Copper(II) chloride

Anhydrous

Anhydrous

Dihydrate

Names
Other names

Cupric chloride

Identifiers

CAS Number

* 7447-39-4 Y
* 10125-13-0 (dihydrate) Y

3D model (JSmol)

* Interactive image
* Interactive image

Beilstein Reference

| 8128168
ChEBI |

* CHEBI:49553 Y

ChEMBL |

* ChEMBL1200553 Y

ChemSpider |

* 148374 Y

DrugBank |

* DB09131

EC Number |

* 231-210-2

Gmelin Reference

| 9300

PubChem CID

* 24014

RTECS number |

* GL7000000

UNII |

* P484053J2Y Y
* S2QG84156O (dihydrate) Y

UN number | 2802

InChI

* InChI=1S/2ClH.Cu/h2*1H;/q;;+2/p-2 Y

Key: ORTQZVOHEJQUHG-UHFFFAOYSA-L Y

* InChI=1/2ClH.Cu/h2*1H;/q;;+2/p-2/rCl2Cu/c1-3-2

Key: ORTQZVOHEJQUHG-LRIOHBSEAE

* InChI=1/2ClH.Cu/h2*1H;/q;;+2/p-2

Key: ORTQZVOHEJQUHG-NUQVWONBAE

SMILES

* Cl[Cu]Cl

* [Cu+2].[Cl-].[Cl-]

Properties

Chemical formula

| CuCl2
Molar mass | 134.45 g/mol (anhydrous)
170.48 g/mol (dihydrate)
Appearance  | yellow-brown solid (anhydrous)
blue-green 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
Hazards
Safety data sheet | Fisher Scientific
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H301, H302, H312, H315, H318, H319, H335, H410, H411

GHS precautionary statements

| P261, P264, P270, P271, P273, P280, P301+310, P301+312, P302+352, P304+340, P305+351+338, P310, P312, P321, P322, P330, P332+313, P337+313, P362, P363, P391, P403+233, P405, P501
NFPA 704 (fire diamond)  |

Flash point | Non-flammable
NIOSH (US health exposure limits):

PEL (Permissible)

| TWA 1 mg/m3 (as Cu)[3]

REL (Recommended)

| TWA 1 mg/m3 (as Cu)[3]

IDLH (Immediate danger)

| TWA 100 mg/m3 (as Cu)[3]
Related compounds

Other anions

| Copper(II) fluoride
Copper(II) bromide

Other cations

| Copper(I) chloride
Silver chloride
Gold(III) chloride

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

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.

## Contents

* 1 Structure
* 2 Properties and reactions
* 2.1 Hydrolysis
* 2.2 Redox and decomposition
* 2.3 Coordination complexes
* 3 Preparation
* 4 Uses
* 4.1 Co-catalyst in Wacker process
* 4.2 In organic synthesis
* 4.3 Catalyst in production of chlorine
* 4.4 Niche uses
* 5 Natural occurrence
* 6 Safety and biological impact
* 7 See also
* 8 References
* 9 Further reading
* 10 External links

## Structure

Structure of copper(II) chloride dihydrate

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):[8][9][10][11]

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 (CuCl2) 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− (it is a dimer in reality, Cu2Cl62−, a couple of tetrahedrons that share an edge), and the green or yellow CuCl42−.[5][14][15]

CuCl2 \+ Cl− ⇌ CuCl−3
CuCl2 \+ 2 Cl− ⇌ CuCl2−4

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)3PO → [CuCl2((C6H5)3PO)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

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 is 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]

1. C2H4 \+ PdCl2 \+ H2O → CH3CHO + Pd + 2 HCl
2. Pd + 2 CuCl2 → 2 CuCl + PdCl2
3. 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

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.[33]

## Safety and biological impact

Copper(II) chloride can be toxic. Only concentrations below 1.3 ppm of aqueous copper ions are allowed in drinking water by the US Environmental Protection Agency.[34] If copper chloride is absorbed, it results in headache, diarrhea, a drop in blood pressure, and fever. Ingestion of large amounts may induce copper poisoning, CNS disorders, and haemolysis.[35][36]

