AMMONIA %25 (AMONYAK %25)

AMMONIA %25 (AMONYAK %25)

AMMONIA %25 (AMONYAK %25)

CAS No. : 7664-41-7

EC No. : 231-635-3

Synonyms:

ammonia; 7664-41-7; azane; Ammonia gas; Spirit of hartshorn; Nitro-sil; Ammonia, anhydrous; Ammoniakgas; Ammonia anhydrous; Anhydrous ammonia; Ammoniak; AM-Fol; Liquid Ammonia; Ammoniak Kconzentrierter; Amoniak [Polish]; Ammoniac [French]; Ammoniak [German]; ammoniac; Ammoniaca [Italian]; Caswell No. 041; Ammonia (conc 20% or greater); NH3; CCRIS 2278; HSDB 162; UN 2073 (>44% solution); UN1005; Aminomethyl Polystyrene Resin; azanediyl (triplet); EPA Pesticide Chemical Code 005302; UNII-5138Q19F1X; R 717; UN 1005 (anhydrous gas or >50% solution); UN 2672 (between 12% and 44% solution); EINECS 231-635-3; CHEBI:16134; MFCD00011418; 5138Q19F1X; Ammonia-14N; Ammonia solution, strong (NF); Ammonia solution, strong [NF]; amoniaco; Ammoniaca; Amoniak; Ammonia, ca. 7N solution in methanol; Ammonia (includes anhydrous ammonia and aqueous ammonia from water dissociable ammonium salts and other sources; 10% of total aqueous ammonia is reportable under this listing); Ammonia, anhydrous, liquefied or ammonia solutions, relative density <0.880 at 15 C in water, with >50% ammonia [UN1005] [Nonflammable gas]; Ammonia, anhydrous, liquefied or ammonia solutions, relative density <0.880 at 15 C in water, with >50% ammonia [UN1005] [Poison gas, Corrosive]; Ammonia, 2M solution in methanol, AcroSeal(R); (Aminomethyl)polystyrene; Ammonia, ca. 7N solution in methanol, AcroSeal(R); Ammonia, 0.5M solution in 1,4-dioxane, AcroSeal(R);tertiaeres Amin; Aminyl radical; ammonia ca; primaeres Amin; Ammonia inhalant; Ammoniacum gummi; sekundaeres Amin; anyhydrous ammonia; (Aminomethyl)polystyrene, 100-200 mesh, extent of labeling: ~0.5 mmol/g amine loading; NH4;UNX; Refrigerent R717; Strong Ammonia Solution; ACMC-1BKZC; Ammonia (8CI,9CI); Ammonia water (JP15); Aromatic ammonia vaporole; Dowex(R) 66 free base; Aromatic Ammonia, Vaporole; EC 231-635-3; Ammonia solution strong (NF); Ammonia solution strong [usan]; INS NO.527; N H3; ammonium isovalerate 30% in pg; CHEMBL1160819; DTXSID0023872; CTK0I1955; Ammonia solution, strong [USAN]; DTXSID40912315; DTXSID80420101; INS-527; [NH3]; NH(3); Ammonia solution, 0.4 M in THF; Ammonia solution, 4 M in methanol; Ammonia solution, 7 N in methanol; Ammonia, anhydrous, >=99.98%; ACT02989; Ammonia solution 2.0 M in ethanol; Ammonia solution 2.0 M in methanol; Ammonia solution, 0.5 M in dioxane; Ammonia solution, 2.0 M in ethanol; AKOS015916403; Ammonia anhydrous 170g Lecture bottle; Ammonia solution, 2.0 M in methanol; Ammonia solution 2.0 M in isopropanol; MCULE-5646000632; Ammonia 0.5M solution in 1,4-Dioxane; Ammonia solution, 2.0 M in isopropanol; Ammonia, puriss., anhydrous, >=99.9%; LS-16633; SC-46302; Ammonia solution 0.25M in tetrahydrofuran; Ammonia, puriss., anhydrous, >=99.95%; E-527; NS00013356; Q4087; R-717; Ammonia, 0.5M solution in THF, AcroSeal(R); C00014; D02916; Dowex(R) Marathon(TM) WBA free base, free base; Q4832241; Q6004010; Q27110025; (Aminomethyl)polystyrene, 100-200 mesh, extent of labeling: ~2 mmol/g amine loading; (Aminomethyl)polystyrene, 200-400 mesh, extent of labeling: ~0.6 mmol/g amine loading; (Aminomethyl)polystyrene, 200-400 mesh, extent of labeling: ~1.5 mmol/g amine loading; (Aminomethyl)polystyrene, 400-500 mum, extent of labeling: 1-2 mmol/g amine loading; (Aminomethyl)polystyrene, 100-200 mesh, extent of labeling: 0.5-1.0 mmol/g N loading, 1 % cross-linked; (Aminomethyl)polystyrene, 100-200 mesh, extent of labeling: 1.0 mmol/g N loading, 1 % cross-linked; (Aminomethyl)polystyrene, 200-400 mesh, extent of labeling: 1.0-1.5 mmol/g N loading, 1 % cross-linked; (Aminomethyl)polystyrene, 200-400 mesh, extent of labeling: 1.0-2.0 mmol/g loading, 2 % cross-linked; (Aminomethyl)polystyrene, 200-400 mesh, extent of labeling: 4.0 mmol/g loading, 2 % cross-linked; (Aminomethyl)polystyrene, 50-100 mesh, extent of labeling: 2.0 mmol/g loading, 1 % cross-linked; (Aminomethyl)polystyrene, 70-90 mesh, extent of labeling: 1.0-1.5 mmol/g N loading, 1 % cross-linked; (Aminomethyl)polystyrene, 70-90 mesh, extent of labeling: 1.5-2.0 mmol/g N loading, 1 % cross-linked; (Aminomethyl)polystyrene, macroporous, 30-60 mesh, extent of labeling: 1.5-3.0 mmol/g loading; (Aminomethyl)polystyrene, macroporous, 70-90 mesh, extent of labeling: 1.5-3.0 mmol/g loading; Ammonia (includes anhydrous ammonia and aqueous ammonia from water dissociable ammonium salts and other sources 10% of total aqueous ammonia is reportable under this listing); Ammonia, anhydrous, liquefied or ammonia solutions, relative density <0.880 at 15 C in water, with >50% ammonia; Ammonia, anhydrous, liquefied or ammonia solutions, relative density <0.880 at 15 C in water, with >50% ammonia [UN1005] [Nonflammable gas]; Ammonia, anhydrous, liquefied or ammonia solutions, relative density <0.880 at 15 C in water, with >50% ammonia [UN1005] [Poison gas, Corrosive];StratoSpheres(TM) PL-AMS resin, 100-200 mesh, extent of labeling: ~1.0 mmol/g loading, 1 % cross-linked with divinylbenzene; StratoSpheres(TM) PL-AMS resin, 100-200 mesh, extent of labeling: 2.0 mmol/g loading, 1 % cross-linked; StratoSpheres(TM) PL-AMS resin, 30-40 mesh, extent of labeling: 1.0 mmol/g loading, 1 % cross-linked; StratoSpheres(TM) PL-AMS resin, 30-40 mesh, extent of labeling: 2.0 mmol/g loading, 1 % cross-linked; StratoSpheres(TM) PL-AMS resin, 50-100 mesh, extent of labeling: 2.0 mmol/g loading, 1 % cross-linked; ÜRE; üre; amonyag; AMONYAG; amanyak; AMANYAK; amoni; AMONI; AMON; ammoni; AMMONI; AMMON; AMONYUM; amonyum; ammoniya; AMMONYA; AMMONIYA; ammonia; 7664-41-7; azane; Ammonia gas; Spirit of hartshorn; Nitro-sil; Ammonia, anhydrous; Ammoniakgas; Ammonia anhydrous; Anhydrous ammonia; Ammoniak; AM-Fol; Liquid Ammonia; Ammoniak Kconzentrierter; Amoniak [Polish]; Ammoniac [French]; Ammoniak [German]; ammoniac; Ammoniaca [Italian]; Caswell No. 041; Ammonia (conc 20% or greater); NH3; CCRIS 2278; HSDB 162; UN 2073 (>44% solution); UN1005; Aminomethyl Polystyrene Resin; azanediyl (triplet); EPA Pesticide Chemical Code 005302; UNII-5138Q19F1X; R 717; UN 1005 (anhydrous gas or >50% solution); UN 2672 (between 12% and 44% solution); EINECS 231-635-3; CHEBI:16134; MFCD00011418; 5138Q19F1X; Ammonia-14N; Ammonia solution, strong (NF); Ammonia solution, strong [NF]; amoniaco; Ammoniaca; Amoniak; Ammonia, ca. 7N solution in methanol; Ammonia (includes anhydrous ammonia and aqueous ammonia from water dissociable ammonium salts and other sources; 10% of total aqueous ammonia is reportable under this listing); Ammonia, anhydrous, liquefied or ammonia solutions, relative density <0.880 at 15 C in water, with >50% ammonia [UN1005] [Nonflammable gas]; Ammonia, anhydrous, liquefied or ammonia solutions, relative density <0.880 at 15 C in water, with >50% ammonia [UN1005] [Poison gas, Corrosive]; Ammonia, 2M solution in methanol, AcroSeal(R); (Aminomethyl)polystyrene; Ammonia, ca. 7N solution in methanol, AcroSeal(R); Ammonia, 0.5M solution in 1,4-dioxane, AcroSeal(R);tertiaeres Amin; Aminyl radical; ammonia ca; primaeres Amin; Ammonia inhalant; Ammoniacum gummi; sekundaeres Amin; anyhydrous ammonia; (Aminomethyl)polystyrene, 100-200 mesh, extent of labeling: ~0.5 mmol/g amine loading; NH4;UNX; Refrigerent R717; Strong Ammonia Solution; ACMC-1BKZC; Ammonia (8CI,9CI); Ammonia water (JP15); Aromatic ammonia vaporole; Dowex(R) 66 free base; Aromatic Ammonia, Vaporole; EC 231-635-3; Ammonia solution strong (NF); Ammonia solution strong [usan]; INS NO.527; N H3; ammonium isovalerate 30% in pg; CHEMBL1160819; DTXSID0023872; CTK0I1955; Ammonia solution, strong [USAN]; DTXSID40912315; DTXSID80420101; INS-527; [NH3]; NH(3); Ammonia solution, 0.4 M in THF; Ammonia solution, 4 M in methanol; Ammonia solution, 7 N in methanol; Ammonia, anhydrous, >=99.98%; ACT02989; Ammonia solution 2.0 M in ethanol; Ammonia solution 2.0 M in methanol; Ammonia solution, 0.5 M in dioxane; Ammonia solution, 2.0 M in ethanol; AKOS015916403; Ammonia anhydrous 170g Lecture bottle; Ammonia solution, 2.0 M in methanol; Ammonia solution 2.0 M in isopropanol; MCULE-5646000632; Ammonia 0.5M solution in 1,4-Dioxane; Ammonia solution, 2.0 M in isopropanol; Ammonia, puriss., anhydrous, >=99.9%; LS-16633; SC-46302; Ammonia solution 0.25M in tetrahydrofuran; Ammonia, puriss., anhydrous, >=99.95%; E-527; NS00013356; Q4087; R-717; Ammonia, 0.5M solution in THF, AcroSeal(R); C00014; D02916; Dowex(R) Marathon(TM) WBA free base, free base; Q4832241; Q6004010; Q27110025; (Aminomethyl)polystyrene, 100-200 mesh, extent of labeling: ~2 mmol/g amine loading; (Aminomethyl)polystyrene, 200-400 mesh, extent of labeling: ~0.6 mmol/g amine loading; (Aminomethyl)polystyrene, 200-400 mesh, extent of labeling: ~1.5 mmol/g amine loading; (Aminomethyl)polystyrene, 400-500 mum, extent of labeling: 1-2 mmol/g amine loading; (Aminomethyl)polystyrene, 100-200 mesh, extent of labeling: 0.5-1.0 mmol/g N loading, 1 % cross-linked; (Aminomethyl)polystyrene, 100-200 mesh, extent of labeling: 1.0 mmol/g N loading, 1 % cross-linked; (Aminomethyl)polystyrene, 200-400 mesh, extent of labeling: 1.0-1.5 mmol/g N loading, 1 % cross-linked; (Aminomethyl)polystyrene, 200-400 mesh, extent of labeling: 1.0-2.0 mmol/g loading, 2 % cross-linked; (Aminomethyl)polystyrene, 200-400 mesh, extent of labeling: 4.0 mmol/g loading, 2 % cross-linked; (Aminomethyl)polystyrene, 50-100 mesh, extent of labeling: 2.0 mmol/g loading, 1 % cross-linked; (Aminomethyl)polystyrene, 70-90 mesh, extent of labeling: 1.0-1.5 mmol/g N loading, 1 % cross-linked; (Aminomethyl)polystyrene, 70-90 mesh, extent of labeling: 1.5-2.0 mmol/g N loading, 1 % cross-linked; (Aminomethyl)polystyrene, macroporous, 30-60 mesh, extent of labeling: 1.5-3.0 mmol/g loading; (Aminomethyl)polystyrene, macroporous, 70-90 mesh, extent of labeling: 1.5-3.0 mmol/g loading; Ammonia (includes anhydrous ammonia and aqueous ammonia from water dissociable ammonium salts and other sources 10% of total aqueous ammonia is reportable under this listing); Ammonia, anhydrous, liquefied or ammonia solutions, relative density <0.880 at 15 C in water, with >50% ammonia; Ammonia, anhydrous, liquefied or ammonia solutions, relative density <0.880 at 15 C in water, with >50% ammonia [UN1005] [Nonflammable gas]; Ammonia, anhydrous, liquefied or ammonia solutions, relative density <0.880 at 15 C in water, with >50% ammonia [UN1005] [Poison gas, Corrosive];StratoSpheres(TM) PL-AMS resin, 100-200 mesh, extent of labeling: ~1.0 mmol/g loading, 1 % cross-linked with divinylbenzene; StratoSpheres(TM) PL-AMS resin, 100-200 mesh, extent of labeling: 2.0 mmol/g loading, 1 % cross-linked; StratoSpheres(TM) PL-AMS resin, 30-40 mesh, extent of labeling: 1.0 mmol/g loading, 1 % cross-linked; StratoSpheres(TM) PL-AMS resin, 30-40 mesh, extent of labeling: 2.0 mmol/g loading, 1 % cross-linked; StratoSpheres(TM) PL-AMS resin, 50-100 mesh, extent of labeling: 2.0 mmol/g loading, 1 % cross-linked; ÜRE; üre; amonyag; AMONYAG; amanyak; AMANYAK; amoni; AMONI; AMON; ammoni; AMMONI; AMMON; AMONYUM; amonyum; ammoniya; AMMONYA; AMMONIYA; 

