Relevant bibliographies by topics / Metal ammonia solutions / Journal articles
To see the other types of publications on this topic, follow the link: Metal ammonia solutions.

Journal articles on the topic 'Metal ammonia solutions'

Author: Grafiati
Published: 4 June 2021
Last updated: 31 January 2023

Create a spot-on reference in APA, MLA, Chicago, Harvard, and other styles

Select a source type:

Consult the top 50 journal articles for your research on the topic 'Metal ammonia solutions.'

Next to every source in the list of references, there is an 'Add to bibliography' button. Press on it, and we will generate automatically the bibliographic reference to the chosen work in the citation style you need: APA, MLA, Harvard, Chicago, Vancouver, etc.

You can also download the full text of the academic publication as pdf and read online its abstract whenever available in the metadata.

Browse journal articles on a wide variety of disciplines and organise your bibliography correctly.

1

Tran, N. E., and J. J. Lagowski. "Metal Ammonia Solutions: Solutions Containing Argentide Ions." Inorganic Chemistry 40, no. 5 (February 2001): 1067–68. http://dx.doi.org/10.1021/ic000333x.

Full text
APA, Harvard, Vancouver, ISO, and other styles
2

Leung, Kevin, and Félix S. Csajka. "Lattice Model for Metal Ammonia Solutions." Physical Review Letters 78, no. 19 (May 12, 1997): 3721–24. http://dx.doi.org/10.1103/physrevlett.78.3721.

Full text
APA, Harvard, Vancouver, ISO, and other styles
3

Deng, Zhihong, Glenn J. Martyna, and Michael L. Klein. "Electronic states in metal-ammonia solutions." Physical Review Letters 71, no. 2 (July 12, 1993): 267–70. http://dx.doi.org/10.1103/physrevlett.71.267.

Full text
APA, Harvard, Vancouver, ISO, and other styles
4

Tran, N. E., and J. J. Lagowski. "ChemInform Abstract: Metal Ammonia Solutions: Solutions Containing Argentide Ions." ChemInform 32, no. 22 (May 26, 2010): no. http://dx.doi.org/10.1002/chin.200122010.

Full text
APA, Harvard, Vancouver, ISO, and other styles
5

Hannongbua, Kiselev, and Heinzinger. "MOLECULAR DYNAMICS SIMULATIONS OF SUPERCRITICAL AMMONIA AND METAL-AMMONIA SOLUTIONS." Condensed Matter Physics 3, no. 2 (2000): 381. http://dx.doi.org/10.5488/cmp.3.2.381.

Full text
APA, Harvard, Vancouver, ISO, and other styles
6

Carlile, Colin, Ian McL Jamie, John W. White, Michael J. Prager, and William Stead. "Rotational tunnelling of ammonia in two-dimensional metal–ammonia solutions." J. Chem. Soc., Faraday Trans. 87, no. 1 (1991): 73–81. http://dx.doi.org/10.1039/ft9918700073.

Full text
APA, Harvard, Vancouver, ISO, and other styles
7

SOLIN, S. A. "TWO-DIMENSIONAL METAL-AMMONIA-SOLUTIONS IN GRAPHITE." Le Journal de Physique IV 01, no. C5 (December 1991): C5–311—C5–324. http://dx.doi.org/10.1051/jp4:1991536.

Full text
APA, Harvard, Vancouver, ISO, and other styles
8

Burkart, Rainer, and Ulrich Schindewolf. "Highly conducting states in metal–ammonia solutions." Physical Chemistry Chemical Physics 2, no. 14 (2000): 3263–68. http://dx.doi.org/10.1039/b002598o.

Full text
APA, Harvard, Vancouver, ISO, and other styles
9

Leung, Kevin, and Félix S. Csajka. "Metal ammonia solutions: A lattice model approach." Journal of Chemical Physics 108, no. 21 (June 1998): 9050–61. http://dx.doi.org/10.1063/1.476351.

Full text
APA, Harvard, Vancouver, ISO, and other styles
10

Heinzinger, K. "Computer simulations of metal-liquid ammonia solutions." Journal of Molecular Liquids 88, no. 1 (October 2000): 77–85. http://dx.doi.org/10.1016/s0167-7322(00)00139-2.