Copper(II) chloride has been demonstrated to cause chromosomal aberrations and mitotic cycle disturbances within A. cepa (onion) cells.[37] Such cellular disturbances lead to genotoxicity. Copper(II) chloride has also been studied as a harmful environmental pollutant. Often present in irrigation-grade water, it can negatively affect water and soil microbes.[38] Specifically, denitrifying bacteria were found to be very sensitive to the presence of copper(II) chloride. At a concentration of 0.95 mg/L, copper(II) chloride was found to cause a 50% inhibition (IC50) of the metabolic activity of denitrifying microbes.[39]

## See also

* Copper(I) chloride

## References

1. ↑ A. F. Wells (1947). "The crystal structure of anhydrous cupric chloride, and the stereochemistry of the cupric atom" (in en). Journal of the Chemical Society: 1670–1675. doi:10.1039/JR9470001670.
2. ↑ Sydney Brownstein; Nam Fong Han; Eric Gabe; Yvon LePage (1989). "A redetermination of the crystal structure of cupric chloride dihydrate" (in en). Zeitschrift für Kristallographie 189 (1): 13–15. doi:10.1524/zkri.1989.189.1-2.13. Bibcode: 1989ZK....189...13B.
3. ↑ 3.0 3.1 3.2 NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0150.html.
4. ↑ Wells, A.F. (1984). Structural Inorganic Chemistry. Oxford: Clarendon Press. p. 253. ISBN 0-19-855370-6.
5. ↑ 5.0 5.1 5.2 5.3 5.4 5.5 Greenwood, N. N. and Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. p. 1183–1185 ISBN 0-7506-3365-4.
6. ↑ Peter Baláž (2008). Mechanochemistry in Nanoscience and Minerals Engineering. Springer. p. 167. ISBN 978-3-540-74854-0. https://books.google.com/books?id=FldqbSffUMgC&pg=PA167.
7. ↑ Carlo Corvaja (2009). Electron paramagnetic resonance: a practitioner's toolkit. John Wiley and Sons. p. 3. ISBN 978-0-470-25882-8. https://books.google.com/books?id=l3F9yUSk-rgC&pg=PA3.
8. ↑ 8.00 8.01 8.02 8.03 8.04 8.05 8.06 8.07 8.08 8.09 8.10 Zhang, J.; Richardson, H. W. (2016). "Copper Compounds". Ullmann's Encyclopedia of Industrial Chemistry. pp. 1–31. doi:10.1002/14356007.a07_567.pub2. ISBN 978-3-527-30673-2.
9. ↑ Shuiliang Zhou; Shaobo Shen; Dalong Zhao; Zhitao Zhang; Shiyu Yan (2017). "Evaporation and decomposition of eutectics of cupric chloride and sodium chloride" (in en). Journal of Thermal Analysis and Calorimetry 129 (3): 1445–1452. doi:10.1007/s10973-017-6360-y.
10. ↑ 10.0 10.1 10.2 Richardson, H. W. (2003). "Copper Compounds". Kirk-Othmer Encyclopedia of Chemical Technology. doi:10.1002/0471238961.0315161618090308.a01.pub2. ISBN 0471238961.
11. ↑ 11.0 11.1 Z. Wang; G. Marin; G. F. Naterer; K. S. Gabriel (2015). "Thermodynamics and kinetics of the thermal decomposition of cupric chloride in its hydrolysis reaction" (in en). Journal of Thermal Analysis and Calorimetry 119 (2): 815–823. doi:10.1007/s10973-014-3929-6. https://research.library.mun.ca/13446/1/2015-JTAC.pdf.
12. ↑ Wilhelm Biltz; Werner Fischer (1927). "Beiträge zur systematischen Verwandtschaftslehre. XLIII. Über das System Cupro-/Cuprichlorid" (in de). Zeitschrift für anorganische und allgemeine Chemie 166 (1): 290–298. doi:10.1002/zaac.19271660126.
13. ↑ A. G. Massey; N. R. Thompson; B. F. G. Johnson (1973) (in en). The Chemistry of Copper, Silver and Gold. Elsevier Science. p. 42. ISBN 9780080188607.
14. ↑ 14.0 14.1 Naida S. Gill; F. B. Taylor (1967). Tetrahalo Complexes of Dipositive Metals in the First Transition Series. Inorganic Syntheses. 9. pp. 136–142. doi:10.1002/9780470132401.ch37. ISBN 978-0-470-13240-1.
15. ↑ 15.0 15.1 H. Wayne Richardson (1997) (in en). Handbook of Copper Compounds and Applications. CRC Press. pp. 24–68. ISBN 9781482277463.
16. ↑ W. Libus; S. K. Hoffmann; M. Kluczkowski; H. Twardowska (1980). "Solution equilibriums of copper(II) chloride in pyridine and pyridine-diluent mixtures" (in en). Inorganic Chemistry 19 (6): 1625–1632. doi:10.1021/ic50208a039.
17. ↑ 17.0 17.1 S. H. Bertz, E. H. Fairchild, in Handbook of Reagents for Organic Synthesis, Volume 1: Reagents, Auxiliaries and Catalysts for C-C Bond Formation, (R. M. Coates, S. E. Denmark, eds.), pp. 220–223, Wiley, New York, 1738.
