関: ammonium

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WordNet

the ion NH4 derived from ammonia; behaves in many respects like an alkali metal ion (同)ammonium_ion
the 14th letter of the Roman alphabet (同)n

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アンモニウム,アンモニア塩基
nitrogenの化学記号

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出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2014/06/08 11:12:57」(JST)

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The ammonium cation is a positively charged polyatomic ion with the chemical formula NH₄⁺.^[1] It is formed by the protonation of ammonia (NH₃). Ammonium is also a general name for positively charged or protonated substituted amines and quaternary ammonium cations (NR₄⁺), where one or more hydrogen atoms are replaced by organic radical groups (indicated by R).

Acid base properties

Fumes from hydrochloric acid and ammonia forming a white cloud of ammonium chloride.

The ammonium ion is generated when ammonia, a weak base, reacts with Brønsted acids (proton donors):

H⁺ + NH₃ → NH₄⁺

The acid dissociation constant (pK_a) of NH₄⁺ is 9.25.

The ammonium ion is mildly acidic, reacting with Brønsted bases to return to the uncharged ammonia molecule:

NH₄⁺ + B⁻ → HB + NH₃

Thus, treatment of concentrated solutions of ammonium salts with strong base gives ammonia. When ammonia is dissolved in water, a tiny amount of it converts to ammonium ions:

H₃O⁺ + NH₃ H₂O + NH₄⁺

The degree to which ammonia forms the ammonium ion depends on the pH of the solution. If the pH is low, the equilibrium shifts to the right: more ammonia molecules are converted into ammonium ions. If the pH is high (the concentration of hydrogen ions is low), the equilibrium shifts to the left: the hydroxide ion abstracts a proton from the ammonium ion, generating ammonia.

Formation of ammonium compounds can also occur in the vapor phase; for example, when ammonia vapor comes in contact with hydrogen chloride vapor, a white cloud of ammonium chloride forms, which eventually settles out as a solid in a thin white layer on surfaces.

The conversion of ammonium back to ammonia is easily accomplished by the addition of a strong base.

Ammonium salts

Formation of ammonium

Ammonium cation is found in a variety of salts such as ammonium carbonate, ammonium chloride, and ammonium nitrate. Most simple ammonium salts are very soluble in water. An exception is ammonium hexachloroplatinate, the formation of which was once used as a test for ammonium. The ammonium salts of nitrate and especially perchlorate are highly explosive, in these cases ammonium is the reducing agent.

In an unusual process, ammonium ions form an amalgam. Such species are prepared by the electrolysis of an ammonium solution using a mercury cathode.^[2] This amalgam eventually decomposes to release ammonia and hydrogen.^[3]

Structure and bonding

The lone electron pair on the nitrogen atom (N) in ammonia, represented as a pair of dots, forms the bond with a proton (H⁺). Thereafter, all four N-H bonds are equivalent, being polar covalent bonds. The ion is isoelectronic with methane and borohydride. In terms of size, the ammonium cation (r_ionic = 175 pm) resembles the caesium cation (r_ionic = 183 pm).

Organic ammonium ions

The hydrogen atoms in the ammonium ion can be substituted with an alkyl group or some other organic group to form a substituted ammonium ion (IUPAC nomenclature": aminium ion). Depending on the number of organic groups, the ammonium cation is called a primary, secondary, tertiary, or quaternary. With the exception of the quaternary ammonium cations, the organic ammonium cations are weak acids.

An example of a reaction forming an ammonium ion is that between dimethylamine, (CH₃)₂NH, and an acid, to give the dimethylaminium cation, (CH₃)₂NH+
2:

Quaternary ammonium cations have four organic groups attached to the nitrogen atom. They lack a hydrogen atom bonded to the nitrogen atom. These cations, such as the tetra-n-butylammonium cation, are sometimes used to replace sodium or potassium ions to increase the solubility of the associated anion in organic solvents. Primary, secondary, and tertiary ammonium salts serve the same function, but are less lipophilic. They are also used as phase-transfer catalysts and surfactants.

