Chemistry:Strontium peroxide
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3D model (JSmol)
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| 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 | |
| Hazards | |
| Safety data sheet | External SDS |
| GHS pictograms |    [3]
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| GHS Signal word | Danger |
| H302, H312, H317, H331, H350 | |
| P220, P261, P280, P305+351+338 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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Strontium peroxide is an inorganic compound with the formula Sr O2 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.[4][5]
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.[citation needed]
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 labile than BaO2.[6][7]
References
- ↑ Middleburgh, Simon C.; Lagerlof, Karl Peter D.; Grimes, Robin W. (2013). "Accommodation of Excess Oxygen in Group II Monoxides". Journal of the American Ceramic Society 96: 308–311. doi:10.1111/j.1551-2916.2012.05452.x.
- ↑ Massalimov, I. A.; Kireeva, M. S.; Sangalov, Yu. A. (2002). "Structure and Properties of Mechanically Activated Barium Peroxide". Inorganic Materials 38 (4): 363–366. doi:10.1023/A:1015105922260.
- ↑ "Strontium Peroxide". American Elements. https://www.americanelements.com/strontium-peroxide-1314-18-7. Retrieved March 7, 2019.
- ↑ 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.
- ↑ Natta, G. "Structure of hydroxides and hydrates. IV. Octahydrated strontium peroxide" Gazzetta Chimica Italiana (1932), 62, 444-56.
- ↑ Middleburgh, Simon C.; Lagerlof, Karl Peter D.; Grimes, Robin W. (2013). "Accommodation of Excess Oxygen in Group II Monoxides". Journal of the American Ceramic Society 96: 308–311. doi:10.1111/j.1551-2916.2012.05452.x.
- ↑ 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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