Zur Konstitution der ammoniakalischen Kupfersalzlösungen

Rosenblatt, F.

doi:10.1002/zaac.19322040404

Cited by 14 publications

(2 citation statements)

References 18 publications

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“…However, it was at the same time also noted that upon addition of a fifth equivalent of ammonia the absorption band shifts in the opposite direction, the so-called pentaammine effect . It was early shown that the rather stable (tetraammine)copper(II) complex is converted to the pentaammine complex in highly concentrated aqueous ammonia solutions. − Furthermore, it was also shown that the UV−visible absorption spectrum of the copper(II) ion in the aqueous ammonia solution is but a little different from that of copper(II) in liquid ammonia . However, it was not possible from these experiments to determine whether the coordination number of five ammonia equivalents around copper(II) could be exceeded or not in a solution .…”

Section: Introductionmentioning

confidence: 99%

Solvation of Copper(II) Ions in Liquid Ammonia

et al. 1996

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X-ray absorption fine structure (XAFS) measurements have been performed at -50 degrees C on a 0.4 mol dm(-)(3) copper(II) nitrate solution in liquid ammonia. Extended X-ray absorption fine structure (EXAFS) spectroscopy was used to determine the coordination number and bond distances for the solvated copper(II) ion in solution. The equatorial ammonia nitrogens are located 2.00 Å from the copper and the axial nitrogen 2.19 Å from the copper. However, it was not possible from the EXAFS analysis alone to conclude whether there was one or two axial nitrogens. Therefore, X-ray absorption near-edge structure (XANES) spectroscopy was combined with discrete variational Xalpha (DV-Xalpha) molecular orbital calculations for a series of five- and six-coordinated models to determine the coordination number and the geometry. The experimental XANES spectrum was best reproduced by a model where the copper(II) ion is pentacoordinated in liquid ammonia in a square pyramidal geometry with the copper(II) ion lifted above the average nitrogen plane.

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Section: Introductionmentioning

confidence: 99%

Solvation of Copper(II) Ions in Liquid Ammonia

et al. 1996

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“…Cupric perchlorate forms various coordination compounds with ammonia which differ in the number of ammonia ligands or by having other ligands. The characterization of these copper perchlorate complexes and the mutual chemical transformations among them were investigated in the first third of the 20 th century [1–4]. The first copper perchlorate‐ammonia complex was probably prepared by Henry Roscoe in 1862.…”

Section: Introductionmentioning

confidence: 99%

Tetraamminecopper Perchlorate (TACP): Explosive Properties

Vodochodský

Künzel

Matyáš

et al. 2020

Propellants Explo Pyrotec

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Tetraamminecopper perchlorate (TACP) is one of the most interesting explosive copper perchlorate‐ammonia complexes. Despite the fact that this complex has been known for more than 100 years there is very little information in the literature about its detonation parameters. Impact sensitivity of TACP is slightly higher than that for PETN while friction sensitivity is between those for PETN and RDX. Detonation velocity for infinite diameter is 3230 m s−1 (density 0.9 g cm−3). Critical diameter of TACP is low – less than 2 mm. Based on the heat of combustion measurement the previously published erroneous enthalpy of formation was corrected to −496 kJ mol−1. Detonation heat of TACP is 4322 kJ kg−1 and Gurney velocity is 1536 m s−1. Experimentally measured detonation parameters of TACP were also compared with theoretically calculated values by the EXPLO5 code.

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Vapor‐liquid equilibrium in ammonia complex systems

1961

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) .Only a postulation of behavior can be made for this region of flow. It may be that the rate of increase in holdup exceeds the rate of increase in area and surface renewal resulting in an over-all It has long been known that aqueous complex systems with volatile ligands, C, H. &fuei&I j. q with E, 1. du Pant de Selke is with Peter J. Schweitzer hivision, Kimberly-Clark Corporation, Lee, Massachusetts. the liquid phase but between the Or complexing goups such as ammo-Nemours & Company, Newport Delaware. W. A. nia, involve equilibrium not only within solution and the vapor over it. When an excess of an insoluble compound of the complexed metal ion is present, equilibria in three phases are involved. Systems of this type are becoming increasingly important in the metallurgical industry. In order to study the behavior of such systems and develop Vol. 7, No. 1 A.1.Ch.E. Journal Washington 2.5, D. C., and may he obtained for $1.25 for photoprints or for 35-inm. microfilm.

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Zur Konstitution der ammoniakalischen Kupfersalzlösungen

Abstract: Die tiefblauen ammoniakalischen Lösungen von Kupfersalzen wurden optisch im Sichtbaren untersucht.

Cited by 14 publications

References 18 publications

Solvation of Copper(II) Ions in Liquid Ammonia

Solvation of Copper(II) Ions in Liquid Ammonia

Tetraamminecopper Perchlorate (TACP): Explosive Properties

Vapor‐liquid equilibrium in ammonia complex systems

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