Full text
APA, Harvard, Vancouver, ISO, and other styles
11

Deng, Zhihong, Glenn J. Martyna, and Michael L. Klein. "Quantum simulation studies of metal–ammonia solutions." Journal of Chemical Physics 100, no. 10 (May 15, 1994): 7590–601. http://dx.doi.org/10.1063/1.466852.

Full text
APA, Harvard, Vancouver, ISO, and other styles
12

Mukhomorov, V. K. "Magnetic properties of electrons in metal-ammonia solutions." Technical Physics 42, no. 8 (August 1997): 855–65. http://dx.doi.org/10.1134/1.1258747.

Full text
APA, Harvard, Vancouver, ISO, and other styles
13

ARENDT, P. "A HIGH-CONDUCTING STATE IN LIQUID METAL-AMMONIA SOLUTIONS." Le Journal de Physique IV 01, no. C5 (December 1991): C5–245—C5–249. http://dx.doi.org/10.1051/jp4:1991529.

Full text
APA, Harvard, Vancouver, ISO, and other styles
14

Howard, Christopher A., and Neal T. Skipper. "Computer Simulations of Fulleride Anions in Metal-Ammonia Solutions." Journal of Physical Chemistry B 113, no. 11 (March 19, 2009): 3324–32. http://dx.doi.org/10.1021/jp8083502.

Full text
APA, Harvard, Vancouver, ISO, and other styles
15

Chuev, Gennady N., and Pascal Quémerais. "Herzfeld instability versus Mott transition in metal–ammonia solutions." Comptes Rendus Physique 8, no. 3-4 (April 2007): 449–55. http://dx.doi.org/10.1016/j.crhy.2007.05.016.

Full text
APA, Harvard, Vancouver, ISO, and other styles
16

Burkart, Rainer, and Ulrich Schindewolf. "ChemInform Abstract: Highly Conducting States in Metal-Ammonia Solutions." ChemInform 31, no. 42 (October 17, 2000): no. http://dx.doi.org/10.1002/chin.200042005.

Full text
APA, Harvard, Vancouver, ISO, and other styles
17

SOLIN, S. A. "ChemInform Abstract: Two-Dimensional Metal-Ammonia-Solutions in Graphite." ChemInform 23, no. 32 (August 21, 2010): no. http://dx.doi.org/10.1002/chin.199232256.

Full text
APA, Harvard, Vancouver, ISO, and other styles
18

Likal’ter, A. A. "The metal-insulator transition and the phase transition in metal-ammonia solutions." Journal of Experimental and Theoretical Physics 84, no. 3 (March 1997): 516–21. http://dx.doi.org/10.1134/1.558170.

Full text
APA, Harvard, Vancouver, ISO, and other styles
19

Zahir, Md Hasan, Shakhawat Chowdhury, Md Abdul Aziz, and Mohammad Mizanur Rahman. "Host–Guest Extraction of Heavy Metal Ions with p-t-Butylcalix[8]arene from Ammonia or Amine Solutions." International Journal of Analytical Chemistry 2018 (July 11, 2018): 1–11. http://dx.doi.org/10.1155/2018/4015878.

Full text
Abstract:
The capacities of the p-t-butylcalix[8]arene (abbreviated as H8L) host to extract toxic divalent heavy metal ions and silver from aqueous solution phases containing ammonia or ethylene diamine to an organic phase (nitrobenzene, dichloromethane, or chloroform) were carried out. When the metal ions were extracted from an aqueous ammonia solution, the metal ion selectivity for extraction was found to decrease in the order Cd2+> Ni2+> Cu2+> Ag+> Co2+> Zn2+. When the aqueous phase contained ethylene diamine, excellent extraction efficiencies of 97% and 90% were observed for the heavy metal ions Cu2+ and Cd2+, respectively. Under the same conditions the extraction of octahedral type metal ions, namely, Co2+ and Ni2+, was suppressed. The extraction of transition metal cations by H8L in ammonia and/or amine was found to be pH dependent. Detailed analysis of extraction behavior was investigated by slope analysis, the continuous variation method, and by loading tests.
APA, Harvard, Vancouver, ISO, and other styles
20

Quemerais, P., J. L. Raimbault, and S. Fratini. "Polarization catastrophe in doped cuprates and metal-ammonia solutions. Metal-to-superconductor transition versus phase separation." Journal de Physique IV 12, no. 9 (November 2002): 227–30. http://dx.doi.org/10.1051/jp4:20020400.

