Tetrakis(acetonitrile)copper(I) hexafluorophosphate

Tetrakis(acetonitrile)copper(I) hexafluorophosphate is a salt with the formula [Cu(CH3CN)4]PF6. It is a colourless solid that is used in the synthesis of other copper complexes. The cation [Cu(CH3CN)4]+ is a well-known example of a transition metal nitrile complex.[1]

Tetrakis(acetonitrile)copper(I) hexafluorophosphate
Names
IUPAC name
Tetrakis(acetonitrile)copper(I) hexafluorophosphate
Identifiers
ECHA InfoCard 100.198.153
Properties
[Cu(CH3CN)4]PF6
Molar mass 372.7198 g/mol
Appearance White powder
Melting point 160 °C (320 °F; 433 K)
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

Structure

As confirmed by X-ray crystallographic studies, copper(I) ion is coordinated to four almost linear acetonitrile ligands in a nearly ideal tetrahedral geometry.[2][3] Related complexes are known with other anions including the perchlorate, tetrafluoroborate, and nitrate. With the weakly coordinating anion B(C6F5)4−, salts of [Cu(CH3CN)2]+ are obtained.[1]

The acetonitrile ligands protect the Cu+ ion from oxidation to Cu2+. Acetonitrile is not bound very strongly to the copper ion, thus the complex is a useful source of Cu(I). With other counteranions, complexes of [Cu(MeCN)3]+ are observed.[4]

Synthesis

The cation was first reported in 1923 with a nitrate anion as a byproduct of the reduction of silver nitrate with a suspension of copper powder in acetonitrile.[5] [Cu(CH3CN)4]PF6 is generally produced by the addition of HPF6 to a suspension of copper(I) oxide in acetonitrile:[6]

Cu2O + 2 HPF6 + 8 CH3CN → 2 [Cu(CH3CN)4]PF6 + H2O

The reaction is highly exothermic, and may bring the solution to a boil. Upon crystallization, the resulting microcrystals should be white, though a blue tinge is common, indicating the presence of Cu2+ impurities.[6]

Reactions and applications

As the coordinated acetonitrile ligands may be displaced in other solvents, the [Cu(CH3CN)4]PF6 compound may serve as a precursor in the non-aqueous syntheses of other Cu(I) compounds.[6]

Water-immiscible organic nitriles have been shown to selectively extract Cu(I) from aqueous chloride solutions.[7] Through this method, copper can be separated from a mixture of other metals. Dilution of acetonitrile solutions with water induces disproportionation:

2 [Cu(CH3CN)4]+ + 6 H2O → [Cu(H2O)6]2+ + Cu + 8 CH3CN
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References
  1. Silvana F. Rach, Fritz E. Kühn "Nitrile Ligated Transition Metal Complexes with Weakly Coordinating Counteranions and Their Catalytic Applications" Chem. Rev., 2009, volume 109, pp 2061–2080. doi:10.1021/cr800270h
  2. Kierkegaard C.P.; Norrestam R. (1975). "Copper(I) tetraacetonitrile perchlorate". Acta Crystallogr. B. 31: 314–317. doi:10.1107/S0567740875002634.
  3. . doi:10.1107/S0108270194012527. Cite journal requires |journal= (help); Missing or empty |title= (help)
  4. . doi:10.1039/C8DT03723J. Cite journal requires |journal= (help); Missing or empty |title= (help)
  5. Morgan, H.H.; Sand, Henry Julics Salomon (1923). "Preparation and Stability of Cuprous Nitrate and Other Cuprous Salts in the Presence of Nitriles". J. Chem. Soc. 19: 2901. doi:10.1039/CT9232302901.
  6. Kubas, G.J. (1990). "Tetrakis(acetonitirile)copper(I) Hexaflurorophosphate". Inorganic Syntheses. 28: 90–91. doi:10.1002/9780470132593.ch15.
  7. Preston, J.S.; Muhr D.M; Parker A.J. (1980). "Cuprous hydrometallurgy: Part VIII. Solvent extraction and recovery of copper(I) chloride with organic nitriles from an iron(III), copper(II) chloride, two-step oxidative leach of chalcopyrite concentrate". Hydrometallurgy. 5: 227. doi:10.1016/0304-386X(80)90041-9.
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