Biology

Ammonium ions are a waste product of the metabolism of 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, because urea 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.^[4]

Ammonium is an important source of nitrogen for many plant species, especially those growing on hypoxic soils. However, it is also toxic to most crop species and is rarely applied as a sole nitrogen source.^[5]

Ammonium metal

The ammonium ion has very similar properties to the heavier alkali metals and is often considered a close relative.^[6]^[7]^[8] Ammonium is expected to behave as a metal (NH+
4 ions in a sea of electrons) at very high pressures, such as inside gas giant planets such as Uranus and Neptune.^[7]^[8]

References

^ In the substitutive nomenclature, NH₄⁺ is denoted by the name "azanium".
^ Pseudo-binary compounds
^ "Ammonium Salts". VIAS Encyclopedia.
^ Campbell, Neil A.; Jane B. Reece (2002). "44". Biology (6th ed.). San Francisco: Pearson Education, Inc. pp. 937–938. ISBN 0-8053-6624-5. Cite uses deprecated parameters (help)
^ Britto, DT; Kronzucker, HJ (2002). "NH₄⁺ toxicity in higher plants: a critical review". Journal of Plant Physiology 159 (6): 567–584. doi:10.1078/0176-1617-0774.
^ Holleman, A. F.; Wiberg, E. (2001), Inorganic Chemistry, San Diego: Academic Press, ISBN 0-12-352651-5
^ ^a ^b Stevenson, D. J. (November 20, 1975). "Does metallic ammonium exist?". Nature (Nature Publishing Group) 258: 222–223. Bibcode:1975Natur.258..222S. doi:10.1038/258222a0. Retrieved January 13, 2012.
^ ^a ^b Bernal, M. J. M.; Massey, H. S. W. (February 3, 1954). "Metallic Ammonium". Monthly Notices of the Royal Astronomical Society (Wiley-Blackwell for the Royal Astronomical Society) 114: 172–179. Bibcode:1954MNRAS.114..172B. Retrieved January 13, 2012.

UpToDate Contents

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English Journal

Structural, spectroscopic, optical, dielectric and mechanical study of pure and l-Proline doped ammonium dihydrogen phosphate single crystals.

Hasmuddin M1, Singh P1, Shkir M2, Abdullah MM3, Vijayan N4, Bhagavannarayana G4, Wahab MA5.Author information 1Crystal Growth Laboratory, Dept. of Physics, Jamia Millia Islamia, New Delhi 110 025, India.2Crystal Growth Laboratory, Dept. of Physics, Jamia Millia Islamia, New Delhi 110 025, India; Department of Physics, School of Science, King Khalid University, P.O. Box. 9004, Abha 61413, Saudi Arabia.3Crystal Growth Laboratory, Dept. of Physics, Jamia Millia Islamia, New Delhi 110 025, India; Promising Centre for Sensors and Electronic Devices (PCSED), Department of Physics, College of Science and Arts, Najran University, P.O. Box 1988, Najran 11001, Saudi Arabia.4CSIR-National Physical Laboratory, Dr. K.S. Krishnan Road, New Delhi 110 012, India.5Crystal Growth Laboratory, Dept. of Physics, Jamia Millia Islamia, New Delhi 110 025, India. Electronic address: mwahab@jmi.ac.in.AbstractSingle crystals of pure and l-Proline (LP) C5H9NO2 doped ammonium dihydrogen phosphate (ADP) (NH4) H2PO4 were grown by slow evaporation solution technique (SEST) at ambient conditions. Powder X-ray diffraction (PXRD) analysis was carried out to confirm the crystal structure and no additional phase was observed due to doping except a systematic variation in peak intensities. FT-Raman analysis also confirms that there is no additional phase formation due to doping. Fourier transform infrared spectral analysis was done to examine the presence of various functional groups in the grown crystals. UV-VIS-NIR spectroscopic analysis was carried out to see the change in optical transparency of pure ADP and crystals due to LP with different doping concentrations. The high-resolution X-ray diffraction (HRXRD) analysis was carried out to examine the crystalline perfection and observed reasonable changes with LP doping. Second harmonic generation (SHG) efficiency measurement was done to examine the enhancement in the nonlinear optical characteristics of the grown crystals. The dielectric behavior of the samples shows that the dielectric constant decreased with increase the value of frequency. The effect of LP dopant on crystal morphology, mechanical properties of ADP has also been presented in this paper. The above studies reveal the effect of incorporation of LP into the lattice of ADP crystals.
Spectrochimica acta. Part A, Molecular and biomolecular spectroscopy.Spectrochim Acta A Mol Biomol Spectrosc.2014 Apr 5;123:376-84. doi: 10.1016/j.saa.2013.12.038. Epub 2013 Dec 21.
Single crystals of pure and l-Proline (LP) C5H9NO2 doped ammonium dihydrogen phosphate (ADP) (NH4) H2PO4 were grown by slow evaporation solution technique (SEST) at ambient conditions. Powder X-ray diffraction (PXRD) analysis was carried out to confirm the crystal structure and no additional phase w
PMID 24412791

Effects of three kinds of organic acids on phosphorus recovery by magnesium ammonium phosphate (MAP) crystallization from synthetic swine wastewater.

