Palladium dichloride, Palladous chloride
3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||177.326 g/mol (anhydrous) |
213.357 g/mol (dihydrate)
|Appearance||dark red solid |
dark brown crystals (dihydrate)
|Melting point||679 °C (1,254 °F; 952 K) (decomposes)|
|soluble in trace amounts, better solubility in cold water|
|Solubility||soluble in organic solvents |
dissolves rapidly in HCl
|Lethal dose or concentration (LD, LC):|
LD50 (median dose)
|2704 mg/kg (rat, oral)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Palladium(II) chloride, also known as palladium dichloride and palladous chloride, are the chemical compounds with the formula PdCl2. PdCl2 is a common starting material in palladium chemistry – palladium-based catalysts are of particular value in organic synthesis. It is prepared by the reaction of chlorine with palladium metal at high temperatures.
Two forms of PdCl2 are known, denoted α and β. In both forms, the palladium centres adopt a square-planar coordination geometry that is characteristic of Pd(II). Furthermore, in both forms, the Pd(II) centers 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 octahedral cluster 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).
crystal structure of α-PdCl2
found in the crystal structure of β-PdCl2
Two further polymorphs, γ-PdCl2 and δ-PdCl2, have been reported and show negative thermal expansion. The high-temperature δ form contains planar ribbons of edge‐connected PdCl4 squares, like α-PdCl2. The low‐temperature γ form has corrugated layers of corner‐connected PdCl4 squares.
Palladium(II) chloride is prepared by dissolving palladium metal in aqua regia or hydrochloric acid in the presence of chlorine. Alternatively, it may be prepared by heating palladium sponge metal with chlorine gas at 500 °C.
Palladium(II) chloride is a common starting point in the synthesis of other palladium compounds. It is not particularly soluble in water or non-coordinating solvents, so the first step in its utilization is often the preparation of labile but soluble Lewis base adducts, such as bis(benzonitrile)palladium dichloride and bis(acetonitrile)palladium dichloride. These complexes are prepared by treating PdCl2 with hot solutions of the nitriles:
- PdCl2 + 2 RCN → PdCl2(RCN)2
Although occasionally recommended, inert-gas techniques are not necessary if the complex is to be used in situ. As an example, bis(triphenylphosphine)palladium(II) dichloride may be prepared from palladium(II) chloride by reacting it with triphenylphosphine in benzonitrile:
- PdCl2 + 2 PPh3 → PdCl2(PPh3)2
- PdCl2(PPh3)2 + 2 PPh3 + 2.5 N2H4 → Pd(PPh3)4 + 0.5 N2 + 2 N2H5+Cl−
Alternatively, palladium(II) chloride may be solubilized in the form of the tetrachloropalladate anion, e.g. sodium tetrachloropalladate, by reacting with the appropriate alkali metal chloride in water: Palladium(II) chloride is insoluble in water, whereas the product dissolves:
- PdCl2 + 2 MCl → M2PdCl4
This compound may also further react with phosphines to give phosphine complexes of palladium.
Palladium(II) chloride is sometimes used in carbon monoxide detectors. Carbon monoxide reduces palladium(II) chloride to palladium:
- PdCl2 + CO + H2O → Pd + CO2 + 2HCl
- PdCl2 + 2 KI → PdI2 + 2 KCl
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- For example, http://www.marinecare.nl/assets/Uploads/Downloads/Leaflet-Passivation-Test-Kit.pdf[permanent dead link]
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