Copper(II) chloride
Copper(II) chloride dihydrate Copper(II) chloride anhydrous Copper(II) chloride is the chemical compound with the chemical formula CuCl2. The anhydrous form is yellowish brown but slowly absorbs moisture to form a blue-green dihydrate. Both the anhydrous and the dihydrate forms occur naturally as the very rare minerals tolbachite and eriochalcite, respectively.[2] Structure[edit]Anhydrous CuCl2 adopts a distorted cadmium iodide structure. In this motif, the copper centers are octahedral. Most copper(II) compounds exhibit distortions from idealized octahedral geometry due to the Jahn-Teller effect, which in this case describes the localization of one d-electron into a molecular orbital that is strongly antibonding with respect to a pair of chloride ligands. In CuCl2·2H2O, the copper again adopts a highly distorted octahedral geometry, the Cu(II) centers being surrounded by two water ligands and four chloride ligands, which bridge asymmetrically to other Cu centers.[3] Copper(II) chloride is paramagnetic. Of historical interest, CuCl2·2H2O was used in the first electron paramagnetic resonance measurements by Yevgeny Zavoisky in 1944.[4][5] Properties and reactions[edit]Aqueous solutions of copper(II) chloride. Greenish when high in [Cl−], more blue when lower in [Cl−]. Aqueous solution prepared from copper(II) chloride contain a range of copper(II) complexes depending on concentration, temperature, and the presence of additional chloride ions. These species include blue color of [Cu(H2O)6]2+ and yellow or red color of the halide complexes of the formula [CuCl2+x]x−.[6] Hydrolysis[edit]Copper(II) hydroxide precipitates upon treating copper(II) chloride solutions with base: CuCl2 + 2 NaOH → Cu(OH)2 + 2 NaClPartial hydrolysis gives dicopper chloride trihydroxide, Cu2(OH)3Cl, a popular fungicide. Redox[edit]Copper(II) chloride is a mild oxidant. It decomposes to copper(I) chloride and chlorine gas near 1000 °C: 2 CuCl2 → 2 CuCl + Cl2Copper(II) chloride (CuCl2) reacts with several metals to produce copper metal or copper(I) chloride (CuCl) with oxidation of the other metal. To convert copper(II) chloride to copper(I) chloride, it can be convenient to reduce an aqueous solution with sulfur dioxide as the reductant: 2 CuCl2 + SO2 + 2 H2O → 2 CuCl + 2 HCl + H2SO4Coordination complexes[edit]CuCl2 reacts with HCl or other chloride sources to form complex ions: the red CuCl3− (it is a dimer in reality, Cu2Cl62−, a couple of tetrahedrons that share an edge), and the green or yellow CuCl42−.[7] 2 + Cl− ⇌ CuCl− 3CuCl 2 + 2 Cl− ⇌ CuCl2− 4 Some of these complexes can be crystallized from aqueous solution, and they adopt a wide variety of structures. Copper(II) chloride also forms a variety of coordination complexes with ligands such as ammonia, pyridine and triphenylphosphine oxide: CuCl2 + 2 C5H5N → [CuCl2(C5H5N)2] (tetragonal)CuCl2 + 2 (C6H5)3PO → [CuCl2((C6H5)3PO)2] (tetrahedral)However "soft" ligands such as phosphines (e.g., triphenylphosphine), iodide, and cyanide as well as some tertiary amines induce reduction to give copper(I) complexes. Preparation[edit]Copper(II) chloride is prepared commercially by the action of chlorination of copper. Copper at red heat (300-400°C) combines directly with chlorine gas, giving (molten) copper (II) chloride. The reaction is very exothermic. Cu(s) + Cl2(g) → CuCl2(l)It is also commercially practical to combine copper(II) oxide with an excess of ammonium chloride at similar temperatures, producing copper chloride, ammonia, and water:[citation needed] CuO + 2NH4Cl → CuCl2 + 2NH3 + H2OAlthough copper metal itself cannot be oxidised by hydrochloric acid, copper-containing bases such as the hydroxide, oxide, or copper(II) carbonate can react to form CuCl2 in an acid-base reaction. Once prepared, a solution of CuCl2 may be purified by crystallization. A standard method takes the solution mixed in hot dilute hydrochloric acid, and causes the crystals to form by cooling in a Calcium chloride (CaCl2)-ice bath.[8][9] There are indirect and rarely used means of using copper ions in solution to form copper(II) chloride. Electrolysis of aqueous sodium chloride with copper electrodes produces (among other things) a blue-green foam that can be collected and converted to the hydrate. While this is not usually done due to the emission of toxic chlorine gas, and the prevalence of the more general chloralkali process, the electrolysis will convert the copper metal to copper ions in solution forming the compound. Indeed, any solution of copper ions can be mixed with hydrochloric acid and made into a copper chloride by removing any other ions. Natural occurrence[edit]Copper(II) chloride occurs naturally as the very rare anhydrous mineral tolbachite and the dihydrate eriochalcite.[2] Both are found near fumaroles and in some Cu mines.[10][11][12] More common are mixed oxyhydroxide-chlorides like atacamite Cu2(OH)3Cl, arising among Cu ore beds oxidation zones in arid climate (also known from some altered slags). Uses[edit]In organic synthesis[edit]Co-catalyst in Wacker process[edit]A major industrial application for copper(II) chloride is as a co-catalyst with palladium(II) chloride in the Wacker process. In this process, ethene (ethylene) is converted to ethanal (acetaldehyde) using water and air. During the reaction, PdCl2 is reduced to Pd, and the CuCl2 serves to re-oxidize this back to PdCl2. Air can then oxidize the resultant CuCl back to CuCl2, completing the cycle.
