Copper oxalate

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Copper oxalate
Names
Other names
Copper (II) oxalate, cupric oxalate, copper(2+) ethanedioate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.011.283 Edit this at Wikidata
EC Number
  • 212-411-4
UNII
UN number 3077
  • Key: QYCVHILLJSYYBD-UHFFFAOYSA-N
  • InChI=1S/C2H2O4.Cu/c3-1(4)2(5)6;/h(H,3,4)(H,5,6);/q;+2
  • O=C([O-])C([O-])=O.[Cu+2]
Properties
CuC
2O
4
Molar mass 151.56
Appearance blue solid
Density 6.57 g/cm3
insoluble
4.43×10−10[1]
Hazards
GHS labelling:
GHS07: Exclamation mark[2]
Warning
H302, H302+H312, H312
P264, P270, P280, P301+P312, P302+P352, P312, P322, P330, P363, P501
Related compounds
Related compounds
 Calcium oxalate
Sodium oxalate
Magnesium oxalate
Strontium oxalate
Barium oxalate
Iron(II) oxalate
Iron(III) oxalate
Lithium oxalate
Praseodymium oxalate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Copper(II) oxalate are inorganic compounds with the chemical formula CuC2O4)(H2O)x. The value of x can range from 0 to approximately 0.44 to 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]

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

Synthesis

Copper oxalate can be produced by precipitation from a mixture of a copper (II) salts and a sodium oxalate oroxalic acid.[6]

Reactions

Upon heating, the hydrates convert to the anhydrous cupric oxalate. Further heating gives copper(II) oxide.

The hydrates bind Lewis bases.

The compound forms complex salts with alkali metal oxalates and ammonium oxalate:

CuC2O4)(H2O)x + C2O4(2-) -> [Cu(C2O4)2]2- + x H2O

Uses

Copper oxalate is used as a catalyst for organic reactions, as a stabilizer for acetylated polyformaldehyde[7] and in seed treatment (to repel birds and rodents).[citation needed]

Related compounds

  • Cuprous oxalates.[8]

See also

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. ^ {{cite journal|title=Zum Strukturprinzip des fehlgeordneten Kupfer(II)-Oxalats CuC2O4·nH2O|journal=Monatsberichte der Deutschen Akademie der Wissenschaften zu Berlin|year=1968|volume=10|page= 581-604|author=Schmittler, H.
  5. ^ "Hazardous Substances Data Bank (HSDB) : 265". National Library of Medicine. Retrieved 17 June 2021.
  6. ^ Gooch, Frank Austin (1909). The precipitation of copper oxalate in analysis. p. 448. OCLC 890741677.
  7. ^ Richardson, H. Wayne (1997). Handbook of Copper Compounds and Applications. CRC Press. p. 84. ISBN 978-0-8247-8998-5.
  8. ^ 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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