Palladium(II) chloride
Palladium 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.
Structure
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. Furthermore, in both forms, the Pd 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.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.
Preparation
Palladium 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 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 bispalladium dichloride and bispalladium dichloride. These complexes are prepared by treating PdCl2 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, bispalladium dichloride may be prepared from palladium chloride by reacting it with triphenylphosphine in benzonitrile:
Further reduction in the presence of more triphenylphosphine gives tetrakispalladium; the second reaction may be carried out without purifying the intermediate dichloride:
Alternatively, palladium 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 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.
File:Tetrachloropalladate ions in aqueous solution.jpg|thumb|250px|left|A solution of 2−
Uses
Even when dry, palladium chloride is able to rapidly stain stainless steel. Thus, palladium chloride solutions are sometimes used to test for the corrosion-resistance of stainless steel.Palladium chloride is sometimes used in carbon monoxide detectors. Carbon monoxide reduces palladium chloride to palladium:
Residual PdCl2 is converted to red PdI2, the concentration of which may be determined colorimetrically:
Palladium chloride is used in the Wacker process for production of aldehydes and ketones from alkenes.
Palladium chloride can also be used for the cosmetic tattooing of leukomas in the cornea.