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Copper(II) oxalate are inorganic compounds with the chemical formula CuC2O4(H2O)x. The value of x can be 0, 0.44, and 1. Two of these species are found as secondary minerals (degradation of minerals), whewellite (monohydrate and moolooite (0.44 hydrate).[3] The anhydrous compound has been characterized by X-ray crystallography.[4] Many transition metal oxalate complexes are known.

Copper(II) monooxalates are practically insoluble in all solvents. They are coordination polymers.[5]

Synthesis

Copper(II) oxalate can be produced by precipitation from acidified aqueous copper(II) salts and oxalic acid.[6][7]

CuSO4 + H2C2O4 + H2O → CuC2O4·H2O + H2SO4

Reactions

Upon heating to 130 °C, the hydrated copper(II) oxalates convert to the anhydrous cupric oxalate. Further heating at higher temperatures under an atmosphere of hydrogen gives copper metal, suitable as a reagent.[6]

The hydrates bind Lewis bases.

Hydrated copper(II) oxalate reacts with alkali metal oxalates and ammonium oxalate to give bis(oxalato)cuprate:[8]

CuC2O4)(H2O)x + C2O2−4 → [Cu(C2O4)2]2− + x H2O

Uses

Copper oxalate is used as a catalyst for organic reactions, as a stabilizer for acetylated polyformaldehyde.[9][10]

Related compounds

  • Cuprous oxalates.[11]

References

  1. ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
  2. ^ "Copper oxalate - Substance Information - ECHA". European Chemical Agency. Retrieved 17 June 2021.
  3. ^ Christensen, Axel Nørlund; Lebech, Bente; Andersen, Niels Hessel; Grivel, Jean-Claude (2014). "The Crystal structure of paramagnetic copper(<SCP>ii</SCP>) oxalate (CuC2O4): Formation and thermal decomposition of randomly stacked anisotropic nano-sized crystallites" (PDF). Dalton Trans. 43 (44): 16754–16768. doi:10.1039/C4DT01689K.
  4. ^ Schmittler, H. (1968). "Zum Strukturprinzip des fehlgeordneten Kupfer(II)-Oxalats CuC2O4·nH2O". Monatsberichte der Deutschen Akademie der Wissenschaften zu Berlin. 10: 581-604.
  5. ^ "Hazardous Substances Data Bank (HSDB) : 265". National Library of Medicine. Retrieved 17 June 2021.
  6. ^ a b O. Glemser; R. Sauer (1963). "Copper(II) Sulfide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=1017-1018. NY,NY: Academic Press.
  7. ^ Gooch, Frank Austin (1909). The precipitation of copper oxalate in analysis. p. 448. OCLC 890741677.
  8. ^ Kirschner, Stanley; McLean, John A.; Meerman, Gerardine (1960). "Potassium Dioxalatocuprate(II) 2-Hydrate". Inorganic Syntheses. Vol. 6. pp. 1–2. doi:10.1002/9780470132371.ch1. ISBN 978-0-470-13165-7.
  9. ^ Richardson, H. Wayne (1997). Handbook of Copper Compounds and Applications. CRC Press. p. 84. ISBN 978-0-8247-8998-5.
  10. ^ Richardson, H. Wayne (2000). "Copper Compounds". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a07_567. ISBN 978-3-527-30385-4.
  11. ^ Royappa, A. Timothy; Royappa, Andrew D.; Moral, Raphael F.; Rheingold, Arnold L.; Papoular, Robert J.; Blum, Deke M.; Duong, Tien Q.; Stepherson, Jacob R.; Vu, Oliver D.; Chen, Banghao; Suchomel, Matthew R.; Golen, James A.; André, Gilles; Kourkoumelis, Nikolaos; Mercer, Andrew D.; Pekarek, Allegra M.; Kelly, Dylan C. (November 2016). "Copper(I) oxalate complexes: Synthesis, structures and surprises". Polyhedron. 119: 563–574. doi:10.1016/j.poly.2016.09.043.
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