Palladium(II) acetate

Palladium(II) acetate
Names
IUPAC name
Palladium(II) acetate
Other names
Palladium diacetate
hexakis(acetato)tripalladium
bis(acetato)palladium
Identifiers
3375-31-3 YesY
3D model (Jmol) Interactive image
ChemSpider 146827 YesY
ECHA InfoCard 100.020.151
PubChem 167845
RTECS number AJ1900000
Properties
Pd(CH3COO)2
Molar mass 224.50 g/mol
Appearance Brown yellow solid
Density 2.19 g/cm3
Melting point 205 °C (401 °F; 478 K) decomposes
Boiling point decomposes
low
Structure
monoclinic
Square Planar
0 D
Hazards
Main hazards considered nonhazardous
Safety data sheet
R-phrases 41
S-phrases 24/25
Related compounds
Other anions
 Palladium(II) chloride
Other cations
 Platinum(II) acetate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Palladium(II) acetate is a chemical compound of palladium described by the formula Pd(O2CCH3)2 or Pd(OAc)2. It is considered more reactive than the analogous platinum compound. It is soluble in many organic solvents, and commonly used as a catalyst for organic reactions and as a precursor for the synthesis of other palladium catalysts.

Structure

Although the compound is a 1:2 stoichiometric ratio of palladium atoms and acetate ligands as their oxidation states suggest, the actual molecular nature of the chemical depends on how it is prepared.

As prepared by Wilkinson and coworkers in 1965, and later studied by Skapski and Smart in 1970 by single crystal X-ray diffraction, palladium(II) acetate is a red-brown solid that crystallizes as monoclinic plates. Its structure was determined to be trimeric, consisting of an equilateral triangle of Pd atoms each pair of which is bridged with two acetate groups in a butterfly conformation. Each metal atom achieves approximate square planar co-ordination.[1][2]

On the other hand, palladium(II) acetate prepared in a slightly different way was isolated as a pale pink powder, whose structure was determined by X-ray powder diffraction to consist of infinite chains of palladium atoms, each linked by an adjacent pair of acetate bridges to the next, in which the coordination geometry around each Pd is true square planar.[3]

Preparation

Palladium acetate, in trimeric form, can be prepared by refluxing palladium sponge with hot glacial acetic acid and nitric acid. An excess of palladium sponge metal or nitrogen gas flow is used to prevent contamination by a material that contains a nitrite ligand in place of one of the acetates (Pd3(OAc)5NO2).[4][5]

Pd + 4 HNO3 → Pd(NO3)2 + 2 NO2 + 2 H2O
Pd(NO3)2 + 2 CH3COOH → Pd(O2CCH3)2 + 2 HNO3

The nitro variant has different solubility and catalytic activity in some reactions. Preventing, or controlling for the amount of, this impurity can be an important aspect for reliable use of palladium(II) acetate.[6]

Palladium(II) propionate is prepared analogously; other carboxylates are prepared by reacting palladium(II) acetate with the appropriate carboxylic acid.[1] Likewise, palladium(II) acetate can be prepared by reacting other palladium(II) carboxylates with acetic acid. This ligand exchange starting with a purified other carboxylate is an alternative way to synthesize palladium(II) acetate free from the nitro contaminant.[6]

Reactions

When warmed with alcohols, or on prolonged boiling with other solvents, palladium(II) acetate decomposes to palladium.[1]

Uses

Catalysis

Palladium acetate is a catalyst for many organic reactions by combining with many common classes of organic compounds such as alkenes, dienes, and alkyl, aryl, and vinyl halides to form reactive adducts. Alkenes and π-allyl coordination to palladium(II) acetate involves sigma-type donation from the pi orbital of the alkene or π-allyl with concomitant pi-backbonding into an empty pi* orbital on the alkene or π-allyl. The greater the sigma donation to the metal is, the greater the pi-backbonding. The greater the pi-backbonding is, the greater the reduction in the bond order of the alkene or π-allyl.[7] Reduction of the alkenes or π-allyl by coordination to palladium(II) acetate reverses the reactivity of the organic ligand allowing them to undergo reactions with nucleophiles rather than electrophiles.[8]

Examples of palladium(II) acetate catalyzed reactions are:

Pd(O2CCH3)2 converts aryl bromides into aryltrimethylsilanes, an important functional group in many organic compounds including the fungicide "Latitude".