Full text
Abstract:
On doping polar dielectrics, such as cuprates (solid) or amonia (liquid), the polarization induces the formation of polarons or solvated electrons. However, the exact role of such entities in the metal-to-insulator transition (MIT) which occurs at some critical densities still remains unclear. We think that their formation together with their long-range Coulomb interactions are responsable for a polarization catastrophe leading to the MIT. Moreover, the accompanishing phenomena is the occurence of a negative sign of the static dielectric constant, which could yield either an insulator-to-superconductor transition in cuprates, either a phase separation in metal-ammonia solutions. The difference of hehavior possibly could come from the nature of the counter ions of the doping charges, which are essentially frozen in oxides, while they remain in a liquid state in metal-ammonia system.
APA, Harvard, Vancouver, ISO, and other styles
21

Mahmudov, F. T. "EXTRACTION OF IONS OF SOME TRANSITION ELEMENTS AND THEIR AMMONIA COMPLEXES FROM SOLUTIONS ON Na-CLINOPTYLOLITE AND Na-MORDENITE." Azerbaijan Chemical Journal, no. 2 (June 2, 2022): 34–39. http://dx.doi.org/10.32737/0005-2531-2022-2-34-39.

Full text
Abstract:
Modified natural zeolites in the Na-form (clinoptilolite tuff of the Aydag and mordenite of the Chananab deposits in Azerbaijan) were studied in order to extract cations of the transition and heavy metals water and industrial liquid waste. The equilibrium and kinetic characteristics of the sorption process under static and dynamic conditions have been studied. Distribution isotherms of exchange ions between Na forms of zeolites with chloride (Ni2+, Co2+, Cu2+, Zn2+, Сd2+) and nitric acid (Hg+, Ag+) solutions have been obtained. It has been found that the increased selectivity of Na-zeolites to metal cations is due to their pronounced selectivity with respect to Ag+ ions over the entire range of concentration changes in solution and solid phase, as well as to cations in the ammonium form ([Ni(NH3)6]2+, [Co(NH3)6]2+, [Cu(NH3)4]2+, [Cd(NH3)6]2+, [Zn(NH3)4]2+) from low selectivity and selectivity to cations in the usual form. This fact makes it possible to extract the studied cations from the mixture in the form of ammonia, in accordance with the established range of selectivity of Na-zeolites to non-ferrous cations and their ammonia complexes
APA, Harvard, Vancouver, ISO, and other styles
22

Terakado, O., T. Kamiyama, and Y. Nakamura. "Low-field EPR study of the metal–non-metal transition in sodium–ammonia solutions." Journal of the Chemical Society, Faraday Transactions 94, no. 7 (1998): 867–69. http://dx.doi.org/10.1039/a708597d.

Full text
APA, Harvard, Vancouver, ISO, and other styles
23

CHIEUX, P. "EVIDENCE FOR COARSE STRUCTURE (INTERMEDIATE RANGE ORDER) IN METAL-AMMONIA SOLUTIONS." Le Journal de Physique IV 01, no. C5 (December 1991): C5–373—C5–375. http://dx.doi.org/10.1051/jp4:1991545.

Full text
APA, Harvard, Vancouver, ISO, and other styles
24

Deng, Zhihong, Michael L. Klein, and Glenn J. Martyna. "Electronic states and the metal–insulator transition in caesium–ammonia solutions." J. Chem. Soc., Faraday Trans. 90, no. 14 (1994): 2009–13. http://dx.doi.org/10.1039/ft9949002009.

