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DESCRIPTION:
Copper chloride appears as a yellowish-brown powder (the anhydrous form) or a green crystalline solid (the dihydrate).
Noncombustible but hydrogen chloride gas may form when heated in a fire.
Copper Chloride is Corrosive to aluminum.
Copper Chloride is Used to manufacture other chemicals, in dyeing, in printing, in fungicides, as a wood preservative.
CAS 1344-67-8
European Community (EC) Number 231-210-2
SYNONYMS
copper(II) chloride,CuCl2,cupric chloride,cupric chloride anhydrous,cupric chloride dihydrate,cupric chloride eriochalcite (CuCl2.2H2O),cupric chloride, 64Cu-labeled cpd,cupric chloride, dihydrate 2H-labeled cpd,CUPRIC CHLORIDE,Copper chloride,Cupric chloride anhydrous,Copper dichloride,Copper bichloride,Copper(2+) chloride,Cupric dichloride,dichlorocopper,CuCl2,Copper chloride,(CuCl2),Copper(2+)chloride,COPPER (II) CHLORIDE,Copper(II) chloride (1:2),Coclor,Copper(II)chloride,CCRIS 6883,HSDB 259,Copper(II) chloride, anhydrous,CHEBI:49553,Cupric chloride in plastic container,EINECS 231-210-2,NSC,AI3-01658,UNII-P484053J2Y,NSC165706,NSC-165706,P484053J2Y,EC 231-210-2,Copper chloride (VAN),copper (II)chloride,copper(II)-chloride,copper (II) cloride,copper (II)-chloride,Epitope ID:156811,Copper (as cupric chloride),Copper(II) chloride, 97%,Copper (II) chloride, 95%,Copper(II) chloride, ultra dry,Copper(II) chloride, powder, 99%,Copper(II) chloride, p.a., 97%,Copper(II) chloride, LR, >=98%,AKOS015902778,DB09131,BP-13443,NCI60_001274,Copper (II) Chloride, Trace metals grade,Copper(II) chloride, SAJ first grade, >=98.0%,Q421781,Copper(II) chloride, 99.999% trace metals basis,Copper(II) chloride, anhydrous, powder, >=99.995% trace metals basis,Copper (II) chloride, ultra dry, powder, ampoule, 99.995% trace metals grade
Copper(II) chloride is an inorganic chloride of copper in which the metal is in the +2 oxidation state.
Copper Chloride has a role as an EC 5.3.3.5 (cholestenol Delta-isomerase) inhibitor.
Copper Chloride is an inorganic chloride and a copper molecular entity.
Copper Chloride contains a copper(2+).
Cupric chloride, for injection, is a sterile, nonpyrogenic solution intended for use as an additive to solutions for Total Parenteral Nutrition (TPN).
Copper(II) chloride, also known as cupric chloride, is an inorganic compound with the chemical formula CuCl2.
The monoclinic yellowish-brown anhydrous form slowly absorbs moisture to form the orthorhombic blue-green dihydrate CuCl2•2H2O, with two water molecules of hydration.
It is industrially produced for use as a co-catalyst in the Wacker process.
Both the anhydrous and the dihydrate forms occur naturally as the rare minerals tolbachite and eriochalcite, respectively.
Structure
Structure of copper(II) chloride dihydrate
Copper, Cu
Oxygen, O
Chlorine, Cl
Hydrogen, H
Anhydrous copper(II) chloride adopts a distorted cadmium iodide structure.
In this structure, 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.[4][5]
Copper(II) chloride is paramagnetic. Of historical interest, CuCl2•2H2O was used in the first electron paramagnetic resonance measurements by Yevgeny Zavoisky in 1944.[6][7]
PROPERTIES AND REACTIONS
Aqueous solutions of copper(II) chloride. Greenish when high in Cl−, more blue when lower in Cl−.
