Palladium(II) chloride

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). 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. ==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 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 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: :PdCl2(PPh3)2 + 2 PPh3 + N2H4 → Pd(PPh3)4 + N2 + 2 Hydrazinium chloride| Alternatively, palladium(II) chloride may be solubilized in the form of the tetrachloropalladate(II) anion, such as in 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. File:Tetrachloropalladate ions in aqueous solution.jpg|thumb|250px|left|A solution of [PdCl4]2−(aq) ==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: : PdCl2 + CO + H2O → Pd + CO2 + 2HCl Residual PdCl2 is converted to red PdI2, the concentration of which may be determined colorimetrically: : PdCl2 + 2 KI → PdI2 + 2 KCl 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. ==References==