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| Names | |||
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IUPAC name
Cadmium dichloride
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| Other names
Cadmium(II) chloride
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| Identifiers | |||
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3D model (JSmol)
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| ChEBI | |||
| ChemSpider | |||
| ECHA InfoCard | 100.030.256 | ||
| EC Number |
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| 912918 | |||
| KEGG | |||
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PubChem CID
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| RTECS number |
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| UNII |
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| UN number | 2570 | ||
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CompTox Dashboard (EPA)
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| Properties | |||
| CdCl2 | |||
| Molar mass | 183.31 g·mol−1 | ||
| Appearance | White solid, hygroscopic | ||
| Odor | Odorless | ||
| Density | 4.047 g/cm3 (anhydrous) 3.327 g/cm3 (Hemipentahydrate) |
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| Melting point | 568 °C (1,054 °F; 841 K) at 760 mmHg |
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| Boiling point | 964 °C (1,767 °F; 1,237 K) at 760 mmHg |
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| Hemipentahydrate: 79.5 g/100 mL (−10 °C) 90 g/100 mL (0 °C) Monohydrate: 119.6 g/100 mL (25 °C) 134.3 g/100 mL (40 °C) 134.2 g/100 mL (60 °C) 147 g/100 mL (100 °C) |
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| Solubility | Soluble in alcohol, selenium(IV) oxychloride, benzonitrile Insoluble in ether, acetone |
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| Solubility in pyridine | 4.6 g/kg (0 °C) 7.9 g/kg (4 °C) 8.1 g/kg (15 °C) 6.7 g/kg (30 °C) 5 g/kg (100 °C) |
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| Solubility in ethanol | 1.3 g/100 g (10 °C) 1.48 g/100 g (20 °C) 1.91 g/100 g (40 °C) 2.53 g/100 g (70 °C) |
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| Solubility in dimethyl sulfoxide | 18 g/100 g (25 °C) | ||
| Vapor pressure | 0.01 kPa (471 °C) 0.1 kPa (541 °C) |
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| −6.87·10−5 cm3/mol | |||
| Viscosity | 2.31 cP (597 °C) 1.87 cP (687 °C) |
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| Structure | |||
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Rhombohedral, hR9 (anhydrous) Monoclinic (hemipentahydrate) |
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| R3m, No. 166 (anhydrous) | |||
| 3 2/m (anhydrous) | |||
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a = 3.846 Å, c = 17.479 Å (anhydrous)
α = 90°, β = 90°, γ = 120°
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| Thermochemistry | |||
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Heat capacity (C)
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74.7 J/mol·K | ||
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Std molar
entropy (S⦵298) |
115.3 J/mol·K | ||
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Std enthalpy of
formation (ΔfH⦵298) |
−391.5 kJ/mol | ||
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Gibbs free energy (ΔfG⦵)
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−343.9 kJ/mol | ||
| Hazards | |||
| GHS labelling: | |||
  
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| Danger | |||
| H301, H330, H340, H350, H360, H372, H410 | |||
| P210, P260, P273, P284, P301+P310, P310 | |||
| NFPA 704 (fire diamond) | |||
| Lethal dose or concentration (LD, LC): | |||
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LD50 (median dose)
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94 mg/kg (rats, oral) 60 mg/kg (mouse, oral) 88 mg/kg (rat, oral) |
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| NIOSH (US health exposure limits): | |||
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PEL (Permissible)
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[1910.1027] TWA 0.005 mg/m3 (as Cd) | ||
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REL (Recommended)
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Ca | ||
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IDLH (Immediate danger)
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Ca [9 mg/m3 (as Cd)] | ||
| Safety data sheet (SDS) | External MSDS | ||
| Related compounds | |||
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Other anions
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Cadmium fluoride Cadmium bromide Cadmium iodide |
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Other cations
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Zinc chloride Mercury(II) chloride Calcium 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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Cadmium chloride is a white crystalline compound of cadmium and chloride, with the formula CdCl2. This salt is a hygroscopic solid that is highly soluble in water and slightly soluble in alcohol. The crystal structure of cadmium chloride (described below), is a reference for describing other crystal structures. Also known are CdCl2•H2O and CdCl2•5H2O.
Structure
Cadmium chloride forms a layered structure consisting of octahedral Cd2+ centers linked with chloride ligands. Cadmium iodide, CdI2, has a similar structure, but the iodide ions are arranged in a HCP lattice, whereas in CdCl2 the chloride ions are arranged in a CCP lattice.
Chemical properties
Cadmium chloride dissolves well in water and other polar solvents. It is a mild Lewis acid.
- CdCl2 + 2 Cl− → [CdCl4]2−
Solutions of equimolar cadmium chloride and potassium chloride give potassium cadmium trichloride. With large cations, it is possible to isolate the trigonal bipyramidal [CdCl5]3− ion.
Preparation
Anhydrous cadmium chloride can be prepared by the reaction of hydrochloric acid and cadmium metal.
- Cd + 2 HCl → CdCl2 + H2
The anhydrous salt can also be prepared from anhydrous cadmium acetate using hydrogen chloride or acetyl chloride.
Uses
Cadmium chloride is used for the preparation of cadmium sulfide, used as "cadmium yellow", a brilliant-yellow stable inorganic pigment.
-
CdCl
2 + H
2S → CdS + 2 HCl
In the laboratory, anhydrous CdCl2 can be used for the preparation of organocadmium compounds of the type R2Cd, where R is an aryl or a primary alkyl. These were once used in the synthesis of ketones from acyl chlorides:
-
CdCl
2 + 2 RMgX → R
2Cd + MgCl
2 + MgX
2
-
R
2Cd + 2R'COCl → 2R'COR + CdCl
2
Such reagents have largely been supplanted by organocopper compounds, which are much less toxic.
Cadmium chloride is also used for photocopying, dyeing and electroplating.
Like all cadmium compounds, CdCl
2 is highly toxic and appropriate safety precautions must be taken when handling it.
External links
- International Chemical Safety Card 0116
- IARC Monograph "Cadmium and Cadmium Compounds"
- National Pollutant Inventory - Cadmium and compounds
