm Scheele in 1770[59] and by Joseph Priestley in 1773 and was termed by him 'alkaline air'.[19][60] Eleven years later in 1785, Claude Louis Berthollet ascertained its composition.[61][19]

The production of ammonia from nitrogen in the air (and hydrogen) was invented by Fritz Haber and Robert LeRossignol. The patent was sent in 1909 (USPTO Nr 1,202,995) and awarded in 1916. Later, Carl Bosch developed the industrial method for ammonia production (Haber–Bosch process). It was first used on an industrial scale in Germany during World War I,[62] following the allied blockade that cut off the supply of nitrates from Chile. The ammonia was used to produce explosives to sustain war efforts.[63] The Nobel Prize in Chemistry 1918 was awarded to Fritz Haber "for the synthesis of ammonia from its elements".

Before the availability of natural gas, hydrogen as a precursor to ammonia production was produced via the electrolysis of water or using the chloralkali process.

With the advent of the steel industry in the 20th century, ammonia became a byproduct of the production of coking coal.

## Applications

### Fertilizer

In the US as of 2019[update], approximately 88% of ammonia was used as fertilisers either as its salts, solutions or anhydrously.[64] When applied to soil, it helps provide increased yields of crops such as maize and wheat.[65] 30% of agricultural nitrogen applied in the US is in the form of anhydrous ammonia, and worldwide, 110 million tonnes are applied each year.[66] Solutions of ammonia ranging from 16% to 25% are used in the fermentation industry as a source of nitrogen for microorganisms and to adjust pH during fermentation.[67] African countries aim to use their potential to produce renewable ammonia to reduce their dependence on fertiliser imports[68][69][70].

### Refrigeration–R717

Because of ammonia's vapourisation properties, it is a useful refrigerant.[62] It was commonly used before the popularisation of chlorofluorocarbons (Freons). Anhydrous ammonia is widely used in industrial refrigeration applications and hockey rinks because of its high energy efficiency and low cost. It suffers from the disadvantage of toxicity, and requiring corrosion resistant components, which restricts its domestic and small-scale use. Along with its use in modern vapour-compression refrigeration it is used in a mixture along with hydrogen and water in absorption refrigerators. The Kalina cycle, which is of growing importance to geothermal power plants, depends on the wide boiling range of the ammonia–water mixture.

Ammonia coolant is also used in the radiators aboard the International Space Station in loops that are used to regulate the internal temperature and enable temperature-dependent experiments.[71][72] The ammonia is under sufficient pressure to remain liquid throughout the process. Single-phase ammonia cooling systems also serve the power electronics in each pair of solar arrays.

The potential importance of ammonia as a refrigerant has increased with the discovery that vented CFCs and HFCs are potent and stable greenhouse gases.[73]

### Antimicrobial agent for food products

As early as in 1895, it was known that ammonia was 'strongly antiseptic; it requires 1.4 grams per litre to preserve beef tea (broth).'[74] In one study, anhydrous ammonia destroyed 99.999% of zoonotic bacteria in three types of animal feed, but not silage.[75][76] Anhydrous ammonia is currently used commercially to reduce or eliminate microbial contamination of beef.[77][78] Lean finely textured beef (popularly known as 'pink slime') in the beef industry is made from fatty beef trimmings (c. 50–70% fat) by removing the fat using heat and centrifugation, then treating it with ammonia to kill E. coli. The process was deemed effective and safe by the US Department of Agriculture based on a study that found that the treatment reduces E. coli to undetectable levels.[79] There have been safety concerns about the process as well as consumer complaints about the taste and smell of ammonia-treated beef.[80]

### Fuel

Ammoniacal Gas Engine Streetcar in New Orleans drawn by Alfred Waud in 1871

Ammonia has been used as fuel, and is a proposed alternative to fossil fuels and hydrogen, especially in maritime transport. Being liquid at ambient temperature under its own vapour pressure and having high volumetric and gravimetric energy density, ammonia is considered a suitable carrier for hydrogen,[81] and may be cheaper than direct transport of liquid hydrogen.[82]

Compared to hydrogen, ammonia is easier to store. Compared to hydrogen as a fuel, ammonia is much more energy efficient, and could be produced, stored and delivered at a much lower cost than hydrogen, which must be kept compressed or as a cryogenic liquid.[83][84] The raw energy density of liquid ammonia is 11.5 MJ/L,[83] which is about a third that of diesel. Ammonia can also be converted back to hydrogen to be used to power hydrogen fuel cells, or it may be used directly within high-temperature solid oxide direct ammonia fuel cells to provide efficient power sources that do not emit greenhouse gases.[85][86] Ammonia to hydrogen conversion can be achieved through the sodium amide process[87] or the catalytic decomposition of ammonia using solid catalysts.[88]

Ammonia production currently creates 1.8% of global CO
2 emissions. 'Green ammonia' is ammonia produced by using green hydrogen (hydrogen produced by electrolysis with electricity from renewable energy), whereas 'blue ammonia' is ammonia produced using blue hydrogen (hydrogen produced by steam methane reforming) where the carbon dioxide has been captured and stored.[89] In a world first in 2020, Saudi Arabia shipped 40 metric tons of liquid 'blue ammonia' to Japan for use as a fuel.[90] It was produced as a by-product by petrochemical industries, and can be burned without giving off greenhouse gases. Its energy density by volume is nearly double that of liquid hydrogen. If the process of creating it can be scaled up via purely renewable resources, producing green ammonia, it could make a major difference in avoiding climate change.[91]

#### Ships and maritime transport

Green ammonia is considered as a potential fuel for new ships, including future container ships. Ammonia is expected to increase in usage as a fuel source for shipping[92] The IEA forecasts that ammonia will meet approximately 45% of shipping fuel demands by 2050.[93]

In 2020, the companies DSME and MAN Energy Solutions announced the construction of an ammonia-based ship, DSME plans to commercialise it by 2025.[94] The use of ammonia as a potential alternative fuel for aircraft jet engines is also being explored.[95] In addition, hybrid engine configurations for supersonic aviation employing ammonia fuel have been investigated.[96] Japan is implementing a plan to develop ammonia co-firing technology that can increase the use of ammonia in power generation, as part of efforts to assist domestic and other Asian utilities to accelerate their transition to carbon neutrality.[97] In October 2021, the first International Conference on Fuel Ammonia (ICFA2021) was held.[98][99]

In June 2022, IHI Corporation succeeded in reducing greenhouse gases by over 99% during combustion of liquid ammonia in a 2,000-kilowatt-class gas turbine achieving truly CO
2-free power generation.[100] In July 2022, Quad nations of Japan, the US, Australia and India agreed to promote technological development for clean-burning hydrogen and ammonia as fuels at the security grouping's first energy meeting.[101] As of 2022[update], however, significant amounts of NO
x are produced.[102] Nitrous oxide may also be a problem as it is a "greenhouse gas that is known to possess up to 300 times the Global Warming Potential (GWP) of carbon dioxide".[103]

#### Vehicles, aviation and space

The X-15 aircraft used ammonia as one component fuel of its rocket engine

Ammonia engines or ammonia motors, using ammonia as a working fluid, have been proposed and occasionally used.[104] The principle is similar to that used in a fireless locomotive, but with ammonia as the working fluid, instead of steam or compressed air. Ammonia engines were used experimentally in the 19th century by Goldsworthy Gurney in the UK and the St. Charles Streetcar Line in New Orleans in the 1870s and 1880s,[105] and during World War II ammonia was used to power buses in Belgium.[106]

Ammonia is sometimes proposed as a practical alternative to fossil fuel for internal combustion engines.[106][107][108][109] However, ammonia cannot be easily used in existing Otto cycle engines because of its very narrow flammability range. Despite this, several tests have been run.[110][111][112] Its high octane rating of 120[113] and low flame temperature[114] allows the use of high compression ratios without a penalty of high NO
x production. Since ammonia contains no carbon, its combustion cannot produce carbon dioxide, carbon monoxide, hydrocarbons, or soot. At high temperature and in the presence of a suitable catalyst, ammonia decomposes into its constituent elements.[115] Decomposition of ammonia is a slightly endothermic process requiring 23 kJ/mol (5.5 kcal/mol) of ammonia, and yields hydrogen and nitrogen gas.

Rocket engines have also been fuelled by ammonia. The Reaction Motors XLR99 rocket engine that powered the X-15 hypersonic research aircraft used liquid ammonia. Although not as powerful as other fuels, it left no soot in the reusable rocket engine, and its density approximately matches the density of the oxidiser, liquid oxygen, which simplified the aircraft's design. Liquid ammonia is also an attractive alternative to liquid hydrogen as a nuclear-thermal rocket propellant, offering increased thrust (at reduced fuel efficiency).[116]

#### Power stations

The company ACWA Power and the city of Neom have announced the construction of a green hydrogen and ammonia plant in 2020.[117]

### Other

#### Remediation of gaseous emissions

Ammonia is used to scrub SO
2 from the burning of fossil fuels, and the resulting product is converted to ammonium sulfate for use as fertiliser. Ammonia neutralises the nitrogen oxide (NO
x ) pollutants emitted by diesel engines. This technology, called SCR (selective catalytic reduction), relies on a vanadia-based catalyst.[118]

Ammonia may be used to mitigate gaseous spills of phosgene.[119]

#### Stimulant

Anti-meth sign on tank of anhydrous ammonia, Otley, Iowa. Anhydrous ammonia is a common farm fertiliser that is also a critical ingredient in making methamphetamine. In 2005, Iowa used grant money to provide thousands of locks to prevent criminals from gaining access to the tanks.[120]

Ammonia, as the vapour released by smelling salts, has found significant use as a respiratory stimulant. Ammonia is commonly used in the illegal manufacture of methamphetamine through a Birch reduction.[121] The Birch method of making methamphetamine is dangerous because the alkali metal and liquid ammonia are both extremely reactive, and the temperature of liquid ammonia makes it susceptible to explosive boiling when reactants are added.[122]

#### Textile

Liquid ammonia is used for treatment of cotton materials, giving properties like mercerisation, using alkalis. In particular, it is used for prewashing of wool.[123]

#### Lifting gas

At standard temperature and pressure, ammonia is less dense than atmosphere and has approximately 45–48% of the lifting power of hydrogen or helium. Ammonia has sometimes been used to fill balloons as a lifting gas. Because of its relatively high boiling point (compared to helium and hydrogen), ammonia could potentially be refrigerated and liquefied aboard an airship to reduce lift and add ballast (and returned to a gas to add lift and reduce ballast).[124]

#### Fuming

Ammonia has been used to darken quartersawn white oak in Arts & Crafts and Mission-style furniture. Ammonia fumes react with the natural tannins in the wood and cause it to change colour.[125]

#### Cleaning agent

Ammonia is used as an ingredient in various cleaning products, such as Windex (until 2006), in the form of ammonia solution.