18. ↑ W. L. F. Armarego; Christina Li Lin Chai (2009-05-22) (Google Books excerpt). Purification of Laboratory Chemicals (6th ed.). Butterworth-Heinemann. pp. 461. ISBN 978-1-85617-567-8. https://books.google.com/books?id=PTXyS7Yj6zUC&pg=PA461.
19. ↑ J. Ji; W. C. Cooper (1990). "Electrochemical preparation of cuprous oxide powder: Part I. Basic electrochemistry" (in en). Journal of Applied Electrochemistry 20 (5): 818–825. doi:10.1007/BF01094312.
20. ↑ 20.0 20.1 20.2 20.3 20.4 20.5 Nicholas D. P. Cosford; Pauline Pei Li; Thierry Ollevier (2015). "Copper(II) Chloride" (in en). Encyclopedia of Reagents for Organic Synthesis: 1–8. doi:10.1002/047084289X.rc214.pub3. ISBN 9780470842898.
21. ↑ C. E. Castro; E. J. Gaughan; D. C. Owsley (1965). "Cupric Halide Halogenations". Journal of Organic Chemistry 30 (2): 587. doi:10.1021/jo01013a069.
22. ↑ J. Brussee; J. L. G. Groenendijk; J. M. Koppele; A. C. A. Jansen (1985). "On the mechanism of the formation of s(−)-(1, 1'-binaphthalene)-2,2'-diol via copper(II)amine complexes". Tetrahedron 41 (16): 3313. doi:10.1016/S0040-4020(01)96682-7.
23. ↑ Chandrasekhar, M.; Kusum L. Chandra; Vinod K. Singh (2003). "Total Synthesis of (+)-Boronolide, (+)-Deacetylboronolide, and (+)-Dideacetylboronolide". Journal of Organic Chemistry 68 (10): 4039–4045. doi:10.1021/jo0269058. PMID 12737588.
24. ↑ Krishna, Palakodety Radha; G. Dayaker (2007). "A stereoselective total synthesis of (−)-andrachcinidine via an olefin cross-metathesis protocol". Tetrahedron Letters (Elsevier) 48 (41): 7279–7282. doi:10.1016/j.tetlet.2007.08.053.
25. ↑ Clark, Jim (August 2018). "Flame Tests". http://www.chemguide.co.uk/inorganic/group1/flametests.html.
26. ↑ Evan Koon Lun Yuuji Hajime, "Adjustable colorimetric moisture indicators", 20150300958 A1  patent US 20150300958 A1, published 2015
27. ↑ "Cobalt dichloride". ECHA. https://echa.europa.eu/substance-information/-/substanceinfo/100.028.718.
28. ↑ B.H. Patel (2011). "11 - Natural dyes". in Clark, M. (in en). Handbook of Textile and Industrial Dyeing. Woodhead Publishing. pp. 412–413. ISBN 9781845696955. https://www.sciencedirect.com/book/9781845696955/handbook-of-textile-and-industrial-dyeing. Retrieved 2 June 2023.
29. ↑ Marlene C. Morris, Howard F. McMurdie, Eloise H. Evans, Boris Paretzkin, Harry S. Parker, and Nicolas C. Panagiotopoulos (1981) Copper chloride hydrate (eriochalcite), in Standard X-ray Diffraction Powder Patterns National Bureau of Standards, Monograph 25, Section 18; page 33.
30. ↑ "Tolbachite" (in en). https://www.mindat.org/min-3990.html.
31. ↑ "Eriochalcite". https://www.mindat.org/min-1398.html.
32. ↑ "The New IMA List of Minerals" (in en). International Mineralogical Association. http://cnmnc.units.it/imalist.htm.
33. ↑ "Atacamite". https://www.mindat.org/min-406.html.
34. ↑ "National Primary Drinking Water Regulations". 30 November 2015. https://www.epa.gov/ground-water-and-drinking-water/national-primary-drinking-water-regulations#Inorganic.
35. ↑ "Copper: Health Information Summary". Environmental Fact Sheet. New Hampshire Department of Environmental Services. 2005. Archived from the original on 20 January 2017. https://web.archive.org/web/20170120014307/http://www.des.nh.gov/organization/commissioner/pip/factsheets/ard/documents/ard-ehp-9.pdf.
36. ↑ "Safety Data Sheet". https://www.sigmaaldrich.com/US/en/sds/aldrich/203149.
37. ↑ Macar, Tuğçe Kalefetoğlu (2020). "Resveratrol ameliorates the physiological, biochemical, cytogenetic, and anatomical toxicities induced by copper (II) chloride exposure in Allium cepa L.". Environmental Science and Pollution Research 27 (1): 657–667. doi:10.1007/s11356-019-06920-2. PMID 31808086. https://link.springer.com/article/10.1007/s11356-019-06920-2.
38. ↑ Shiyab, Safwan (2018). "Phytoaccumulation of copper from irrigation water and its effect on the internal structure of lettuce.". Agriculture 8 (2): 29. doi:10.3390/agriculture8020029.
39. ↑ Ochoa-Herrera, Valeria (2011). "Toxicity of copper (II) ions to microorganisms in biological wastewater treatment systems.". Science of the Total Environment 412 (1): 380–385. doi:10.1016/j.scitotenv.2011.09.072. PMID 22030247. Bibcode: 2011ScTEn.412..380O. https://www.sciencedirect.com/science/article/pii/S0048969711011065.