Aqueous solutions 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 the blue color of [Cu(H2O)6]2+ and the yellow or red color of the halide complexes of the formula [CuCl2+x]x−.[5]
Hydrolysis
When copper(II) chloride solutions are treated with a base, a precipitation of copper(II) hydroxide occurs:[8]
CuCl2 + 2 NaOH → Cu(OH)2 + 2 NaCl
Partial hydrolysis gives dicopper chloride trihydroxide, Cu2(OH)3Cl, a popular fungicide.[8]
When an aqueous solution of copper(II) chloride is left in the air and isn't stabilized by a small amount of acid, it is prone to undergo slight hydrolysis.[5]
Redox and decomposition
Copper(II) chloride is a mild oxidant.
It starts to decompose to copper(I) chloride and chlorine gas around 400 °C (752 °F) and is completely decomposed near 1,000 °C (1,830 °F):
2 CuCl2 → 2 CuCl + Cl2
The reported melting point of copper(II) chloride of 498 °C (928 °F) is a melt of a mixture of copper(I) chloride and copper(II) chloride.
The true melting point of 630 °C (1,166 °F) can be extrapolated by using the melting points of the mixtures of CuCl and CuCl2.[12][13]
Copper(II) chloride 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:[8]
2 CuCl2 + SO2 + 2 H2O → 2 CuCl + 2 HCl + H2SO4
Coordination complexes
CuCl2 reacts with HCl or other chloride sources to form complex ions: the red [CuCl3]− (found in potassium trichloridocuprate(II) K[CuCl3]) (it is a dimer in reality, [Cu2Cl6]2−, a couple of tetrahedrons that share an edge), and the green or yellow [CuCl4]2− (found in potassium tetrachloridocuprate(II) K2[CuCl4]).[5][14][15]
CuCl2 + Cl− ⇌ [CuCl3]−
CuCl2 + 2 Cl− ⇌ [CuCl4]2−
Some of these complexes can be crystallized from aqueous solution, and they adopt a wide variety of structures.[14]
Copper(II) chloride also forms a variety of coordination complexes with ligands such as ammonia, pyridine and triphenylphosphine oxide:[8][5][16]
CuCl2 + 2 C5H5N → [CuCl2(C5H5N)2] (tetragonal)
CuCl2 + 2 (C6H5)3P=O → [CuCl2((C6H5)3P=O)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.[5]
Preparation
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.[8][15]
Cu(s) + Cl2(g) → CuCl2(l)
A solution of copper(II) chloride is commercially produced by adding chlorine gas to a circulating mixture of hydrochloric acid and copper.
From this solution, the dihydrate can be produced by evaporation.[8][10]
Although copper metal itself cannot be oxidized 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 which can subsequently be heated above 100 °C (212 °F) to produce the anhydrous derivative.[8][10]
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.[17][18]
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.[19]
USES
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 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.[20]
C2H4 + PdCl2 + H2O → CH3CHO + Pd + 2 HCl
Pd + 2 CuCl2 → 2 CuCl + PdCl2
4 CuCl + 4 HCl + O2 → 4 CuCl2 + 2 H2O
The overall process is:[20]
2 C2H4 + O2 → 2 CH3CHO
In organic synthesis
Copper(II) chloride has some highly specialized applications in the synthesis of organic compounds.[17]
It affects the 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:[20][21]
This reaction is performed in a polar solvent such as dimethylformamide, often in the presence of lithium chloride, which accelerates the reaction.[20]
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:[22]
Such compounds are intermediates in the synthesis of BINAP and its derivatives.[20]
Copper(II) chloride dihydrate promotes the hydrolysis of acetonides, i.e., for deprotection to regenerate diols[23] or aminoalcohols, as in this example (where TBDPS = tert-butyldiphenylsilyl):[24]
CuCl2 also catalyses the free radical addition of sulfonyl chlorides to alkenes; the alpha-chlorosulfone may then undergo elimination with a base to give a vinyl sulfone product.[20]
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:[8]
4 HCl + O2 → 2 Cl2 + 2 H2O
Copper(II) chloride catalyzes the chlorination in the production of vinyl chloride and dichloromethane.[8]
Copper(II) chloride is used in the copper–chlorine cycle where it reacts with steam into copper(II) oxide dichloride and hydrogen chloride and is later recovered in the cycle from the electrolysis of copper(I) chloride.[11]
Niche uses
Copper(II) chloride is used in pyrotechnics as a blue/green coloring agent. In a flame test, copper chlorides, like all copper compounds, emit green-blue light.[25]
In humidity indicator cards (HICs), cobalt-free brown to azure (copper(II) chloride base) HICs can be found on the market.[26]
In 1998, the European Community 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).
