Cuprous chloride
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| Names | |
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IUPAC name
Copper(I) chloride
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| Other names
Cuprous chloride
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| Identifiers | |
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3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.028.948 |
| EC Number | 231-842-9 |
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PubChem CID
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| RTECS number | GL6990000 |
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| Properties | |
| CuCl | |
| Molar mass | 98.999 g/mol |
| Appearance | white powder, slightly green from oxidized impurities |
| Density | 4.14 g/cm3 |
| Melting point | 423 °C (793 °F; 696 K) |
| Boiling point | 1,490 °C (2,710 °F; 1,760 K) (decomposes) |
| 0.047 g/L (20 °C) | |
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Solubility product (Ksp)
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1.72×10−7 |
| Solubility | insoluble in ethanol acetone; soluble in concentrated HCl, NH4OH |
| Band gap | 3.25 eV (300 K, direct) |
| -40.0·10−6 cm3/mol | |
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Refractive index (nD)
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1.930 |
| Structure | |
| Zincblende, cF20 | |
| F43m, No. 216 | |
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a = 0.54202 nm
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Lattice volume (V)
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0.1592 nm3 |
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Formula units (Z)
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4 |
| Hazards | |
| Safety data sheet | JT Baker |
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EU classification (DSD) (outdated)
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Harmful (Xn) Dangerous for the environment (N) |
| R-phrases (outdated) | R22, R50/53 |
| S-phrases (outdated) | (S2), S22, S60, S61 |
| NFPA 704 | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
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LD50 (median dose)
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140 mg/kg |
| US health exposure limits (NIOSH): | |
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PEL (Permissible)
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TWA 1 mg/m3 (as Cu) |
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REL (Recommended)
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TWA 1 mg/m3 (as Cu) |
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IDLH (Immediate danger)
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TWA 100 mg/m3 (as Cu) |
| Related compounds | |
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Other anions
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Copper(I) bromide Copper(I) iodide |
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Other cations
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Copper(II) chloride Silver(I) chloride |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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 (what is   ?) |
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| Infobox references | |
Copper(I) chloride, commonly called cuprous chloride, is the lower chloride of copper, with the formula CuCl. The substance is a white solid sparingly soluble in water, but very soluble in concentrated hydrochloric acid. Impure samples appear green due to the presence of copper(II) chloride.
Copper(I) chloride was first prepared by Robert Boyle in the mid-seventeenth century from mercury(II) chloride ("Venetian sublimate") and copper metal:
In 1799, J.L. Proust characterized the two different chlorides of copper. He prepared CuCl by heating CuCl2 at red heat in the absence of air, causing it to lose half of its combined chlorine followed by removing residual CuCl2 by washing with water.
An acidic solution of CuCl was formerly used for analysis of carbon monoxide content in gases, for example in Hempel's gas apparatus. This application was significant during the time that coal gas was widely used for heating and lighting, during the nineteenth and early twentieth centuries.
Copper(I) chloride is produced industrially by the direct combination of copper metal and chlorine at 450–900 °C:
Cu + 0.5 Cl2 → CuCl
Copper(I) chloride can also be prepared by reducing copper(II) chloride, e.g. with sulfur dioxide:
2 CuCl2 + SO2 + 2 H2O → 2 CuCl + H2SO4 + 2 HCl
Many other reducing agents can be used.
Copper(I) chloride has the cubic zincblende crystal structure at ambient conditions. Upon heating to 408 °C the structure changes to hexagonal. Several other crystalline forms of CuCl appear at high pressures (several GPa).
Copper(I) chloride is a Lewis acid, which is classified as soft according to the Hard-Soft Acid-Base concept. Thus, it tends to form stable complexes with soft Lewis bases such as triphenylphosphine:
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