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Barium peroxide

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Barium peroxide
Names
IUPAC name
barium peroxide
Other names
Barium binoxide,
Barium dioxide,
Barium superoxide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.013.754 Edit this at Wikidata
EC Number
  • 215-128-4
RTECS number
  • CR0175000
  • InChI=1S/Ba.O2/c;1-2/q+2;-2 checkY
    Key: ZJRXSAYFZMGQFP-UHFFFAOYSA-N checkY
  • InChI=1/Ba.O2/c;1-2/q+2;-2
    Key: ZJRXSAYFZMGQFP-UHFFFAOYAZ
  • [Ba+2].[O-][O-]
Properties
BaO2
Molar mass 169.33 g/mol
Appearance Grey-white crystalline solid
Density 5.68 g/cm3
Melting point 450 °C (723 K)
Boiling point 800 °C (1073 K) (decomp. to BaO & O2)
insoluble [1]
Structure
Tetragonal [2]
D174h, I4/mmm, tI6
6
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g. hydrogen peroxideSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
3
0
3
OX
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Barium peroxide is the chemical compound with the formula BaO2. This grey-white solid is one of the most common inorganic peroxides. Barium peroxide is an oxidizing agent, which is used for bleaching. It is used in fireworks as an oxidizer,[3] which also gives a vivid green colour, as do all barium compounds.

Barium peroxide is a peroxide, containing O22− subunits wherein the oxygen atoms bond to each other as well as to the barium. The solid adopts the same structure as calcium carbide, CaC2.

Barium peroxide arises by the reversible absorption of O2 by barium oxide. The oxygen is released above 500°C.

2 BaO + O2 ⇌ 2 BaO2

This reaction is the basis for the now-obsolete Brin process for separating oxygen from the atmosphere. Other oxides, e.g. Na2O, behave similarly.[4]

Hydrogen peroxide can also be prepared via the related reaction:

BaO2 + H2SO4 → H2O2 + BaSO4

The insoluble barium sulfate is filtered from the mixture.

Footnotes

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
  2. ^ Massalimov, I. A.; Kireeva, M. S.; Sangalov, Yu. A. (2002). Inorganic Materials. 38 (4): 363. doi:10.1023/A:1015105922260. {{cite journal}}: Missing or empty |title= (help)
  3. ^ "Data Sheet". Data Sheet. Hummel Croton Inc. Retrieved 2007-02-01.
  4. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.

See also


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