Consequently, new cobalt-free humidity indicator cards containing copper have been developed.[27]
Copper(II) chloride is used as a mordant in the textile industry, petroleum sweetener, wood preservative, and water cleaner.[8][28]
Natural occurrence
Eriochalcite
Copper(II) chloride occurs naturally as the very rare anhydrous mineral tolbachite and the dihydrate eriochalcite.[29]
Both are found near fumaroles and in some copper mines.[30][31][32]
Mixed oxyhydroxide-chlorides like atacamite (Cu2(OH)3Cl) are more common, arising among Cu ore beds oxidation zones in arid climates.
CHEMICAL AND PHYSICAL PROPERTIES
Molecular Weight
134.45 g/mol
Computed by PubChem 2.2 (PubChem release 2021.10.14)
Hydrogen Bond Donor Count
0
Computed by Cactvs 3.4.8.18 (PubChem release 2021.10.14)
Hydrogen Bond Acceptor Count
0
Computed by Cactvs 3.4.8.18 (PubChem release 2021.10.14)
Rotatable Bond Count
0
Computed by Cactvs 3.4.8.18 (PubChem release 2021.10.14)
Exact Mass
132.867303 g/mol
Computed by PubChem 2.2 (PubChem release 2021.10.14)
Monoisotopic Mass
132.867303 g/mol
Computed by PubChem 2.2 (PubChem release 2021.10.14)
Topological Polar Surface Area
0Ų
Computed by Cactvs 3.4.8.18 (PubChem release 2021.10.14)
Heavy Atom Count
3
Computed by PubChem
Formal Charge
0
Computed by PubChem
Complexity
2.8
Computed by Cactvs 3.4.8.18 (PubChem release 2021.10.14)
Isotope Atom Count
0
Computed by PubChem
Defined Atom Stereocenter Count
0
Computed by PubChem
Undefined Atom Stereocenter Count
0
Computed by PubChem
Defined Bond Stereocenter Count
0
Computed by PubChem
Undefined Bond Stereocenter Count
0
Computed by PubChem
Covalently-Bonded Unit Count
1
Computed by PubChem
Compound Is Canonicalized
Yes
Chemical formula CuCl2
Molar mass 134.45 g/mol (anhydrous)
170.48 g/mol (dihydrate)
Appearance dark brown solid (anhydrous)
light blue solid (dihydrate)
Odor odorless
Density 3.386 g/cm3 (anhydrous)
2.51 g/cm3 (dihydrate)
Melting point 630 °C (1,166 °F; 903 K) (extrapolated)
100 °C (dehydration of dihydrate)
Boiling point 993 °C (1,819 °F; 1,266 K) (anhydrous, decomposes)
Solubility in water 70.6 g/(100 mL) (0 °C)
75.7 g/(100 mL) (25 °C)
107.9 g/(100 mL) (100 °C)
Solubility methanol:
68 g/(100 mL) (15 °C)
ethanol:
53 g/(100 mL) (15 °C)
soluble in acetone
Magnetic susceptibility (χ) +1080•10−6 cm3/mol
Structure[1][2]
Crystal structure monoclinic (β = 121°) (anhydrous)
orthorhombic (dihydrate)
Space group C2/m (anhydrous)
Pbmn (dihydrate)
Lattice constant
a = 6.85 Å (anhydrous)
7.41 Å (dihydrate), b = 3.30 Å (anhydrous)
8.09 Å (dihydrate), c = 6.70 Å (anhydrous)
3.75 Å (dihydrate)
Coordination geometry Octahedral
SAFETY INFORMATION ABOUT COPPER CHLORIDE
First aid measures:
Description of first aid measures:
General advice:
Consult a physician.
Show this safety data sheet to the doctor in attendance.
Move out of dangerous area:
If inhaled:
If breathed in, move person into fresh air.