EN

AMMONIA IUPAC Name azane

AMMONIA InChI InChI=1S/H3N/h1H3

AMMONIA InChI Key QGZKDVFQNNGYKY-UHFFFAOYSA-N

AMMONIA Canonical SMILES N

AMMONIA Molecular Formula NH3

AMMONIA CAS 7664-41-7

AMMONIA Deprecated CAS 208990-07-2, 214478-05-4, 8007-57-6, 558443-52-0, 1026405-88-8

AMMONIA European Community (EC) Number 231-635-3

AMMONIA ICSC Number 0414

AMMONIA RTECS Number BO0875000

AMMONIA UN Number 2073

AMMONIA UNII 5138Q19F1X

AMMONIA FEMA Number 4494

AMMONIA DSSTox Substance ID DTXSID0023872

AMMONIA Molecular Weight 17.031 g/mol

AMMONIA XLogP3-AA -0.7

AMMONIA Hydrogen Bond Donor Count 1

AMMONIA Hydrogen Bond Acceptor Count 1

AMMONIA Rotatable Bond Count 0

AMMONIA Exact Mass 17.026549 g/mol

AMMONIA Monoisotopic Mass 17.026549 g/mol

AMMONIA Topological Polar Surface Area 1 Ų

AMMONIA Heavy Atom Count 1

AMMONIA Formal Charge 0

AMMONIA Complexity 0

AMMONIA Isotope Atom Count 0

AMMONIA Defined Atom Stereocenter Count 0

AMMONIA Undefined Atom Stereocenter Count 0

AMMONIA Defined Bond Stereocenter Count 0

AMMONIA Undefined Bond Stereocenter Count 0

AMMONIA Covalently-Bonded Unit Count 1

AMMONIA Compound Is Canonicalized Yes

Ammonia is a compound of nitrogen and hydrogen with the formula NH3. A stable binary hydride, and the simplest pnictogen hydride, ammonia is a colourless gas with a characteristic pungent smell. It is a common nitrogenous waste, particularly among aquatic organisms, and it contributes significantly to the nutritional needs of terrestrial organisms by serving as a precursor to food and fertilizers. Ammonia, either directly or indirectly, is also a building block for the synthesis of many pharmaceutical products and is used in many commercial cleaning products. It is mainly collected by downward displacement of both air and water.Although common in nature—both terrestrially and in the outer planets of the Solar System—and in wide use, ammonia is both caustic and hazardous in its concentrated form. It is classified as an extremely hazardous substance in the United States, and is subject to strict reporting requirements by facilities which produce, store, or use it in significant quantities.[12]The global industrial production of ammonia in 2018 was 175 million tonnes,[13] with no significant change relative to the 2013 global industrial production of 175 million tonnes.[14] Industrial ammonia is sold either as ammonia liquor (usually 28% ammonia in water) or as pressurized or refrigerated anhydrous liquid ammonia transported in tank cars or cylinders.[15]NH3 boils at −33.34 °C (−28.012 °F) at a pressure of one atmosphere, so the liquid must be stored under pressure or at low temperature. Household ammonia or ammonium hydroxide is a solution of NH3 in water. The concentration of such solutions is measured in units of the Baumé scale (density), with 26 degrees Baumé (about 30% (by weight) ammonia at 15.5 °C or 59.9 °F) being the typical high-concentration commercial product.[16]Pliny, in Book XXXI of his Natural History, refers to a salt produced in the Roman province of Cyrenaica named hammoniacum, so called because of its proximity to the nearby Temple of Jupiter Amun (Greek Ἄμμων Ammon).[17] 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.[18] In any case, that salt ultimately gave ammonia and ammonium compounds their name.Ammonia is a chemical found in trace quantities in nature, being produced from nitrogenous animal and vegetable matter. Ammonia and ammonium salts are also found in small quantities in rainwater, whereas ammonium chloride (sal ammoniac), and ammonium sulfate are found in volcanic districts; crystals of ammonium bicarbonate have been found in Patagonia guano.[19] The kidneys secrete ammonia to neutralize excess acid.[20] Ammonium salts are found distributed through fertile soil and in seawater.Ammonia is also found throughout the Solar System on 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 173 K (−100 °C; −148 °F) 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.[21][22] Substances containing ammonia, or those that are similar to it, are called ammoniacal.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; the liquid boils at −33.3 °C (−27.94 °F), and freezes to white crystals[19] at −77.7 °C (−107.86 °F).Ammonia may be conveniently deodorized by reacting it with either sodium bicarbonate or acetic acid. Both of these reactions form an odourless ammonium salt.The crystal symmetry is cubic, Pearson symbol cP16, space group P213 No.198, lattice constant 0.5125 nm.[23]Liquid ammonia possesses strong ionising powers reflecting its high ε of 22. Liquid ammonia has a very high standard enthalpy change of vaporization (23.35 kJ/mol, cf. water 40.65 kJ/mol, methane 8.19 kJ/mol, phosphine 14.6 kJ/mol) and can therefore be used in laboratories in uninsulated vessels without additional refrigeration. See liquid ammonia as a solvent.Ammonia readily dissolves in water. In an aqueous solution, it can be expelled by boiling. The aqueous solution of ammonia is basic. The maximum concentration of ammonia in water (a saturated solution) has a density of 0.880 g/cm3 and is often known as ‘.880 ammonia’.Ammonia does not burn readily or sustain combustion, except under narrow fuel-to-air mixtures of 15–25% air. 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 (NCl3) is also formed.At high temperature and in the presence of a suitable catalyst, ammonia is decomposed into its constituent elements. Decomposition of ammonia is slightly endothermic process requiring 5.5 kcal/mol of ammonia, and yields hydrogen and nitrogen gas. Ammonia can also be used as a source of hydrogen for acid fuel cells if the unreacted ammonia can be removed. Ruthenium and Platinum catalysts were found to be the most active, whereas supported Ni catalysts were the less active.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°.[24] 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°.[24] 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 NH4+. 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.[25]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 salts; thus with hydrochloric acid it forms ammonium chloride (sal ammoniac); with nitric acid, ammonium nitrate, etc. Perfectly dry ammonia will not combine with perfectly dry hydrogen chloride; moisture is necessary to bring about the reaction.[26][27] As a demonstration experiment, opened bottles of concentrated ammonia and hydrochloric acid produce clouds of ammonium chloride, which seem to appear “out of nothing” as the salt forms where the two diffusing clouds of molecules meet, somewhere between the two bottles.The salts produced by the action of ammonia on acids are known as the ammonium salts and all contain the ammonium ion (NH4+).[26]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 NH2− ion). For example, lithium dissolves in liquid ammonia to give a solution of lithium amide: 2Li + 2NH3 → 2LiNH2 + H2 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 vaporization, 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.[28] The flammable range of ammonia in dry air is 15.15%-27.35% and in 100% relative humidity air is 15.95%-26.55%.[29] For studying the kinetics of ammonia combustion a detailed reliable reaction mechanism is required, however knowledge about ammonia chemical kinetics during combustion process has been challenging.[30]In organic chemistry, ammonia can act as a nucleophile in substitution reactions. Amines can be formed by the reaction of ammonia with alkyl halides, although the resulting -NH2 group is also nucleophilic and secondary and tertiary amines are often formed as byproducts. An excess of ammonia helps minimise multiple substitution and neutralises the hydrogen halide formed. Methylamine is prepared commercially by the reaction of ammonia with chloromethane, and the reaction of ammonia with 2-bromopropanoic acid has been used to prepare racemic alanine in 70% yield. Ethanolamine is prepared by a ring-opening reaction with ethylene oxide: the reaction is sometimes allowed to go further to produce diethanolamine and triethanolamine.Amides can be prepared by the reaction of ammonia with carboxylic acid derivatives. 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 so long as there are no thermally sensitive groups present: temperatures of 150–200 °C are required.The hydrogen in ammonia is susceptible to replacement by myriad substituents. When heated with sodium it converts to sodamide, NaNH2.[26] With chlorine, monochloramine is formed.Pentavalent ammonia is known as λ5-amine or, more commonly, ammonium hydride. This crystalline solid is only stable under high pressure and decomposes back into trivalent ammonia and hydrogen gas at normal conditions. This substance was once investigated as a possible solid rocket fuel in 1966.[31]Ammonia can act as a ligand in transition metal complexes. It is a pure σ-donor, in the middle of the spectrochemical series, and shows intermediate hard-soft behaviour (see also ECW model). Its relative donor strength toward a series of acids, versus other Lewis bases, can be illustrated by C-B plots.