Copper sulfate structure

It represents the case of the reaction at the metal electrode in which ions of the same metal discharge at the electrode from the electrolyte. It can be said that copper ions in the electrolyte (copper sulfate solution) possess a free energy GCu(ej, and those in the copper metal electrode possess a free energy Ci(ll(-ril.. Then, if a copper ion is to leave its place in the copper sulfate electrolyte structure and occupy a position in the structure of the copper electrode, the free energy change accompanying this process will be ... 

Roncero, V., E. Duran, F. Soler, J. Masot, and L. Gomez. 1992. Morphometric, structural, and ultrastructural studies of tench (Tinea tinea L.) hepatocytes after copper sulfate administration. Environ. Res. 57 45-58. 

Figure 4.1 Copper sulfate pentaquo complex. In solution, CuS04 exists as a Cu2 + ion in octahedral co-ordination surrounded by the S042- ion and five water molecules orientated so that the oxygen atom points towards the copper ion. It is the effect of this hydration sphere on the electronic orbital structure of the copper which gives rise to d-d band transitions, and hence the blue color of the solution.

FIG. 28. The formation of upd layers often involves complex interactions between the anion, upd metal, and substrate. An example is provided by the (Vs X vVs) R30° STM image of the copper/sulfate upd layer formed on Au(lll) and the SXS of the interfacial structure. (Adapted from Refs. 148, 351, 353.)... 

AFM image of Cu adlayer on Au(lll) in copper perchlorate solution, showing close-packed structure with a rotation to the Au(lll) substrate, (b) Schematic of the incommensurate structure of the Cu adlayer. (c) ( J3 X y/3 )/ 30° structure of the Cu adlayer on Au(lll), in copper sulfate solution, (d) Schematic diagram of that structure. The open circle represents Au atom at the topmost layer, the hatched circle represents the Cu adatom. (Reproduced from Manne et al., 1991a, with permission.)... 

Mercuric-5-nitrotetrazole [Structure (2.13)] was prepared according to the methods reported by Gilligan et al. [14] and Redman and Spear [15]. Thus, 5-aminotetrazole was treated with sodium nitrite and copper sulfate to obtain Cu(NT)2HNT-4H20 (where NT nitrotetrazole). The copper salt was subsequently converted to the ethylene diamine complex MNT was then obtained by treating the complex with mercuric nitrate in HN03 medium. The precursors and final product were air dried. The synthesis of these compounds is carried out in a fume hood behind a protective polycarbonate shield in a stainless steel reaction vessel. 

Copper Complexes of Substantive Azo Dyes Under certain structural conditions, azo dyes are capable of forming metal complexes (see Sections 2.9, 3.11). A process for the complexing of o,o - dihydroxyazo dyes with copper by reaction of these dyes with copper sulfate in a weakly acid solution was described for the first time in 1915 [8],... 

A mixture of 2-chloroadenosine (13 g, 43 mM), 1,3-dichloro-l,1,3,3-tetraisopropyldisiloxane (15 g, 47.6 mM) and pyridine (150 mL) is stirred at room temperature under nitrogen for 3 hours. The solvent volume is reduced in vacuo and the resulting residue is dissolved in CH2CI2 (250 mL), washed with a saturated copper sulfate solution (2x150 mL) and dried with sodium sulfate. The organic layer is concentrated in vacuo and purified by column chromatography on silica gel (200 g) with ethyl acetate/hexane (1 1) to yield the title compound as a white powder (14.7 g, 63%, MP 198-200°C). NMR, IR and elemental analysis are confirmed the structure of the title compound. 

The hydrate contains water as an integral part of the crystalline structure of the compound. When salt crystallizes from an aqueous solution, the number of water molecules bound to the metal ion are characteristic of the metal and are in a definite proportion. Thus when copper sulfate crystallizes from water, the blue salt copper(II) sulfate pentahydrate, CuS04-5H20, forms. As indicated by the formula, 5 waters of hydration are bound to the copper(II) ion in copper sulfate. Notice how the formula is written—the waters of hydration are separated from the formula of the salt by a dot. 

In the course of a study of the condensation of D-ribose with acetone, Levene and his coworkers61 88 found that an anhydroisopropylidene-D-ribose, melting at 93-94°, was obtained when hydrogen chloride was used as a catalyst, while an isomeric compound, melting at 61-62°, resulted when a mixture of sulfuric acid and anhydrous copper sulfate was employed. The structure of neither of these anhydrides has received further attention. 

Water of crystallisation may also be associated with anions (for example, sulfate and oxalate). A good example of such anion water is found in the hydrate of copper sulfate, CuS04 5H20. Four of the five waters are associated with the cation, the fifth with the anion. The sketch of a portion of the structure given below is found in many texts it is quite crude, but conveys the idea well. 

Ores of copper native copper, cuprite, chalcocite, chalcopyrite, malachite, azurite. Metallurgy of ores containing native copper, oxide and carbonate ores, sulfide ores. Gangue, flux, flotation, roasting of ores, matte, blister copper. Cupric compounds copper sulfate (blue vitriol, bluestone), Bordeaux mixture, cupric chloride, cupric bromide, cupric hydroxide. Test for cupric ion with Fehling s solution. Cuprous compounds cuprous chloride, cuprous bromide, cuprous iodide, cuprous oxide. Covalent-bond structure of cuprous compounds. 

Copper sulfate is a beautiful crystalline structure of formula... 

Furthermore Levene and Tipson discovered that uridine will condense with acetone in the presence of sulfuric acid and anhydrous copper sulfate to give a mono-isopropylidene-uridine. On treatment with tosyl chloride it gave a tosyl-isopropylidene-uridine which reacted readily with sodium iodide in acetone to give a crystalline monoiodo-isopropyli-dene-uridine, showing that the tosyl group is at position (5) of the sugar chain. Hence the isopropylidene derivative is 2,3-isopropylidene-uridine with a furanose ring structure, and uridine is D-ribofuranosyl-uracil. 

FIGURE 8.15. (a) Copper sulfate pentahydrate Patterson map with (b) Cu-Cu and Cu S vectors shown, and (c) the crystal structure (Ref. 58). Cu black circles, S open circles, O stippled circles, H atoms omitted for clarity. 

In the biuret test, the sample is treated with an alkaline copper sulfate reagent that produces a violet color and requires a peptide with at least two peptide bonds. The violet color is produced through formation of a coordination complex (between peptide nitrogen atoms and cupric ion) that is analogous to the structure of the complex of biuret with cupric ion, as shown below ... 

A prerequisite for the interpretation of metal precipitations is the term ion and the simple structure of the atom with the atom nucleus and differentiated electron shells. If the ion term has already been introduced as in Chap. 5, then the colors of salt solutions are already known - for instance the light blue color of diluted copper sulfate solutions or of diluted copper chloride solutions. Armed with this information, there are good prerequisites for the problem-oriented interpretation of the following experiments. If an iron nail is dipped into copper sulfate solution, then a copper-colored coating appears on the part that has been dipped (see E8.1). If iron wool is placed in copper sulfate solution, then the solution warms up and the blue color of the solution disappears (see E8.2). 

The third large group of donor-acceptor reactions are the complex reactions. If we consider the bright-blue colored solution of copper sulfate in water and add concentrated hydrochloric acid, the blue color changes to green. The blue solution contains complex ions called hexaaquacopper complexes with the symbol [Cu(H20)6]2+(aq). The structure of the complex shows an octahedron (see Fig. 9.2) the Cu2+ ion is called central ion, 6 H20 molecules are the ligands. Through the reaction with chloride ions the complex releases one water molecule and a chloride ion replaces it in the complex ... 

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