Full text
APA, Harvard, Vancouver, ISO, and other styles
25

Pashitskiı̆, É. A. "Did Ogg really observe high-temperature superconductivity in metal-ammonia solutions?" Low Temperature Physics 24, no. 11 (November 1998): 835–36. http://dx.doi.org/10.1063/1.593686.

Full text
APA, Harvard, Vancouver, ISO, and other styles
26

Chuev, Gennady N., and Marina V. Fedotova. "Electron–electron attraction caused by dispersion forces in metal–ammonia solutions." Chemical Physics Letters 556 (January 2013): 138–41. http://dx.doi.org/10.1016/j.cplett.2012.12.005.

Full text
APA, Harvard, Vancouver, ISO, and other styles
27

Chuev, Gennady N., Pascal Quémerais, and Jason Crain. "Nature of the metal–nonmetal transition in metal–ammonia solutions. I. Solvated electrons at low metal concentrations." Journal of Chemical Physics 127, no. 24 (December 28, 2007): 244501. http://dx.doi.org/10.1063/1.2812244.

Full text
APA, Harvard, Vancouver, ISO, and other styles
28

Ross, Claudia B., Travis Wade, Richard M. Crooks, and Douglas M. Smith. "Electrochemical synthesis of metal nitride ceramic precursors in liquid ammonia electrolyte solutions." Chemistry of Materials 3, no. 5 (September 1991): 768–71. http://dx.doi.org/10.1021/cm00017a002.

Full text
APA, Harvard, Vancouver, ISO, and other styles
29

Hung, Chang-Mao, Jie-Chung Lou, and Chia-Hua Lin. "Wet Air Oxidation of Aqueous Ammonia Solutions Catalyzed by Composite Metal Oxide." Environmental Engineering Science 20, no. 6 (November 2003): 547–56. http://dx.doi.org/10.1089/109287503770736069.

Full text
APA, Harvard, Vancouver, ISO, and other styles
30

Buttersack, Tillmann, Philip E. Mason, Ryan S. McMullen, H. Christian Schewe, Tomas Martinek, Krystof Brezina, Martin Crhan, et al. "Photoelectron spectra of alkali metal–ammonia microjets: From blue electrolyte to bronze metal." Science 368, no. 6495 (June 4, 2020): 1086–91. http://dx.doi.org/10.1126/science.aaz7607.

Full text
Abstract:
Experimental studies of the electronic structure of excess electrons in liquids—archetypal quantum solutes—have been largely restricted to very dilute electron concentrations. We overcame this limitation by applying soft x-ray photoelectron spectroscopy to characterize excess electrons originating from steadily increasing amounts of alkali metals dissolved in refrigerated liquid ammonia microjets. As concentration rises, a narrow peak at ~2 electron volts, corresponding to vertical photodetachment of localized solvated electrons and dielectrons, transforms continuously into a band with a sharp Fermi edge accompanied by a plasmon peak, characteristic of delocalized metallic electrons. Through our experimental approach combined with ab initio calculations of localized electrons and dielectrons, we obtain a clear picture of the energetics and density of states of the ammoniated electrons over the gradual transition from dilute blue electrolytes to concentrated bronze metallic solutions.
APA, Harvard, Vancouver, ISO, and other styles
31

Nicholas, Thomas C., Thomas F. Headen, Jonathan C. Wasse, Christopher A. Howard, Neal T. Skipper, and Andrew G. Seel. "Intermediate Range Order in Metal–Ammonia Solutions: Pure and Na-Doped Ca-NH3." Journal of Physical Chemistry B 125, no. 27 (July 2, 2021): 7456–61. http://dx.doi.org/10.1021/acs.jpcb.1c03843.

Full text
APA, Harvard, Vancouver, ISO, and other styles
32

NAKAMURA, Y. "PHYSICAL PROPERTIES OF ALKALI METAL-AMMONIA (AMINE) SOLUTIONS STUDIED BY MAGNETIC RESONANCE METHODS." Le Journal de Physique IV 01, no. C5 (December 1991): C5–61—C5–70. http://dx.doi.org/10.1051/jp4:1991507.

