![]() ![]() ![]() Īqueous solutions prepared from copper(II) chloride contain a range of copper(II) complexes depending on concentration, temperature, and the presence of additional chloride ions. Greenish when high in, more blue when lower in. Properties and reactions Aqueous solutions of copper(II) chloride. Of historical interest, CuCl 2♲H 2O was used in the first electron paramagnetic resonance measurements by Yevgeny Zavoisky in 1944. In CuCl 2♲H 2O, 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. 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 this motif, the copper centers are octahedral. Structure Structure of copper(II) chloride dihydrateĪnhydrous CuCl 2 adopts a distorted cadmium iodide structure. It is industrially produced for use as a co-catalyst in the Wacker process.īoth the anhydrous and the dihydrate forms occur naturally as the rare minerals tolbachite and eriochalcite, respectively. The monoclinic yellowish-brown anhydrous form slowly absorbs moisture to form the orthorhombic blue-green dihydrate CuCl 2♲H 2O, with two water molecules of hydration. Copper(II) chloride, also known as cupric chloride, is an inorganic compound with the chemical formula CuCl 2. ![]()
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