Copper chloride is a brownish-yellow powder.
white or pale grey powder
White cubic crystal which turns blue when heated at 178°C; density 4.14 g/cm3; the mineral nantokite (CuCl) has density 4.14 g/cm3, hardness 2.5 (Mohs), refractive index 1.930; melts at 430°C becoming a deep, green liquid; vaporizes around 1,400°C; vapor pressure 5 torr at 645°C and 400 torr at 1250°C; low solubility in water (decomposes partially); Ksp 1.72x10-7; insoluble in ethanol and acetone; soluble in concentrated HCl and ammonium hydroxide.The space lattice of CuCl belongs to the cubic system, and its zinc-blende structure has a lattice
constant of a=0.541 nm and Cu–Cl=0.235 nm below 407°C, and it belongs to the hexagonal
system and has a wurtzite structure at 407°C–422°C.
The reflection peaks at room temperature are positioned at λ: 58 and 65.4 mm. The transmission
peak is located at λ: 18.5 mm. The absorption spectrum near the absorption edge λ: 370.0 nm at liquid He temperature shows
many structures because of exciton absorption.
It is used for absorption of carbon monoxide in gas analysis. Cuprous chloride is used as a light modulator for λ: 0.43–2.5 mm.
As catalyst for organic reactions; catalyst, decolorizer and desulfuring agent in petroleum industry; in denitration of cellulose; as condensing agent for soaps, fats and oils; in gas analysis to absorb carbon monoxide.
Copper chloride is also known as cupric chloride, this substance was made
by treating copper carbonate with hydrochloric acid. The
greenish blue crystals are soluble in water, alcohol, and ether.
This halide was added to printing-out and silver bromide
emulsions for increased contrast.
Shows unique character as an initiator of radical reactions such as the hydrostannation of α,β-unsaturated ketones.1
Copper(I) chloride (CuCl) or cuprous chloride is a white powder used as an absorbing agent
for carbon dioxide gas in enclosed breathing areas such as space vehicles.
ChEBI: An inorganic chloride of copper in which the metal is in the +1 oxidation state.
Copper(I) chloride is prepared by reduction of copper(II) chloride in solution: 2CuCl2 + H2 2CuCl + 2HCl Alternatively, it can be prepared by boiling an acidic solution of copper(II) chloride with copper metal, which on dilution yields white CuCl: Cu + CuCl2 2CuCl Copper(I) chloride dissolved in concentrated HCl absorbs carbon monoxide under pressure forming an adduct, CuCl(CO). The complex decomposes on heating releasing CO. Copper(I) chloride is slightly soluble in water. However, in the presence of Cl- ion, it forms soluble complexes of discrete halogeno anions such as, CuCl2-, CuCl3 2-, and CuCl4 3-. Formation of complexes and organocopper derivatives as outlined below are not confined only to copper(I) chloride, but typify Cu+ in general. Reaction with ethylenediamine (en) in aqueous potassium chloride solution forms Cu(II)-ethylenediamine complex, while Cu+ ion is reduced to its metallic state: 2CuCl + 2en → [Cuen2]2+ + 2Cl- + Cu° It dissolves in acetonitrile, CH3CN forming tetrahedral complex ion [Cu(CH3CN)4]+ which can be precipitated with large anions such as ClO4 - or PF6- . Reactions with alkoxides of alkali metals produce yellow copper(I) alkoxides. For example, reaction with sodium ethoxide yield copper(I) ethoxide, a yellow compound that can be sublimed from the product mixture: CuCl + NaOC2H5 → CuOC2H5 + NaCl Copper(I) chloride forms complexes with ethylene and other alkenes in solutions that may have compositions such as [Cu(C2H4)(H2O)2]+ or [Cu(C2H4)(bipy)]+. (bipy = bipyridyl) Reactions with lithium or Grignard reagent yield alkyl or aryl copper(I) derivatives, respectively. Such organocopper compounds containing Cu-Cu bonds are formed only by Cu+ and not Cu2+ ions.
Cuprous chloride crystal is grown by direct deposition on the substrate from vapor (vapor phase
growth). Small, zinc-blende crystals without deformation can be obtained from solution.
Large single crystals are grown by the Czochralski method. The first grown crystal takes a
wurtzite structure, which changes to a zinc-blende structure below 407℃. It is inevitable to keep a
constant strain.
Cuprous chloride is soluble in water and ethyl alcohol is used for cutting and polishing.
The structure of copper(I) chloride is similar to zinc-blende crystal at room temperature; the structure is wurtzite at 407 °C and at higher temperatures it forms copper(I) chloride vapor as per mass spectroscopy.
Copper(I) chloride is moderately toxic by ingestion and possibly other routes of entry into the body. The oral LD50 in mouse is reported to be 347 mg/kg; and subcutaneous LD50 in guinea pigs is 100 mg/kg.
UN2802 Copper chloride, Hazard class: 8; Labels: 8-Corrosive material.
Wash the solid with ethanol and diethyl ether, then dry it and store it in a vacuum desiccator [.sterl.f Acta Chem Scand 4 375 1950]. Alternatively, to an aqueous solution of CuCl2.2H2O is added, with stirring, an aqueous solution of anhydrous sodium sulfite. The colourless product is dried at 80o for 30minutes and stored under N2. Cu2Cl2 can be purified by zone-refining [Hall et al. J Chem Soc, Faraday Trans 1 79 343 1983]. [Glemser & Sauer in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol II p 1005 1965.]
Contact with strong acids forms monovalent copper salts and toxic hydrogen chloride gas. Forms shock-sensitive and explosive compounds with potassium, sodium, sodium hypobromite, nitromethane, acetylene. Keep away from moisture and alkali metals. Attacks metals in the presence of moisture. Reacts with moist air to form cupric chloride dihydrate. May attack some metals, paints, and coatings. May be able to ignite combustible materials.
