Palladium(II) chloride
Palladium(II) chloride, also known as palladium dichloride and palladous chloride, are the chemical compounds with the formula PdCl. PdCl 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. Structure. Two forms of PdCl 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 μ-chloride bridges. The α-form of PdCl is  a polymer, consisting of "infinite" slabs or chains. The β-form of PdCl is molecular, consisting of an octahedral cluster of six Pd atoms. Each of the twelve edges of this octahedron is spanned by Cl. PtCl adopts similar structures, whereas NiCl adopts the CdCl motif, featuring hexacoordinated Ni(II). Two further polymorphs, γ-PdCl and δ-PdCl, have been reported and show negative thermal expansion. The high-temperature δ form contains planar ribbons of edge-connected PdCl squares, like α-PdCl. The low-temperature γ form has corrugated layers of corner-connected PdCl squares. Preparation. 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. Reactions. 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 PdCl with hot solutions of the nitriles: 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: Further reduction in the presence of more triphenylphosphine gives tetrakis(triphenylphosphine)palladium(0); the second reaction may be carried out without purifying the intermediate dichloride: 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: This compound may also further react with phosphines to give phosphine  complexes of palladium. Palladium chloride may also be used to give heterogeneous palladium catalysts: palladium on barium sulfate, palladium on carbon, and palladium chloride on carbon. Uses. 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. Carbon monoxide reduces palladium(II) chloride to palladium: Residual PdCl is converted to red PdI, the concentration of which may be determined colorimetrically: Palladium(II) chloride is used in the Wacker process for production of aldehydes and ketones  from alkenes. Palladium(II) chloride can also be used for the cosmetic tattooing of leukomas in the cornea.