Potassium tetraperoxochromate(V)

Chemical compound

Potassium tetraperoxochromate(V)

Names
IUPAC name

Potassium tetraperoxochromate(V)

Other names

* Potassium perchromate
* Potassium peroxochromate

Identifiers

CAS Number

* 12331-76-9 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 106513

PubChem CID

* 139134081

CompTox Dashboard (EPA)

* DTXSID5059531

InChI

* InChI=1S/Cr.3K.4O2/c;;;;4*1-2/q+5;3*+1;4*-2

Key: JSURYJVAXIVWCV-UHFFFAOYSA-N

SMILES

* [O-][O-].[O-][O-].[O-][O-].[O-][O-].[K+].[K+].[K+].[Cr+5]

Properties

Chemical formula

| K3[Cr(O2)4]
Molar mass | 297.286 g/mol
Appearance  | black
Melting point | 70 °C (158 °F; 343 K)[1] (decomposes)

Solubility in water

| 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).

Y verify (what is YN ?)

Infobox references

Chemical compound

Potassium peroxochromate, potassium tetraperoxochromate(V), or simply potassium perchromate, is an inorganic compound having the chemical formula K3[Cr(O2)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

[edit]

Potassium peroxochromate is prepared by treating potassium chromate with hydrogen peroxide at 0 °C:

2 CrO2−4 \+ 8 H2O2 → 2 [Cr(O2)4]2− \+ 8 H2O

The intermediate tetraperoxochromate(VI) is reduced by hydrogen peroxide, forming tetraperoxochromate(V):[3][4]

2 [Cr(O2)4]2− \+ 2 OH− \+ H2O2 → 2 [Cr(O2)4]3− \+ 2 H2O + O2

Thus, the overall reaction is:

2 CrO2−4 \+ 9 H2O2 \+ 2 OH− → 2 [Cr(O2)4]3− \+ 10 H2O + O2

The compound decomposes spontaneously at higher temperatures.

## References

[edit]

1. ^ a b c John W. Peters; Paul J. Bekowies; Arthur M. Winer; James N. Pitts Jr. (1975). "Potassium perchromate as a source of singlet oxygen". Journal of the American Chemical Society. 97 (12). ACS Publications: 3299–3306\. doi:10.1021/ja00845a003.
2. ^ 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\. Bibcode:2007CryRp..52..639S. doi:10.1134/S1063774507040116. S2CID 95018505.
3. ^ Haxhillazi, Gentiana. "Preparation, Structure and Vibrational Spectroscopy of Tetraperoxo Complexes of CrV+, VV+, NbV+ and TaV+". Archived from the original on 2011-07-18. Retrieved 2009-03-07.
4. ^ 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.

* v
* t
* e

Chromium compounds

Chromium(0)|

* Cr(CO)6

| Organochromium(0) compounds|

* Cr(C6H6)2
* CrC6H6(CO)3

|

Chromium(I)|

* CrH

| Organochromium(I) compounds|

* Cr2(C5H5)2(CO)6

|

Chromium(II)|

* CrH2
* Cr3C2
* Cr(C2O4)
* Cr(CH3CO2)2
* CrSi2
* CrO
* CrS
* CrSO4
* CrSe
* CrF2
* CrCl2
* CrBr2
* CrI2

| Organochromium(II) compounds|

* Cr(C5H5)2

|

Chromium(II, III)|

* Cr3C2

Chromium(III)|

* CrB
* [Cr3O(CH3CO2)6(H2O)3]+[CH3CO2]−
* CrN
* Cr(NO3)3
* CrPO4
* Cr2O3
* Cr(OH)3
* Cr2S3
* Cr2(SO4)3
* Cr2Te3
* CrF3
* CrCl3
* Cr(ClO4)3
* CrBr3
* CrI3

Chromium(IV)|

* CrSi
* CrO2
* CrF4
* CrCl4
* CrBr4
* CrI4

Chromium(V)|

* K3Cr(O2)4
* CrF5

Chromium(VI)|

* CrO3
* CrO(O2)2
* H2CrO4/H2Cr2O7
* CrO2F2
* CrOF4
* CrO2Cl2
* CrO2Br2
* [C5H5NH]+CrO3Cl−
* CrF6 (hypothetical)

Polyatomic ion|

* Chromate and dichromate

*[CID]: Compound ID
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