[32][33] For historical reasons, ammonia is named ammine in the nomenclature of coordination compounds. Some notable ammine complexes include tetraamminediaquacopper(II) ([Cu(NH3)4(H2O)2]2+), a dark blue complex formed by adding ammonia to a solution of copper(II) salts. Tetraamminediaquacopper(II) hydroxide is known as Schweizer’s reagent, and has the remarkable ability to dissolve cellulose. Diamminesilver(I) ([Ag(NH3)2]+) is the active species in Tollens’ reagent. Formation of this complex can also help to distinguish between precipitates of the different silver halides: silver chloride (AgCl) is soluble in dilute (2M) ammonia solution, silver bromide (AgBr) is only soluble in concentrated ammonia solution, whereas silver iodide (AgI) is insoluble in aqueous ammonia.Ammine complexes of chromium(III) were known in the late 19th century, and 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 [CrCl3(NH3)3] could be formed, and concluded the ligands must be arranged around the metal ion at the vertices of an octahedron. This proposal has since been confirmed by X-ray crystallography.An ammine ligand bound to a metal ion is markedly more acidic than a free ammonia molecule, although deprotonation in aqueous solution is still rare. One example is the Calomel reaction, where the resulting amidomercury(II) compound is highly insoluble.Ammonia forms 1:1 adducts with a variety of Lewis acids such as I2, phenol, and Al(CH3)3. Ammonia is a hard base and its E & C parameters are EB = 2.31 and C B = 2.04. Its relative donor strength toward a series of acids, versus other Lewis bases, can be illustrated by C-B plots.Ammonia and ammonium salts can be readily detected, in very minute traces, by the addition of Nessler’s solution, which gives a distinct yellow colouration in the presence of the slightest trace of ammonia or ammonium salts. The amount of ammonia in ammonium salts can be estimated quantitatively by distillation of the salts with sodium or potassium hydroxide, the ammonia evolved being absorbed in a known volume of standard sulfuric acid and the excess of acid then determined volumetrically; or the ammonia may be absorbed in hydrochloric acid and the ammonium chloride so formed precipitated as ammonium hexachloroplatinate, (NH4)2PtCl6.[34]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).[37][38] 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.[39] Hammoniacus sal appears in the writings of Pliny,[40] although it is not known whether the term is identical with the more modern sal ammoniac (ammonium chloride).[19][41][42]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 dying cloth, and to remove rust from iron.[43]In the form of sal ammoniac, ammonia was important to the Muslim alchemists as early as the 8th century, first mentioned by the Persian-Arab chemist Jābir ibn Hayyān,[44] and to the European alchemists since 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.[45] At a later period, when sal ammoniac was obtained by distilling the hooves and horns of oxen and neutralizing the resulting carbonate with hydrochloric acid, the name “spirit of hartshorn” was applied to ammonia.[19][46]Gaseous ammonia was first isolated by Joseph Black in 1756 by reacting sal ammoniac (Ammonium Chloride) with calcined magnesia (Magnesium Oxide).[47][48] It was isolated again by Peter Woulfe in 1767,[49][50] by Carl Wilhelm Scheele in 1770[51] and by Joseph Priestley in 1773 and was termed by him “alkaline air”.[19][52] Eleven years later in 1785, Claude Louis Berthollet ascertained its composition.[53][19]The Haber–Bosch process to produce ammonia from the nitrogen in the air was developed by Fritz Haber and Carl Bosch in 1909 and patented in 1910. It was first used on an industrial scale in Germany during World War I,[54] following the allied blockade that cut off the supply of nitrates from Chile. The ammonia was used to produce explosives to sustain war efforts.[55]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.In the US as of 2019, approximately 88% of ammonia was used as fertilizers either as its salts, solutions or anhydrously.[13] When applied to soil, it helps provide increased yields of crops such as maize and wheat.[56] 30% of agricultural nitrogen applied in the US is in the form of anhydrous ammonia and worldwide 110 million tonnes are applied each year.[57]Ammonia is directly or indirectly the precursor to most nitrogen-containing compounds. Virtually all synthetic nitrogen compounds are derived from ammonia. An important derivative is nitric acid. This key material 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 is an intermediate in this conversion:[58] NH3 + 2 O2 → HNO3 + H2O Household ammonia is a solution of NH3 in water, and is used as a general purpose cleaner for many surfaces. Because ammonia results in a relatively streak-free shine, one of its most common uses is to clean glass, porcelain and stainless steel. It is also frequently used for cleaning ovens and soaking items to loosen baked-on grime. Household ammonia ranges in concentration by weight from 5 to 10% ammonia.[59] United States manufacturers of cleaning products are required to provide the product’s material safety data sheet which lists the concentration used.[60]As early as in 1895, it was known that ammonia was “strongly antiseptic … it requires 1.4 grams per litre to preserve beef tea.”[61] In one study, anhydrous ammonia destroyed 99.999% of zoonotic bacteria in 3 types of animal feed, but not silage.[62][63] Anhydrous ammonia is currently used commercially to reduce or eliminate microbial contamination of beef.[64][65] 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.[66] There have been safety concerns about the process as well as consumer complaints about the taste and smell of beef treated at optimal levels of ammonia.[67] The level of ammonia in any final product has not come close to toxic levels to humans.Because of ammonia’s vaporization properties, it is a useful refrigerant.[54] 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 vapor-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 S1 radiator aboard the International Space Station in two loops which are used to regulate the internal temperature and enable temperature dependent experiments.[68][69]The potential importance of ammonia as a refrigerant has increased with the discovery that vented CFCs and HFCs are extremely potent and stable greenhouse gases.[70] The contribution to the greenhouse effect of CFCs and HFCs in current use, if vented, would match that of all CO2 in the atmosphere.The raw energy density of liquid ammonia is 11.5 MJ/L,[73] which is about a third that of diesel. There is the opportunity to convert ammonia back to hydrogen, where it can be used to power hydrogen fuel cells or directly within high-temperature fuel cells.[74] The conversion of ammonia to hydrogen via the sodium amide process,[75] either for combustion or as fuel for a proton exchange membrane fuel cell,[73] is possible. Conversion to hydrogen would allow the storage of hydrogen at nearly 18 wt% compared to ≈5% for gaseous hydrogen under pressure.Ammonia engines or ammonia motors, using ammonia as a working fluid, have been proposed and occasionally used.[76] 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 Avenue Streetcar line in New Orleans in the 1870s and 1880s,[77] and during World War II ammonia was used to power buses in Belgium.[78]Ammonia is sometimes proposed as a practical alternative to fossil fuel for internal combustion engines.[78][79][80] Its high octane rating of 120[81] and low flame temperature[82] allows the use of high compression ratios without a penalty of high NOx production. Since ammonia contains no carbon, its combustion cannot produce carbon dioxide, carbon monoxide, hydrocarbons, or soot.Even though ammonia production currently creates 1.8% of global CO2 emissions, the Royal Society report[83] claims that “green” ammonia can be produced by using low-carbon hydrogen (blue hydrogen and green hydrogen). Total decarbonization of ammonia production and the accomplishment of net-zero targets are possible by 2050.However ammonia cannot be easily used in existing Otto cycle engines because of its very narrow flammability range, and there are also other barriers to widespread automobile usage. In terms of raw ammonia supplies, plants would have to be built to increase production levels, requiring significant capital and energy sources. Although it is the second most produced chemical (after sulfuric acid), the scale of ammonia production is a small fraction of world petroleum usage. It could be manufactured from renewable energy sources, as well as coal or nuclear power. The 60 MW Rjukan dam in Telemark, Norway produced ammonia for many years from 1913, providing fertilizer for much of Europe.Despite this, several tests have been done. In 1981, a Canadian company converted a 1981 Chevrolet Impala to operate using ammonia as fuel.[84][85] In 2007, a University of Michigan pickup powered by ammonia drove from Detroit to San Francisco as part of a demonstration, requiring only one fill-up in Wyoming.[86]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 as a cryogenic liquid.[73][87]Rocket engines have also been fueled 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 oxidizer, liquid oxygen, which simplified the aircraft’s design.Ammonia, as the vapor 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.[89] 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.[90]Liquid ammonia is used for treatment of cotton materials, giving properties like mercerisation, using alkalis. In particular, it is used for prewashing of wool.[91]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 weather 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).The U.S. 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.[95] The National Institute for Occupational Safety and Health (NIOSH) recently reduced the IDLH (Immediately Dangerous to Life and Health, the level to which a healthy worker can be exposed for 30 minutes without suffering irreversible health effects) from 500 to 300 based on recent more conservative interpretations of original research in 1943. Other organizations have varying exposure levels. U.S. Navy Standards [U.S. Bureau of Ships 1962] maximum allowable concentrations (MACs): continuous exposure (60 days): 25 ppm / 1 hour: 400 ppm.