Cobalt(II) oxalate

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Cobalt(II) oxalate
Cobalt (II) oxalate.jpg
Cobalt(II)-oxalate-dihydrate-from-xtal-2005-CM-3D-balls.png
Identifiers
3D model (JSmol)
ChemSpider
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PubChem CID
UNII
  • InChI=1S/C2H2O4.Co/c3-1(4)2(5)6;/h(H,3,4)(H,5,6);/q;+2/p-2 X mark.svgN
    Key: MULYSYXKGICWJF-UHFFFAOYSA-L X mark.svgN
  • InChI=1/C2H2O4.Co/c3-1(4)2(5)6;/h(H,3,4)(H,5,6);/q;+2/p-2
    Key: MULYSYXKGICWJF-NUQVWONBAF
  • C(=O)(C(=O)[O-])[O-].[Co+2]
Properties
CoC2O4
Molar mass 146.9522 g/mol
Appearancegray/pink powder
Odor odorless
Density 3.01 g/cm3
Melting point 250 °C (482 °F; 523 K) (decomposes)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Cobalt(II) oxalate is the inorganic compound with the formula of CoC2O4. Like other simple inorganic oxalates, it is a coordination polymer. The oxalate ligands bridge of Co(OH2)2 centres. Each cobalt adopts octahedral coordination geometry. [1]

It is used in the preparation of cobalt catalysts, and cobalt metal powder for powder-metallurgical applications. It is made in process of recycling lithium-ion batteries, where the cobalt is obtained from cathode material (LiCoO2) by leaching with sulfuric acid and then precipitated with ammonium oxalate. [2]

Many cobalt(III) oxalate complexes are known, including [Co(C2O4)3]3- and [Co(C2H4(NH2)2)C2O4)2]−. [3] [4]

References

  1. ↑ Bacsa, J.; Eve, D.; Dunbar, K. R. (2005). "catena-Poly[[diaquacobalt(II)]-μ-oxalato]". Acta Crystallogr. C . 61 (Pt 1): m58 –m60. Bibcode:2005AcCrC..61M..58B. doi:10.1107/S0108270104030409. PMID   15640580.
  2. ↑ Meng, Qi; Zhang, Yingjie; Dong, Peng (2018). "A combined process for cobalt recovering and cathode material regeneration from spent LiCoO2 batteries: Process optimization and kinetics aspects" . Waste Management. 71: 372–380. doi:10.1016/j.wasman.2017.10.030.
  3. ↑ Kauffman, George B.; Takahashi, Lloyd T.; Sugisaka, Nobuyuki (1966). "Resolution of the Trioxalatocobaltate(III) Ion". Inorganic Syntheses. Vol. 8. pp. 207–211. doi:10.1002/9780470132395.ch55. ISBN   978-0-470-13167-1.
  4. ↑ Worrell, J. H.; Kipp, E. B. (1972). "Resolution of the (Ethylenediamine)bis(oxalato)cobaltate(III) Ion". Inorganic Syntheses. Vol. 13. pp. 195–202. doi:10.1002/9780470132449.ch40. ISBN   978-0-470-13172-5.


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