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Palladium(II) chloride

Palladium(II) chloride
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
Density and phase 4 g/cm³, solid
Solubility in water insol
Other solvents hydrochloric acid
Melting point 675 °C decomp
Coordination geometry square planar
Structure (i) infinite chain with
bridging chloride ions
(i) cubic cluster
Thermodynamic data
Standard enthalpy
of formation
 ? kJ/mol
Standard molar entropy
 ? J.K–1.mol–1
Safety data
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

Palladium(II) chloride, also known as palladium dichloride, 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 chlorination of palladium.



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 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).[1]



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 labile but soluble Lewis base adducts, such as those derived from acetonitrile or benzonitrile.[2]

The acetonitrile complex is prepared by treating PdCl2 in refluxing acetonitrile:

PdCl2 + 2 MeCN → 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.[citation needed] Palladium(II) chloride is sometimes used in carbon monoxide detectors.


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.


  1. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  2. ^ Gordon K. Anderson, Minren Lin. "Bis(Benzonitrile)Dichloro Complexes of Palladium and Platinum". Inorganic Syntheses 28: 60-63. doi:10.1002/9780470132593.ch13.
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Palladium(II)_chloride". A list of authors is available in Wikipedia.
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