## Safety

The world's longest ammonia pipeline (roughly 2400 km long),[126] running from the TogliattiAzot plant in Russia to Odesa in Ukraine

The US Occupational Safety and Health Administration (OSHA) has set a 15-minute exposure limit for gaseous ammonia of 35 ppm by volume in the environmental air and an 8-hour exposure limit of 25 ppm by volume.[127] The National Institute for Occupational Safety and Health (NIOSH) recently reduced the IDLH (Immediately Dangerous to Life or Health, the level to which a healthy worker can be exposed for 30 minutes without suffering irreversible health effects) from 500 to 300 ppm based on recent more conservative interpretations of original research in 1943. Other organisations have varying exposure levels. US Navy Standards [US Bureau of Ships 1962] maximum allowable concentrations (MACs): for continuous exposure (60 days) is 25 ppm; for exposure of 1 hour is 400 ppm.[128]

Ammonia is an irritant and irritation increases with concentration; the permissible exposure limit is 25 ppm, and lethal above 500 ppm by volume.[129]

Ammonia vapour has a sharp, irritating, pungent odour that acts as a warning of potentially dangerous exposure. The average odour threshold is 5 ppm, well below any danger or damage. Exposure to very high concentrations of gaseous ammonia can result in lung damage and death.[127] Ammonia is regulated in the US as a non-flammable gas, but it meets the definition of a material that is toxic by inhalation and requires a hazardous safety permit when transported in quantities greater than 3,500 US gallons (13,000 l; 2,900 imp gal).[130]

## Toxicity

The toxicity of ammonia solutions does not usually cause problems for humans and other mammals because they possess metabolic pathways that prevent ammonia from accumulating in the bloodstream. Ammonia is converted to carbamoyl phosphate by the enzyme carbamoyl phosphate synthetase and then enters the urea cycle, where it is incorporated into amino acids or excreted as urea.[131]

Fish and amphibians lack this internal detoxification mechanism because they normally eliminate ammonia directly into the surrounding water. As a result, they are highly sensitive to elevated environmental concentrations: even dilute levels in the water can impede excretion and lead to toxic accumulation. For this reason, ammonia in aquatic environments is classified as dangerous for the environment. Atmospheric ammonia also plays a key role in the formation of fine particulate matter.[132]

Ammonia is also a constituent of tobacco smoke.[133]

### Coking wastewater

Ammonia is present in coking wastewater streams, as a liquid by-product of the production of coke from coal.[134] In some cases, the ammonia is discharged to the marine environment where it acts as a pollutant. The Whyalla Steelworks in South Australia is one example of a coke-producing facility that discharges ammonia into marine waters.[135]

### Aquaculture

Ammonia toxicity is believed to be a cause of otherwise unexplained losses in fish hatcheries. Excess ammonia may accumulate and cause alteration of metabolism or increases in the body pH of the exposed organism. Tolerance varies among fish species.[136] At lower concentrations, around 0.05 mg/L, un-ionised ammonia is harmful to fish species and can result in poor growth and feed conversion rates, reduced fecundity and fertility and increase stress and susceptibility to bacterial infections and diseases.[137] Exposed to excess ammonia, fish may suffer loss of equilibrium, hyper-excitability, increased respiratory activity and oxygen uptake and increased heart rate.[136] At concentrations exceeding 2.0 mg/L, ammonia causes gill and tissue damage, extreme lethargy, convulsions, coma, and death.[136][138] Experiments have shown that the lethal concentration for a variety of fish species ranges from 0.2 to 2.0 mg/L.[138]

During winter, when reduced feeds are administered to aquaculture stock, ammonia levels can be higher. Lower ambient temperatures reduce the rate of algal photosynthesis so less ammonia is removed by any algae present. Within an aquaculture environment, especially at large scale, there is no fast-acting remedy to elevated ammonia levels. Prevention rather than correction is recommended to reduce harm to farmed fish[138] and in open water systems, the surrounding environment.

### Storage information

Similar to propane, anhydrous ammonia boils below room temperature when at atmospheric pressure. A storage vessel capable of 250 psi (1.7 MPa) is suitable to contain the liquid.[139] Ammonia is used in numerous different industrial applications requiring carbon or stainless steel storage vessels. Ammonia with at least 0.2% by weight water content is not corrosive to carbon steel. NH
3 carbon steel construction storage tanks with 0.2% by weight or more of water could last more than 50 years in service.[140] Experts warn that ammonium compounds not be allowed to come in contact with bases (unless in an intended and contained reaction), as dangerous quantities of ammonia gas could be released.

### Laboratory

A standard laboratory solution of 28% ammonia

The hazards of ammonia solutions depend on the concentration: 'dilute' ammonia solutions are usually 5–10% by weight (< 5.62 mol/L); 'concentrated' solutions are usually prepared at >25% by weight. A 25% (by weight) solution has a density of 0.907 g/cm3, and a solution that has a lower density will be more concentrated. The European Union classification of ammonia solutions is given in the table.

Concentration
by weight (w/w)  | Molarity  | Concentration
mass/volume (w/v)  | GHS pictograms  | H-phrases

|
|
|
|

5–10%  | 2.87–5.62 mol/L  | 48.9–95.7 g/L  |  | H314
10–25%  | 5.62–13.29 mol/L  | 95.7–226.3 g/L  |  | H314, H335, H400
>25%  | >13.29 mol/L  | >226.3 g/L  |  | H314, H335, H400, H411

The ammonia vapour from concentrated ammonia solutions is severely irritating to the eyes and the respiratory tract, and experts warn that these solutions only be handled in a fume hood. Saturated ('0.880'–see § Properties) solutions can develop a significant pressure inside a closed bottle in warm weather, and experts also warn that the bottle be opened with care. This is not usually a problem for 25% ('0.900') solutions.

Experts warn that ammonia solutions not be mixed with halogens, as toxic and/or explosive products are formed. Experts also warn that prolonged contact of ammonia solutions with silver, mercury or iodide salts can also lead to explosive products: such mixtures are often formed in qualitative inorganic analysis, and that it needs to be lightly acidified but not concentrated (<6% w/v) before disposal once the test is completed.

### Laboratory use of anhydrous ammonia (gas or liquid)

Anhydrous ammonia is classified as toxic (T) and dangerous for the environment (N). The gas is flammable (autoignition temperature: 651 °C) and can form explosive mixtures with air (16–25%). The permissible exposure limit (PEL) in the United States is 50 ppm (35 mg/m3), while the IDLH concentration is estimated at 300 ppm. Repeated exposure to ammonia lowers the sensitivity to the smell of the gas: normally the odour is detectable at concentrations of less than 50 ppm, but desensitised individuals may not detect it even at concentrations of 100 ppm. Anhydrous ammonia corrodes copper\- and zinc-containing alloys, which makes brass fittings not appropriate for handling the gas. Liquid ammonia can also attack rubber and certain plastics.

Ammonia reacts violently with the halogens. Nitrogen triiodide, a primary high explosive, is formed when ammonia comes in contact with iodine. Ammonia causes the explosive polymerisation of ethylene oxide. It also forms explosive fulminating compounds with compounds of gold, silver, mercury, germanium or tellurium, and with stibine. Violent reactions have also been reported with acetaldehyde, hypochlorite solutions, potassium ferricyanide and peroxides.

## Production

Main article: Chemistry:Ammonia production

{{#chart:Global Ammonia Production.chart}}

Global ammonia production 1950–2020 (expressed as fixed nitrogen in US tons)[141]

Ammonia has one of the highest rates of production of any inorganic chemical. Production is sometimes expressed in terms of "fixed nitrogen". Global production was estimated as being 160 million tonnes in 2020 (147 tons of fixed nitrogen).[142] China accounted for 26.5% of that, followed by Russia at 11.0%, the United States at 9.5%, and India at 8.3%.[142]

Before the start of World War I, most ammonia was obtained by the dry distillation[143] of nitrogenous vegetable and animal waste products, including camel dung, where it was distilled by the reduction of nitrous acid and nitrites with hydrogen; in addition, it was produced by the distillation of coal, and also by the decomposition of ammonium salts by alkaline hydroxides[144] such as quicklime:[19]

2 [NH
4]Cl + 2 CaO → CaCl
2 \+ Ca(OH)
2 \+ 2 NH
3(g)

For small scale laboratory synthesis, one can heat urea and calcium hydroxide or sodium hydroxide:

(NH

2CO + Ca(OH)
2 → CaCO
3 \+ 2 NH

### Haber–Bosch

This section is an excerpt from Haber–Bosch process[ edit ]

### Electrochemical

The electrochemical synthesis of ammonia involves the reductive formation of lithium nitride, which can be protonated to ammonia, given a proton source. The first use of this chemistry was reported in 1930, where lithium solutions in ethanol were used to produce ammonia at pressures of up to 1000 bar, with ethanol acting as the proton source.[145] Beyond simply mediating proton transfer to the nitrogen reduction reaction, ethanol has been found to play a multifaceted role, influencing electrolyte transformations and contributing to the formation of the solid electrolyte interphase, which enhances overall reaction efficiency.[146][147]

In 1994, Tsuneto et al. used lithium electrodeposition in tetrahydrofuran to synthesize ammonia at more moderate pressures with reasonable Faradaic efficiency.[148] Subsequent studies have further explored the ethanol–tetrahydrofuran system for electrochemical ammonia synthesis.[147][149]

In 2020, a solvent-agnostic gas diffusion electrode was shown to improve nitrogen transport to the reactive lithium. NH
3 production rates of up to 30 ± 5 nmol/(s⋅cm2) and Faradaic efficiencies of up to 47.5 ± 4% at ambient temperature and 1 bar pressure were achieved.[150]

In 2021, it was demonstrated that ethanol could be replaced with a tetraalkyl phosphonium salt.[151] The study observed NH
3 production rates of 53 ± 1 nmol/(s⋅cm2) at 69 ± 1% Faradaic efficiency experiments under 0.5 bar hydrogen and 19.5 bar nitrogen partial pressure at ambient temperature.[151] Technology based on this electrochemistry is being developed for commercial fertiliser and fuel production.[152][153]

In 2022, ammonia was produced via the lithium mediated process in a continuous-flow electrolyzer also demonstrating the hydrogen gas as proton source. The study synthesised ammonia at 61 ± 1% Faradaic efficiency at a current density of −6 mA/cm2 at 1 bar and room temperature.[154]

## Biochemistry and medicine

Main symptoms of hyperammonemia (ammonia reaching toxic concentrations).[155]

Ammonia is essential for life.[156] For example, it is required for the formation of amino acids and nucleic acids, fundamental building blocks of life. Ammonia is however quite toxic. Nature thus uses carriers for ammonia. Within a cell, glutamate serves this role. In the bloodstream, glutamine is a source of ammonia.[157]

Ethanolamine, required for cell membranes, is the substrate for ethanolamine ammonia-lyase, which produces ammonia:[158]

2NCH
2CH
2OH → NH
3 \+ CH
3CHO

Ammonia is both a metabolic waste and a metabolic input throughout the biosphere. It is an important source of nitrogen for living systems. Although atmospheric nitrogen abounds (more than 75%), few living creatures are capable of using atmospheric nitrogen in its diatomic form, N
2 gas. Therefore, nitrogen fixation is required for the synthesis of amino acids, which are the building blocks of protein. Some plants rely on ammonia and other nitrogenous wastes incorporated into the soil by decaying matter. Others, such as nitrogen-fixing legumes, benefit from symbiotic relationships with rhizobia bacteria that create ammonia from atmospheric nitrogen.[159]

In humans, inhaling ammonia in high concentrations can be fatal. Exposure to ammonia can cause headaches, edema, impaired memory, seizures and coma as it is neurotoxic in nature.[160]

### Biosynthesis

See also: Biology:Diazotroph

In certain organisms, ammonia is produced from atmospheric nitrogen by enzymes called nitrogenases. The overall process is called nitrogen fixation. Intense effort has been directed toward understanding the mechanism of biological nitrogen fixation. The scientific interest in this problem is motivated by the unusual structure of the active site of the enzyme, which consists of an Fe
7MoS
9 ensemble.[161]

Ammonia is also a metabolic product of amino acid deamination catalysed by enzymes such as glutamate dehydrogenase 1. Ammonia excretion is common in aquatic animals. In humans, it is quickly converted to urea (by liver), which is much less toxic, particularly less basic. This urea is a major component of the dry weight of urine. Most reptiles, birds, insects, and snails excrete uric acid solely as nitrogenous waste.

### Physiology

Ammonia plays a role in both normal and abnormal animal physiology. It is biosynthesised through normal amino acid metabolism and is toxic in high concentrations. The liver converts ammonia to urea through a series of reactions known as the urea cycle. Liver dysfunction, such as that seen in cirrhosis, may lead to elevated amounts of ammonia in the blood (hyperammonemia). Likewise, defects in the enzymes responsible for the urea cycle, such as ornithine transcarbamylase, lead to hyperammonemia. Hyperammonemia contributes to the confusion and coma of hepatic encephalopathy, as well as the neurological disease common in people with urea cycle defects and organic acidurias.[162]

Ammonia is important for normal animal acid/base balance. After formation of ammonium from glutamine, α-ketoglutarate may be degraded to produce two bicarbonate ions, which are then available as buffers for dietary acids. Ammonium is excreted in the urine, resulting in net acid loss. Ammonia may itself diffuse across the renal tubules, combine with a hydrogen ion, and thus allow for further acid excretion.[163]

### Excretion

Main article: Biology:Excretion

Ammonium ions are a toxic waste product of metabolism in animals. In fish and aquatic invertebrates, it is excreted directly into the water. In mammals, sharks, and amphibians, it is converted in the urea cycle to urea, which is less toxic and can be stored more efficiently. In birds, reptiles, and terrestrial snails, metabolic ammonium is converted into uric acid, which is solid and can therefore be excreted with minimal water loss.[164]

## Extraterrestrial occurrence

Ammonia occurs in the atmospheres of the outer giant planets such as Jupiter (0.026% ammonia), Saturn (0.012% ammonia), and in the atmospheres and ices of Uranus and Neptune.