RC6H4Br + Si2(CH3)6 → RC6H4Si(CH3)3 + Si(CH3)3Br

Pd(O2CCH3)2 is compatible with the electronic properties of aryl bromides, and unlike other methods of synthesis, this method does not require high pressure equipment.[12]

Precursor to other Pd compounds

Palladium acetate is used to produce other palladium(II) compounds. For example, phenylpalladium acetate, used to isomerize allylic alcohols to aldehydes, is prepared by the following reaction:

Hg(C6H5)(CH3COO) + Pd(CH3COO)2 → Pd(C6H5)(O2CCH3) + Hg(O2CCH3)2[13]

Palladium(II) acetate reacts with acetylacetone (the "acac" ligand) to produce Pd(acac)2, a monomeric molecule that is a precursor to Pd(0).

Light or heat reduce palladium acetate to give thin layers of palladium and can produce nanowires and colloids.[4]

See also

References

  1. 1 2 3 T. A. Stephenson; S. M. Morehouse; A. R. Powell; J. P. Heffer and G. Wilkinson (1965). "667. Carboxylates of palladium, platinum, and rhodium, and their adducts". Journal of the Chemical Society (Resumed): 3632. doi:10.1039/jr9650003632.
  2. ↑ Skapski, A C.; M. L. Smart (1970). "The Crystal Structure of Trimeric Palladium(II) Acetate". J. Chem. Soc. D (11): 658b–659. doi:10.1039/C2970000658b.
  3. ↑ Kirik, S.D.; Mulagaleev, S.F.; Blokhin, A.I. (2004). "[Pd(CH 3 COO) 2 ] n from X-ray powder diffraction data". Acta Crystallogr. C. 60 (9): m449–m450. doi:10.1107/S0108270104016129.
  4. 1 2 Bakhmutov, V. I.,; Berry, J. F.; Cotton, F. A.; Ibragimov, S.; Murillo, C. A. (2005). "Non-Trivial Behavior of Palladium(II) Acetate". Dalton Transactions (11): 1989–1992. doi:10.1039/b502122g. PMID 15909048.
  5. ↑ "High Purity Homogeneous Catalyst" (PDF). Engelhard. September 2005. Archived from the original (PDF) on 17 March 2006. Retrieved 24 February 2006.
  6. 1 2 Ritter, Stephen K. (May 2, 2016). "Chemists introduce a user's guide for palladium acetate". Chemical & Engineering News. 94 (18): 20–21.
  7. ↑ Toreki, R. "Allyl Ligands." The Organometallic HyperTextBook. 20 Nov. 2003. Chemglass. 01 Apr. 2006<http://www.ilpi.com/organomet/allyl.html>.
  8. ↑ Suggs, J W. "Palladium: Organometallic Chemistry." Encyclopedia of Inorganic Chemistry. Ed. R B. King. 8 vols. Chichester: Wiley, 1994.
  9. ↑ Nikitin, Kirill V.; Andryukhova, N.P.; Bumagin, N.A.; Beletskaya, I.P. (1991). "Synthesis of Aryl Esters by Pd-catalysed Carbonylation of Aryl Iodides". Mendeleev Communications. 1 (4): 129–131. doi:10.1070/MC1991v001n04ABEH000080.
  10. ↑ Basu, B., Satadru J., Mosharef H. B., and Pralay D. (2003). "A Simple Protocol for the Direct Reductive Amination of Aldehydes and Ketones Using Potassium Formate and Catalytic Palladium Acetate". ChemInform. 34 (30): 555–557. doi:10.1002/chin.200330069.
  11. ↑ "Buchwald-Hartwig Cross Coupling Reaction". Organic Chemistry Portal.
  12. ↑ Gooben, L J. "Research Area "New Pd-Catalyzed Cross-Coupling Reactions"" 28 Feb. 2006<http://www.mpi-muelheim.mpg.de/kofo/bericht2002/pdf/2.1.8_gossen.pdf> Archived July 12, 2007, at the Wayback Machine..
  13. ↑ Richard F. Heck. "Aldehydes from Allylic Alcohols and Phenylpalladium Acetate: 2-Methyl-3-Phenylpropionaldehyde". Org. Synth.; Coll. Vol., 6, p. 815
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