Full text
APA, Harvard, Vancouver, ISO, and other styles
33

Arendt, P. "Dissipationless electric current flow through decomposing liquid metal-ammonia solutions between copper electrodes." Electrochimica Acta 30, no. 6 (June 1985): 709–18. http://dx.doi.org/10.1016/0013-4686(85)80117-1.

Full text
APA, Harvard, Vancouver, ISO, and other styles
34

Bardina, E. S., Y. B. Elchishcheva, L. G. Chekanova, and A. S. Maksimov. "Research of the complex formation of neopentanic acid hydrazide with non-ferrous metal ions." Вестник Пермского университета. Серия «Химия» = Bulletin of Perm University. CHEMISTRY 10, no. 2 (2020): 143–49. http://dx.doi.org/10.17072/2223-1838-2020-2-143-149.

Full text
Abstract:
The processes of complexation of neopentanic acid hydrazide (GnPC) with Cu(II), Co(II), Ni(II),Fe(III), Ag(I) ions in ammonia and hydrochloric acid solutions by spectrophotometric methodhave been studied. The optimal conditionsfor the formation of complexes have been found; the molar ratios [Me(II)]:[GnPC] have beenestablishedby saturation and shift of equilibriummethods.
APA, Harvard, Vancouver, ISO, and other styles
35

Bobik, Magdalena, Irena Korus, and Lidia Dudek. "The effect of magnetite nanoparticles synthesis conditions on their ability to separate heavy metal ions." Archives of Environmental Protection 43, no. 2 (June 27, 2017): 3–9. http://dx.doi.org/10.1515/aep-2017-0017.

Full text
Abstract:
Abstract Magnetite nanoparticles have become a promising material for scientific research. Among numerous technologies of their synthesis, co-precipitation seems to be the most convenient, less time-consuming and cheap method which produces fine and pure iron oxide particles applicable to environmental issues. The aim of the work was to investigate how the co-precipitation synthesis parameters, such as temperature and base volume, influence the magnetite nanoparticles ability to separate heavy metal ions. The synthesis were conducted at nine combinations of different ammonia volumes - 8 cm3, 10 cm3, 15 cm3 and temperatures - 30°C, 60°C, 90°C for each ammonia volume. Iron oxides synthesized at each combination were examined as an adsorbent of seven heavy metals: Cr(VI), Pb(II), Cr(III), Cu(II), Zn(II), Ni(II) and Cd(II). The representative sample of magnetite was characterized using XRD, SEM and BET methods. It was observed that more effective sorbent for majority of ions was produced at 30°C using 10 cm3 of ammonia. The characterization of the sample produced at these reaction conditions indicate that pure magnetite with an average crystallite size of 23.2 nm was obtained (XRD), the nanosized crystallites in the sample were agglomerated (SEM) and the specific surface area of the aggregates was estimated to be 55.64 m2·g-1 (BET). The general conclusion of the work is the evidence that magnetite nanoparticles have the ability to adsorb heavy metal ions from the aqueous solutions. The effectiveness of the process depends on many factors such as kind of heavy metal ion or the synthesis parameters of the sorbent.
APA, Harvard, Vancouver, ISO, and other styles
36

Zhao, Ting Kai, Le Hao Liu, Guang Ming Li, and Mo Tang Tang. "Zinc and Cobalt Recovery from Co-Ni Residue of Zinc Hydrometallurgy by an Ammonia Process." Advanced Materials Research 396-398 (November 2011): 48–51. http://dx.doi.org/10.4028/www.scientific.net/amr.396-398.48.

Full text
Abstract:
A new process for treating a Co-Ni residue of zinc metallurgy to produce zinc powder and recover cobalt in ammonia and ammonium sulfate(AAS) solutions was proposed. In this process, the baked Co-Ni residue was leached in AAS solutions. The leached solution was purified to remove the impurities by adding zinc powder and to separate Zn and Co from Cu, and Zn from Co and Cd. Under the optimal technical parameters, the metal leaching rate was 91.18 Zn, 96.98 Cu, 99.38 Cd and 89.35 Co in wt% respectively. The high cobalt-residue bearing 3.79wt% cobalt that of 8.4 times the raw Co-Ni residue can be used as a raw material for extracting cobalt or cobalt-salt. An active zinc powder could be obtained by using electrolysis from zinc purification solution, and current efficiency of the electrolysis is more than 88.19%. It’s a practical technology for treating waste-residue in zinc hydrometallurgy and will be a feasible process to recover valuable metals.
APA, Harvard, Vancouver, ISO, and other styles
37