Ammonia has been detected in the atmospheres of the giant planets Jupiter, Saturn, Uranus and Neptune, along with other gases such as methane, hydrogen, and helium. The interior of Saturn may include frozen ammonia crystals.[165]

### Interstellar space

Ammonia was first detected in interstellar space in 1968, based on microwave emissions from the direction of the galactic core.[166] This was the first polyatomic molecule to be so detected. The sensitivity of the molecule to a broad range of excitations and the ease with which it can be observed in a number of regions has made ammonia one of the most important molecules for studies of molecular clouds.[167] The relative intensity of the ammonia lines can be used to measure the temperature of the emitting medium.

The following isotopic species of ammonia have been detected: NH
3,15

3, NH
2D, NHD
2, and ND
3. The detection of triply deuterated ammonia was considered a surprise as deuterium is relatively scarce. It is thought that the low-temperature conditions allow this molecule to survive and accumulate.[168]

Since its interstellar discovery, NH
3 has proved to be an invaluable spectroscopic tool in the study of the interstellar medium. With a large number of transitions sensitive to a wide range of excitation conditions, NH
3 has been widely astronomically detected–its detection has been reported in hundreds of journal articles. Listed below is a sample of journal articles that highlights the range of detectors that have been used to identify ammonia.

The study of interstellar ammonia has been important to a number of areas of research in the last few decades. Some of these are delineated below and primarily involve using ammonia as an interstellar thermometer.

#### Interstellar formation mechanisms

The interstellar abundance for ammonia has been measured for a variety of environments. The [NH
3]/[H
2] ratio has been estimated to range from 10−7 in small dark clouds[169] up to 10−5 in the dense core of the Orion molecular cloud complex.[170] Although a total of 18 total production routes have been proposed,[171] the principal formation mechanism for interstellar NH
3 is the reaction:

[NH
4]+
\+ e−
→ NH
3 \+ H

The rate constant, k, of this reaction depends on the temperature of the environment, with a value of 5.2×10−6 at 10 K.[172] The rate constant was calculated from the formula k=a(T/300)B. For the primary formation reaction, a = 1.05×10−6 and B = −0.47. Assuming an NH+
4 abundance of 3×10−7and an electron abundance of 10−7 typical of molecular clouds, the formation will proceed at a rate of 1.6×10−9 cm−3s−1 in a molecular cloud of total density 105 cm−3.[173]

All other proposed formation reactions have rate constants of between two and 13 orders of magnitude smaller, making their contribution to the abundance of ammonia relatively insignificant.[174] As an example of the minor contribution other formation reactions play, the reaction:

2 \+ NH
2 → NH
3 \+ H

has a rate constant of 2.2×10−15. Assuming H
2 densities of 105 and [NH
2]/[H
2] ratio of 10−7, this reaction proceeds at a rate of 2.2×10−12, more than three orders of magnitude slower than the primary reaction above.

Some of the other possible formation reactions are:

\+ [NH
4]+
→ NH
3 \+ H

[PNH
3]+
\+ e−
→ P + NH

#### Interstellar destruction mechanisms

There are 113 total proposed reactions leading to the destruction of NH
3. Of these, 39 were tabulated in extensive tables of the chemistry among C, N and O compounds.[175] A review of interstellar ammonia cites the following reactions as the principal dissociation mechanisms:[167]

3 \+ [H
3]+
→ [NH
4]+
\+ H

|
|

(1)

3 \+ HCO+
→ [NH
4]+
\+ CO

|
|

(2)

with rate constants of 4.39×10−9[176] and 2.2×10−9,[177] respectively. The above equations (1, 2) run at a rate of 8.8×10−9 and 4.4×10−13, respectively. These calculations assumed the given rate constants and abundances of [NH
3]/[H
2] = 10−5, [[H
3]+
]/[H
2] = 2×10−5, [HCO+
]/[H
2] = 2×10−9, and total densities of n = 105, typical of cold, dense, molecular clouds.[178] Clearly, between these two primary reactions, equation (1) is the dominant destruction reaction, with a rate ≈10,000 times faster than equation (2). This is due to the relatively high abundance of [H
3]+

#### Single antenna detections

Radio observations of NH
3 from the Effelsberg 100-m Radio Telescope reveal that the ammonia line is separated into two components–a background ridge and an unresolved core. The background corresponds well with the locations previously detected CO.[179] The 25 m Chilbolton telescope in England detected radio signatures of ammonia in H II regions, HNH2O masers, H–H objects, and other objects associated with star formation. A comparison of emission line widths indicates that turbulent or systematic velocities do not increase in the central cores of molecular clouds.[180]

Microwave radiation from ammonia was observed in several galactic objects including W3(OH), Orion A, W43, W51, and five sources in the galactic centre. The high detection rate indicates that this is a common molecule in the interstellar medium and that high-density regions are common in the galaxy.[181]

#### Interferometric studies

VLA observations of NH
3 in seven regions with high-velocity gaseous outflows revealed condensations of less than 0.1 pc in L1551, S140, and Cepheus A. Three individual condensations were detected in Cepheus A, one of them with a highly elongated shape. They may play an important role in creating the bipolar outflow in the region.[182]

Extragalactic ammonia was imaged using the VLA in IC 342. The hot gas has temperatures above 70 K, which was inferred from ammonia line ratios and appears to be closely associated with the innermost portions of the nuclear bar seen in CO.[183] NH
3 was also monitored by VLA toward a sample of four galactic ultracompact HII regions: G9.62+0.19, G10.47+0.03, G29.96−0.02, and G31.41+0.31. Based upon temperature and density diagnostics, it is concluded that in general such clumps are probably the sites of massive star formation in an early evolutionary phase prior to the development of an ultracompact HII region.[184]

#### Infrared detections

Absorption at 2.97 micrometres due to solid ammonia was recorded from interstellar grains in the Becklin–Neugebauer Object and probably in NGC 2264-IR as well. This detection helped explain the physical shape of previously poorly understood and related ice absorption lines.[185]

A spectrum of the disk of Jupiter was obtained from the Kuiper Airborne Observatory, covering the 100 to 300 cm−1 spectral range. Analysis of the spectrum provides information on global mean properties of ammonia gas and an ammonia ice haze.[186]

A total of 149 dark cloud positions were surveyed for evidence of 'dense cores' by using the (J,K) = (1,1) rotating inversion line of NH3. In general, the cores are not spherically shaped, with aspect ratios ranging from 1.1 to 4.4. It is also found that cores with stars have broader lines than cores without stars.[187]

Ammonia has been detected in the Draco Nebula and in one or possibly two molecular clouds, which are associated with the high-latitude galactic infrared cirrus. The finding is significant because they may represent the birthplaces for the Population I metallicity B-type stars in the galactic halo that could have been borne in the galactic disk.[188]

#### Observations of nearby dark clouds

By balancing and stimulated emission with spontaneous emission, it is possible to construct a relation between excitation temperature and density. Moreover, since the transitional levels of ammonia can be approximated by a 2-level system at low temperatures, this calculation is fairly simple. This premise can be applied to dark clouds, regions suspected of having extremely low temperatures and possible sites for future star formation. Detections of ammonia in dark clouds show very narrow lines - indicative not only of low temperatures, but also of a low level of inner-cloud turbulence. Line ratio calculations provide a measurement of cloud temperature that is independent of previous CO observations. The ammonia observations were consistent with CO measurements of rotation temperatures of ≈10 K. With this, densities can be determined, and have been calculated to range between 104 and 105 cm−3 in dark clouds. Mapping of NH
3 gives typical clouds sizes of 0.1 pc and masses near 1 solar mass. These cold, dense cores are the sites of future star formation.

#### UC HII regions

Ultra-compact HII regions are among the best tracers of high-mass star formation. The dense material surrounding UCHII regions is likely primarily molecular. Since a complete study of massive star formation necessarily involves the cloud from which the star formed, ammonia is an invaluable tool in understanding this surrounding molecular material. Since this molecular material can be spatially resolved, it is possible to constrain the heating/ionising sources, temperatures, masses, and sizes of the regions. Doppler-shifted velocity components allow for the separation of distinct regions of molecular gas that can trace outflows and hot cores originating from forming stars.

#### Extragalactic detection

Ammonia has been detected in external galaxies,[189][190] and by simultaneously measuring several lines, it is possible to directly measure the gas temperature in these galaxies. Line ratios imply that gas temperatures are warm (≈50 K), originating from dense clouds with sizes of tens of parsecs. This picture is consistent with the picture within our Milky Way galaxy - hot dense molecular cores form around newly forming stars embedded in larger clouds of molecular material on the scale of several hundred parsecs (giant molecular clouds; GMCs).

## See also

* Chemistry:Ammonia fountain - Type of chemical demonstration
* Chemistry:Ammonia production - Overview of history and methods to produce NH3
* Chemistry:Ammonia solution - Chemical compound
* Finance:Cost of electricity by source - Comparison of costs of different electricity generation sources
* Physics:Forming gas - Mixture of hydrogen and nitrogen
* Chemistry:Haber process - Industrial process for ammonia production
* Chemistry:Hydrazine
* Earth:Water purification - Process of removing impurities from water