[96] 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.[95] Ammonia is regulated in the United States 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 13,248 L (3,500 gallons).[97]Liquid ammonia is dangerous because it is hygroscopic and because it can cause caustic burns. See Gas carrier § Health effects of specific cargoes carried on gas carriers for more information.The toxicity of ammonia solutions does not usually cause problems for humans and other mammals, as a specific mechanism exists to prevent its build-up in the bloodstream. Ammonia is converted to carbamoyl phosphate by the enzyme carbamoyl phosphate synthetase, and then enters the urea cycle to be either incorporated into amino acids or excreted in the urine.[98] Fish and amphibians lack this mechanism, as they can usually eliminate ammonia from their bodies by direct excretion. Ammonia even at dilute concentrations is highly toxic to aquatic animals, and for this reason it is classified as dangerous for the environment.Ammonia is a constituent of tobacco smoke.[99]Ammonia is present in coking wastewater streams, as a liquid by-product of the production of coke from coal.[100] 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 which discharges ammonia into marine waters.[101]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.[102] 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.[103] Exposed to excess ammonia, fish may suffer loss of equilibrium, hyper-excitability, increased respiratory activity and oxygen uptake and increased heart rate.[102] At concentrations exceeding 2.0 mg/L, ammonia causes gill and tissue damage, extreme lethargy, convulsions, coma, and death.[102][104] Experiments have shown that the lethal concentration for a variety of fish species ranges from 0.2 to 2.0 mg/l.[104]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[104] and in open water systems, the surrounding environment.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.[105] Ammonia is used in numerous different industrial application requiring carbon or stainless steel storage vessels. Ammonia with at least 0.2 percent by weight water content is not corrosive to carbon steel. NH3 carbon steel construction storage tanks with 0.2 percent by weight or more of water could last more than 50 years in service.[106] Ammonium compounds should never be allowed to come in contact with bases (unless in an intended and contained reaction), as dangerous quantities of ammonia gas could be released.The ammonia vapour from concentrated ammonia solutions is severely irritating to the eyes and the respiratory tract, and these solutions should 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 the bottle should be opened with care; this is not usually a problem for 25% (“0.900”) solutions.Ammonia solutions should not be mixed with halogens, as toxic and/or explosive products are formed. 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 should be lightly acidified but not concentrated (<6% w/v) before disposal once the test is completed.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, and so brass fittings should not be used 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.Ammonia has alkaline properties and is corrosive.Ammonia gas dissolves easily in water to form ammonium hydroxide, a caustic solution and weak base.Ammonia gas is easily compressed and forms a clear liquid under pressure.Ammonia is usually shipped as a compressed liquid in steel containers.Ammonia is not highly flammable, but containers of ammonia may explode when exposed to high heat.About 80% of the ammonia produced by industry is used in agriculture as fertilizer. Ammonia is also used as a refrigerant gas, for purification of water supplies, and in the manufacture of plastics, explosives, textiles, pesticides, dyes and other chemicals. It is found in many household and industrial-strength cleaning solutions. Household ammonia cleaning solutions are manufactured by adding ammonia gas to water and can be between 5 and 10% ammonia. Ammonia solutions for industrial use may be concentrations of 25% or higher and are corrosive.Inhalation: Ammonia is irritating and corrosive. Exposure to high concentrations of ammonia in air causes immediate burning of the nose, throat and respiratory tract. This can cause bronchiolar and alveolar edema, and airway destruction resulting in respiratory distress or failure. Inhalation of lower concentrations can cause coughing, and nose and throat irritation. Ammonia’s odor provides adequate early warning of its presence, but ammonia also causes olfactory fatigue or adaptation, reducing awareness of one’s prolonged exposure at low concentrations.There is no antidote for ammonia poisoning, but ammonia’s effects can be treated, and most people recover. Immediate decontamination of skin and eyes with copious amounts of water is very important. Treatment consists of supportive measures and can include administration of humidified oxygen, bronchodilators and airway management. Ingested ammonia is diluted with milk or water.Ammonia, a colorless gas with a distinct odor, is a building-block chemical and a key component in the manufacture of many products people use every day. It occurs naturally throughout the environment in the air, soil and water and in plants and animals, including humans. The human body makes ammonia when the body breaks down foods containing protein into amino acids and ammonia, then converting the ammonia into urea.When using cleaning products containing ammonia, follow all instructions on the product label, make sure the area is well ventilated (open windows and doors) and wear proper clothing and eye protection. Ammonia exposure can irritate skin, eyes and lungs. Do not mix ammonia with chlorine bleach, as this produces toxic gases called chloramines. Exposure to chloramine gases can cause coughing, shortness of breath, chest pain, nausea, irritation to the throat, nose and eyes or pneumonia and fluid in the lungs.Ammonia is a chemical consisting of one atom of nitrogen and three atoms of hydrogen. It is designated in chemical notation as NH3. Ammonia is extremely soluble in water and is frequently used as a water solution called aqua ammonia. Ammonia chemically combines with water to form ammonium hydroxide. Household ammonia is a diluted water solution containing 5 to 10 percent ammonia. On the other hand, anhydrous ammonia is essentially pure (over 99 percent) ammonia. “Anhydrous” is a Greek word meaning “without water;” therefore, anhydrous ammonia in ammonia without water.Anhydrous ammonia is a clear liquid that boils at a temperature of -28°F. In refrigeration systems, the liquid is stored in closed containers under pressure. When the pressure is released, the liquid evaporates rapidly, generally forming an invisible vapor or gas. The rapid evaporation causes the temperature of the liquid to drop until it reaches the normal boiling point of -28°F, a similar effect occurs when water evaporates off the skin, thus cooling it. This is why ammonia is used in refrigeration systems.Liquid anhydrous ammonia weighs less than water. About eight gallons of ammonia weighs the same as five gallons of water.Liquid and gas ammonia expand and contract with changes in pressure and temperature. For example, if liquid anhydrous ammonia is in a partially filled, closed container it is heated from 0°F to 68°F, the volume of the liquid will increase by about 10 percent. If the tank is 90 percent full at 0°F, it will become 99 percent full at 68°F. At the same time, the pressure in the container will increase from 16 pounds per square inch (psi) to 110 psi.Liquid ammonia will expand by 850 times when evaporating:Anhydrous ammonia gas is considerably lighter than air and will rise in dry air. However, because of ammonias tremendous affinity for water, it reacts immediately with the humidity in the air and may remain close to the ground.The odor threshold for ammonia is between 5 – 50 parts per million (ppm) of air. The permissible exposure limit (PEL) is 50 ppm averaged over an 8 hour shift. It is recommended that if an employee can smell it they ought to back off and determine if they need to be using respiratory protection.Ammonia, like CO2 is a waste product of fish metabolism and tends to accumulate in transport water. Ammonia is directly toxic to fish in the unionized form, which is favored at high temperatures and pH, and it also reduces the ability of fish to utilize oxygen. To avoid the accumulation of excessive ammonia, feed should be withheld from fish before transport and proper loading rates should be used. To reduce the effects of ammonia, fish should be transported in reduced water temperatures, when possible. Weirich et al. (1993) noted that calcium addition seems to provide some benefits regarding ammonia toxicity, as the 96 h LC50 of ammonia for sunshine bass increased significantly when calcium concentrations were raised from 5 to 80 mg/L.Ammonia (NH3) is available as a liquid in cylinders (49 kg and 65 kg) or drums (530 kg). It is withdrawn as a gas at 0.5 kg/h from a cylinder or 2 kg/h from a drum at 15°C, or as a liquid to evaporators. Apparatus used is very similar to that used for chlorine. Ammonia is very soluble in water and is corrosive. Steel piping is suitable for conveyance of ammonia liquid and dry gas. Iron, copper, zinc and aluminium are attacked by ammonia solution, but PVC-U is suitable. Motive water for ammonia dosing units should be softened to a hardness value of less than 25 mg/l as CaCO3 to prevent calcium carbonate scaling of fittings.