The overall process is: 2 C2H4 + O2 → 2 CH3CHOOther organic synthetic applications[edit]Copper(II) chloride has some highly specialized applications in the synthesis of organic compounds.[8] It affects chlorination of aromatic hydrocarbons—this is often performed in the presence of aluminium oxide. It is able to chlorinate the alpha position of carbonyl compounds:[13] This reaction is performed in a polar solvent such as dimethylformamide (DMF), often in the presence of lithium chloride, which accelerates the reaction. CuCl2, in the presence of oxygen, can also oxidize phenols. The major product can be directed to give either a quinone or a coupled product from oxidative dimerization. The latter process provides a high-yield route to 1,1-binaphthol:[14] Such compounds are intermediates in the synthesis of BINAP and its derivatives. Copper(II) chloride dihydrate promotes the hydrolysis of acetonides, i.e., for deprotection to regenerate diols[15] or aminoalcohols, as in this example (where TBDPS = tert-butyldiphenylsilyl):[16] CuCl2 also catalyses the free radical addition of sulfonyl chlorides to alkenes; the alpha-chlorosulfone may then undergo elimination with base to give a vinyl sulfone product.[citation needed] In inorganic synthesis[edit]Catalyst in production of chlorine[edit]Copper(II) chloride is used as a catalyst in a variety of processes that produce chlorine by oxychlorination. The Deacon process takes place at about 400 to 450 °C in the presence of a copper chloride: 4 HCl + O2 → 2 Cl2 + 2 H2OCopper(II) chloride catalyzes the chlorination in the production of vinyl chloride and dichloroethane.[17] Copper(II) chloride is used in the Copper–chlorine cycle in which it splits steam into a copper oxygen compound and hydrogen chloride, and is later recovered in the cycle from the electrolysis of copper(I) chloride. Niche uses[edit]Copper(II) chloride is also used in pyrotechnics as a blue/green coloring agent. In a flame test, copper chlorides, like all copper compounds, emit green-blue. In humidity indicator cards (HICs), cobalt-free brown to azure (copper(II) chloride base) HICs can be found on the market. In 1998, the European Community (EC) classified items containing cobalt(II) chloride of 0.01 to 1% w/w as T (Toxic), with the corresponding R phrase of R49 (may cause cancer if inhaled). As a consequence, new cobalt-free humidity indicator cards have been developed that contain copper. Safety[edit]
Copper(II) chloride can be toxic. Only concentrations below 5 ppm are allowed in drinking water by the US Environmental Protection Agency.[citation needed] References[edit]
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Is copper chloride insoluble or soluble?Copper(I) chloride, commonly called cuprous chloride, is the lower chloride of copper, with the formula CuCl. The substance is a white solid sparingly soluble in water, but very soluble in concentrated hydrochloric acid.
Is CuCl2 soluble or insoluble in water?CuCl2 completely ionises in water hence it is completely soluble in water.
Why does copper chloride dissolve in water?Since water molecules have slightly positive hydrogens and slightly negative oxygens, the positive part of copper chloride is attracted to the oxygen in water and the negative part of copper chloride is attracted to the hydrogens in water. So it's ionic because of its ability to dissolve in water.
Is CuCl2 aqueous or solid?Copper (II) is the chemical compound that contains the chemical formula CuCl2. It is a light brown solid, gradually absorbing moisture to form a green-blue dihydrate.
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