## References

1. ↑ 1.0 1.1 1.2 Myers, Richard L. (2007). The 100 Most Important Chemical Compounds: A Reference Guide. ABC-CLIO. pp. 27–29. ISBN 978-0-313-33758-1. https://books.google.com/books?id=0AnJU-hralEC. Retrieved 21 November 2015.
2. ↑ Ammonia as energy vector round table discussion https://web.archive.org/web/20251222231225/https://bmbf-client.de/en/news/coalco2-x-round-table-discussion-ammonia-energy-vector
3. ↑ Watermann, Clara Maria; Nitsche, Tim; Csepei, Lénárd‐István; Menne, Andreas; Zeidler‐Fandrich, Barbara (June 2025). "Green Ammonia as a Decentralized, Cross‐Sector Energy Vector for the German Energy Transition". Chemie Ingenieur Technik 97 (6): 599–607. doi:10.1002/cite.202500020. https://onlinelibrary.wiley.com/doi/10.1002/cite.202500020.
4. ↑ Ritchie, Hannah (7 November 2017). "How many people does synthetic fertilizer feed?". https://ourworldindata.org/how-many-people-does-synthetic-fertilizer-feed.
5. ↑ "Ammonia Technology Roadmap – Analysis". IEA. 11 October 2021. https://www.iea.org/reports/ammonia-technology-roadmap.
6. ↑ "40 C.F.R.: Appendix A to Part 355—The List of Extremely Hazardous Substances and Their Threshold Planning Quantities". United States: Government Printing Office. https://www.ecfr.gov/current/title-40/chapter-I/subchapter-J/part-355#Appendix-A-to-Part-355.
7. ↑ "Global ammonia annual production capacity". https://www.statista.com/statistics/1065865/ammonia-production-capacity-globally/.
8. ↑ "Mitsubishi Heavy Industries BrandVoice: Scaling Ammonia Production for the World's Food Supply". 29 October 2021. https://www.forbes.com/sites/mitsubishiheavyindustries/2021/10/29/scaling-ammonia-production-for-the-worlds-food-supply/.
9. ↑ Shreve, R. Norris; Brink, Joseph (1977). Chemical Process Industries (4th ed.). McGraw-Hill. p. 276. ISBN 978-0-07-057145-7.
10. ↑ "Pliny the Elder, The Natural History, BOOK XXXI. REMEDIES DERIVED FROM THE AQUATIC PRODUCTION, CHAP. 39. (7.)—THE VARIOUS KINDS OF SALT; THE METHODS OF PREPARING IT, AND THE REMEDIES DERIVED FROM IT. TWO HUNDRED AND FOUR OBSERVATIONS THERE UPON.". https://www.perseus.tufts.edu/hopper/text?doc=urn:cts:latinLit:phi0978.phi001.perseus-eng1:31.39.
11. ↑ Agricola, Georg (1986). Hoover, Herbert. ed. De re metallica. New York: Dover Publications. p. 560. ISBN 978-0-486-60006-2.
12. ↑ "ammoniacal (adj.)". July 2023. doi:10.1093/OED/3565252514. https://www.oed.com/dictionary/ammoniacal_adj.
13. ↑ Shannon, Francis Patrick (1938) Tables of the properties of aqua–ammonia solutions. Part 1 of The Thermodynamics of Absorption Refrigeration. Lehigh University studies. Science and technology series
14. ↑ An ammonia–water slurry may swirl below Pluto's icy surface. Purdue University (9 November 2015)
15. ↑ 15.0 15.1 15.2 Behera, Sailesh N.; Sharma, Mukesh; Aneja, Viney P.; Balasubramanian, Rajasekhar (1 November 2013). "Ammonia in the atmosphere: a review on emission sources, atmospheric chemistry and deposition on terrestrial bodies" (in en). Environmental Science and Pollution Research 20 (11): 8092–8131. doi:10.1007/s11356-013-2051-9. ISSN 0944-1344. PMID 23982822. Bibcode: 2013ESPR...20.8092B. http://link.springer.com/10.1007/s11356-013-2051-9.
16. ↑ Lin, Yongxin; Hu, Hang-Wei; Ye, Guiping; Fan, Jianbo; Ding, Weixin; He, Zi-Yang; Zheng, Yong; He, Ji-Zheng (15 December 2021). "Ammonia-oxidizing bacteria play an important role in nitrification of acidic soils: A meta-analysis". Geoderma 404. doi:10.1016/j.geoderma.2021.115395. ISSN 0016-7061. Bibcode: 2021Geode.40415395L.
17. ↑ 17.0 17.1 17.2 17.3 17.4 Pai, Sidhant J.; Heald, Colette L.; Murphy, Jennifer G. (15 July 2021). "Exploring the Global Importance of Atmospheric Ammonia Oxidation" (in en). ACS Earth and Space Chemistry 5 (7): 1674–1685. doi:10.1021/acsearthspacechem.1c00021. ISSN 2472-3452. Bibcode: 2021ESC.....5.1674P. https://pubs.acs.org/doi/10.1021/acsearthspacechem.1c00021.
18. ↑ Yu, Fangqun; Nadykto, Alexey B.; Herb, Jason; Luo, Gan; Nazarenko, Kirill M.; Uvarova, Lyudmila A. (10 December 2018). "H 2 SO 4 –H 2 O–NH 3 ternary ion-mediated nucleation (TIMN): kinetic-based model and comparison with CLOUD measurements" (in en). Atmospheric Chemistry and Physics 18 (23): 17451–17474. doi:10.5194/acp-18-17451-2018. ISSN 1680-7324. https://acp.copernicus.org/articles/18/17451/2018/.
19. ↑ 19.0 19.1 19.2 19.3 19.4 19.5 19.6 Chisholm 1911, p. 861.
20. ↑ Pimputkar, Siddha; Nakamura, Shuji (January 2016). "Decomposition of supercritical ammonia and modeling of supercritical ammonia–nitrogen–hydrogen solutions with applicability toward ammonothermal conditions". The Journal of Supercritical Fluids 107: 17–30. doi:10.1016/j.supflu.2015.07.032.
21. ↑ Hewat, A. W.; Riekel, C. (1979). "The crystal structure of deuteroammonia between 2 and 180 K by neutron powder profile refinement". Acta Crystallographica Section A 35 (4): 569. doi:10.1107/S0567739479001340. Bibcode: 1979AcCrA..35..569H.
22. ↑ Billaud, Gerard; Demortier, Antoine (December 1975). "Dielectric constant of liquid ammonia from -35 to + 50.deg. and its influence on the association between solvated electrons and cation" (in en). The Journal of Physical Chemistry 79 (26): 3053–3055. doi:10.1021/j100593a053. ISSN 0022-3654. Bibcode: 1975JPhCh..79.3053B. https://pubs.acs.org/doi/abs/10.1021/j100593a053.
23. ↑ Ammonia in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD), http://webbook.nist.gov
24. ↑ Jepsen, S. Dee; McGuire, Kent (27 November 2017). "Safe Handling of Anhydrous Ammonia". https://ohioline.osu.edu/factsheet/aex-594.
25. ↑ "Medical Management Guidelines for Ammonia". 12 January 2017. https://wwwn.cdc.gov/TSP/MMG/MMGDetails.aspx?mmgid=7&toxid=2.
26. ↑ Hawkins, Nehemiah (1909) (in en). Hawkins' Mechanical Dictionary: A Cyclopedia of Words, Terms, Phrases and Data Used in the Mechanic Arts, Trades and Sciences. T. Audel. p. 15. https://books.google.com/books?id=Z14wAAAAMAAJ.
27. ↑ 27.0 27.1 27.2 Neufeld, R.; Michel, R.; Herbst-Irmer, R.; Schöne, R.; Stalke, D. (2016). "Introducing a Hydrogen-Bond Donor into a Weakly Nucleophilic Brønsted Base: Alkali Metal Hexamethyldisilazides (MHMDS, M = Li, Na, K, Rb and Cs) with Ammonia". Chem. Eur. J. 22 (35): 12340–12346. doi:10.1002/chem.201600833. PMID 27457218. Bibcode: 2016ChEuJ..2212340N.
28. ↑ 28.0 28.1 28.2 Combellas, C; Kanoufi, F; Thiébault, A (2001). "Solutions of solvated electrons in liquid ammonia". Journal of Electroanalytical Chemistry 499: 144–151. doi:10.1016/S0022-0728(00)00504-0.
29. ↑ Audrieth, Ludwig F.; Kleinberg, Jacob (1953). Non-aqueous solvents. New York: John Wiley & Sons. p. 45. https://archive.org/details/cftri.2662nonaqueoussolven0000ludw/page/45/.
30. ↑ Edwin M. Kaiser (2001). "Calcium–Ammonia". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rc003. ISBN 978-0-471-93623-7.
31. ↑ 31.0 31.1 Haynes, William M., ed (2013). CRC Handbook of Chemistry and Physics (94th ed.). CRC Press. pp. 9–26. ISBN 978-1-4665-7114-3.
32. ↑ Cleeton, C. E.; Williams, N. H. (1934). "Electromagnetic Waves of 1.1 cm (0 in). Wave-Length and the Absorption Spectrum of Ammonia". Physical Review 45 (4): 234. doi:10.1103/PhysRev.45.234. Bibcode: 1934PhRv...45..234C.
33. ↑ Chisholm 1911, p. 862.
34. ↑ Baker, H. B. (1894). "Influence of moisture on chemical change". J. Chem. Soc. 65: 611–624. doi:10.1039/CT8946500611. https://zenodo.org/record/1863586.
35. ↑ "Ammonia". https://pubchem.ncbi.nlm.nih.gov/source/hsdb/162#section=Flammable-Limits.
36. ↑ Kobayashi, Hideaki; Hayakawa, Akihiro; Somarathne, K.D. Kunkuma A.; Okafor, Ekenechukwu C. (2019). "Science and technology of ammonia combustion". Proceedings of the Combustion Institute 37 (1): 109–133. doi:10.1016/j.proci.2018.09.029. Bibcode: 2019PComI..37..109K.
37. ↑ Khan, A.S.; Kelley, R.D.; Chapman, K.S.; Fenton, D.L. (1995). Flammability limits of ammonia–air mixtures. U.S.: U.S. DOE Office of Scientific and Technical Information.
38. ↑ Shrestha, Krishna P.; Seidel, Lars; Zeuch, Thomas; Mauss, Fabian (7 July 2018). "Detailed kinetic mechanism for the oxidation of ammonia including the formation and reduction of nitrogen oxides". Energy & Fuels 32 (10): 10202–10217. doi:10.1021/acs.energyfuels.8b01056. ISSN 0887-0624. Bibcode: 2018EnFue..3210202S. https://hal.archives-ouvertes.fr/hal-02629067/file/Shrestha_Ammonia_NOx_2018.pdf.
39. ↑ Holleman, A. F.; Wiberg, E. (2001). Inorganic Chemistry. San Diego: Academic Press. ISBN 978-0-12-352651-9.
40. ↑ Sterrett, K. F.; Caron, A. P. (1966). "High pressure chemistry of hydrogenous fuels". Northrop Space Labs. http://oai.dtic.mil/oai/oai?verb=getRecord&metadataPrefix=html&identifier=AD0373800.
41. ↑ Holleman, A. F., ed (2001). Holleman-Wiberg inorganic chemistry. San Diego, Calif. London: Academic. ISBN 978-0-12-352651-9.
42. ↑ Herodotus with George Rawlinson, trans., The History of Herodotus (New York City: Tandy-Thomas Co., 1909), vol.2, Book 4, § 181, pp. 304–305.
43. ↑ The land of the Ammonians is mentioned elsewhere in Herodotus' History and in Pausanias' Description of Greece:
* Herodotus with George Rawlinson, trans., The History of Herodotus (New York City: Tandy-Thomas Co., 1909), vol. 1, Book 2, § 42, p. 245, vol. 2, Book 3, § 25, p. 73, and vol. 2, Book 3, § 26, p. 74.
* Pausanias with W.H.S. Jones, trans., Description of Greece (London, England: William Heinemann Ltd., 1979), vol. 2, Book 3, Ch. 18, § 3, pp. 109 and 111 and vol. 4, Book 9, Ch. 16, § 1, p. 239.
44. ↑ Kopp, Hermann, Geschichte der Chemie [History of Chemistry] (Braunschweig, (Germany): Friedrich Vieweg und Sohn, 1845), Part 3, p. 237. [in German]
45. ↑ Chisholm 1911 cites Pliny Nat. Hist. xxxi. 39. See: Pliny the Elder with John Bostock and H. T. Riley, ed.s, The Natural History (London, England: H. G. Bohn, 1857), vol. 5, Book 31, § 39, p. 502.
46. ↑ "Sal-ammoniac". Webmineral. http://webmineral.com/data/Sal-ammoniac.shtml.
47. ↑ Pliny also mentioned that when some samples of what was purported to be natron (Latin: nitrum, impure sodium carbonate) were treated with lime (calcium carbonate) and water, the natron would emit a pungent smell, which some authors have interpreted as signifying that the natron either was ammonium chloride or was contaminated with it. See:
* Pliny with W.H.S. Jones, trans., Natural History (London, England: William Heinemann Ltd., 1963), vol. 8, Book 31, § 46, pp. 448–449. From pp. 448–449: "Adulteratur in Aegypto calce, deprehenditur gusto. Sincerum enim statim resolvitur, adulteratum calce pungit et asperum [or aspersum] reddit odorem vehementer." (In Egypt it [i.e., natron] is adulterated with lime, which is detected by taste; for pure natron melts at once, but adulterated natron stings because of the lime, and emits a strong, bitter odour [or: when sprinkled [(aspersum) with water] emits a vehement odour])
* Kidd, John, Outlines of Mineralogy (Oxford, England: N. Bliss, 1809), vol. 2, p. 6.
* Moore, Nathaniel Fish, Ancient Mineralogy: Or, An Inquiry Respecting Mineral Substances Mentioned by the Ancients: ... (New York, New York: G. & C. Carvill & Co., 1834), pp. 96–97.
48. ↑ See:
* Forbes, R.J., Studies in Ancient Technology, vol. 5, 2nd ed. (Leiden, Netherlands: E.J. Brill, 1966), pp. 19, 48, and 65.
* Moeller, Walter O., The Wool Trade of Ancient Pompeii (Leiden, Netherlands: E.J. Brill, 1976), p. 20.
* Faber, G.A. (pseudonym of: Goldschmidt, Günther) (May 1938) "Dyeing and tanning in classical antiquity," Ciba Review, 9 : 277–312. Available at: Elizabethan Costume
* Smith, William, A Dictionary of Greek and Roman Antiquities (London, England: John Murray, 1875), article: "Fullo" (i.e., fullers or launderers), pp. 551–553.
* Rousset, Henri (31 March 1917) "The laundries of the Ancients," Scientific American Supplement, 83 (2152) : 197.
* Bond, Sarah E., Trade and Taboo: Disreputable Professions in the Roman Mediterranean (Ann Arbor, Michigan: University of Michigan Press, 2016), p. 112.
* Binz, Arthur (1936) "Altes und Neues über die technische Verwendung des Harnes" (Ancient and modern [information] about the technological use of urine), Zeitschrift für Angewandte Chemie, 49 (23) : 355–360. [in German]
* Witty, Michael (December 2016) "Ancient Roman urine chemistry," Acta Archaeologica, 87 (1) : 179–191. Witty speculates that the Romans obtained ammonia in concentrated form by adding wood ash (impure potassium carbonate) to urine that had been fermented for several hours. Struvite (magnesium ammonium phosphate) is thereby precipitated, and the yield of struvite can be increased by then treating the solution with bittern, a magnesium-rich solution that is a byproduct of making salt from sea water. Roasting struvite releases ammonia vapours.
49. ↑ Lenkeit, Roberta Edwards (23 October 2018) (in en). High Heels and Bound Feet: And Other Essays on Everyday Anthropology, Second Edition. Waveland Press. p. 72. ISBN 978-1-4786-3841-4. https://books.google.com/books?id=sapxDwAAQBAJ&dq=Teeth+whitening+ancient+Rome&pg=PA72.
50. ↑ Perdigão, Jorge (3 August 2016) (in en). Tooth Whitening: An Evidence-Based Perspective. Springer. p. 170. ISBN 978-3-319-38849-6. https://books.google.com/books?id=lB3KDAAAQBAJ&dq=Teeth+whitening+ancient+Rome&pg=PA170.
51. ↑ Bonitz, Michael; Lopez, Jose; Becker, Kurt; Thomsen, Hauke (9 April 2014) (in en). Complex Plasmas: Scientific Challenges and Technological Opportunities. Springer Science & Business Media. p. 465. ISBN 978-3-319-05437-7. https://books.google.com/books?id=EzW8BAAAQBAJ&dq=Teeth+whitening+ancient+Rome&pg=PA465.