TR

AMONYAK IUPAC Ad azane

AMONYAK InChI InChI = 1S / H3N / h1H3

AMONYAK InChI Anahtar QGZKDVFQNNGYKY-UHFFFAOYSA-N

AMONYAK Canonical SMILES N

AMONYAK Moleküler Formül NH3

AMONYAK CAS 7664-41-7

AMONYAK Kullanmdan kaldrlan CAS 208990-07-2, 214478-05-4, 8007-57-6, 558443-52-0, 1026405-88-8

AMONYAK Avrupa Topluluu (EC) Numaras 231-635-3

AMONYAK ICSC Numaras 0414

AMONYAK RTECS Numaras BO0875000

AMONYAK UN Numaras 2073

AMONYAK UNII 5138Q19F1X

AMONYAK FEMA Numaras 4494

AMONYAK DSSTox Madde Kimlii DTXSID0023872

AMONYAK Moleküler Arlk 17.031 g / mol

AMONYAK XLogP3-AA -0,7

AMONYAK Hidrojen Ba Donör Says 1

AMONYAK Hidrojen Ba Alcs Says 1

AMONYAK Döndürülebilir Tahvil Says 0

AMONYAK Tam Kütle 17.026549 g / mol

AMONYAK Monoizotopik Kütle 17.026549 g / mol

AMONYAK Topolojik Polar Yüzey Alan 1 Ų

AMONYAK Ar Atom Says 1

AMONYAK Resmi Ücret 0

AMONYAK Karmaklk 0

AMONYAK zotop Atom Says 0

AMONYAK Tanml Atom Stereo Merkez Says 0

AMONYAK Tanmsz Atom Stereo Merkez Says 0

AMONYAK Tanml Bond Stereocenter Says 0

AMONYAK Tanmsz Ba Stereocenter Says 0

AMONYAK Kovalent Bal Birim Says 1

AMONYAK Bileik Kanonikletirilmitir Evet

Amonyak, formülü NH3 olan; azot atomu ve hidrojen atomundan oluan renksiz , keskin ve ho olmayan kokuya sahip bir gaz bileiidir. OH- iyonu içermedii halde suda zayf baz özellii gösterir. Bir amonyak molekülü, bir azot ve üç hidrojen atomundan oluur.Amonyak, kovalent bal (ametal + ametal) bir bileiktir. Molekülleri polar olduundan su içinde yüksek oranda çözünür. Amonyak molekülleri kendi aralarnda olduu gibi su molekülleri ile de zayf hidrojen ba oluturur. Bu nedenle suda çözünür.Amonyak, gübre, ilaç, boya, parfüm gibi maddelerin sentezlenmesinde ilk aamada kullanlmaktadr. Amonyak canllar için zehirli bir maddedir, kullanlrken dikkat edilmesi gerekir. Piyasada amonyak ad altnda satlan maddeler amonyan sulu çözeltisi olan amonyum hidroksittir.Amonyak, gübre, ilaç, boya, parfüm gibi maddelerin sentezlenmesinde ilk aamada kullanlmaktadr. Amonyak canllar için zehirli bir maddedir, kullanlrken dikkat edilmesi gerekir. Piyasada amonyak ad altnda satlan maddeler amonyan sulu çözeltisi olan amonyum hidroksittir.Amonyak, gübre, ilaç, boya, parfüm gibi maddelerin sentezlenmesinde ilk aamada kullanlmaktadr. Amonyak canllar için zehirli bir maddedir, kullanlrken dikkat edilmesi gerekir. Piyasada amonyak ad altnda satlan maddeler amonyan sulu çözeltisi olan Amonyum Hidroksittir.Amonyak, formülü NH3 olan; azot atomu ve hidrojen atomundan oluan renksiz , keskin ve ho olmayan kokuya sahip bir gaz bileiidir. OH- iyonu içermedii halde suda zayf baz özellii gösterir. Bir amonyak molekülü, bir azot ve üç hidrojen atomundan oluur. Amonyak, formülü NH3 olan; azot atomu ve hidrojen atomundan oluan renksiz , keskin ve ho olmayan kokuya sahip bir gaz bileiidir. OH- iyonu içermedii halde suda zayf baz özellii gösterir. Bir amonyak molekülü, bir azot ve üç hidrojen atomundan oluur.Amonyak, kovalent bal (ametal + ametal) bir bileiktir. Molekülleri polar olduundan su içinde yüksek oranda çözünür. Amonyak molekülleri kendi aralarnda olduu gibi su molekülleri ile de zayf hidrojen ba oluturur. Bu nedenle suda çözünür.Oda scaklnda, amonyak keskin ve boucu bir kokuya sahip renksiz, oldukça tahri edici bir gazdr. Genellikle varl hakknda yeterli sinyali verir; ancak koku alma yorgunluu oluturabilir.Saf halde susuz amonyak olarak bilinir ve nemi kolayca emer.Amonyak alkali özelliklere sahiptir ve yüksek konsantrasyonlarda andrcdr.Amonyak gaz su içinde kolayca çözünür ve amonyum hidroksit, kostik bir çözelti ve zayf bir baz oluturur.Amonyak gaz kolayca sktrlr ve basnç altnda berrak bir sv oluturur.Amonyak genellikle çelik kaplarda sktrlm bir sv olarak sevk edilir.Amonyak çok yanc deildir, ancak yüksek sya maruz kaldnda patlama riski vardr.Amonyak doal olarak bulunduundan ve temizlik ürünlerinde de sklkla kullanldndan, endüstriyel maruziyetin yannda bu kaynaklardan da maruziyet meydana gelebilir. Çiftlikler ve endüstriyel alanlarda yaygn olarak kullanlmas olas kazalarla maruziyet ihtimalini arttrmaktadr. Maruziyet kastl bir terör saldrsndan da kaynaklanabilir.Susuz amonyak gaz havadan daha hafiftir, böylece yükselerek alanda dalr ve alçakta kalan bölgelere yerlemez. Bununla birlikte, nemin varlnda (yüksek bal nem gibi), svlatrlm susuz amonyak gaz havadan ar buharlar oluturur. Bu buharlar, zeminde veya insanlarn maruz kalabilecei zayf hava akm olan ve alçakta kalan alanlara yaylabilir.Amonyak maruziyetinin neden olduu etkilenme derecesi maruz kalma süresine ve gaz veya svnn konsantrasyonuna baldr. Amonyak, göze nüfuz etme ve göze zarar verme eiliminde olup, etkisi dier alkalilere göre daha fazladr. Havadaki düük konsantrasyonlarda bile (50 ppm) hzl bir ekilde göz, burun ve boaz tahriine, öksürme ve bronlarn daralmasna sebep olur.  Yüksek konsantrasyonda gazla veya konsantre amonyum hidroksitle temas, gözün yüzey hücrelerinin imesine ve kaymasna ve geçici veya kalc körlüe neden olabilir.Amonyan koku eii, varl hakknda yeterli sinyali vermek için oldukça düüktür (koku eii = 5 ppm; OSHA PEL = 50 ppm). Bununla birlikte amonyak, koku alma yorgunluuna veya adaptasyonuna neden olarak maruziyet süresini uzatarak tespitini zorlatrr. sal ve güvenlii anlamnda ülke mevzuatnda, amonyak maruziyeti snr deeri Kimyasal Maddelerle Çalmalarda Salk Ve Güvenlik Önlemleri Hakknda Yönetmelik ile belirlenmitir. Bu yönetmelie göre mesleki maruziyet snr deerleri 8 saatlik(TWA) maruziyet için  20 ppm,  15 dakikalk (STEL) maruziyet içinse 50 ppmdir.Baz endüstriyel temizleyicilerin (% 25) gibi konsantre amonyak çözeltileriyle cildin temas, cilt yanklar, kalc göz hasar veya körlük gibi ciddi andrc yaralanmalara neden olabilir. Svlatrlm amonyakla temas souk srmasna neden olabilir. Uzun süreli cilt temas (birkaç dakikadan fazla) arya ve andrc yaralanmalara neden olabilir. Seyreltik sulu çözeltiler (%5’ten az) nadiren ciddi yanklara neden olur ancak orta derecede tahri edici olabilir. Konsantre buhar veya çözeltiye maruz kalma, özellikle nemli cilt bölgelerinde ar, iltihaplanma, kabarcklar ve derin delici yanklara neden olabilir.Son 20 yl içinde ülkemizde ve dünyada yaanan amonyak maruziyeti kaynakl kazalara bakldnda yüksek rakamlarla karlalmaktadr. 2003 ylnda Mersin’de gübre fabrikasnda amonyak borusunda meydana gelen patlama sonucu 40 kii zehirlenmitir. 2012 ylnda ise Manisa’da salça ve kurutulmu domates fabrikasnda amonyak kazanndan yaanan sznt ile 50 kii zehirlenmitir. 2013 ylnda Çin’de bir fabrikada meydana gelen amonyak szntsnda ise 15 kii ölmü 30 kii yaralanmtr. Amonyak ile ilgili bunlar ve benzeri yaanan kazalar ile ilgili son 10 ylda yaanm olan ciddi kazalar düünülünce maruziyet durumunda alnacak acil önlemlerin bilinmesi faydal olacaktr.  Gözlerde amonyak maruziyeti: Gözler hemen bol miktarda su ile ara sra üst ve alt göz kapaklarn kaldrlarak ykanmaldr.Deride amonyak maruziyeti: Tahri meydana gelirse, fazla kimyasallar nazikçe alnmaldr ve amonyak temas olan bölge bol suyla ykanmaldr. Kimyasallar giysilere nüfuz ederse, derhal giysi çkartlmal ve cilt yine ykanmaldr.Solunum sisteminde amonyak maruziyeti: Bir içi çok miktarda amonyak solursa, hemen temiz havaya çkarlmaldr.Amonyak: (NH3), Sanayide en fazla azotlu gübreler ve nitrik asidin üretiminde ilk maddesi olarak kullanlr. Laboratuarlarda zayf baz ve birçok kimyasal maddenin elde edilmesi içinde kullanlr. Amonyak bilhassa nitrik asit ile amonyum tuzlarnn imal, üre, boya, ilaç ve plastik benzeri organik madde üretiminde kullanlr. Amonyak gaz normal sda basnç uyguland zaman kolayca svlar, meydana çkan bu svnn buharlama ss ise yüksektir (327 kcal/g), bunun için endüstride soutucu olarak kullanlr.