Chemistry:Potassium tetraperoxochromate(V)
| |
| Names | |
|---|---|
| IUPAC name
Potassium tetraperoxochromate(V)
| |
Other names
| |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
PubChem CID
|
|
| |
| |
| Properties | |
| K 3[Cr(O 2) 4] | |
| Molar mass | 297.286 g/mol |
| Appearance | red brown |
| Melting point | 70 °C (158 °F; 343 K)[1] (decomposes) |
| Poorly soluble (0 °C) Reacts (45 °C)[1] | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
| |
| Infobox references | |
Potassium peroxochromate, potassium tetraperoxochromate(V), or simply potassium perchromate, is an inorganic compound having the chemical formula K
3[[[Chromium|Cr]](O
2)
4]. It is a red-brown paramagnetic solid. It is the potassium salt of tetraperoxochromate(V), one of the few examples of chromium in the +5 oxidation state and one of the rare examples of a complex stabilized only by peroxide ligands.[2] This compound is used as a source of singlet oxygen.[1]
Preparation
Potassium peroxochromate is prepared by treating potassium chromate with hydrogen peroxide at 0 °C:
- 2 CrO2−
4 + 8 H
2O
2 → 2 [Cr(O
2)
4]2− + 8 H
2O
The intermediate tetraperoxochromate(VI) is reduced by hydrogen peroxide, forming tetraperoxochromate(V):[3][4]
- 2 [Cr(O
2)
4]2− + 2 OH−
+ H
2O
2 → 2 [Cr(O
2)
4]3− + 2 H
2O + O
2
Thus, the overall reaction is:
- 2 CrO2−
4 + 9 H
2O
2 + 2 OH−
→ 2 [Cr(O
2)
4]3− + 10 H
2O + O
2
The compound decomposes spontaneously at higher temperatures.
References
- ↑ 1.0 1.1 1.2 John W. Peters; Paul J. Bekowies; Arthur M. Winer; James N. Pitts Jr. (1975). "Potassium perchromate as a source of singlet oxygen" (in English). Journal of the American Chemical Society (ACS Publications) 97 (12): 3299–3306. doi:10.1021/ja00845a003.
- ↑ Sergienko, V. S. (2007). "Structural chemistry of peroxo compounds of group VI transition metals: I. Peroxo complexes of chromium". Crystallography Reports 52 (4): 639–646. doi:10.1134/S1063774507040116. Bibcode: 2007CryRp..52..639S.
- ↑ Haxhillazi, Gentiana. "Preparation, Structure and Vibrational Spectroscopy of Tetraperoxo Complexes of CrV+, VV+, NbV+ and TaV+". http://deposit.ddb.de/cgi-bin/dokserv?idn=969592612&dok_var=d1&dok_ext=pdf&fi....
- ↑ Riesenfeld, E. H.; Wohlers, H.E.; Kutsch, W.A. (1905). "Höhere Oxydationsproducte des Chroms". Berichte der Deutschen Chemischen Gesellschaft 38 (2): 1885–1898. doi:10.1002/cber.190503802113. https://zenodo.org/record/1426142.
 |  |