52. ↑ Haq, Syed Nomanul (1995). Names, Natures and Things: The Alchemist Jabir Ibn Hayyan and His Kitab Al-Ahjar (Book of Stones). Springer. ISBN 978-0-7923-3254-1. https://books.google.com/books?id=P-70YjP0nj8C.
53. ↑ Spiritus salis urinæ (spirit of the salt of urine, i.e., ammonium carbonate) had apparently been produced before Valentinus, although he presented a new, simpler method for preparing it in his book: Valentinus, Basilius, Vier Tractätlein Fr. Basilii Valentini ... [Four essays of Brother Basil Valentine ... ] (Frankfurt am Main, (Germany): Luca Jennis, 1625), "Supplementum oder Zugabe" (Supplement or appendix), pp. 80–81: "Der Weg zum Universal, damit die drei Stein zusammen kommen." (The path to the Universal, so that the three stones come together.). From p. 81: "Der Spiritus salis Urinæ nimbt langes wesen zubereiten / dieser proceß aber ist waß leichter unnd näher auß dem Salz von Armenia, ... Nun nimb sauberen schönen Armenischen Salz armoniac ohn alles sublimiren / thue ihn in ein Kolben / giesse ein Oleum Tartari drauff / daß es wie ein Muß oder Brey werde / vermachs baldt / dafür thu auch ein grosen vorlag / so lege sich als baldt der Spiritus Salis Urinæ im Helm an Crystallisch ... " (Spirit of the salt of urine [i.e., ammonium carbonate] requires a long method [i.e., procedure] to prepare; this [i.e., Valentine's] process [starting] from the salt from Armenia [i.e., ammonium chloride], however, is somewhat easier and shorter ... Now take clean nice Armenian salt, without sublimating all [of it]; put it in a [distillation] flask; pour oil of tartar [i.e., potassium carbonate that has dissolved only in the water that it has absorbed from the air] on it, [so] that it [i.e., the mixture] becomes like a mush or paste; assemble it [i.e., the distilling apparatus (alembic)] quickly; for that [purpose] connect a large receiving flask; then soon spirit of the salt of urine deposits as crystals in the "helmet" [i.e., the outlet for the vapours, which is atop the distillation flask] ...)
See also: Kopp, Hermann, Geschichte der Chemie [History of Chemistry] (Braunschweig, (Germany): Friedrich Vieweg und Sohn, 1845), Part 3, p. 243. [in German]
54. ↑ Maurice P. Crosland (2004). Historical Studies in the Language of Chemistry. Courier Dover Publications. p. 72. ISBN 978-0-486-43802-3. https://books.google.com/books?id=kwQQaltqByAC&pg=PA72.
55. ↑ Black, Joseph (1893). Experiments upon magnesia alba, quick-lime, and other alcaline substances. Edinburgh: W.F. Clay. https://archive.org/details/b21730738.
56. ↑ Jacobson, Mark Z. (23 April 2012) (in en). Air Pollution and Global Warming: History, Science, and Solutions. Cambridge University Press. ISBN 978-1-107-69115-5. https://books.google.com/books?id=UeGlmU2F8_8C&pg=PA14.
57. ↑ "Woulfe's bottle" (in en). Chemistry World. https://www.chemistryworld.com/opinion/woulfes-bottle/2500114.article.
58. ↑ Woulfe, Peter (1 January 1767). "Experiments on the Distillation of Acids, Volatile Alkalies, &c. Shewing How They May be Condensed without Loss, and How Thereby We May Avoid Disagreeable and Noxious Fumes: In a Letter from Mr. Peter Woulfe, F. R. S. to John Ellis, Esq; F. R. S." (in en). Philosophical Transactions 57 (57): 517–536. doi:10.1098/rstl.1767.0052. ISSN 0261-0523. Bibcode: 1767RSPT...57..517W. https://zenodo.org/record/1432252.
59. ↑ Urdang, George (1942). Pictorial life history of the apothecary chemist Carl Wilhelm Scheele. American Institute of the History of Pharmacy.
60. ↑ See:
* Priestley, Joseph (1773) "Extrait d'une lettre de M. Priestley, en date du 14 Octobre 1773" (Extract of a letter from Mr. Priestley, dated 14 October 1773), Observations sur la Physique ..., 2 : 389.
* Priestley, Joseph, Experiments and Observations on Different Kinds of Air, vol. 1, 2nd ed. (London, England: 1775), Part 2, § 1: Observations on Alkaline Air, pp. 163–177.
* Schofield, Robert E., The Enlightened Joseph Priestley: A Study of His Life and Work from 1773 to 1804 (University Park, Pennsylvania: Pennsylvania State University Press, 2004), pp. 93–94.
* By 1775, Priestley had observed that electricity could decompose ammonia ("alkaline air"), yielding a flammable gas (hydrogen). See: Priestley, Joseph, Experiments and Observations on Different Kinds of Air, vol. 2 (London, England: J. Johnson, 1775), pp. 239–240.
61. ↑ Berthollet (1785) "Analyse de l'alkali volatil" (Analysis of volatile alkali), Mémoires de l'Académie Royale des Sciences, 316–326.
62. ↑ 62.0 62.1 Max Appl (2006). "Ammonia". Ammonia, in Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a02_143.pub2. ISBN 978-3-527-30673-2.
63. ↑ Smith, Roland (2001). Conquering Chemistry. Sydney: McGraw-Hill. ISBN 978-0-07-470146-1.
64. ↑ "Mineral Commodity Summaries 2020, p. 117 – Nitrogen". USGS. 2020. https://pubs.usgs.gov/periodicals/mcs2020/mcs2020.pdf.
65. ↑ Lassaletta, Luis; Billen, Gilles; Grizzetti, Bruna; Anglade, Juliette; Garnier, Josette (2014). "50-year trends in nitrogen use efficiency of world cropping systems: the relationship between yield and nitrogen input to cropland" (in en). Environmental Research Letters 9 (10). doi:10.1088/1748-9326/9/10/105011. ISSN 1748-9326. Bibcode: 2014ERL.....9j5011L.
66. ↑ David Brown (18 April 2013). "Anhydrous ammonia fertilizer: abundant, important, hazardous". Washington Post. https://www.washingtonpost.com/national/health-science/anhydrous-ammonia-fertilizer-abundant-important-hazardous/2013/04/18/c2d4c69c-a85a-11e2-a8e2-5b98cb59187f_story.html.
67. ↑ "Applications of Anhydrous Ammonia and Aqueous Ammonia". https://www.mysoreammonia.com/applications/.
68. ↑ Conversion of CO2 from South African coal-fired power plants using green ammonia and hydrogen https://www.igb.fraunhofer.de/en/reference-projects/coalco2x.html;
69. ↑ Skills development workshop for hydrogen and ammonia https://www.igb.fraunhofer.de/en/reference-projects/ptx-skills-development-in-tunisia.html;
70. ↑ Green Ammonia – Production of green ammonia in Morocco https://www.igb.fraunhofer.de/en/reference-projects/green-ammonia.html;
71. ↑ Wright, Jerry (13 April 2015). "Cooling System Keeps Space Station Safe, Productive" (in en). NASA. https://www.nasa.gov/content/cooling-system-keeps-space-station-safe-productive.
72. ↑ "International Space Station's Cooling System: How It Works (Infographic)". Space.com. http://www.space.com/21059-space-station-cooling-system-explained-infographic.html.
73. ↑ "Reducing Hydrofluorocarbon (HFC) Use and Emissions in the Federal Sector through SNAP". https://www.epa.gov/sites/default/files/2016-12/documents/epa_hfc_federal_sector.pdf.
74. ↑ Samuel Rideal (1895). Disinfection and Disinfectants: An Introduction to the Study of. London: Charles Griffin and Company. p. 109. https://archive.org/details/disinfectiondisi00rideuoft.
75. ↑ Tajkarimi, Mehrdad et al. (2008). "Ammonia disinfection of animal feeds – Laboratory study". International Journal of Food Microbiology 122 (1–2): 23–28. doi:10.1016/j.ijfoodmicro.2007.11.040. PMID 18155794.
76. ↑ Kim, J. S.; Lee, Y. Y.; Kim, T. H. (January 2016). "A review on alkaline pretreatment technology for bioconversion of lignocellulosic biomass.". Bioresource Technology 199: 42–48. doi:10.1016/j.biortech.2015.08.085. PMID 26341010. Bibcode: 2016BiTec.199...42K.
77. ↑ "Evaluation of Treatment Methods for Reducing Bacteria in Textured Beef", Jensen, Jean L et al., American Society of Agricultural and Biological Engineers Annual Meeting 2009
78. ↑ Reference Document: Antimicrobial Interventions for Beef , Dawna Winkler and Kerri B. Harris, Center for Food Safety, Department of Animal Science, Texas A&M University, May 2009, page 12
79. ↑ Moss, Michael (3 October 2009). "The Burger That Shattered Her Life". The New York Times. https://www.nytimes.com/2009/10/04/health/04meat.html.
80. ↑ Moss, Michael (31 December 2009). "Safety of Beef Processing Method Is Questioned". The New York Times. https://www.nytimes.com/2009/12/31/us/31meat.html.
81. ↑ "MOL studies ammonia FSRU concept" (in en-US). 3 February 2022. https://www.offshore-energy.biz/mol-studies-ammonia-fsru-concept/.
82. ↑ Collins (l_collins), Leigh (27 January 2022). "SPECIAL REPORT | Why shipping pure hydrogen around the world might already be dead in the water | Recharge" (in en). https://www.rechargenews.com/energy-transition/special-report-why-shipping-pure-hydrogen-around-the-world-might-already-be-dead-in-the-water/2-1-1155434.
83. ↑ 83.0 83.1 Lan, Rong; Tao, Shanwen (28 August 2014). "Ammonia as a suitable fuel for fuel cells". Frontiers in Energy Research 2: 35. doi:10.3389/fenrg.2014.00035. Bibcode: 2014FrER....2...35L.
84. ↑ Lindzon, Jared (27 February 2019). "He's Creating a New Fuel Out of Thin Air – for 85 Cents per Gallon". http://www.ozy.com/rising-stars/hes-creating-a-new-fuel-out-of-thin-air-for-85-cents-per-gallon/92686.
85. ↑ Giddey, S.; Badwal, S. P. S.; Munnings, C.; Dolan, M. (10 October 2017). "Ammonia as a Renewable Energy Transportation Media". ACS Sustainable Chemistry & Engineering 5 (11): 10231–10239. doi:10.1021/acssuschemeng.7b02219. Bibcode: 2017ASCE....510231G.
86. ↑ Afif, Ahmed; Radenahmad, Nikdilila; Cheok, Quentin; Shams, Shahriar; Hyun Kim, Jung; Azad, Abul (12 February 2016). "Ammonia-fed fuel cells: a comprehensive review". Renewable and Sustainable Energy Reviews 60: 822–835. doi:10.1016/j.rser.2016.01.120. Bibcode: 2016RSERv..60..822A. https://www.researchgate.net/publication/294579196. Retrieved 1 January 2021.
87. ↑ David, William I. F.; Makepeace, Joshua W.; Callear, Samantha K.; Hunter, Hazel M. A.; Taylor, James D.; Wood, Thomas J.; Jones, Martin O. (24 September 2014). "Hydrogen Production from Ammonia Using Sodium Amide". Journal of the American Chemical Society 136 (38): 13082–13085. doi:10.1021/ja5042836. ISSN 0002-7863. PMID 24972299. Bibcode: 2014JAChS.13613082D.
88. ↑ Lucentini, Ilaria; García Colli, Germán; Luzi, Carlos D.; Serrano, Isabel; Martínez, Osvaldo M.; Llorca, Jordi (5 June 2021). "Catalytic ammonia decomposition over Ni–Ru supported on CeO2 for hydrogen production: Effect of metal loading and kinetic analysis" (in en). Applied Catalysis B: Environmental 286. doi:10.1016/j.apcatb.2021.119896. ISSN 0926-3373. Bibcode: 2021AppCB.28619896L. https://www.sciencedirect.com/science/article/pii/S0926337321000229.
89. ↑ "Green ammonia | Royal Society". https://royalsociety.org/topics-policy/projects/low-carbon-energy-programme/green-ammonia/.
90. ↑ "Saudi Arabia Sends Blue Ammonia to Japan in World-First Shipment". 27 September 2020. https://www.bloomberg.com/news/articles/2020-09-27/saudi-arabia-sends-blue-ammonia-to-japan-in-world-first-shipment.
91. ↑ Service, Robert F. (12 July 2018). "Ammonia—a renewable fuel made from sun, air, and water—could power the globe without carbon" (in en). https://www.science.org/content/article/ammonia-renewable-fuel-made-sun-air-and-water-could-power-globe-without-carbon.
92. ↑ Kypriotaki, Anastasia (10 October 2024). "DNV Energy Transition Outlook 2024: Maritime energy demand will only grow slightly". https://safety4sea.com/dnv-energy-transition-outlook-2024-maritime-energy-demand-will-only-grow-slightly/.
93. ↑ Mehta, Amgeli (15 May 2023). "In the voyage to net-zero, which green shipping fuel will rule the seas?". Reuters. https://www.reuters.com/sustainability/climate-energy/voyage-net-zero-which-green-shipping-fuel-will-rule-seas-2023-05-15/.
94. ↑ "DSME gets LR AIP for ammonia-fueled 23,000 TEU boxship". 6 October 2020. https://www.offshore-energy.biz/dsme-gets-lr-aip-for-ammonia-fueled-23000-teu-boxship/.
95. ↑ "What will power aircraft in the future?". 30 March 2022. https://aviafuture.com/index.php/2022/03/30/what-will-power-aircraft-in-the-future/#ammonia.
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102. ↑ "On the use of ammonia as a fuel – A perspective". https://hal-cnrs.archives-ouvertes.fr/hal-03675905/file/2022 NH3 perspective.pdf.
103. ↑ "Nitrogen Oxides as a By-product of Ammonia/Hydrogen Combustion Regimes". https://orca.cardiff.ac.uk/id/eprint/144277/3/ICLCA21_0206 ed V3 without comments.pdf.
104. ↑ Douglas Self (1 October 2007). "Ammonia Motors". http://www.douglas-self.com/MUSEUM/POWER/ammonia/ammonia.htm.
105. ↑ Louis C. Hennick; Elbridge Harper Charlton (1965). The Streetcars of New Orleans. Pelican Publishing. pp. 14–16. ISBN 978-1-4556-1259-8.
106. ↑ 106.0 106.1 "Ammonia as a Transportation Fuel IV". Norm Olson – Iowa Energy Center. 15–16 October 2007. http://www.energy.iastate.edu/Renewable/ammonia/ammonia/2007/Olson2_NH3.pdf.
107. ↑ Lee, Dongeun; Min, Hyungeun; Park, Hyunho; Song, Han Ho (1 November 2017). "Development of new combustion strategy for internal combustion engine fueled by pure ammonia". Seoul National University, Department of Mechanical Engineering. https://nh3fuelassociation.org/wp-content/uploads/2017/11/NH3-Energy-2017-Donggeun-Lee.pdf.
108. ↑ Brohi, Emtiaz Ali (2014). "Ammonia as fuel for internal combustion engines?". Chalmers University of Technology. http://publications.lib.chalmers.se/records/fulltext/207145/207145.pdf.
109. ↑ Elucidare (2 February 2008). "Ammonia: New possibilities for hydrogen storage and transportation". http://www.elucidare.co.uk/news/Ammonia as H2 carrier.pdf.
110. ↑ Ammonia Powered Car on YouTube