Song Y1, Dai Y2, Hu Q3, Yu X4, Qian F2.Author information 1State Key Laboratory of Environmental Criteria and Risk Assessment, Chinese Research Academy of Environmental Sciences, 100012 Beijing, China; Department of Urban Water Environmental Research, Chinese Research Academy of Environmental Sciences, 100012 Beijing, China. Electronic address: songyh@craes.org.cn.2State Key Laboratory of Environmental Criteria and Risk Assessment, Chinese Research Academy of Environmental Sciences, 100012 Beijing, China; Department of Urban Water Environmental Research, Chinese Research Academy of Environmental Sciences, 100012 Beijing, China.3State Key Laboratory of Environmental Criteria and Risk Assessment, Chinese Research Academy of Environmental Sciences, 100012 Beijing, China; Department of Urban Water Environmental Research, Chinese Research Academy of Environmental Sciences, 100012 Beijing, China; School of Civil Engineering, Beijing Jiaotong University, 100044 Beijing, China.4School of Civil Engineering, Beijing Jiaotong University, 100044 Beijing, China.AbstractP recovery from swine wastewater has become a great concern as a result of the high demand for P resources and its potential eutrophication effects on water ecosystems. The method of magnesium ammonium phosphate (MAP) crystallization was used to recover P from simulated swine wastewater, and the effects of three organic acids (citric acid, succinic acid and acetic acid) on P removal efficiency and rate at different pH values were investigated. The results indicated that the P removal efficiency was worst affected by citric acid in the optimal pH range of 9.0-10.5, followed by succinic acid and acetic acid, and the influencing extent of organic acids decreased with the increasing pH value. Due to the complexation between organic acid and Mg(2+)/NH4(+), all of three organic acids could inhibit the P removal rate at the beginning of the reaction, which showed positive correlation between the inhibition effects and the concentration of organic acids. The high concentration of citric acid could completely suppress the MAP crystallization reaction. Moreover, citric acid and succinic acid brought obvious effects on the morphology of the crystallized products. The experimental results also demonstrated that MAP crystals could be obtained in the presence of different kinds and concentrations of organic acids.
Chemosphere.Chemosphere.2014 Apr;101:41-8. doi: 10.1016/j.chemosphere.2013.11.019. Epub 2013 Dec 2.
P recovery from swine wastewater has become a great concern as a result of the high demand for P resources and its potential eutrophication effects on water ecosystems. The method of magnesium ammonium phosphate (MAP) crystallization was used to recover P from simulated swine wastewater, and the eff
PMID 24296029

Fe/S doped granular activated carbon as a highly active heterogeneous persulfate catalyst toward the degradation of Orange G and diethyl phthalate.