Chuev, Gennady N., and Pascal Quémerais. "Nature of metal–nonmetal transition in metal–ammonia solutions. II. From uniform metallic state to inhomogeneous electronic microstructure." Journal of Chemical Physics 128, no. 14 (April 14, 2008): 144503. http://dx.doi.org/10.1063/1.2883695.

Full text
APA, Harvard, Vancouver, ISO, and other styles
38

Mironov, V. E., G. L. Pashkov, and T. V. Stupko. "Thermodynamics of formation reaction and hydrometallurgical application of metal–ammonia complexes in aqueous solutions." Russian Chemical Reviews 61, no. 9 (September 30, 1992): 944–58. http://dx.doi.org/10.1070/rc1992v061n09abeh001008.

Full text
APA, Harvard, Vancouver, ISO, and other styles
39

Imamura, Hayao, Takashi Yoshimura, and Yoshihisa Sakata. "Alloying of Yb–Cu and Yb–Ag utilizing liquid ammonia metal solutions of ytterbium." Journal of Solid State Chemistry 171, no. 1-2 (February 2003): 254–56. http://dx.doi.org/10.1016/s0022-4596(02)00161-5.

Full text
APA, Harvard, Vancouver, ISO, and other styles
40

Uyama, Haruo, Yasushi Kanzaki, and Osamu Matsumoto. "Ion-exchange on synthetic zeolites in non-aqueous ammonia solutions of alkali metal nitrates." Materials Research Bulletin 22, no. 2 (February 1987): 157–64. http://dx.doi.org/10.1016/0025-5408(87)90066-3.

Full text
APA, Harvard, Vancouver, ISO, and other styles
41

Arendt, P. "Distribution of Fröhlich supercurrents through a gel made from decomposing liquid metal-ammonia solutions." Solid State Communications 70, no. 11 (June 1989): 1001–5. http://dx.doi.org/10.1016/0038-1098(89)90181-6.

Full text
APA, Harvard, Vancouver, ISO, and other styles
42

Ksandrov, Nikolai V., and Olga R. Ozhogina. "ADSORPTION OF AMMONIA WITH ACTIVATED COAL AG-3." IZVESTIYA VYSSHIKH UCHEBNYKH ZAVEDENIY KHIMIYA KHIMICHESKAYA TEKHNOLOGIYA 61, no. 8 (August 21, 2018): 53. http://dx.doi.org/10.6060/ivkkt201861008.5726.

Full text
Abstract:
The problem of NH3 extraction from wet gases and returning it to the process may take place in the technologies which use aqueous ammonia solutions. The extraction of non-ferrous metal oxides forming soluble ammoniates from industrial wastes with the solution of ammonium chloride and ammonia in water is an example of such technologies. The oxides of non-ferrous metals are then precipitated, driving the mixture of water vapor and ammonia off the solution. Waste purification reduces the pollution of natural water resources and expands the raw material base of metallurgy of copper and zinc. To return NH3 to the waste treatment it is efficient to use adsorption of ammonia from the gas-vapor mixture. The silica gel used in ammonia plants is not applicable to absorption NH3 from wet gases. The data on the adsorption NH3 from the gas-vapor mixture with hydrophobic activated coals are not sufficient for practical purposе. The dependence of the equilibrium adsorption capacity of activated coal AG-3 on ammonia wapors on their partial pressure at 0.1−15 kPa and a tempеrature of 288−323 K in the sorption of ammonia from wet gases is studied with a dynamic method. The micropore volume of the coal samples is equal to 0.31±0.02 cm3/g. The presented equation provides the calculation of the sorption capacity of coal in the studied range of adsorption parameter change with an average error less than 5% for each isotherme. The heat of adsorption is equal to 37 -39 kJ/mol which is larger than the heat of condensation of ammonia vapors by about 20 kJ/mol, which is typical for physical adsorption. During the regeneration of the coal which absorbed the ammonia the adsorption capacity was stable.
APA, Harvard, Vancouver, ISO, and other styles
43

Dye, James L. "The alkali metals: 200 years of surprises." Philosophical Transactions of the Royal Society A: Mathematical, Physical and Engineering Sciences 373, no. 2037 (March 13, 2015): 20140174. http://dx.doi.org/10.1098/rsta.2014.0174.