## Further reading

* Lide, David R. (1990). CRC handbook of chemistry and physics: a ready-reference book of chemical and physical data. Boca Raton: CRC Press. ISBN 0-8493-0471-7. https://archive.org/details/handbookofchemis00crcp.
* The Merck Index, 7th edition, Merck & Co, Rahway, New Jersey, USA, 1960.
* D. Nicholls, Complexes and First-Row Transition Elements, Macmillan Press, London, 1973.
* A. F. Wells, 'Structural Inorganic Chemistry, 5th ed., Oxford University Press, Oxford, UK, 1984.
* J. March, Advanced Organic Chemistry, 4th ed., p. 723, Wiley, New York, 1992.
* Fieser & Fieser Reagents for Organic Synthesis Volume 5, p158, Wiley, New York, 1975.
* D. W. Smith (1976). "Chlorocuprates(II)". Coordination Chemistry Reviews 21 (2–3): 93–158. doi:10.1016/S0010-8545(00)80445-2.

## External links

* Copper Chloride at The Periodic Table of Videos (University of Nottingham)
* Copper (II) Chloride – Description and Pictures
* National Pollutant Inventory – Copper and compounds fact sheet

* v
* t
* e

Copper compounds

Cu(0,I)|

* Cu5Si

Cu(I)|

* CuBr
* CuCN
* CuCl
* CuF
* CuH
* CuI
* Cu2C2
* Cu2Cr2O5
* Cu2O
* CuOH
* CuNO3
* Cu3P
* Cu2S
* CuSCN

Cu(I,II)|

* Cu3H4O8S2

Cu(II)|

* Cu(BF4)2
* CuBr2
* CuC2
* CuCO3
* Cu(CN)2
* Cu(ClO3)2
* CuCl2
* CuF2
* Cu(NO3)2
* Cu3(PO4)2
* Cu(N3)2
* CuO
* CuO2
* Cu(OH)2
* CuI2
* CuS
* CuSO4
* Cu3(AsO4)2