111. ↑ "Watch 'Ammonia Fuel'". Greg Vezina. http://www.gregvezina.ca.
112. ↑ "Welcome to NH3 Car". NH3Car.com. http://www.nh3car.com/.
113. ↑ "Ammonia". chm.bris.ac.uk. http://www.chm.bris.ac.uk/motm/ammonia/Ammonia MOTM.htm.
114. ↑ Zacharakis-Jutz, George; Kong, Song-Charng (2013). "Characteristics of an SI Engine Using Direct Ammonia Injection". Department of Mechanical Engineering, Iowa State University. https://nh3fuelassociation.org/wp-content/uploads/2013/10/nh3fcx-song-charng-kong.pdf.
115. ↑ White, Alfred H.; Melville, Wm. (April 1905). "The Decomposition of Ammonia at High Temperatures" (in en). Journal of the American Chemical Society 27 (4): 373–386. doi:10.1021/ja01982a005. ISSN 0002-7863. Bibcode: 1905JAChS..27..373W. https://pubs.acs.org/doi/abs/10.1021/ja01982a005.
116. ↑ Nikitaeva, Daria; Thomas, Dale L. (July 2022). "Alternative Propellant Nuclear Thermal Propulsion Engine Architectures". Journal of Spacecraft and Rockets 59 (4): 1149–1160. doi:10.2514/1.A35289. ISSN 0022-4650. https://arc.aiaa.org/doi/10.2514/1.A35289.
117. ↑ "Will Saudi Arabia build the world's largest green hydrogen and ammonia plant?". 17 September 2020. https://energypost.eu/will-saudi-arabia-build-the-worlds-largest-green-hydrogen-and-ammonia-plant/.
118. ↑ "Diesel: Greener Than You Think". http://www.businessweek.com/bwdaily/dnflash/content/mar2008/db20080321_748642_page_3.htm.
119. ↑ "Phosgene: Health and Safety Guide". International Programme on Chemical Safety. 1998. http://www.inchem.org/documents/hsg/hsg/hsg106.htm.
120. ↑ "Anhydrous ammonia tank locks have flaws". Cedar Rapids Gazette. 6 October 2009. http://thegazette.com/2009/10/06/anhydrous-ammonia-tank-locks-have-flaws.
121. ↑ "Illinois Attorney General | Basic Understanding of Meth". Illinoisattorneygeneral.gov. http://www.illinoisattorneygeneral.gov/methnet/understandingmeth/basics.html.
122. ↑ Greenberg, Michael I. (1 January 2003) (in en). Occupational, Industrial, and Environmental Toxicology. Elsevier Health Sciences. ISBN 978-0-323-01340-6. https://books.google.com/books?id=NnZ23IqU4SoC&q=ammonia+birch+method+danger&pg=PA759.
123. ↑ Włochowicz, A.; Stelmasiak, E. (1983). "Change in thermal properties of wool after treatment with liquid ammonia". Journal of Thermal Analysis and Calorimetry 26 (1): 17. doi:10.1007/BF01914084.
124. ↑ Horkheimer, Donald (2005). "Ammonia – A Solution for Airships Demanding Rapid Changes in Net Buoyancy". AIAA 5th ATIO and 16th Lighter-Than-Air Sys Tech. And Balloon Systems Conferences. doi:10.2514/6.2005-7393. ISBN 978-1-62410-067-3. https://doi.org/10.2514/6.2005-7393. Retrieved 27 October 2022.
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126. ↑ minerals year book, vol. 3
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128. ↑ Ammonia, IDLH Documentation
129. ↑ (OSHA) Source: Sax, N. Irving (1984) Dangerous Properties of Industrial Materials. 6th Ed. Van Nostrand Reinhold. ISBN 0-442-28304-0.
130. ↑ Is Anhydrous Ammonia covered under the Hazardous Materials Safety Permit Program? from the website of the United States Department of Transportation (DOT)
131. ↑ Berg, J. M.; Tymoczko, J. L.; Stryer, L. (2002). Biochemistry (5th ed.). https://www.ncbi.nlm.nih.gov/books/NBK22450/.
132. ↑ Wang, Mingyi; Kong, Weimeng; Marten, Ruby; He, Xu-Cheng; Chen, Dexian; Pfeifer, Joschka; Heitto, Arto; Kontkanen, Jenni et al. (13 May 2020). "Rapid growth of new atmospheric particles by nitric acid and ammonia condensation" (in en). Nature 581 (7807): 184–189. doi:10.1038/s41586-020-2270-4. ISSN 1476-4687. PMID 32405020. Bibcode: 2020Natur.581..184W.
133. ↑ Talhout, Reinskje; Schulz, Thomas; Florek, Ewa; Van Benthem, Jan; Wester, Piet; Opperhuizen, Antoon (2011). "Hazardous Compounds in Tobacco Smoke". International Journal of Environmental Research and Public Health 8 (12): 613–628. doi:10.3390/ijerph8020613. ISSN 1660-4601. PMID 21556207.
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135. ↑ Vasudevan Rajaram; Subijoy Dutta; Krishna Parameswaran (30 June 2005). Sustainable Mining Practices: A Global Perspective. CRC Press. p. 113. ISBN 978-1-4398-3423-7. https://books.google.com/books?id=5uTM2jFMzH4C&pg=PA113.
136. ↑ 136.0 136.1 136.2 Oram, Brian. "Ammonia in Groundwater, Runoff, and Streams". http://www.water-research.net/index.php/ammonia-in-groundwater-runoff-and-streams.
137. ↑ Hargreaves, J.A.; Tucker, C.S. (2004). Managing ammonia in fish ponds. Southern Regional Aquaculture Center.
138. ↑ 138.0 138.1 138.2 Sergeant, Chris (5 February 2014). "The Management of Ammonia Levels in an Aquaculture Environment". Water/Wastewater. http://www.pollutionsolutions-online.com/articles/water-wastewater/17/chris_sergeant/the_management_of_ammonia_levels_in_an_aquaculture_environment/1557/. Retrieved 3 December 2014.
139. ↑ Electronic Code of Federal Regulations: . Ecfr.gpoaccess.gov. Retrieved on 22 December 2011.
140. ↑ "Ammonia Tanks – Carbon and Stainless Steel Construction". https://ammoniatanks.com/.
141. ↑ "Nitrogen Statistics and Information U.S. Geological Survey". https://www.usgs.gov/centers/national-minerals-information-center/nitrogen-statistics-and-information.
142. ↑ 142.0 142.1 "Nitrogen (Fixed)--Ammonia (2022)". https://pubs.usgs.gov/periodicals/mcs2022/mcs2022-nitrogen.pdf.
143. ↑ "Nobel Prize in Chemistry (1918) – Haber–Bosch process". http://nobelprize.org/chemistry/laureates/1918/press.html.
144. ↑ "Chemistry of the Group 2 Elements – Be, Mg, Ca, Sr, Ba, Ra". BBC.co.uk. https://h2g2.com/edited_entry/A1002934.
145. ↑ Fichter, Fr.; Girard, Pierre; Erlenmeyer, Hans (1 December 1930). "Elektrolytische Bindung von komprimiertem Stickstoff bei gewöhnlicher Temperatur" (in en). Helvetica Chimica Acta 13 (6): 1228–1236. doi:10.1002/hlca.19300130604. Bibcode: 1930HChAc..13.1228F. https://onlinelibrary.wiley.com/doi/10.1002/hlca.19300130604.
146. ↑ Bjarke Valbæk Mygind, Jon; Pedersen, Jakob B.; Li, Katja; Deissler, Niklas H.; Saccoccio, Mattia; Fu, Xianbiao; Li, Shaofeng; Sažinas, Rokas et al. (22 November 2023). "Is Ethanol Essential for the Lithium-Mediated Nitrogen Reduction Reaction?" (in en). ChemSusChem 16 (22). doi:10.1002/cssc.202301011. ISSN 1864-5631. PMID 37681646. Bibcode: 2023ChSCh..16E1011B.
147. ↑ 147.0 147.1 Lazouski, Nikifar; Schiffer, Zachary J.; Williams, Kindle; Manthiram, Karthish (17 April 2019). "Understanding Continuous Lithium-Mediated Electrochemical Nitrogen Reduction" (in en). Joule 3 (4): 1127–1139. doi:10.1016/j.joule.2019.02.003. ISSN 2542-4351. Bibcode: 2019Joule...3.1127L.
148. ↑ Tsuneto, Akira; Kudo, Akihiko; Sakata, Tadayoshi (4 March 1994). "Lithium-mediated electrochemical reduction of high pressure N2 to NH3" (in en). Journal of Electroanalytical Chemistry 367 (1): 183–188. doi:10.1016/0022-0728(93)03025-K. ISSN 1572-6657.
149. ↑ Andersen, Suzanne Z.; Čolić, Viktor; Yang, Sungeun; Schwalbe, Jay A.; Nielander, Adam C.; McEnaney, Joshua M.; Enemark-Rasmussen, Kasper; Baker, Jon G. et al. (June 2019). "A rigorous electrochemical ammonia synthesis protocol with quantitative isotope measurements" (in en). Nature 570 (7762): 504–508. doi:10.1038/s41586-019-1260-x. ISSN 1476-4687. PMID 31117118. Bibcode: 2019Natur.570..504A. https://www.nature.com/articles/s41586-019-1260-x.
150. ↑ Lazouski, Nikifar; Chung, Minju; Williams, Kindle; Gala, Michal L.; Manthiram, Karthish (1 May 2020). "Non-aqueous gas diffusion electrodes for rapid ammonia synthesis from nitrogen and water-splitting-derived hydrogen" (in en). Nature Catalysis 3 (5): 463–469. doi:10.1038/s41929-020-0455-8. ISSN 2520-1158. Bibcode: 2020NatCa...3..463L. https://www.nature.com/articles/s41929-020-0455-8.
151. ↑ 151.0 151.1 Suryanto, Bryan H. R.; Matuszek, Karolina; Choi, Jaecheol; Hodgetts, Rebecca Y.; Du, Hoang-Long; Bakker, Jacinta M.; Kang, Colin S. M.; Cherepanov, Pavel V. et al. (11 June 2021). "Nitrogen reduction to ammonia at high efficiency and rates based on a phosphonium proton shuttle" (in en). Science 372 (6547): 1187–1191. doi:10.1126/science.abg2371. ISSN 0036-8075. PMID 34112690. Bibcode: 2021Sci...372.1187S. https://www.science.org/doi/10.1126/science.abg2371.
152. ↑ Lavars, Nick (30 November 2021). "Green ammonia electrolysis breakthrough could finally kill Haber–Bosch" (in en-US). https://newatlas.com/energy/green-ammonia-phosphonium-production/.
153. ↑ Blaine, Loz (19 November 2021). "FuelPositive promises green ammonia at 60% the cost of today's gray" (in en-US). https://newatlas.com/energy/fuelpositive-green-ammonia/.
154. ↑ Fu, Xianbiao; Pedersen, Jakob B.; Zhou, Yuanyuan; Saccoccio, Mattia; Li, Shaofeng; Sažinas, Rokas; Li, Katja; Andersen, Suzanne Z. et al. (16 February 2022). "Continuous-flow electrosynthesis of ammonia by nitrogen reduction and hydrogen oxidation" (in en). Science 379 (6633): 707–712. doi:10.1126/science.adf4403. PMID 36795804. https://www.science.org/doi/10.1126/science.adf4403.
155. ↑ Roth, Karl S.. "eMedicine Specialties > Metabolic Diseases > Hyperammonemia". http://emedicine.medscape.com/article/944996-overview.
156. ↑ Mohiuddin, S. S.; Khattar, D. (2023). Biochemistry, Ammonia. Treasure Island. PMID 31082083. https://www.ncbi.nlm.nih.gov/books/NBK541039/#:~:text=Ammonia is loaded via glutamine,low concentrations in the liver..
157. ↑ Nelson, David L.; Cox, Michael M. (2005), Principles of Biochemistry (4th ed.), New York: W. H. Freeman, p. 632-633, ISBN 0-7167-4339-6
158. ↑ Shibata, Naoki; Tamagaki, Hiroko; Hieda, Naoki; Akita, Keita; Komori, Hirofumi; Shomura, Yasuhito; Terawaki, Shin-Ichi; Mori, Koichi et al. (2010). "Crystal Structures of Ethanolamine Ammonia-lyase Complexed with Coenzyme B12 Analogs and Substrates". Journal of Biological Chemistry 285 (34): 26484–26493. doi:10.1074/jbc.M110.125112. PMID 20519496.
159. ↑ "Nitrogen Fixation and Inoculation of Forage Legumes". University of Florida IFAS Extension. June 2002. http://edis.ifas.ufl.edu/AG152.
160. ↑ Identifying the direct effects of ammonia on the brain – PubMed
161. ↑ Igarashi, Robert Y.; Laryukhin, Mikhail; Dos Santos, Patricia C.; Lee, Hong-In; Dean, Dennis R.; Seefeldt, Lance C.; Hoffman, Brian M. (May 2005). "Trapping H- Bound to the Nitrogenase FeMo-Cofactor Active Site during H2 Evolution: Characterization by ENDOR Spectroscopy". Journal of the American Chemical Society 127 (17): 6231–6241. doi:10.1021/ja043596p. PMID 15853328. Bibcode: 2005JAChS.127.6231I.
162. ↑ Zschocke, Johannes; Hoffman, Georg (2004). Vademecum Metabolism. Schattauer Verlag. ISBN 978-3-7945-2385-6.
163. ↑ Rose, Burton; Helmut Rennke (1994). Renal Pathophysiology. Baltimore: Williams & Wilkins. ISBN 978-0-683-07354-6. https://archive.org/details/renalpathophysio0000rose.
164. ↑ Campbell, Neil A.; Jane B. Reece (2002). "44". Biology (6th ed.). San Francisco: Pearson Education, Inc. pp. 937–938. ISBN 978-0-8053-6624-2. https://archive.org/details/biologyc00camp.
165. ↑ Edited by Kirk Munsell. Image page credit Lunar and Planetary Institute. NASA. "NASA's Solar Exploration: Multimedia: Gallery: Gas Giant Interiors ". Retrieved 26 April 2006.
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167. ↑ 167.0 167.1 Ho, P. T. P.; Townes, C. H. (1983). "Interstellar ammonia". Annu. Rev. Astron. Astrophys. 21 (1): 239–70. doi:10.1146/annurev.aa.21.090183.001323. Bibcode: 1983ARA&A..21..239H.
168. ↑ Millar, T. J. (2003). "Deuterium Fractionation in Interstellar Clouds". Space Science Reviews 106 (1): 73–86. doi:10.1023/A:1024677318645. Bibcode: 2003SSRv..106...73M.
169. ↑ Ungerechts, H.; Walmsley, C. M.; Winnewisser, G. (1980). "Ammonia and cyanoacetylene observations of the high-density core of L-183 (L-134-N)". Astron. Astrophys. 88: 259. Bibcode: 1980A&A....88..259U. http://cdsads.u-strasbg.fr/cgi-bin/nph-journal_query?volume=88&plate_select=NO&page=259&plate=&cover=&journal=A+A...
170. ↑ Genzel, R.; Downes, D.; Ho, P. T. P. (1982). "NH3 in Orion-KL – A new interpretation". Astrophysical Journal 259: L103. doi:10.1086/183856. Bibcode: 1982ApJ...259L.103G.
171. ↑ "The UMIST data for Astrochemistry". http://udfa.net/.
172. ↑ Vikor, L.; Al-Khalili, A.; Danared, H.; Djuric, N.; Dunn, G. H.; Larsson, M.; Le Padellec, A.; Rosen, S. et al. (1999). "Branching fractions of dissociative recombination of NH4+ and NH2+ molecular ions". Astronomy and Astrophysics 344: 1027. Bibcode: 1999A&A...344.1027V. http://cdsads.u-strasbg.fr/cgi-bin/nph-journal_query?volume=344&plate_select=NO&page=1027&plate=&cover=&journal=A+A...
173. ↑ van Dishoeck, E. F.; Black, J. H. (1986). "Comprehensive models of diffuse interstellar clouds – Physical conditions and molecular abundances". Astrophys. J. Suppl. Ser. 62: 109–145. doi:10.1086/191135. Bibcode: 1986ApJS...62..109V. https://openaccess.leidenuniv.nl/bitstream/handle/1887/1980/8_352_018.pdf?sequence=1.
174. ↑ "astrochemistry.net". astrochemistry.net. http://astrochemistry.net.
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177. ↑ Smith, D.; Adams, N. G. (1977). "Reactions of CH+n IONS with ammonia at 300 K". Chemical Physics Letters 47 (1): 145. doi:10.1016/0009-2614(77)85326-8. Bibcode: 1977CPL....47..145S.
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181. ↑ Morris, M.; Zuckerman, B.; Palmer, P.; Turner, B. E. (1973). "Interstellar ammonia". Astrophysical Journal 186: 501. doi:10.1086/152515. Bibcode: 1973ApJ...186..501M.
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### Works cited

