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Copper Chloride

Copper(II) chloride is the chemical compound with the formula CuCl2. This a yellow-brown solid which slowly absorbs moisture to form a blue-green dihydrate.

- Copper Dichloride
- Copper Monochloride
- Cuprous Dichloride
- Cuprous Monochloride
- Cupric Dichloride
- Cupric Monochloride
- Copper Bichloride
- Cuprous Chloride
- Cuprous Bichloride
- Cupric Chloride
- Cupric Bichloride


  Copper Dichloride

Anhydrous cucl2 adopts a distorted cadmium iodide structure. Most copper(ii) compounds exhibit distortions from idealized octahedral geometry due to the jahn-teller effect, which in this case describes the localisation of one d-electron into a molecular orbital that is strongly antibonding with respect to a pair of ligands. In cucl2(h2o)2 the copper can be described as a highly distorted octahedral complex, the cu(ii) center being surrounded by two water ligands and four chloride ligands, which bridge asymmetrically to other cu centers.


  Copper Bichloride

Anhydrous cucl2 adopts a distorted cadmium iodide structure. Most copper(ii) compounds exhibit distortions from idealized octahedral geometry due to the jahn-teller effect, which in this case describes the localisation of one d-electron into a molecular orbital that is strongly antibonding with respect to a pair of ligands. In cucl2(h2o)2 the copper can be described as a highly distorted octahedral complex, the cu(ii) center being surrounded by two water ligands and four chloride ligands, which bridge asymmetrically to other cu centers.


  Copper Monochloride

Anhydrous CuCl2 adopts a distorted cadmium iodide structure. Most copper(II) compounds exhibit distortions from idealized octahedral geometry due to the Jahn-Teller effect, which in this case describes the localisation of one d-electron into a molecular orbital that is strongly antibonding with respect to a pair of ligands. In CuCl2(H2O)2 the copper can be described as a highly distorted octahedral complex, the Cu(II) center being surrounded by two water ligands and four chloride ligands, which bridge asymmetrically to other Cu centers.



  Cuprous Chloride

Copper(II) chloride dissociates in aqueous solution to give the blue color of [Cu(H2O)6]2+ and yellow or red color of the halide complexes of the formula [CuCl2+x]x-. Concentrated solutions of CuCl2 appear green because of the combination of these various chromophores. The color of the dilute solution depends on temperature, being green around 100 °C and blue at room temperature.[2] When copper(II) chloride is heated in a flame, it emits a green-blue color.



  Cuprous Dichloride

Copper(II) chloride dissociates in aqueous solution to give the blue color of [Cu(H2O)6]2+ and yellow or red color of the halide complexes of the formula [CuCl2+x]x-. Concentrated solutions of CuCl2 appear green because of the combination of these various chromophores. The color of the dilute solution depends on temperature, being green around 100 °C and blue at room temperature.[2] When copper(II) chloride is heated in a flame, it emits a green-blue colour.



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