Copper (I) chloride
Crystal structure | ||||||||||||||||
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__ Cu + __ Cl - | ||||||||||||||||
General | ||||||||||||||||
Surname | Copper (I) chloride | |||||||||||||||
Ratio formula | CuCl | |||||||||||||||
Brief description |
white crystal powder |
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External identifiers / databases | ||||||||||||||||
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properties | ||||||||||||||||
Molar mass | 99.00 g mol −1 | |||||||||||||||
Physical state |
firmly |
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density |
4.14 g cm −3 |
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Melting point |
430 ° C |
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boiling point |
1490 ° C (decomposition) |
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Vapor pressure |
0.1 hPa (440 ° C) |
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solubility | ||||||||||||||||
Refractive index |
1.9727 |
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safety instructions | ||||||||||||||||
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MAK |
0.1 mg m −3 |
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Toxicological data | ||||||||||||||||
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . Refractive index: Na-D line , 20 ° C |
Copper (I) chloride is a chemical compound of copper and chlorine with the formula CuCl. It is a Lewis acid . Copper (I) chloride crystallizes in the sphalerite structure.
Occurrence
Copper (I) chloride occurs naturally as the mineral nantokit .
Extraction and presentation
Copper (I) chloride can be obtained by reduction of copper (II) sulfate with sodium metabisulfite in half-concentrated hydrochloric acid are produced. Further production options are the reduction of copper (II) chloride with electrolytic copper in boiling hydrochloric acid or with zinc , hypophosphorous acid , hydrazine or sodium sulfite
as well as by precipitation from sodium chloride- containing copper sulfate solution by means of sulfur dioxide passed through .
Alternatively, copper (I) chloride is formed when copper (II) chloride is heated with metallic copper in concentrated hydrochloric acid as the complex acid H [CuCl 2 ]. When the solution is diluted, it decomposes with the elimination of hydrochloric acid and the formation of a white, poorly soluble precipitate of CuCl.
On an industrial scale, it is obtained by reacting copper with chlorine at temperatures between 450 and 900 ° C.
properties
Pure copper (I) chloride is snow-white, but often greenish in color due to oxidation to basic copper (II) chloride Cu (OH) Cl.
A solution of copper (I) chloride in ammonia is able to absorb carbon monoxide with the formation of the complex compound [CuCl (CO) (H 2 O) 2 ]. In addition to ammonia, acetylene and olefins also form corresponding complex compounds. It has a crystal structure of the zinc blende type with the space group F 4 3 m (space group no. 216) (a = 541.6 pm). At 407 ° C there is a transition to a high-temperature modification of the wurtzite type with the space group P 6 3 mc (No. 186) (a = 391, c = 642 pm). The enthalpy of formation is −138.1 kJ / mol.
use
Copper (I) chloride is used:
- as a catalyst for many organic reactions ( MCS synthesis )
- for phosgene-free polycarbonate production
- in the Sandmeyer reaction
- in olefin oxidation
- in ammoxidation to acrylonitrile
- for the production of phthalocyanine blue pigments
- for the absorption of carbon monoxide in a gas burette
Web links
- OECD : Screening Information Dataset (SIDS) Initial Assessment Report (SIAR) for Copper monochloride
Individual evidence
- ↑ a b Georg Brauer (Ed.), With the collaboration of Marianne Baudler u a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume II, Ferdinand Enke, Stuttgart 1978, ISBN 3-432-87813-3 , p. 973.
- ↑ a b c d e f g h i Entry on copper (I) chloride in the GESTIS substance database of the IFA , accessed on February 1, 2016(JavaScript required) .
- ↑ a b c d e H. Wayne Richardson: Handbook of copper compounds and applications , ISBN 978-0-8247-8998-5 .
- ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Index of Refraction of Inorganic Crystals, pp. 10-246.
- ↑ Entry on Copper chloride in the Classification and Labeling Inventory of the European Chemicals Agency (ECHA), accessed on February 1, 2016. Manufacturers or distributors can expand the harmonized classification and labeling .
- ↑ Cotton / Wilkinson: Inorganische Chemie, Verlag Chemie Weinheim 1967, p. 837.