Full text
Abstract:
Alkali metal compounds have been known since antiquity. In 1807, Sir Humphry Davy surprised everyone by electrolytically preparing (and naming) potassium and sodium metals. In 1808, he noted their interaction with ammonia, which, 100 years later, was attributed to solvated electrons. After 1960, pulse radiolysis of nearly any solvent produced solvated electrons, which became one of the most studied species in chemistry. In 1968, alkali metal solutions in amines and ethers were shown to contain alkali metal anions in addition to solvated electrons. The advent of crown ethers and cryptands as complexants for alkali cations greatly enhanced alkali metal solubilities. This permitted us to prepare a crystalline salt of Na − in 1974, followed by 30 other alkalides with Na − , K − , Rb − and Cs − anions. This firmly established the −1 oxidation state of alkali metals. The synthesis of alkalides led to the crystallization of electrides, with trapped electrons as the anions. Electrides have a variety of electronic and magnetic properties, depending on the geometries and connectivities of the trapping sites. In 2009, the final surprise was the experimental demonstration that alkali metals under high pressure lose their metallic character as the electrons are localized in voids between the alkali cations to become high-pressure electrides!
APA, Harvard, Vancouver, ISO, and other styles
44

Zemskova, Larisa, Vladimir Silant’ev, Eduard Tokar, and Andrei Egorin. "Synthesis of Inorganic Compounds in the Matrix of Polysaccharide Chitosan." Biomimetics 6, no. 3 (July 5, 2021): 45. http://dx.doi.org/10.3390/biomimetics6030045.

Full text
Abstract:
Data related to the fabrication of hybrid materials based on the polysaccharide chitosan were systematized and reviewed. The possibility of using chitosan as a “host” matrix for in situ synthesis of inorganic compounds for the preparation of various types of composite materials were investigated. Coprecipitation of metal oxides/hydroxides (Fe, Ni, Al, Zr, Cu and Mn) with chitosan was carried out through the alkalinization of solutions containing metal salts and chitosan, with the addition of ammonia or alkali solutions, homogeneous hydrolysis of urea, or electrophoretic deposition on the cathode. The synthesis of transition metal ferrocyanides and hydroxyapatite was achieved from precursor salts in a chitosan solution with simultaneous alkalinization. The mechanism of composite formation during the coprecipitation process of inorganic compounds with chitosan is discussed. Composite materials are of interest as sorbents, coatings, sensors, and precursors for the production of ceramic and electrode materials.
APA, Harvard, Vancouver, ISO, and other styles
45

Imamura, Hayao, Koji Nishimura, Takashi Yoshimura, Hiroshi Yoshimochi, Masakazu Ueno, Yoshihisa Sakata, and Susumu Tsuchiya. "Catalysis of lanthanides deposited on oxide from Eu or Yb metal solutions in liquid ammonia." Journal of Molecular Catalysis A: Chemical 165, no. 1-2 (January 2001): 189–97. http://dx.doi.org/10.1016/s1381-1169(00)00414-3.

Full text
APA, Harvard, Vancouver, ISO, and other styles
46

Bilewicz, A., R. Dybczynski, and J. Narbutt. "Ion exchange of some transition metal cations on hydrated titanium dioxide in aqueous ammonia solutions." Journal of Radioanalytical and Nuclear Chemistry Articles 158, no. 2 (April 1992): 273–82. http://dx.doi.org/10.1007/bf02047114.

