Strontium peroxide

Strontium peroxide
Identifiers
CAS Number	1314-18-7 ;
3D model (JSmol)	Interactive image;
ECHA InfoCard	100.013.841
EC Number	215-224-6;
PubChem CID	14807;
UNII	E0830P344P ;
CompTox Dashboard (EPA)	DTXSID80905100 ;
	InChI InChI=1S/O2.Sr/c1-2;/q-2;+2;
	SMILES [O-] [O-].[Sr+2];
Properties
Chemical formula	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)
Solubility in water	slightly soluble
Solubility	very soluble in alcohol, ammonium chloride ; insoluble in acetone
Structure
Crystal structure	Tetragonal
Space group	D174h, I4/mmm, tI6
Coordination geometry	6
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H302, H312, H317, H331, H350
Precautionary statements	P220, P261, P280, P305+P351+P338
Safety data sheet (SDS)	External SDS
	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

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. S2CID 91881752.
^ "Strontium Peroxide". American Elements. 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

Uses

Production

References

See also