Cadmium chloride
From Wikipedia, the free encyclopedia
| Cadmium chloride | |
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| Identifiers | |
| CAS number | [10108-64-2] |
| Properties | |
| Molecular formula | CdCl2 |
| Molar mass | 183.316 |
| Appearance | white solid, hygroscopic |
| Density | 4.08 g/cm3 (solid) |
| Melting point |
564 °C |
| Boiling point |
960 °C |
| Hazards | |
| MSDS | External MSDS |
| EU classification | Highly toxic (T+) Carc. Cat. 2 Muta. Cat. 2 Repr. Cat. 2 Dangerous for the environment (N) |
| NFPA 704 |
 4
4
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| R-phrases | R45, R46, R60, R61, R25, R26, R48/23/25, R50/53 |
| S-phrases | S53, S45, S60, S61 |
| Related compounds | |
| Other anions | Cadmium fluoride Cadmium bromide Cadmium iodide |
| Other cations | Zinc chloride Mercury(II) chloride |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Cadmium chloride is a white crystalline compound of cadmium and chlorine, with the formula CdCl2. It is a hygroscopic solid that is highly soluble in water and slightly soluble in alcohol. Although it is considered to be ionic, it has considerable covalent character to its bonding. The crystal structure of cadmium chloride (described below), composed of two-dimensional layers of ions, is often used as a reference for describing other crystal structures.
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[edit] Crystal structure
Cadmium chloride forms crystals with cubic symmetry. The structure is based on the sodium chloride crystal structure, but with half of the metal ions removed (the "missing" ions are shown as hatched light-blue balls in the drawing) so that the resultant structure consists of a layered lattice. This same basic structure is found in many other salts and minerals, in particular those that display some degree of covalent bonding, such as in manganese(II) chloride, cobalt(II) chloride, or magnesium chloride.
Cadmium iodide, CdI2, has a very similar crystal structure to CdCl2. The individual layers in the two structures are identical, but in CdCl2 the chloride ions are arranged in a CCP lattice, whereas in CdI2 the iodide ions are arranged in a HCP lattice.
[edit] Chemical properties
Cadmium chloride has a high solubility in water, and it dissociates into ions. A certain amount of hydrolysis to species such as [CdOH(H2O)x]+ may occur. The high solubility may be due in part to formation of complex ions such as [CdCl4]2− (i.e, CdCl2 is a Lewis acid). With excess chloride ions in water or acetonitrile it forms mainly [CdCl3]− and the tetrahedral anion, [CdCl4]2−:
CdCl2(aq) + 2 Cl−(aq) → [CdCl4]2−(aq)
With large cations, it is possible to isolate the trigonal bipyramidal [CdCl5]3− ion.
[edit] Preparation
Anhydrous cadmium chloride can be prepared by the action of anhydrous chlorine or hydrogen chloride gas on heated cadmium metal.
Cd(s) + 2 HCl(g) → CdCl2(s) + H2(g)
Hydrochloric acid may be used to make hydrated CdCl2 from the metal, or alternatively from cadmium oxide or cadmium carbonate.
[edit] Uses
Cadmium chloride is used for the preparation of cadmium sulfide, used as "Cadmium Yellow", a brilliant-yellow pigment, which is stable to heat and sulfide fumes.
CdCl2(aq) + H2S(g) → CdS(s) + 2 HCl(aq)
In the laboratory, anhydrous CdCl2 can be used for the preparation of organocadmium compounds of the type R2Cd where R = aryl or primary alkyl. These were once used in the synthesis of ketones from acyl chlorides (see below), but nowadays they have largely been supplanted by organocopper compounds, which are much less toxic.
CdCl2 + 2 RMgX → R2Cd + MgCl2 + MgX2
Cadmium chloride is also used for electroplating.
[edit] References
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The references in this article would be clearer with a different or consistent style of citation, footnoting, or external linking. |
- N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, 2nd ed., Butterworth-Heinemann, Oxford, UK, 1997.
- Handbook of Chemistry and Physics, 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
- 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.
