Movatterモバイル変換

[0]ホーム
URL:

Jump to content
WikipediaThe Free Encyclopedia
Search

Strontium peroxide

From Wikipedia, the free encyclopedia
Strontium peroxide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard100.013.841Edit this at Wikidata
EC Number
  • 215-224-6
UNII
UN number1509 (STRONTIUM PEROXIDE)
  • Key: UHCGLDSRFKGERO-UHFFFAOYSA-N
  • InChI=1S/O2.Sr/c1-2;/q-2;+2
  • [O-] [O-].[Sr+2]
Properties
SrO2
Molar mass119.619 g/mol
Appearancewhite powder
Odorodorless
Density4.56 g/cm3 (anhydrous) 1.91 g/cm3 (octahydrate)
Melting point215 °C (419 °F; 488 K) (decomposes)[1]
slightly soluble
Solubilityvery soluble inalcohol,ammonium chloride
insoluble inacetone
Structure
Tetragonal[2]
D174h, I4/mmm,tI6
6
Hazards
GHS labelling:
GHS03: OxidizingGHS05: CorrosiveGHS07: Exclamation mark[3]
Danger
H302,H312,H317,H331,H350
P220,P261,P280,P305+P351+P338
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)
Chemical compound

Strontium peroxide is aninorganic compound with the formulaSrO2 that exists in both anhydrous and octahydrate form, both of which are white solids. The anhydrous form adopts a structure similar to that ofcalcium carbide.[4][5]

Uses

[edit]

It is anoxidizing agent used forbleaching. It is used in somepyrotechnic compositions as an oxidizer and a vivid redpyrotechnic colorant. It can also be used as anantiseptic and in tracer munitions.[citation needed]

Production

[edit]

Strontium peroxide is produced by passing oxygen over heatedstrontium oxide. Upon heating in the absence of O2, it degrades to SrO and O2. It is more thermally labile than BaO2.[6][7]

References

[edit]
  1. ^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.
  2. ^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.
  3. ^"Strontium Peroxide".American Elements. RetrievedMarch 7, 2019.
  4. ^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.
  5. ^Natta, G. "Structure of hydroxides and hydrates. IV. Octahydrated strontium peroxide" Gazzetta Chimica Italiana (1932), 62, 444-56.
  6. ^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.
  7. ^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

[edit]

External links

[edit]
Compounds of theperoxide ion
H2O2He
Li2O2BeBCNOO2F2
O4F2		Ne
Na2O2MgO2AlSiPH2OSClOOCl
Cl2O5		Ar
K2O2CaO2ScTiVCrO(O2)2MnFeCoNiCuO2ZnO2GaGeAsSeBrKr
Rb2O2SrO2YZrNbMoTcRuRhPdAgCdInSnSbTeIXe
Cs2O2BaO2*LuHfTaWReOsIrPtAuHgTlPbBiPoAtRn
FrRa**LrRfDbSgBhHsMtDsRgCnNhFlMcLvTsOg
 
*LaCePrNdPmSmEuGdTbDyHoErTmYb
**AcThPaUO4·nH2ONpPuAmCmBkCfEsFmMdNo
Authority control databasesEdit this at Wikidata
Retrieved from "https://en.wikipedia.org/w/index.php?title=Strontium_peroxide&oldid=1300699001"
Categories:
Hidden categories:
[8]ページ先頭
©2009-2025 Movatter.jp