In chemistry, peroxycarbonate (sometimes peroxocarbonate, IUPAC name: oxocarbonate or oxidocarbonate) or percarbonate is a divalent anion with formula CO2−
4. It is an oxocarbon anion that consists solely of carbon and oxygen. It would be the anion of a hypothetical peroxycarbonic acid HO−CO−O−OH (sometimes peroxocarbonic acid).[1][2] or the real hydroperoxyformic acid, HO−O−CO−OH (a.k.a. percarbonic acid, carbonoperoxoic acid, hydroxycarbonic acid).
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| Names | |
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| Preferred IUPAC name
Oxidocarbonate | |
| Systematic IUPAC name
Oxocarbonate | |
| Other names
Peroxycarbonate (Peroxocarbonate)
Percarbonate Peroxidocarboxylate Peroxidoformate Dioxidan-2-idecarboxylate | |
| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| CO42− | |
| Molar mass | 76.01 g/mol |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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The peroxycarbonate anion is formed, together with peroxydicarbonate C2O2−6, at the negative electrode during electrolysis of molten lithium carbonate.[3] Lithium peroxycarbonate can be produced also by combining carbon dioxide CO2 with lithium hydroxide in concentrated hydrogen peroxide H2O2 at −10 °C.[4]
Electrolysis of a solution of lithium carbonate at -30° to -40 °C yields a solution of the Lithium percarbonate, which can liberate iodine from potassium iodide instantaneously. The crystalline salt has not been isolated.
The peroxycarbonate anion has been proposed as an intermediate to explain the catalytic effect of CO2 on the oxidation of organic compounds by O2.[5]
The potassium and rubidium salts of the monovalent hydrogenperoxycarbonate anion (aka. hydroxycarbonate, biperoxycarbonate) H−O−O−CO−2 have also been obtained.[6][7][8][9]
See also
edit- Sodium percarbonate, actually a perhydrate of sodium carbonate.
- Sodium peroxycarbonate
- Orthocarbonate anion CO4−
4 - Dipropyl peroxydicarbonate
References
edit- ^ Riesenfeld, E. H.; Reinhold, B. (1909). "Die Existenz echter Percarbonate und ihre Unterscheidung von Carbonaten mit Krystall-Wasserstoffsuperoxyd". Berichte der Deutschen Chemischen Gesellschaft. 42 (4): 4377–4383. doi:10.1002/cber.19090420428.
- ^ Riesenfeld, E. H.; Mau, W. (1911). "Isomere Percarbonate". Berichte der Deutschen Chemischen Gesellschaft. 44 (3): 3595–3605. doi:10.1002/cber.191104403244.
- ^ Chen, Li-Jiang; Lin, Chang-Jian; Zuo, Juan; Song, Ling-Chun; Huang, Chao-Ming (2004). "First Spectroscopic Observation of Peroxocarbonate/ Peroxodicarbonate in Molten Carbonate". The Journal of Physical Chemistry B. 108 (23): 7553–7556. doi:10.1021/jp035749l.
- ^ Firsova, T. P.; Kvlividze, V. I.; Molodkina, A. N.; Morozova, T. G. (1975). "Synthesis and some properties of lithium peroxocarbonate". Bulletin of the Academy of Sciences of the USSR, Division of Chemical Science. 24 (6): 1318–1319. doi:10.1007/BF00922073.
- ^ Park, Sang-Eon; Yoo, Jin S. (2004), "New CO2 chemistry – Recent advances in utilizing CO2 as an oxidant and current understanding on its role", Studies in Surface Science and Catalysis, Carbon Dioxide Utilization for Global Sustainability, 153, Elsevier: 303–314, doi:10.1016/s0167-2991(04)80269-6, ISBN 9780444516008
- ^ Mimoza Gjikaj (2001), "Darstellung und strukturelle Charakterisierung neuer Alkali- bzw. Erdalkalimetallperoxide, -hydrogenperoxide, -peroxocarbonate und -peroxohydrate" Archived 2012-02-25 at the Wayback Machine. Doctoral Thesis, University of Köln. 115 pages.
- ^ Adam, Arnold; Mehta, Mathias (1998). "KH(O2)CO2·H2O2—An Oxygen-Rich Salt of Monoperoxocarbonic Acid". Angewandte Chemie International Edition. 37 (10): 1387–1388. doi:10.1002/(SICI)1521-3773(19980605)37:10<1387::AID-ANIE1387>3.0.CO;2-3. ISSN 1521-3773. PMID 29710903.
- ^ M. Mehta and A. Adam (1998), Z. Kristallogr., Suppl. Issue 15 p. 53. Cited by Gjikaj.
- ^ M. Mehta and A. Adam (1998), Z. Kristallogr., Suppl. Issue 15 p. 46. Cited by Gjikaj.
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