* "Aqua Ammonia". airgasspecialtyproducts.com. http://www.airgasspecialtyproducts.com/Libraries/Aqua_Ammonia_Technical_Data_Manual/Physical_Properties.sflb.ashx.
* This article incorporates text from a publication now in the public domain: Chisholm, Hugh, ed (1911). "Ammonia". Encyclopædia Britannica. 1 (11th ed.). Cambridge University Press. pp. 861–863.
* Clark, Jim (April 2013). "The Haber Process" (in en). https://chemguide.co.uk/physical/equilibria/haber.html.

## Further reading

* Bretherick, L., ed (1986). Hazards in the Chemical Laboratory (4th ed.). London: Royal Society of Chemistry. ISBN 978-0-85186-489-1. OCLC 16985764. https://archive.org/details/hazardsinchemica0004unse.
* Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
* Template:Housecroft1st
* Weast, R. C., ed (1972). Handbook of Chemistry and Physics (53rd ed.). Cleveland, OH: Chemical Rubber Co..
* Schmidt, Eckart W. (2022). Encyclopedia of Liquid Fuels. De Gruyter. pp. 703–844. doi:10.1515/9783110750287-008. ISBN 978-3-11-075028-7.

## External links

* International Chemical Safety Card 0414 (anhydrous ammonia), ilo.org.
* International Chemical Safety Card 0215 (aqueous solutions), ilo.org.
* CID 222 from PubChem
* "Ammoniac et solutions aqueuses" (in fr). Institut National de Recherche et de Sécurité. http://www.inrs.fr/fichetox/ft16.html.
* Emergency Response to Ammonia Fertiliser Releases (Spills) for the Minnesota Department of Agriculture.ammoniaspills.org
* National Institute for Occupational Safety and Health–Ammonia Page, cdc.gov
* NIOSH Pocket Guide to Chemical Hazards–Ammonia, cdc.gov
* Ammonia, video

* v
* t
* e

Nitrogen species

* Hydrides:
* NH3
* NH4+
* NH2− MNH2
* N3−
* NH2OH
* N2H4
* N3–
* Organic:
* -NH2
* -CHR=NHR
* -CONHR2
* HCN
* CN−
* C2N2
* H2NCN
* CH2N2
* Oxides:
* N2O
* NO
* NO2
* N2O3
* N2O4
* N2O5
* H2N2O2
* H4N2O4
* HNO2
* HNO3
* HONO3
* HN2O2−
* N2O22−
* NO2−
* ONOO−
* NO3−
* NO43−
* O2NOO−
* NO+
* NO2+
* Halides:
* NF3
* NCl3
* NBr3
* NI3
* FN3
* ClN3
* BrN3
* NH2Cl
* NHCl2

Chemical formulas

* v
* t
* e

Binary compounds of hydrogen

Alkali metal (Group 1) hydrides|

* LiH
* NaH
* KH
* RbH
* CsH

Lithium hydride, LiH
ionic metal hydride

Beryllium hydride
Left (gas phase): BeH2
covalent metal hydride
Right: (BeH2)n (solid phase)
polymeric metal hydride