Özellii; renksiz, kendine özgü keskin kokusu olup ayrca zehirli ve andrcdr. Oda scaklnda gaz halindedir ve düük scaklklarda alevlenme özellii tar. Kimyasal olarak bazik’ tir. Normal sda, basnç altnda kolay bir ekilde svlar. Amonyak Kullanm Alanlar: Gübre Sanayi, Nitrik asit üretimi, ilk balangç maddesi olarak endüstriyel soutma sistemleri ile soutma gayesiyle kimya sanayinde ilaç, boya, naylon, tuz ve plastik üretim malzemelerin sl ilemlerinde hidrojen ve azot kayna olarak, Gaz Nitrür ilemi için ise parça yüzeylerine azot emdirme gayesiyle kullanlr.Amonyak formulü NH3 olan; azot atomu ile hidrojen atomundan meydana gelen renksiz, keskin ve ho olmayan bir kokuya sahip, gaz bileiinden meydana gelir. OH- iyonu bulunmad halde zayf baz özellii gösterir. Gazlama gizli ss çok yüksek olduu için sanayi tesislerinde soutucu madde olarak kullanlr. 17,0304 g/mol molekül arl, 1 Atmosfer basnç ta kaynama noktas -33.34 °C (239.81 K). -78 derecede donmas nedeniyle oda ssnda gaz eklinde bulunur. Bileikteki N atomu sp3 hibritleme yapmtr. Ba yapmam bir çift elektronu olduu için, molekül ekli üçgen piramittir. Bundan dolay polar bir moleküldür. Molekülleri polar olmasndan dolay, su içinde yüksek oranda çözülmektedir.Amonyak sminin kökeni eski msra kadar dayanr. Amon tapnan stmak için kullanlan deve tezeinden çkan gazlardan, tapnak duvarlarnda, tavannda sofra tuzuna benzer, beyaz kristaller halindeki amonyum klorür yani niadr birikmitir. Bu oluuma da o devirlerde “Amonun Tuzu” diye söylenirmi.Amonyak, ilaç, boya, gübre, parfüm gibi maddelerin sentezlenmesi olaynda ilk basamak olarak kullanlr. Amonyak ayrca temizlik maddelerinin içerisinde de kullanlr. Amonyakcanllar için çok zehirli bir maddedir, kullanrken dikkat çok fazla etmek gerekir.Amonyak kovalent bal bileiktir. Ametal ve Ametal badr. Molekülleri polar olduu için su içinde yüksek oranda çözülmektedir. Amonyak molekülü kendi arasnda olduu gibi, su molekülleri ile de zayf hidrojen ba oluturmaktadr. Bu nedenden suda çok fazla çözünür. 1 atmosfer basnçta ve 0 derecede 1 litre su içinde 1300 litre, 20 derece sda ise 700 litre amonyak çözülmektedir. Oda koullar altnda doymu amonyak çözeltisi %34’ lük olup, younluu 0,88 g/ml dir.Piyasada amonyak ad altnda bulunan ve satlan bu maddeler amonyan sulu çözeltisi olan amonyum hidroksittir.Temizlik malzemeleri ile gübre ve patlayc yapmnda kullanlr.Amonyak, gübre, ilaç, boya, parfüm gibi maddelerin sentezlenmesinde ilk aamada kullanlmaktadr. Amonyak canllar için zehirli bir maddedir, kullanlrken dikkat edilmesi gerekir. Piyasada amonyak ad altnda satlan maddeler amonyan sulu çözeltisi olan Amonyum Hidroksittir.Amonyak, en fazla gübre üretiminde ve gübre olarak kullanlr. Azotlu gübre ve nitrik asit üretiminde balangç maddesidir.Sv amonyak, topraa dorudan dökülebilir. Amonyum nitrat ve amonyum fosfat gibi tuzlar da gübre olarak kullanlabilir.Rafine petrolün asit içeren yan ürünlerinin nötrletirilmesinde, lastik üretiminde phtlamay önlemek için amonyak kullanlr.Balca kullanld ürünler unlardr; boyalar, plastikler, naylon, temizlik ürünleri, patlayclar, soutucular (klima gibi), sentetik elyaflar, pamuk ve ipek temizlii, bakalit ve sentetik reçine üretimi, soda, patlayc maddeler, sentetik fiber, ilaç sentezleri…Amonyak gaz, yiyecek ve içecek fabrikalarnda, üretim-proses ve depolama bölümlerinde soutucu gaz olarak kullanlmaktadr. Bu ve buna benzer yerlerde veya amonyak gaznn dondurucuya doldurulduu lokasyonlarda çalan personelin, bu gaz tehlikesinden korunmaya ihtiyac vardr. Gaz konsantrasyonunu izleme çözümleri içinde, çalanlarn portatif gaz dedektörü kullanm veya hedef alandaki sabit gaz alglama sisteminin montaj-kurulumu seçenekleri yer almaktadr. Tipik olarak alglanan gazlarn içinde 0-100 ppm NH3, 0-3 % vol aralnda CO2, oksijen seviyesinin azalmasnn kontrolü ve yanc buharlarn 0-100 % LEL aralndaki ölçümleri yer almaktadr.Yiyecek üretim tesislerinde ürün depo alanlarndaki soutucularda bulunan ürünlerin bozulmas, büyük maddi kayplara ve üretim hacminin küçülmesine sebep olmaktadr. Ürünlerin bozulmasna neden olan soutucu seviyesi, ürünün çeidine ve yaplan paketlemenin tipine göre farkllk göstermektedir. Ancak bu paketleme ve üretim proseslerinde düük konsantrasyonlarda paketlenmeyen yiyeceklerin bozulmas muhtemeldir. 1-10 ppm arasndaki bir deerde bozulma meydana gelir. Bu nedenle amonyak kontrolünün yaplmas gereklidir.Saf amonyak genellikle SIVI – SUSUZ amonyak olarak bilinir. Amonyak gaz keskin kokulu, renksiz bir gazdr.Sv amonyak sktrlm ve/ veya svlatrlm amonyak gazdr. Amonyak gaz normal atmosfer basncnda ve – 33 C’nin altnda svlar ve basnç kaldrlnca da sv, gaz fazna döner.Bu özellik gaz basnç altnda bir sv olarak depolama ve tama imkan salar.Amonyak gümü, civa, klor,iyot, brom kalsiyum ve hipokloritler gibi maddelerle temas halinde olduunda patlayc bileikler meydana getirir. Sv Amonyak çelii ve demiri paslandrmaz ;ancak çinko,kalay,bakr ve pirinç gibi bakr esasl alamlarla reaksiyona girer. Dier metallerin bir çou da amonyakla deien derecelerde reaksiyona girer.Bu sebeple iletmelerde kullanlan baz basnç, sv gibi göstergelerde ve benzeri donatlarda genellikle kullanlan galvenize ve balant elemanlaryla demir ihtiva etmeyen metallerin çou amonyaa dayanmazlar.letmelerde Amonyak gaz ile ilgili yaplacak olan her hangi bir tesisatn daha çok paslanmaz metallerle yaplmas daha uygun olacaktr.Topraklardan ortaya çkan amonyak tçmas, sistemin özelliklerinin bir fonksiyonu olarak teorik ye deneysel yollarla ana/iz edilmitir. Toprak tarafndan tutulan nihai amonyum konsantrasyonu; hidrojen iyon aktivitesi,balangçtaki am.0nyum konsantrasyonu ve havadaki ksmi amonyak basncnaba” olarak artmaktadr. Topran tamponluk kapasitesindeki bir art ise, nihai amonyum konsantrasyonunda bir azalmaya yol açmaktadr.Kieçli topraklara amonyakhgübreler ilave edildii taktirde, amonyan önemli bir ksm uçmaktadr (1, 2, 5).Bu gibi kayplar ekonomik yönden önemli olduu gibi, çevredeki sularn da azot yönünden zenginlemesine yol açabilmektedir (6).Amonyak koronavirüse kar etkisizdir, virüsleri öldürmez. Cam temizliini, döemeleri, sabun kirini gidermek için ev temizliinde skça kullanlr. Yüzey temizleyiciler ya da banyo temizleyicileri gibi temizlik ürünleri amonyak içerir.Amonyak ile evinizin yüzeylerini temizleyerek koronavirüs (COVD-19) ya da baka virüslere kar korunabilir misiniz? Bunun yant hayr. Amonyak virüsleri öldürmez.Ball State Üniversitesi Salk Bilimleri Doçenti ve Profesörü Jagdish Khubchandani , “Amonyak virüslere kar neredeyse etkisizdir veya çok az etkisi vardr . E. Coli gibi baz yaygn bakteriler için yaygn olarak kullanlan bir dezenfektandr.” diyor.Amonyak, NH3 formülüne sahip bir nitrojen ve hidrojen bileiidir. Kararl bir ikili hidrit ve en basit pnictogen hidrit olan amonyak, karakteristik keskin kokusu olan renksiz bir gazdr. Özellikle suda yaayan organizmalar arasnda yaygn bir azotlu atktr ve gda ve gübrelerin öncüsü olarak hizmet ederek karasal organizmalarn beslenme ihtiyaçlarna önemli ölçüde katkda bulunur. Dorudan veya dolayl olarak amonyak, birçok farmasötik ürünün sentezi için bir yap tadr ve birçok ticari temizlik ürününde kullanlr. Esas olarak hem havann hem de suyun aaya doru yer deitirmesiyle toplanr. Doada – hem karada hem de Güne Sisteminin d gezegenlerinde yaygn olmasna ramen ve geni kullanmda amonyak, konsantre biçiminde hem yakc hem de tehlikelidir. Amerika Birleik Devletleri’nde son derece tehlikeli bir madde olarak snflandrlr ve onu önemli miktarlarda üreten, depolayan veya kullanan tesislerin kat raporlama gerekliliklerine tabidir. [12] 2018’de küresel endüstriyel amonyak üretimi 175 milyon tondu, [13] 175 milyon tonluk 2013 küresel endüstriyel üretimine göre önemli bir deiiklik olmadan. [14] Endüstriyel amonyak, amonyak likörü (genellikle suda% 28 amonyak) olarak veya tank arabalarnda veya silindirlerde tanan basnçl veya soutulmu susuz sv amonyak olarak satlr. [15] NH3, bir basnçta -33,34 ° C’de (-28,012 ° F) kaynar bir atmosfer, bu nedenle sv basnç altnda veya düük scaklkta depolanmaldr. Ev tipi amonyak veya