Palladium(II) chloride
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| Palladium(II) chloride | |
|---|---|
 |
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| General | |
| Other names | Palladium dichloride |
| Molecular formula | PdCl2 |
| Molar mass | 177.33 g/mol |
| Appearance | dark red solid |
| CAS number | [7647-10-1] |
| EINECS number | 231-596-2 |
| Properties | |
| Density and phase | 4 g/cm3, solid |
| Solubility in water | insol |
| Other solvents | hydrochloric acid |
| Melting point | 675 °C decomp |
| Structure | |
| Coordination geometry | square planar |
| Structure | (i) infinite chain with bridging chloride ions (i) cubic cluster |
| Thermodynamic data | |
| Standard enthalpy of formation ΔfH°solid |
? kJ/mol |
| Standard molar entropy S°solid |
? J.K–1.mol–1 |
| Safety data | |
| PEL-TWA (OSHA) | — |
| RTECS number | RT3500000 |
| Supplementary data page | |
| Structure & properties | n, εr, etc. |
| Thermodynamic data | Phase behaviour Solid, liquid, gas |
| Spectral data | UV, IR, NMR, MS |
| Related compounds | |
| Other anions | Palladium(II) fluoride Palladium(II) bromide Palladium(II) iodide |
| Other cations | Nickel(II) chloride Platinum(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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Palladium(II) chloride, also known as palladium dichloride, is the chemical compound with the formula PdCl2. It is a common starting material in palladium chemistry – palladium-based catalysts are of particular value in organic synthesis. It is prepared by chlorination of palladium.
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[edit] Structure
Two forms of PdCl2 are known. In both forms, the palladium centres adopt the square-planar coordination geometry that is characteristic of Pd(II). Furthermore, in both forms, the Pd(II) centres are linked by μ2-chloride bridges. The α-form of PdCl2 is a polymer, consisting of "infinite" slabs or chains. The β-form of PdCl2 is molecular, consisting of an octahedron of six Pd atoms. Each of the twelve edges of this octahedron is spanned by Cl-. PtCl2 adopts similar structures, whereas NiCl2 adopts the CdCl2 motif, featuring hexacoordinated Ni(II).[1]
[edit] Uses
Starting point in the synthesis of other palladium compounds. Palladium(II) chloride is not particularly soluble in water or non-coordinating solvents, so the first step in its utilization is often the preparation labile but soluble Lewis base adducts, such as those derived from acetonitrile or benzonitrile. The acetonitrile complex is prepared by treating PdCl2 in refluxing acetonitrile:
- PdCl2 + 2MeCN → PdCl2(MeCN)2
Although occasionally recommended, inert-gas techniques are not necessary if the complex is to be used in situ.
Even when dry, palladium(II) chloride is able to rapidly stain stainless steel. Thus, palladium(II) chloride solutions are sometimes used to test for the corrosion-resistance of stainless steel. Palladium(II) chloride is sometimes used in carbon monoxide detectors.
[edit] Safety
The related nickel and platinum compounds are known to be irritants of the skin and the respiratory system and, in some cases, carcinogenic, and its is generally accepted as prudent to assume that palladium compounds share these risks.
[edit] References
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
