Strontium peroxide

Strontium peroxide
Identifiers
1314-18-7 YesY
3D model (Jmol) Interactive image
ECHA InfoCard 100.013.841
EC Number 215-224-6
PubChem 14807
Properties
SrO2
Molar mass 119.619 g/mol
Appearance white powder
Odor odorless
Density 4.56 g/cm3 (anhydrous) 1.91 g/cm3 (octahydrate)
Melting point 215 °C (419 °F; 488 K) (decomposes)[1]
slightly soluble
Solubility very soluble in alcohol, ammonium chloride
insoluble in acetone
Structure
Tetragonal [2]
D174h, I4/mmm, tI6
6
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Strontium peroxide is an inorganic compound with the formula SrO2 that exists in both anhydrous and octahydrate form, both of which are white solids. The anhydrous form adopts a structure similar to that of calcium carbide.[3][4]

Uses

It is an oxidizing agent used for bleaching. It is used in some pyrotechnic compositions as an oxidizer and a vivid red pyrotechnic colorant. It can also be used as an antiseptic and in tracer munitions.

Production

Strontium peroxide is produced by passing oxygen over heated strontium oxide. Upon heating in the absence of O2, it degrades to SrO and O2. It is more thermally labilethan BaO2.[5][6]

References

  1. ↑ Accommodation of Excess Oxygen in Group II Monoxides - S.C. Middleburgh, R.W. Grimes, K.P.D. Lagerlof http://onlinelibrary.wiley.com/doi/10.1111/j.1551-2916.2012.05452.x/abstract
  2. ↑ Massalimov, I. A.; Kireeva, M. S.; Sangalov, Yu. A. (2002). Inorganic Materials. 38 (4): 363. doi:10.1023/A:1015105922260. Missing or empty |title= (help)
  3. ↑ Bernal, J. D.; D'yatlova, E.; Kasarnovskii, I.; Raikhstein, S. I.; Ward, A. G. "The structure of strontium and barium peroxides" Zeitschrift für Kristallographie, Kristallgeometrie, Kristallphysik, Kristallchemie (1935), 92, 344-54.
  4. ↑ Natta, G. "Structure of hydroxides and hydrates. IV. Octahydrated strontium peroxide" Gazzetta Chimica Italiana (1932), 62, 444-56.
  5. ↑ Accommodation of Excess Oxygen in Group II Monoxides - S.C. Middleburgh, R.W. Grimes, K.P.D. Lagerlof http://onlinelibrary.wiley.com/doi/10.1111/j.1551-2916.2012.05452.x/abstract
  6. ↑ Bauschlicher, Charles W., Jr.; Partridge, Harry; Sodupe, Mariona; Langhoff, Stephen R. "Theoretical study of the alkaline-earth metal superoxides BeO2 through SrO2" Journal of Physical Chemistry 1992, volume 96, pp. 9259-64. doi:10.1021/j100202a036

See also


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