Tetrakis(acetonitrile)copper(I) hexafluorophosphate

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Tetrakis(acetonitrile)copper(I) hexafluorophosphate
Tetrakis(acetonitrile)copper(I) hexafluorophosphate.png
Tetrakis(acetonitrile)copper(I) hexafluorophosphate 3D spacefill.png
Names
IUPAC name
Tetrakis(acetonitrile)copper(I) hexafluorophosphate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.198.153 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 672-617-9
PubChem CID
  • InChI=1S/4C2H3N.Cu.F6P/c4*1-2-3;;1-7(2,3,4,5)6/h4*1H3;;/q;;;;+1;-1
    Key: GNQXUMGHBSAQBV-UHFFFAOYSA-N
  • CC#N.CC#N.CC#N.CC#N.F[P-](F)(F)(F)(F)F.[Cu+]
Properties
[Cu(CH3CN)4]PF6
Molar mass 372.7198 g/mol
AppearanceWhite powder
Melting point 160 °C (320 °F; 433 K)
Hazards
GHS labelling:
GHS-pictogram-exclam.svg
Warning
H315, H319, H335
P261, P264, P264+P265, P271, P280, P302+P352, P304+P340, P305+P351+P338, P319, P321, P332+P317, P337+P317, P362+P364, P403+P233, P405, P501
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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]

Contents

Structure

As confirmed by X-ray crystallographic studies, the copper(I) ion is coordinated to four almost linear acetonitrile ligands in a nearly ideal tetrahedral geometry. [2] [3] Similar complexes with other anions including the perchlorate, tetrafluoroborate, and nitrate are known. [1]

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. [4] [Cu(CH3CN)4]PF6 is generally produced by the addition of HPF6 to a suspension of copper(I) oxide in acetonitrile: [5]

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. [5]

Reactions and applications

The acetonitrile ligands protect the Cu+ ion from oxidation to Cu2+, but are rather poorly bound: with other counterions, the complex forms di- [1] and tri-acetonitrilo [6] complexes and is also a useful source of unbound Cu(I). [5]

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

See also

References

  1. 1 2 3 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 (1): 314–317. Bibcode:1975AcCrB..31..314C. doi:10.1107/S0567740875002634.
  3. ↑ Black, J. R.; Levason, W.; Webster, M. (1995). "Tetrakis(acetonitrile-N)copper(I) Hexafluorophosphate(V) Acetonitrile Solvate". Acta Crystallographica Section C Crystal Structure Communications. 51 (4): 623–625. Bibcode:1995AcCrC..51..623B. doi:10.1107/S0108270194012527.
  4. ↑ 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.
  5. 1 2 3 Kubas, G.J. (1990). "Tetrakis(Acetonitrile)Copper(1+) Hexafluorophosphate(1-)". Inorganic Syntheses. Inorganic Syntheses. Vol. 28. pp. 68–69. doi:10.1002/9780470132593.ch15. ISBN   978-0-471-52619-3.
  6. ↑ Elsayed Moussa, Mehdi; Piesch, Martin; Fleischmann, Martin; Schreiner, Andrea; Seidl, Michael; Scheer, Manfred (2018). "Highly soluble Cu(i)-acetonitrile salts as building blocks for novel phosphorus-rich organometallic-inorganic compounds" (PDF). Dalton Transactions. 47 (45): 16031–16035. doi:10.1039/C8DT03723J. PMID   30321246.
  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 (2): 227. Bibcode:1980HydMe...5..227P. doi:10.1016/0304-386X(80)90041-9.
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