| 词条 | Palladium(II) chloride | ||||
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 431915305 | Name = Palladium(II) chloride | ImageFile = Palladium chloride.jpg | ImageName = Palladium(II) chloride Palladium dichloride | OtherNames = Palladium dichloride, Palladous chloride |Section1={{Chembox Identifiers | CASNo_Ref = {{cascite|correct|CAS}} | CASNo = 7647-10-1 | UNII_Ref = {{fdacite|changed|FDA}} | UNII = N9214IR8N7 | EINECS = 231-596-2 | RTECS = RT3500000 | PubChem = 24290 | SMILES = Cl[Pd]Cl | SMILES_Comment = monomer | SMILES1 = [Cl+]0[Pd-2]12[Cl+][Pd-2]34[Cl+][Pd-2]05[Cl+][Pd-2]6([Cl+]1)[Cl+][Pd-2]([Cl+]2)([Cl+]3)[Cl+][Pd-2]([Cl+]4)([Cl+]5)[Cl+]6 | SMILES1_Comment = hexamer | InChI = 1S/2ClH.Pd/h2*1H;/q;;+2/p-2 | InChIKey = PIBWKRNGBLPSSY-UHFFFAOYSA-L | ChemSpiderID = 22710 |Section2={{Chembox Properties | Formula = PdCl2 | MolarMass = 177.326 g/mol (anhydrous) 213.357 g/mol (dihydrate) | Appearance = dark red solid hygroscopic (anhydrous) dark brown crystals (dihydrate) | Density = 4.0 g/cm3 | Solubility = soluble in trace amounts, better solubility in cold water | SolubleOther = soluble in organic solvents dissolves rapidly in HCl | MeltingPtC = 679 | MeltingPt_notes = (decomposes) | MagSus = −38.0·10−6 cm3/mol |Section3={{Chembox Structure | Coordination = square planar | CrystalStruct = rhombohedral |Section4={{Chembox Thermochemistry | DeltaHf = | Entropy = |Section7={{Chembox Hazards | ExternalSDS = | EUClass = | MainHazards = | NFPA-H = | NFPA-F = | NFPA-R = | NFPA-S = | RPhrases = | SPhrases = | FlashPt = Non-flammable | PEL = | LD50 = 2704 mg/kg (rat, oral) |Section8={{Chembox Related | OtherAnions = Palladium(II) fluoride Palladium(II) bromide Palladium(II) iodide | OtherCations = Nickel(II) chloride Platinum(II) chloride Platinum(II,IV) chloride Platinum(IV) chloride }} Palladium(II) 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. StructureTwo 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).[1]
PreparationPalladium(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. ReactionsPalladium(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.[2] 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:[3] 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:[4] PdCl2(PPh3)2 + 2 PPh3 + 2.5 N2H4 → Pd(PPh3)4 + 0.5 N2 + 2 N2H5+Cl− 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:[5] 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.[5] Palladium chloride may also be used to give heterogeneous palladium catalysts: palladium on barium sulfate, palladium on carbon, and palladium chloride on carbon.[6] UsesEven 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.[7] 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:[8] 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. References1. ^Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}. {{Palladium compounds}}2. ^{{cite journal | title = Bis(Benzonitrile)Dichloro Complexes of Palladium and Platinum | pages =60–63 | journal = Inorg. Synth. | volume = 28 | author = Gordon K. Anderson, Minren Lin | doi = 10.1002/9780470132593.ch13 | year = 1990}} 3. ^{{OrgSynth | title = Palladium-catalyzed reaction of 1-alkenylboronates with vinylic halides: (1Z,3E)-1-Phenyl-1,3-octadiene | collvol = 8 | collvolpages = 532 | author = Norio Miyaura and Akira Suzuki | year = 1993 | prep = cv8p0532}} 4. ^{{cite journal | journal = Inorg. Synth. | volume = 13 | pages = 121 | title = 23. Tetrakis(triphenylphosphine)palladium(0) | author = D. R. Coulson | doi = 10.1002/9780470132449.ch23 | year = 1972 | last2 = Satek | first2 = L. C. | last3 = Grim | first3 = S. O.}} 5. ^1 {{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 | url = https://books.google.com/books?id=mTMA2hExAaIC&pg=PA47 | format = Google Books excerpt}} 6. ^{{OrgSynth | title = Palladium Catalysts | author = Ralph Mozingo | collvol = 3 | collvolpages = 685 | year = 1955 | prep = cv3p0685}} 7. ^For example, http://www.marinecare.nl/assets/Uploads/Downloads/Leaflet-Passivation-Test-Kit.pdf{{dead link|date=March 2018 |bot=InternetArchiveBot |fix-attempted=yes }} 8. ^{{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}} 3 : Palladium compounds|Chlorides|Metal halides |
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