Pu M1, Ma Y1, Wan J2, Wang Y1, Huang M1, Chen Y3.Author information 1College of Environment and Energy, South China University of Technology, Guangzhou 510006, China; The Key Laboratory of Pollution Control and Ecosystem Restoration in Industry Clusters, Ministry of Education, South China University of Technology, Guangzhou 510006, China.2College of Environment and Energy, South China University of Technology, Guangzhou 510006, China; State Key Laboratory of Pulp and Paper Engineering, South China University of Technology, Guangzhou 510640, China. Electronic address: ppjqwan@scut.edu.cn.3State Key Laboratory of Pulp and Paper Engineering, South China University of Technology, Guangzhou 510640, China; School of Chemistry and Chemical Engineering, South China University of Technology, Guangzhou 510640, China.AbstractFe/S doped granular activated carbon (Fe/SGAC) was synthesized with ferric nitrate, Na2S2O3 and (NH4)2S2O8 via an impregnation-precipitation, reduction-oxidation combining with aqueous-phase synthesis method treatment. Surface density of functional groups, surface area changes as well as the chemical state inside Fe/SGAC catalyst were studied by Boehm titration, N2 adsorption and X-ray photoelectron spectroscopy (XPS). The reactivity of the catalysts was tested by degrading Orange G (OG) and diethyl phthalate (DEP). The Fe/SGAC catalysts could significantly enhance the removal rate of OG as compared to persulfate alone and PS/GAC. And the catalytic capacity was also enhanced by S doping. But the degradation of DEP under the similar condition was inhibited by adsorption process because of the different hydrophobicities of OG and DEP molecule. Fe2O3/FeOOH (Fe(3+)) (represents ferrihydrite) together with FeO/Fe3O4 (Fe(2+)) and Fe2O3-satellite, which provide the new active site for persulfate catalyst was found to be the major components of iron element in Fe/SGAC catalyst; the existence of FeS2(S(-)) for sulfur element verified the assumption that the doped S element promoted the electron transfer between the persulfate species and iron oxide at the interface. COD removal experiment further confirmed that mostly contaminant removal was owed to the Fe/SGAC catalytic persulfate oxidation process.
Journal of colloid and interface science.J Colloid Interface Sci.2014 Mar 15;418:330-7. doi: 10.1016/j.jcis.2013.12.034. Epub 2013 Dec 20.
Fe/S doped granular activated carbon (Fe/SGAC) was synthesized with ferric nitrate, Na2S2O3 and (NH4)2S2O8 via an impregnation-precipitation, reduction-oxidation combining with aqueous-phase synthesis method treatment. Surface density of functional groups, surface area changes as well as the chemica
PMID 24461853

Japanese Journal

Effects of preservation period of fertilized eggs and high concentrations of nitrogen in nutrient sources on germling growth of Sargassum horneri

Journal of Applied Phycology 28(5), 2883-2890, 2016-10-01
NAID 120005743912

Contrasting effects of exogenous phosphorus application on N2O emissions from two tropical forest soils with contrasting phosphorus availability

SpringerPlus 5, 2016-08-02
NAID 120005829441

Groundwater geochemistry of a nitrate-contaminated agricultural site

Environmental Earth Sciences 75(15), 1145, 2016-08
NAID 120005905672

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Ammonium
	Systematic name Ammonium
Identifiers
CAS number	14798-03-9
PubChem	16741146
ChemSpider	218
MeSH	D000644
ChEBI	CHEBI:CHEBI:28938
Jmol-3D images	Image 1
	SMILES [NH4+] ;
	InChI InChI=1S/H3N/h1H3/p+1; Key: QGZKDVFQNNGYKY-UHFFFAOYSA-O InChI=1/H3N/h1H3/p+1; Key: QGZKDVFQNNGYKY-IKLDFBCSAZ ;
Properties
Molecular formula	NH+; 4
Molar mass	18.03851 g mol−1
	Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
	Infobox references

　　[★]

アスパラギン asparagine
窒素(原子、分子)

[1] In the substitutive nomenclature, NH₄⁺ is denoted by the name "azanium".

[2] Pseudo-binary compounds

[3] "Ammonium Salts". VIAS Encyclopedia.

[4] Campbell, Neil A.; Jane B. Reece (2002). "44". Biology (6th ed.). San Francisco: Pearson Education, Inc. pp. 937–938. ISBN 0-8053-6624-5. Cite uses deprecated parameters (help)

[5] Britto, DT; Kronzucker, HJ (2002). "NH₄⁺ toxicity in higher plants: a critical review". Journal of Plant Physiology 159 (6): 567–584. doi:10.1078/0176-1617-0774.

[Holleman.26Wiberg-6] Holleman, A. F.; Wiberg, E. (2001), Inorganic Chemistry, San Diego: Academic Press, ISBN 0-12-352651-5

[Stevenson-7] Stevenson, D. J. (November 20, 1975). "Does metallic ammonium exist?". Nature (Nature Publishing Group) 258: 222–223. Bibcode:1975Natur.258..222S. doi:10.1038/258222a0. Retrieved January 13, 2012.

[Bernal.26Massey-8] Bernal, M. J. M.; Massey, H. S. W. (February 3, 1954). "Metallic Ammonium". Monthly Notices of the Royal Astronomical Society (Wiley-Blackwell for the Royal Astronomical Society) 114: 172–179. Bibcode:1954MNRAS.114..172B. Retrieved January 13, 2012.

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案内

NH4+