Full text
APA, Harvard, Vancouver, ISO, and other styles
47

Kułażyński, Marek, Krystyna Bratek, and Jerzy Walendziewski. "Optimization of an active phase composition in the low-temperature nitric oxide reduction catalyst." Polish Journal of Chemical Technology 9, no. 3 (January 1, 2007): 33–37. http://dx.doi.org/10.2478/v10026-007-0049-0.

Full text
Abstract:
Optimization of an active phase composition in the low-temperature nitric oxide reduction catalyst In the first research studies series a selection of the quantitative composition of catalyst active phase composition (iron, copper and manganese) deposited on mineral-carbon support was carried out. It was found on the basis of the selection studies series that the best results were attained when copper and manganese were used as catalyst components. The quantitative composition of the denitrogention catalyst was estimated using a statistical method of experiment planning and metals content changed in the range 0.5 - 1.5wt % for both metals. Catalyst activity in nitric oxide reduction by ammonia was determined in the dependence on an active phase composition in the temperature range 100 - 200°C, at GHSV (Gas Hour Space Velocity) 6 000 and 10 000 Nm3/m3h, NO concentration 400 ppm, NH3/NO ratio 1:1. A graphic presentation of the obtained results was made using the UNIPLOT program. The highest activity in nitric oxide reduction by ammonia presented copper - manganese catalysts prepared by the impregnation of mineral-carbon support with active metals salts solutions and calcination after each metal impregnation with copper (up to 1.5 wt %) and manganese (up to 1.5 wt %).
APA, Harvard, Vancouver, ISO, and other styles
48

Zabel, H., and D. A. Neumann. "Neutron scattering studies of potassium-ammonia layers in graphite." Canadian Journal of Chemistry 66, no. 4 (April 1, 1988): 666–71. http://dx.doi.org/10.1139/v88-115.

Full text
Abstract:
Neutron scattering investigations of the structural and dynamical properties of ammonia molecules in the stage 1 compound KC24(NH3)4.3 are discussed. The K–NH3 intercalate layers represent the two-dimensional analogue of the well-known metal–ammonia solutions. At room temperature the intercalate liquid structure factor can be described by a model in which the K ions are surrounded on the average by four NH3 molecules, and the remaining molecules are essentially free. Quasi-elastic neutron scattering revealed two independent rotational motions of the NH3 molecule, one associated with the rotation about the C3 symmetry axis and the other one about the K ions. Above 200 K translational diffusion also becomes noticeable. The phonon dispersion of the [00q] longitudinal modes show clear signs of a phonon–libron coupling which causes the acoustic branch to split.
APA, Harvard, Vancouver, ISO, and other styles
49

Tang, Xiaohui, Marc Debliquy, Driss Lahem, Yiyi Yan, and Jean-Pierre Raskin. "A Review on Functionalized Graphene Sensors for Detection of Ammonia." Sensors 21, no. 4 (February 19, 2021): 1443. http://dx.doi.org/10.3390/s21041443.

Full text
Abstract:
Since the first graphene gas sensor has been reported, functionalized graphene gas sensors have already attracted a lot of research interest due to their potential for high sensitivity, great selectivity, and fast detection of various gases. In this paper, we summarize the recent development and progression of functionalized graphene sensors for ammonia (NH3) detection at room temperature. We review graphene gas sensors functionalized by different materials, including metallic nanoparticles, metal oxides, organic molecules, and conducting polymers. The various sensing mechanism of functionalized graphene gas sensors are explained and compared. Meanwhile, some existing challenges that may hinder the sensor mass production are discussed and several related solutions are proposed. Possible opportunities and perspective applications of the graphene NH3 sensors are also presented.
APA, Harvard, Vancouver, ISO, and other styles
50

Kaewpuang-Ngam, Sutasinee, Koji Inazu, and Ken-Ichi Aika. "Selective wet air oxidation of diluted aqueous ammonia solutions over co-precipitated transition metal-aluminium catalysts." Research on Chemical Intermediates 28, no. 5 (July 2002): 471–77. http://dx.doi.org/10.1163/156856702760346888.

Full text
APA, Harvard, Vancouver, ISO, and other styles
We offer discounts on all premium plans for authors whose works are included in thematic literature selections. Contact us to get a unique promo code!

To the bibliography