amonyum hidroksit, sudaki bir NH3 çözeltisidir. Bu tür çözeltilerin konsantrasyonu, tipik yüksek konsantrasyonlu ticari ürün olan 26 derece Baumé (arlkça yaklak% 30 (arlkça) amonyak, 15.5 ° C veya 59.9 ° F) ile Baumé ölçei (younluk) birimleriyle ölçülür. [16 ] Pliny, Doa Tarihi’nin XXXI Kitabnda, Roma’nn Cyrenaica eyaletinde üretilen ve yakndaki Jüpiter Amun Tapna’na (Yunan Ἄμμων Ammon) yaknlndan dolay hammoniacum adl bir tuzu ifade eder. [17] Bununla birlikte, Pliny’nin tuzla ilgili verdii açklama, amonyum klorürün özelliklerine uymamaktadr.Herbert Hoover’n Georgius Agricola’nn De re metallica eserinin ngilizce çevirisindeki yorumuna göre, muhtemelen deniz tuzu olabilir. [18] Her halükarda, bu tuz nihayetinde amonyak ve amonyum bileiklerine isimlerini verdi.Amonia, azotlu hayvansal ve bitkisel maddelerden üretilen, doada eser miktarlarda bulunan bir kimyasaldr. Amonyak ve amonyum tuzlar da yamur suyunda küçük miktarlarda bulunurken, volkanik bölgelerde amonyum klorür (sal amonyak) ve amonyum sülfat bulunur; Patagonia guano’da amonyum bikarbonat kristalleri bulunmutur. [19] Böbrekler fazla asidi nötralize etmek için amonyak salglar. [20] Amonyum tuzlar, verimli topraklarda ve deniz suyunda dalm halde bulunur.Amonia ayrca Güne Sistemi boyunca Mars, Jüpiter, Satürn, Uranüs, Neptün ve Plüton’da bulunur: Plüton gibi daha küçük, buzlu cisimlerde amonyak etki edebilir. Jeolojik açdan önemli bir antifriz olarak, amonyak konsantrasyonu yeterince yüksekse ve bu nedenle bu tür cisimlerin iç okyanuslar tutmasna izin verirse, su ve amonyak karm 173 K (−100 ° C; −148 ° F) kadar düük bir erime noktasna sahip olabilir. ve sadece suyla mümkün olabileceinden çok daha düük bir scaklkta aktif jeoloji. [21] [22] Amonyak içeren veya ona benzeyen maddelere amonyak denir.Amonia, karakteristik olarak keskin bir kokuya sahip renksiz bir gazdr. Havadan daha hafiftir, younluu havannkinin 0,589 katdr. Moleküller arasndaki güçlü hidrojen ba nedeniyle kolayca svlatrlr; Sv -33.3 ° C’de (-27.94 ° F) kaynar ve -77.7 ° C’de (-107.86 ° F) beyaz kristallere [19] donar. Amonyak sodyum bikarbonat veya asetik asit ile reaksiyona sokularak uygun ekilde kokusu giderilebilir. . Bu reaksiyonlarn her ikisi de kokusuz bir amonyum tuzu oluturur. Kristal simetrisi kübiktir, Pearson sembolü cP16, boluk grubu P213 No. 198, kafes sabiti 0.5125 nm. [23] Sv amonyak, yüksek ε 22’sini yanstan güçlü iyonlatrc güçlere sahiptir. Sv amonyak buharlama standardnda çok yüksek bir entalpi deiimine sahiptir (23.35 kJ / mol, cf. su 40.65 kJ / mol, metan 8.19 kJ / mol, fosfin 14.6 kJ / mol) ve bu nedenle, laboratuvarlarda ek soutma olmakszn yaltlmam kaplarda laboratuarlarda kullanlabilir. Çözücü olarak sv amonya görün.Amonia, suda kolayca çözünür. Sulu bir çözelti içinde kaynatlarak atlabilir. Sulu amonyak çözeltisi baziktir. Sudaki maksimum amonyak konsantrasyonu (doymu bir çözelti) 0.880 g / cm3 younlua sahiptir ve genellikle ‘.880 amonyak’ olarak bilinir. Amonyak, yakttan havaya dar karmlar dnda, kolayca yanmaz veya yanmay sürdürmez. % 15–25 hava. Oksijenle kartrldnda soluk sarms yeil bir alevle yanar. Tutuma, klor amonyaa geçerek nitrojen ve hidrojen klorür oluturduunda meydana gelir; Klor fazlal varsa, o zaman oldukça patlayc nitrojen triklorür (NCl3) de oluur. Yüksek scaklkta ve uygun bir katalizör varlnda, amonyak bileen elementlerine ayrr.Amonyan ayrmas, 5.5 kcal / mol amonyak gerektiren hafif endotermik bir süreçtir ve hidrojen ve nitrojen gaz verir. Reaksiyona girmemi amonyak uzaklatrlabiliyorsa, amonyak asit yakt hücreleri için bir hidrojen kayna olarak da kullanlabilir. Rutenyum ve Platin katalizörlerinin en aktif olduu, desteklenmi Ni katalizörlerinin ise daha az aktif olduu bulundu. 106.7 °. [24] Merkezi nitrojen atomu, her hidrojen atomundan ek bir elektron ile be d elektrona sahiptir. Bu, toplamda sekiz elektron veya dört yüzlü olarak düzenlenmi dört elektron çifti verir. Bu elektron çiftlerinden üçü, tek bir çift elektron brakan ba çiftleri olarak kullanlr. Yalnz çift, ba çiftlerinden daha güçlü iter, bu nedenle ba açs, normal bir tetrahedral düzenlemeden beklendii gibi 109,5 ° deil, 106,7 ° ‘dir. [24] Bu ekil moleküle bir çift kutuplu moment verir ve onu kutupsal hale getirir. Molekülün polaritesi ve özellikle hidrojen balar oluturma yetenei, amonya suyla oldukça karabilir hale getirir. Yalnz çift, amonya bir baz, bir proton alcs yapar. Amonyak orta derecede baziktir; 1.0 M sulu çözeltinin pH’si 11.6’dr ve çözelti nötr olana kadar (pH = 7) böyle bir çözeltiye güçlü bir asit eklenirse, amonyak moleküllerinin% 99.4’ü protonlanr. Scaklk ve tuzluluk da NH4 + orann etkiler. kincisi, normal bir tetrahedron ekline sahiptir ve metan ile izoelektroniktir. Amonyak molekülü, oda scaklnda nitrojen inversiyonuna kolayca maruz kalr; yararl bir benzetme, kuvvetli bir rüzgarda kendini tersine çeviren bir emsiyedir. Bu inversiyonun enerji engeli 24.7 kJ / mol ve rezonans frekans 23.79 GHz olup, 1.260 cm dalga boyundaki mikrodalga radyasyonuna karlk gelir. Bu frekanstaki absorpsiyon, gözlemlenen ilk mikrodalga spektrumuydu. [25] Amonyan en karakteristik özelliklerinden biri de bazikliidir.Amonyak zayf bir baz olarak kabul edilir. Tuzlar oluturmak için asitlerle birleir; bu nedenle hidroklorik asit ile amonyum klorür (sal amonyak) oluturur; nitrik asit, amonyum nitrat, vb. ile. Mükemmel kuru amonyak, mükemmel kuru hidrojen klorür ile birlemez; reaksiyonu meydana getirmek için nem gereklidir. [26] [27] Bir gösteri deneyi olarak, açlm konsantre amonyak ve hidroklorik asit ieleri, iki ie arasnda bir yerde iki dank molekül bulutu birletii yerde tuz olutuunda “yoktan” görünen amonyum klorür bulutlar üretir. Amonyan asitler üzerindeki etkisiyle amonyum tuzlar olarak bilinir ve hepsi amonyum iyonunu (NH4 +) içerir. [26] Amonyak, zayf bir baz olarak iyi bilinmesine ramen, ayn zamanda ar derecede zayf bir asit görevi görebilir. Protik bir maddedir ve amidler oluturabilir (NH2− iyonu içerir). Örnein, lityum sv amonyak içinde çözülerek bir lityum amid solüsyonu verir: 2Li + 2NH3 → 2LiNH2 + H2 Bir katalizör (platin gazl bez veya scak krom (III) oksit gibi) olmadnda havadaki amonyan yanmas çok zordur. ), nispeten düük yanma ss, daha düük laminer yanma hz, yüksek kendiliinden tutuma scakl, yüksek buharlama ss ve dar bir yanma aral nedeniyle. Bununla birlikte, son aratrmalar, amonyan verimli ve istikrarl yanmasnn girdapl yanma cihazlar kullanlarak elde edilebileceini ve bu sayede termal enerji üretimi için bir yakt olarak amonyaa yönelik aratrma ilgisini yeniden canlandrdn göstermitir. [28] Kuru havada yanclk aral% 15,15 -% 27,35 ve% 100 bal nemde havada% 15,95 -% 26,55’dir. [29] Amonyak yanma kinetiini incelemek için ayrntl bir güvenilir reaksiyon mekanizmas gereklidir, ancak yanma ilemi srasnda amonyak kimyasal kinetii hakknda bilgi almak zordur. [30] Organik kimyada, amonyak ikame reaksiyonlarnda bir nükleofil görevi görebilir. Aminler, amonyan alkil halojenürlerle reaksiyonuyla oluturulabilir, bununla birlikte ortaya çkan -NH2 grubu da nükleofiliktir ve ikincil ve üçüncül aminler genellikle yan ürünler olarak oluturulur. Fazla amonyak, çoklu ikameyi en aza indirmeye yardmc olur ve oluan hidrojen halojenürü nötralize eder. Metilamin, ticari olarak amonyan klorometan ile reaksiyonu ile hazrlanr ve amonyan 2-bromopropanoik asit ile reaksiyonu% 70 verimle rasemik alanin hazrlamak için kullanlmtr. Etanolamin, etilen oksit ile bir halka açma reaksiyonu ile hazrlanr: reaksiyonun bazen dietanolamin ve trietanolamin üretmek için daha ileri gitmesine izin verilir.Amitler, amonyan karboksilik asit türevleri ile reaksiyona sokulmasyla hazrlanabilir. Asil klorürler en reaktif olanlardr, ancak oluan hidrojen klorürü nötralize etmek için amonyak en az iki kat fazla olmaldr. Esterler ve anhidritler ayrca amidler oluturmak için amonyakla reaksiyona girer. Karboksilik asitlerin amonyum