Borane and diborane
Left: BH3 (special conditions), covalent metalloid hydride
Right: B2H6 (standard conditions), dimeric metalloid hydride

Methane, CH4
covalent nonmetal hydride

Ammonia, NH3
covalent nonmetal hydride

Water, H2O
covalent nonmetal hydride

Hydrogen fluoride, HF
covalent nonmetal hydride

Alkaline (Group 2) earth hydrides|

| Monohydrides|

* BeH
* MgH
* CaH
* SrH
* BaH

|

Dihydrides|

* BeH2
* MgH2
* CaH2
* SrH2
* BaH2

|

Group 13 hydrides|

| Boranes|

* BH3
* B2H6
* B2H2
* B2H4
* B4H10
* B5H9
* B5H11
* B6H10
* B6H12
* B10H14
* B18H22

|

Alanes|

* AlH3
* Al2H6

|

Gallanes|

* GaH3
* Ga2H6

|

Indiganes|

* InH3
* In2H6

|

Thallanes|

* TlH3
* Tl2H6

|

Group 14 hydrides|

| Linear alkanes|

* CH4
* C2H6
* C3H8
* C4H10
* C5H12
* C6H14
* C7H16
* C8H18
* C9H20
* C10H22
* more...

|

Linear alkenes|

* C2H4
* C3H6
* C4H8
* C5H10
* C6H12
* C7H14
* C8H16
* C9H18
* C10H20
* more...

|

Linear alkynes|

* C2H2
* C3H4
* C4H6
* C5H8
* C6H10
* C7H12
* C8H14
* C9H16
* C10H18
* more...

|

Silanes|

* SiH4
* Si2H6
* Si3H8
* Si4H10
* Si5H12
* Si6H14
* Si7H16
* Si8H18
* Si9H20
* Si10H22
* more...

|

Silenes|

* Si2H4

|

Silynes|

* Si2H2
* SiH

|

Germanes|

* GeH4
* Ge2H6
* Ge3H8
* Ge4H10
* Ge5H12

|

Stannanes|

* SnH4
* Sn2H6

|

Plumbanes|

* PbH4

|

* CH
* CH2
* CH3
* C2H
* Cycloalkanes
* Cycloalkenes
* Annulenes
* Many more

Pnictogen (Group 15) hydrides|

| Azanes|

* NH3
* N2H4
* N3H5
* N4H6
* N5H7
* N6H8
* N7H9
* N8H10
* N9H11
* N10H12
* more...

|

Azenes|

* N2H2
* N3H3
* N4H4

|

Phosphanes|

* PH3
* P2H4
* P3H5
* P4H6
* P5H7
* P6H8
* P7H9
* P8H10
* P9H11
* P10H12
* more...

|

Phosphenes|

* P2H2
* P3H3
* P4H4

|

Arsanes|

* AsH3
* As2H4

|

Stibanes|

* SbH3

|

Bismuthanes|

* BiH3

|

* HN3
* NH
* radical

Hydrogen chalcogenides (Group 16 hydrides)|

| Polyoxidanes|

* H2O
* H2O2
* H2O3
* H2O4
* H2O5
* H2O6
* H2O7
* H2O8
* H2O9
* H2O10
* more...

|

Polysulfanes|

* H2S
* H2S2
* H2S3
* H2S4
* H2S5
* H2S6
* H2S7
* H2S8
* H2S9
* H2S10
* more...

|

Selanes|

* H2Se
* H2Se2

|

Tellanes|

* H2Te
* H2Te2

|

Polanes|

* PoH2

|

* HO
* HO2
* HO3
* H2O+–O–
* H2S=S
* (HS)2S+–S–
* HS
* HDO
* D2O
* T2O

Hydrogen halides (Group 17 hydrides)|

* HF
* HCl
* HBr
* HI
* HAt

Transition metal hydrides|

* ScH2
* YH2
* YH3
* TiH2
* ZrH2
* HfH2
* VH
* VH2
* NbH
* NbH2
* TaH
* CrH
* CrH2
* CrHx
* NiH
* PdHx (x < 1)
* FeH
* FeH2
* FeH5
* CuH
* ZnH2
* CdH2
* HgH2

Lanthanide hydrides|

* LaH2
* LaH3
* LaH10
* CeH2
* CeH3
* PrH2
* PrH3
* NdH2
* NdH3
* SmH2
* SmH3
* EuH2
* GdH2
* GdH3
* TbH2
* TbH3
* DyH2
* DyH3
* HoH2
* HoH3
* ErH2
* ErH3
* TmH2
* TmH3
* YbH2
* YbH2.5
* LuH2
* LuH3

Actinide hydrides|

* AcH2
* ThH2
* Th4H15
* PaH3
* UH3
* NpH2
* NpH3
* PuH2
* PuH3
* AmH2
* AmH3
* CmH2

* v
* t
* e

Molecules detected in outer space

Molecules|

| Diatomic|

* Aluminium monochloride
* Aluminium monofluoride
* Aluminium monoxide
* Argonium
* Carbon monophosphide
* Carbon monosulfide
* Carbon monoxide
* Carborundum
* Cyanogen radical
* Diatomic carbon
* Fluoromethylidynium
* Helium hydride ion
* Hydrogen chloride
* Hydrogen fluoride
* Hydrogen (molecular)
* Hydroxyl radical
* Iron(II) oxide
* Magnesium monohydride cation
* Methylidyne radical
* Nitric oxide
* Nitrogen (molecular)
* Nitrogen monohydride
* Nitrogen sulfide
* Oxygen (molecular)
* Phosphorus monoxide
* Phosphorus mononitride
* Potassium chloride
* Silicon carbide
* Silicon mononitride
* Silicon monoxide
* Silicon monosulfide
* Sodium chloride
* Sodium iodide
* Sulfur monohydride
* Sulfur monoxide
* Titanium oxide

|
|

Triatomic|

* Aluminium hydroxide
* Aluminium isocyanide
* Amino radical
* Carbon dioxide
* Carbonyl sulfide
* CCP radical
* Chloronium
* Diazenylium
* Dicarbon monoxide
* Disilicon carbide
* Ethynyl radical
* Formyl radical
* Hydrogen cyanide (HCN)
* Hydrogen isocyanide (HNC)
* Hydrogen sulfide
* Hydroperoxyl
* Iron cyanide
* Isoformyl
* Magnesium cyanide
* Magnesium isocyanide
* Methylene radical
* N2H+
* Nitrous oxide
* Nitroxyl
* Ozone
* Phosphaethyne
* Potassium cyanide
* Protonated molecular hydrogen
* Sodium cyanide
* Sodium hydroxide
* Silicon carbonitride
* c-Silicon dicarbide
* SiNC
* Sulfur dioxide
* Thioformyl
* Thioxoethenylidene
* Titanium dioxide
* Tricarbon
* Water

Four
atoms|

* Acetylene
* Ammonia
* Cyanic acid
* Cyanoethynyl
* Cyclopropynylidyne
* Formaldehyde
* Fulminic acid
* HCCN
* Hydrogen peroxide
* Hydromagnesium isocyanide
* Isocyanic acid
* Isothiocyanic acid
* Ketenyl
* Methylene amidogen
* Methyl radical
* Propynylidyne
* Protonated carbon dioxide
* Protonated hydrogen cyanide
* Silicon tricarbide
* Thioformaldehyde
* Tricarbon monoxide
* Tricarbon sulfide
* Thiocyanic acid

Five
atoms|

* Ammonium ion
* Butadiynyl
* Carbodiimide
* Cyanamide
* Cyanoacetylene
* Cyanoformaldehyde
* Cyanomethyl
* Cyclopropenylidene
* Formic acid
* Isocyanoacetylene
* Ketene
* Methane
* Methoxy radical
* Methylenimine
* Propadienylidene
* Protonated formaldehyde
* Protonated formaldehyde
* Silane
* Silicon-carbide cluster

Six
atoms|

* Acetonitrile
* Cyanobutadiynyl radical
* E-Cyanomethanimine
* Cyclopropenone
* Diacetylene
* Ethylene
* Formamide
* HC4N
* Ketenimine
* Methanethiol
* Methanol
* Methyl isocyanide
* Pentynylidyne
* Propynal
* Protonated cyanoacetylene

Seven
atoms|

* Acetaldehyde
* Acrylonitrile
* Vinyl cyanide
* Cyanodiacetylene
* Ethylene oxide
* Glycolonitrile
* Hexatriynyl radical
* Methylacetylene
* Methylamine
* Methyl isocyanate
* Vinyl alcohol

Eight
atoms|

* Acetic acid
* Aminoacetonitrile
* Cyanoallene
* Ethanimine
* Glycolaldehyde
* Heptatrienyl radical
* Hexapentaenylidene
* Methylcyanoacetylene
* Methyl formate
* Propenal

Nine
atoms|

* Acetamide
* Cyanohexatriyne
* Cyanotriacetylene
* Dimethyl ether
* Ethanol
* Methyldiacetylene
* Octatetraynyl radical
* Propene
* Propionitrile

Ten
atoms
or more|

* Acetone
* Benzene
* Benzonitrile
* Buckminsterfullerene (C60, C60+, fullerene, buckyball)
* C70 fullerene
* Cyanodecapentayne
* Cyanopentaacetylene
* Cyanotetra-acetylene
* Ethylene glycol
* Ethyl formate
* Methyl acetate
* Methyl-cyano-diacetylene
* Methyltriacetylene
* Propanal
* n-Propyl cyanide
* Pyrimidine

Deuterated
molecules|

* Ammonia
* Ammonium ion
* Formaldehyde
* Formyl radical
* Heavy water
* Hydrogen cyanide
* Hydrogen deuteride
* Hydrogen isocyanide
* Methylacetylene
* N2D+
* Trihydrogen cation

Unconfirmed|

* Anthracene
* Dihydroxyacetone
* Ethyl methyl ether
* Glycine
* Graphene
* H2NCO+
* Linear C5
* Naphthalene cation
* Phosphine
* Pyrene
* Silylidine

Related|

* Abiogenesis
* Astrobiology
* Astrochemistry
* Atomic and molecular astrophysics
* Chemical formula
* Circumstellar envelope
* Cosmic dust
* Cosmic ray
* Cosmochemistry
* Diffuse interstellar band
* Earliest known life forms
* Extraterrestrial life
* Extraterrestrial liquid water
* Forbidden mechanism
* Homochirality
* Intergalactic dust
* Interplanetary medium
* Interstellar medium
* Photodissociation region
* Iron–sulfur world theory
* Kerogen
* Molecules in stars
* Nexus for Exoplanet System Science
* Organic compound
* Outer space
* PAH world hypothesis
* Panspermia
* Polycyclic aromatic hydrocarbon (PAH)
* RNA world hypothesis
* Spectroscopy
* Tholin

* Category:Astrochemistry
*   *   *

* v
* t
* e

Salts and covalent derivatives of the nitride ion

NH3 |  |  |  | He(N2)11

|
|
|
|

Li3N | Be3N2 | BN | β-C3N4
g-C3N4 | N2 | NxOy | NF3 | Ne
Na3N | Mg3N2 | AlN | Si3N4 | PN
P3N5 | SxNy

S4N4 | NCl3 | Ar
K3N | Ca3N2 | ScN | TiN | VN | CrN
Cr2N | MnxNy | FexNy | CoN | Ni3N | CuN | Zn3N2 | GaN | Ge3N4 | As  | Se  | NBr3 | Kr
Rb3N | Sr3N2 | YN | ZrN | NbN | β-Mo2N | Tc  | Ru  | Rh  | PdN | Ag3N | CdN | InN | Sn  | Sb  | Te  | NI3 | Xe
Cs3N | Ba3N2 |  | Hf3N4 | TaN | WN | Re  | Os  | Ir  | Pt  | Au  | Hg3N2 | TlN | Pb  | BiN | Po  | At  | Rn
Fr3N | Ra3N |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
La  | CeN | Pr  | Nd  | Pm  | Sm  | Eu  | GdN | Tb  | Dy  | Ho  | Er  | Tm  | Yb  | Lu
Ac  | Th  | Pa  | UN | Np  | Pu  | Am  | Cm  | Bk  | Cf  | Es  | Fm  | Md  | No  | Lr

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Original source: https://en.wikipedia.org/wiki/Ammonia. Read more

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*[H335]: May cause respiratory irritation
*[H400]: Very toxic to aquatic life
*[H411]: Toxic to aquatic life with long lasting effects
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