Copper II Compounds

In both cases, the precipitate must be filtered and dried quickly, by washing first with alcohol and then with ether (to prevent formation of the copper(II) compound). 

This copper(I) compound, unlike the above, is soluble in water and therefore in the presence of water liberates copper and forms a copper(II) compound ... 

Cupri-. cupric, copper(II). -azetst, n. cupric acetate, copper(II) acetate, -carbonat, n. cupric carbonate, copper(II) carbonate, -chlorid, n. cupric chloride, copper(II) chloride. -hydroxyd, n. cupric hydroxide, cop-per(II) hydroxide. -ion, n. cupric ion, copper(II) ion. -ozalat, n. cupric oxalate, copper(II) oxalate, -oxyd, n. cupric oxide, copper(II) oxide. -salz, n. cupric salt, copper(II) salt, -suifat, n. cupric sulfate. copper(II) sulfate, -sulfid, n. cupric sulfide, copper(II) sulfide, -verbihdung, /. cupric compound, copper(II) compound, -wein-saure, /. cupritartaric acid. 

Kupfer-oxydverbindung, /. cupric compound, copper(II) compound. -pecherz,n. = Kupferbraun. -platte, /. copper plate, copperplate. 

Copper(II) compounds. Many other metallic ions which are capable of undergoing oxidation by potassium iodate can also be determined. Thus, for example, copper(II) compounds can be analysed by precipitation of copper)I) thiocyanate which is titrated with potassium iodate ... 

Ligand field splittings in copper(II) compounds. D. W. Smith, Struct. Bonding (Berlin), 1972, 12, 49-112 (220). 

Study of the relationship between the structural data and magnetic interaction in cxo-bridged binu-cleaT copper(II) compounds. M. Melnik, Coord. Chem. Rev., 1982,42,259-293 (147). 

Suggest a reason why copper(II) compounds are often colored but copper(I) compounds are colorless. Which oxidation number results in paramagnetic compounds ... 

Smith DW (1972) Ligand Field Splittings in Copper(II) Compounds. 12 49-112... 

RUey MJ (2001) Geometric and Electronic Information From the Spectroscopy of Six-Coordinate Copper(II) Compounds. 214 57-80 Rissanen K, see Nummelin S (2000) 210 1-67... 

The amount of Lewis acid to be used is depicted as an effective amount and a minimum limit of 0.5 mole equivalent with respect to the sulfmated compound concentration was mentioned. A wide variety of Lewis acids was mentioned to be useful for the present invention in the patent document, but only copper (II) compounds were claimed. The way in which the Lewis acid is used (either as a homogeneous or a heterogeneous phase), was reported to be irrelevant. So, it could be employed in solution in the reaction medium or insoluble as powders or on a solid support, such as alumina or a zeolite. The Lewis acid is supposed to be acting as a catalyst in the desulfination process. The temperature and pressure conditions for this reaction are substantially higher than the microbial conditions. The temperature and pressure conditions did not form part of any claim, but the document stipulates values between 50°C and 100°C, and 10 and 15psi, respectively. The quantitative effectiveness or conversion values of this reaction were not given, but it looks like it would diminish the advantages of a biocatalytic process. 

Metal ions play an important role in several of these oxidative reactions as well as in biological dioxygen metabolism. As an example, copper(II) acetate and hydrogen peroxide have been used to produce a stable oxidizing agent, hydroperoxy copper(II) compound. The same oxidation system is also obtained from copper(II) nitrate and hydrogen peroxide (Eq. 1) [103] but requires the neutralization of ensuing nitric acid by potassium bicarbonate to maintain a pH 5. 

Iron(II) salts, usually in conjunction with catalytic amounts of copper(II) compounds, have also been used to mediate radical additions to dienes91,92. Radicals are initially generated in these cases by reductive cleavage of peroxyesters of hydroperoxides to yield, after rearrangement, alkyl radicals. Addition to dienes is then followed by oxidation of the allyl radical and trapping by solvent. Hydroperoxide 67, for example, is reduced by ferrous sulfate to acyclic radical 68, which adds to butadiene to form adduct radical 69. Oxidation of 69 by copper(H) and reaction of the resulting allyl cation 70 with methanol yield product 71 in 61% yield (equation 29). 

The d-d spectra of copper(II) compounds have provided a fruitful field for practitioners of the AOM. A wealth of structural data is available, and a rich variety of coordination geometries has been revealed. If we can make allowance for the dependence of the AOM parameters on the intemuclear distance, we are provided with excellent opportunities to test the validity of AOM parameters over a range of related systems. However, the progress of such studies over the years has illustrated the fact that a simple model may be very successful in explaining a limited amount of dubious experimental data as more crystal structures appear and as better spectroscopic data become available, the simple model may require considerable refurbishment, perhaps to the extent that it loses some of its appeal and utility. 

To date, the organometallic chemistry of copper, in terms of isolation and structural characterization of compounds, is essentially limited to the Cu(I) oxidation state. Only a very few examples of other oxidation states are known. The older literature offers a reported synthetic procedure for the synthesis of bis(aryl)copper(II) compounds [33, 34] (see Scheme 1.2), but this result has never been reproduced by others. 

Riley MJ (2001) Geometric and Electronic Information From the Spectroscopy of Six-Co-ordinate Copper(II) Compounds. 214 57-80 Rissanen K, see Nummelin S (2000) 210 1-67 Roeggen I (1999) Extended Geminal Models. 203 89-103 Rockendorf N, Lindhorst TK (2001) Glycodendrimers. 217 201-238 Roeda D, see Lasne M-C (2002) 222 201-258... 

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