Cu(III)|

* K3CuF6
* Cu2O3

Cu(IV)|

* Cs2CuF6
* Rb2CuF6

* v
* t
* e

Salts and covalent derivatives of the chloride ion

HCl |  |  |  | He

|
|
|
|

LiCl | BeCl2 | BCl3
B2Cl4 | CCl4 | NCl3
ClN3 | Cl2O
ClO2
Cl2O7 | ClF
ClF3
ClF5 | Ne
NaCl | MgCl2 | AlCl
AlCl3 | SiCl4 | P2Cl4
PCl3
PCl5 | S2Cl2
SCl2
SCl4 | Cl2 | Ar
KCl | CaCl
CaCl2 | ScCl3 | TiCl2
TiCl3
TiCl4 | VCl2
VCl3
VCl4
VCl5 | CrCl2
CrCl3
CrCl4 | MnCl2 | FeCl2
FeCl3 | CoCl2
CoCl3 | NiCl2 | CuCl
CuCl2 | ZnCl2 | GaCl2
GaCl3 | GeCl2
GeCl4 | AsCl3
AsCl5 | Se2Cl2
SeCl4 | BrCl | KrCl
RbCl | SrCl2 | YCl3 | ZrCl3
ZrCl4 | NbCl4
NbCl5 | MoCl2
MoCl3
MoCl4
MoCl5
MoCl6 | TcCl4 | RuCl3 | RhCl3 | PdCl2 | AgCl | CdCl2 | InCl
InCl2
InCl3 | SnCl2
SnCl4 | SbCl3
SbCl5 | Te3Cl2
TeCl4 | ICl
ICl3 | XeCl
XeCl2
CsCl | BaCl2 |  | HfCl4 | TaCl5 | WCl2
WCl3
WCl4
WCl5
WCl6 | Re3Cl9
ReCl4
ReCl5
ReCl6 | OsCl4 | IrCl2
IrCl3
IrCl4 | PtCl2
PtCl4 | AuCl
AuCl3 | Hg2Cl2,
HgCl2 | TlCl | PbCl2,
PbCl4 | BiCl3 | PoCl2,
PoCl4 | AtCl  | RnCl2
FrCl | RaCl2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaCl3 | CeCl3 | PrCl3 | NdCl2,
NdCl3 | PmCl3 | SmCl2,
SmCl3 | EuCl2,
EuCl3 | GdCl3 | TbCl3 | DyCl2,
DyCl3 | HoCl3 | ErCl3 | TmCl2
TmCl3 | YbCl2
YbCl3 | LuCl3
AcCl3 | ThCl4 | PaCl5 | UCl3
UCl4
UCl5
UCl6 | NpCl4 | PuCl3 | AmCl2
AmCl3 | CmCl3 | BkCl3 | CfCl3 | EsCl3 | Fm  | Md  | No  | LrCl3

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Original source: https://en.wikipedia.org/wiki/Copper(II) chloride. Read more

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Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Copper(II)_chloride&oldid=248145"
*[CID]: Compound ID
*[H301]: Toxic if swallowed
*[H302]: Harmful if swallowed
*[H312]: Harmful in contact with skin
*[H315]: Causes skin irritation
*[H318]: Causes serious eye damage
*[H319]: Causes serious eye irritation
*[H335]: May cause respiratory irritation
*[H410]: Very toxic to aquatic life with long lasting effects
*[H411]: Toxic to aquatic life with long lasting effects
*[P261]: Avoid breathing dust/fume/gas/mist/vapours/spray
*[P264]: Wash … thoroughly after handling
*[P270]: Do not eat, drink or smoke when using this product
*[P271]: Use only outdoors or in a well-ventilated area
*[P273]: Avoid release to the environment
*[P280]: Wear protective gloves/protective clothing/eye protection/face protection
*[P301+310]: IF SWALLOWED: Immediately call a POISON CENTER or doctor/physician
*[P301+312]: IF SWALLOWED: Call a POISON CENTER or doctor/physician if you feel unwell
*[P302+352]: IF ON SKIN: Wash with soap and water
*[P304+340]: IF INHALED: Remove victim to fresh air and keep at rest in a position comfortable for breathing
*[P305+351+338]: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do – continue rinsing
*[P310]: Immediately call a POISON CENTER or doctor/physician
*[P312]: Call a POISON CENTER or doctor/physician if you feel unwell
*[P321]: Specific treatment (see … on this label)
*[P322]: Specific measures (see … on this label)
*[P330]: Rinse mouth
*[P332+313]: If skin irritation occurs: Get medical advice/attention
*[P337+313]: Get medical advice/attention
*[P362]: Take off contaminated clothing and wash before reuse
*[P363]: Wash contaminated clothing before reuse
*[P391]: Collect spillage
*[P403+233]: Store in a well ventilated place. Keep container tightly closed
*[P405]: Store locked up
*[P501]: Dispose of contents/container to …
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