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).Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.

Image:Beta-PdCl2.png

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.{{cite journal | author = J. Evers, W. Beck, M. Göbel, S. Jakob, P. Mayer, G. Oehlinger, M. Rotter, T. M. Klapötke | title = The Structures of δ-PdCl₂ and γ-PdCl₂: Phases with Negative Thermal Expansion in One Direction | doi = 10.1002/anie.201000680 | journal = Angew. Chem. Int. Ed. | year = 2010 | volume = 49 | pages = 5677–5682 | issue = 33 | pmid = 20602377 }}

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.{{cite book |last1=Patnaik |first1=Pradyot |title=Handbook of inorganic chemicals |date=2003 |publisher=McGraw-Hill |location=New York |isbn=978-0-07-049439-8 |page=687 |edition=1 |chapter=Palladium}}{{cite book |last1=Patnaik |first1=Pradyot |title=Handbook of inorganic chemicals |date=2003 |publisher=McGraw-Hill |location=New York |isbn=978-0-07-049439-8 |pages=688–689 |edition=1 |chapter=Palladium Dichloride}}{{cite book |last1=Armarego |first1=W. L. F. |title=Purification of laboratory chemicals |date=2017 |publisher=Elsevier |location=Amsterdam |isbn=978-0-12-805457-4 |page=687 |edition=Eighth |chapter=4. Purification of Inorganic and Metal-Organic Chemicals}}{{cite journal |last1=Kharasch |first1=Morris S. |last2=Seyler |first2=Ralph C. |last3=Mayo |first3=Frank R. |title=Coördination Compounds of Palladous Chloride |journal=J. Am. Chem. Soc. |date=1938 |volume=60 |issue=4 |pages=882–884 |doi=10.1021/ja01271a035 |publisher=American Chemical Society}}

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.{{cite book | chapter = Bis(Benzonitrile)Dichloro Complexes of Palladium and Platinum | pages =60–63 | journal = Inorg. Synth. | volume = 28 | author = Gordon K. Anderson, Minren Lin | title =Inorganic Syntheses | doi = 10.1002/9780470132593.ch13 | date =2007 | isbn =9780470132593 }} 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:{{OrgSynth | title = Palladium-catalyzed reaction of 1-alkenylboronates with vinylic halides: (1Z,3E)-1-Phenyl-1,3-octadiene | collvol = 8 | collvolpages = 532|author1-link=Norio Miyaura | author1 = Norio Miyaura|author2-link=Akira Suzuki (chemist)| author2= Akira Suzuki | year = 1993 | prep = cv8p0532}}

: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:{{cite book | journal = Inorg. Synth. | volume = 13 | pages = 121–124 | author = D. R. Coulson | doi = 10.1002/9780470132449.ch23 | year = 1972 | last2 = Satek | first2 = L. C. | last3 = Grim | first3 = S. O.| title = Inorganic Syntheses | chapter = Tetrakis(triphenylphosphine)palladium(0) | isbn = 9780470132449 }}

:PdCl₂(PPh₃)₂ + 2 PPh₃ + {{sfrac|5|2}} N₂H₄ → Pd(PPh₃)₄ + {{sfrac|1|2}} 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:{{cite book | title = Handbook of Organopalladium Chemistry for Organic Synthesis | editor = Ei-ichi Negishi | isbn = 0-471-31506-0 | year = 2002 | publisher = John Wiley & Sons, Inc. | chapter = II.2.3 Pd(0) and Pd(II) Complexes Containing Phosphorus and Other Group 15 Atom Ligands | author = Daniele Choueiry and Ei-ichi Negishi | chapter-url = https://books.google.com/books?id=mTMA2hExAaIC&pg=PA47 | chapter-format = Google Books excerpt}} 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 chloride may also be used to give heterogeneous palladium catalysts: palladium on barium sulfate, palladium on carbon, and palladium chloride on carbon.{{OrgSynth | title = Palladium Catalysts | author = Ralph Mozingo | collvol = 3 | collvolpages = 685 | year = 1955 | prep = cv3p0685}}

File:Tetrachloropalladate ions in aqueous solution.jpg

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.For example, http://www.marinecare.nl/assets/Uploads/Downloads/Leaflet-Passivation-Test-Kit.pdf{{dead link|date=March 2018 |bot=InternetArchiveBot |fix-attempted=yes }}

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:{{cite journal | author = T. H. Allen, W. S. Root | title = Colorimetric Determination of Carbon Monoxide in Air by an improved Palladium Chloride Method | url = http://www.jbc.org/content/216/1/309 | journal = J. Biol. Chem. | year = 1955 | volume = 216 | pages = 309–317 | pmid = 13252030 | issue = 1| doi = 10.1016/S0021-9258(19)52307-9 | doi-access = free }}

: 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.

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{{Palladium compounds}}

{{Chlorides}}

Category:Palladium compounds

Category:Chlorides

Category:Platinum group halides