tuzlar, termal olarak duyarl gruplar olmad sürece amidlere dehidre edilebilir: 150–200 ° C scaklklar gereklidir.Amonyaktaki hidrojen, saysz ikame ediciyle yer deitirmeye duyarldr. Sodyum ile stldnda sodamide, NaNH2’ye dönüür. [26] Klor ile monokloramin oluur. Be deerli amonyak, λ5-amin veya daha yaygn olarak amonyum hidrit olarak bilinir. Bu kristal kat, yalnzca yüksek basnç altnda stabildir ve normal koullarda üç deerlikli amonyak ve hidrojen gazna ayrr. Bu madde bir zamanlar 1966’da olas bir kat roket yakt olarak aratrlmt. [31] Amonyak, geçi metal komplekslerinde bir ligand görevi görebilir. Spektrokimyasal serinin ortasnda saf bir σ-vericidir ve orta derecede sert-yumuak davran gösterir (ayrca bkz. ECW modeli). Dier Lewis bazlarna kar bir dizi aside kar bal donör gücü C-B grafikleri ile gösterilebilir. [32] [33] Tarihsel nedenlerden dolay, amonyak koordinasyon bileiklerinin isimlendirmesinde ammin olarak adlandrlr. Baz önemli ammin kompleksleri arasnda, bir bakr (II) tuzlar çözeltisine amonyak ilave edilerek oluturulan koyu mavi bir kompleks olan tetraamminediaquacopper (II) ([Cu (NH3) 4 (H2O) 2] 2+) bulunur. Tetraamminediaquacopper (II) hidroksit, Schweizer reaktifi olarak bilinir ve olaanüstü selülozu çözme kabiliyetine sahiptir. Diamminesilver (I) ([Ag (NH3) 2] +), Tollens reaktifindeki aktif türdür. Bu kompleksin oluumu, farkl gümü halojenürlerin çökeltilerini ayrt etmeye de yardmc olabilir: gümü klorür (AgCl) seyreltik (2M) amonyak çözeltisinde çözünür, gümü bromür (AgBr) yalnzca konsantre amonyak çözeltisinde çözünür, gümü iyodür (AgI ) sulu amonyakta çözünmez. 19. yüzyln sonlarnda krom (III) ‘ün amin kompleksleri biliniyordu ve Alfred Werner’n koordinasyon bileiklerinin yaps hakkndaki devrimci teorisinin temelini oluturdu. Werner, [CrCl3 (NH3) 3] kompleksinin yalnzca iki izomerinin (faktör ve mer-) oluturulabileceini kaydetti ve ligandlarn bir oktahedronun köelerinde metal iyonu etrafnda düzenlenmesi gerektii sonucuna vard. Bu öneri, o zamandan beri X-n kristalografisi ile dorulanmtr. Bir metal iyonuna balanan bir ammin ligand, sulu çözeltide protonsuzlama hala nadir olmasna ramen, serbest bir amonyak molekülünden belirgin ekilde daha asidiktir.Bir örnek, ortaya çkan amidomerkür (II) bileiinin yüksek oranda çözünmez olduu Calomel reaksiyonudur.Ammonia, I2, fenol ve Al (CH3) 3 gibi çeitli Lewis asitleri ile 1: 1 eklentiler oluturur. Amonyak sert bir tabandr ve E & C parametreleri EB = 2.31 ve C B = 2.04’tür. Dier Lewis bazlarna kar bir dizi aside kar bal donör gücü, CB grafikleri ile gösterilebilir.Amonyum ve amonyum tuzlar, çok küçük izlerde, Nessler çözeltisinin eklenmesiyle kolayca tespit edilebilir, bu da farkl bir sar renk verir. en ufak bir amonyak veya amonyum tuzlarnn varl. Amonyum tuzlanndaki amonyak miktar, tuzlarn sodyum veya potasyum hidroksit ile damtlmasyla niceliksel olarak tahmin edilebilir, ortaya çkan amonyak bilinen bir hacimde standart sülfürik asit içinde emilir ve daha sonra asit fazlas hacimsel olarak belirlenir; veya amonyak hidroklorik asitte emilebilir ve bu ekilde oluan amonyum klorür, amonyum hekzakloroplatinat, (NH4) 2PtCl6 olarak çökeltilir. [34] Antik Yunan tarihçi Herodot, Libya’nn bir insanlar “Ammonyallar” (imdi: Msr’n kuzeybatsndaki, tuz göllerinin hala var olduu Siwa vahas) adn verdiler. [37] [38] Yunan corafyac Strabo da bu bölgeden gelen tuzdan bahsetti. Ancak, antik yazarlar Dioscorides, Apicius, Arrian, Synesius ve Amida’l Aëtius, bu tuzu, yemek piirmek için kullanlabilecek ve esasen kaya tuzu olan berrak kristaller oluturuyor olarak tanmladlar. [39] Hammoniacus sal, Pliny’nin yazlarnda görünmektedir [40], ancak daha modern sal amonyakla (amonyum klorür) ayn olup olmad bilinmemekle birlikte, [19] [41] [42] drarn bakteriler tarafndan fermantasyonu amonyak çözeltisi; bu nedenle Fermente idrar Klasik Antik Ça’da kuma ve giysiyi ykamak, tabaklama hazrl srasnda derilerden tüyleri çkarmak, boyanan kumata mordan olarak hizmet etmek ve demirden pas çkarmak için kullanld. [43] Sal amonyak formunda, Amonyak, 8. yüzyln balarnda Müslüman simyaclar için önemliydi, ilk olarak Fars-Arap kimyager Jbir ibn Hayyān [44] ve 13. yüzyldan beri Avrupal ​​simyaclar için Albertus Magnus [19] tarafndan bahsediliyordu. Ayrca Orta Ça’da boyaclar tarafndan bitkisel boyalarn rengini deitirmek için fermente idrar formunda kullanlmtr. 15. yüzylda Basilius Valentinus, amonyan, alkalilerin sal amonyak üzerindeki etkisiyle elde edilebileceini gösterdi. [45] Daha sonraki bir dönemde, öküzlerin toynak ve boynuzlarnn damtlmas ve elde edilen karbonatn hidroklorik asit ile nötralize edilmesiyle sal amonyak elde edildiinde, amonyaa “hartshorn ruhu” ad verildi. [19] [46] Gazl amonyak ilk izole edildi. Joseph Black tarafndan 1756’da sal amonyak (Amonyum Klorür) ile kalsine magnezya (Magnezyum Oksit) reaksiyona girerek. [47] [48] 1767’de Peter Woulfe tarafndan, [49] [50] 1770’de [51] Carl Wilhelm Scheele ve 1773’te Joseph Priestley tarafndan tekrar izole edilmi ve onun tarafndan “alkali hava” olarak adlandrlmtr. [19] [52]On bir yl sonra 1785’te Claude Louis Berthollet bileimini dorulad. [53] [19] Haber – Bosch’un havadaki nitrojenden amonyak üretme ilemi 1909’da Fritz Haber ve Carl Bosch tarafndan gelitirildi ve 1910’da patentlendi. ili’den nitrat tedarikini kesen müttefik ablukasn takiben, ilk olarak 1. Dünya Sava srasnda Almanya’da endüstriyel ölçekte kullanld [54]. Amonyak, sava çabalarn sürdürmek için patlayclar üretmek için kullanld. [55] Doal gazn bulunmasndan önce, amonyak üretiminin öncüsü olarak hidrojen, suyun elektrolizi veya kloralkali ilemi kullanlarak üretiliyordu. 20. yüzylda amonyak, koklaabilir ta kömürü üretiminin bir yan ürünü haline geldi. 2019 itibariyle ABD’de amonyan yaklak% 88’i gübre olarak tuz, solüsyon veya susuz olarak kullanld. [13] Topraa uygulandnda, msr ve buday gibi mahsullerin veriminin artmasna yardmc olur. [56] ABD’de uygulanan tarmsal nitrojenin% 30’u susuz amonyak eklindedir ve dünya çapnda her yl 110 milyon ton uygulanmaktadr. [57] Amonyak, nitrojen içeren çou bileiin dorudan veya dolayl olarak öncüsüdür. Neredeyse tüm sentetik nitrojen bileikleri amonyaktan elde edilir. Önemli bir türev nitrik asittir. Bu temel malzeme Ostwald ilemi yoluyla amonyan hava ile platin katalizör üzerinde 700–850 ° C (1.292–1.562 ° F), ≈9 atm’de oksidasyonu ile üretilir. Nitrik oksit bu dönüümde bir ara maddedir: [58] NH3 + 2 O2 → HNO3 + H2O Ev tipi amonyak sudaki bir NH3 solüsyonudur ve birçok yüzey için genel amaçl bir temizleyici olarak kullanlr. Amonyak nispeten iz brakmayan bir parlaklk saladndan, en yaygn kullanmlarndan biri cam, porselen ve paslanmaz çelii temizlemektir. Ayrca frnlarn temizliinde ve pimi kiri gevetmek için slatma maddelerinde sklkla kullanlr. Ev tipi amonyak, arlkça% 5 ile% 10 arasnda amonyak arasnda deimektedir. [59] Amerika Birleik Devletleri temizlik ürünleri üreticilerinin, kullanlan konsantrasyonu listeleyen ürünün malzeme güvenlik veri sayfasn salamalar gerekmektedir. [60] 1895’in balarnda, amonyan “kuvvetli antiseptik olduu biliniyordu … litre bana 1,4 gram gerektirir sr çayn koruyun. “[61] Bir çalmada susuz amonyak, 3 tür hayvan yeminde zoonotik bakterilerin% 99,999’unu yok etti, ancak silaj yok etti. [62] [63] Susuz amonyak u anda ticari olarak sr etinin mikrobiyal kontaminasyonunu azaltmak veya ortadan kaldrmak için kullanlmaktadr. [64] [65] Sr eti endüstrisindeki yasz ince dokulu sr eti (halk arasnda “pembe balçk” olarak bilinir), yal sr etlerinden (yaklak% 50-70 ya) s ve santrifüjleme kullanlarak yan çkarlmas ve ardndan E. coli. lem, tedavinin E. coli’yi tespit edilemeyen seviyelere düürdüünü bulan bir aratrmaya dayanarak ABD Tarm Bakanl tarafndan etkili ve güvenli kabul edildi. [66] Optimal amonyak seviyelerinde ilenmi sr etinin tad ve kokusu ile ilgili tüketici ikayetlerinin yan sra süreçle ilgili güvenlik endieleri de olmutur.