If not breathing, give artificial respiration.
Consult a physician.
In case of skin contact:
Take off contaminated clothing and shoes immediately.
Wash off with soap and plenty of water.
Consult a physician.
In case of eye contact:
Rinse thoroughly with plenty of water for at least 15 minutes and consult a physician.
Continue rinsing eyes during transport to hospital.
If swallowed:
Do NOT induce vomiting.
Never give anything by mouth to an unconscious person.
Rinse mouth with water.
Consult a physician.
Firefighting measures:
Extinguishing media:
Suitable extinguishing media:
Use water spray, alcohol-resistant foam, dry chemical or carbon dioxide.
Special hazards arising from the substance or mixture
Carbon oxides, Nitrogen oxides (NOx), Hydrogen chloride gas
Advice for firefighters:
Wear self-contained breathing apparatus for firefighting if necessary.
Accidental release measures:
Personal precautions, protective equipment and emergency procedures
Use personal protective equipment.
Avoid breathing vapours, mist or gas.
Evacuate personnel to safe areas.
Environmental precautions:
Prevent further leakage or spillage if safe to do so.
Do not let product enter drains.
Discharge into the environment must be avoided.
Methods and materials for containment and cleaning up:
Soak up with inert absorbent material and dispose of as hazardous waste.
Keep in suitable, closed containers for disposal.
Handling and storage:
Precautions for safe handling:
Avoid inhalation of vapour or mist.
Conditions for safe storage, including any incompatibilities:
Keep container tightly closed in a dry and well-ventilated place.
Containers which are opened must be carefully resealed and kept upright to prevent leakage.
Storage class (TRGS 510): 8A: Combustible, corrosive hazardous materials
Exposure controls/personal protection:
Control parameters:
Components with workplace control parameters
Contains no substances with occupational exposure limit values.
Exposure controls:
Appropriate engineering controls:
Handle in accordance with good industrial hygiene and safety practice.
Wash hands before breaks and at the end of workday.
Personal protective equipment:
Eye/face protection:
Tightly fitting safety goggles.
Faceshield (8-inch minimum).
Use equipment for eye protection tested and approved under appropriate government standards such as NIOSH (US) or EN 166(EU).
Skin protection:
Handle with gloves.
Gloves must be inspected prior to use.
Use proper glove
removal technique (without touching glove's outer surface) to avoid skin contact with this product.
Dispose of contaminated gloves after use in accordance with applicable laws and good laboratory practices.
Wash and dry hands.
Full contact:
Material: Nitrile rubber
Minimum layer thickness: 0.11 mm
Break through time: 480 min
Material tested:Dermatril (KCL 740 / Aldrich Z677272, Size M)
Splash contact
Material: Nitrile rubber
Minimum layer thickness: 0.11 mm
Break through time: 480 min
Material tested:Dermatril (KCL 740 / Aldrich Z677272, Size M)
It should not be construed as offering an approval for any specific use scenario.
Body Protection:
Complete suit protecting against chemicals, The type of protective equipment must be selected according to the concentration and amount of the dangerous substance at the specific workplace.
Respiratory protection:
Where risk assessment shows air-purifying respirators are appropriate use a fullface respirator with multi-purpose combination (US) or type ABEK (EN 14387) respirator cartridges as a backup to engineering controls.
If the respirator is the sole means of protection, use a full-face supplied air respirator.
Use respirators and components tested and approved under appropriate government standards such as NIOSH (US) or CEN (EU).
Control of environmental exposure
Prevent further leakage or spillage if safe to do so.
Do not let product enter drains.
Discharge into the environment must be avoided.
Stability and reactivity:
Chemical stability:
Stable under recommended storage conditions.
Incompatible materials:
Strong oxidizing agents:
Hazardous decomposition products:
Hazardous decomposition products formed under fire conditions.
Carbon oxides, Nitrogen oxides (NOx), Hydrogen chloride gas.
Disposal considerations:
Waste treatment methods:
Product:
Offer surplus and non-recyclable solutions to a licensed disposal company.
Contact a licensed professional waste disposal service to dispose of this material.
Contaminated packaging:
Dispose of as unused product.
