Barium peroxide

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Barium peroxide
Peroxid barnaty.JPG
BaO2structure.jpg
  Barium cations Ba2+
  Peroxide anions O2−2
Names
IUPAC name
barium peroxide
Other names
Barium binoxide,
Barium dioxide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.013.754 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 215-128-4
PubChem CID
RTECS number
  • CR0175000
UNII
UN number 1449
  • InChI=1S/Ba.O2/c;1-2/q+2;-2 Yes check.svgY
    Key: ZJRXSAYFZMGQFP-UHFFFAOYSA-N Yes check.svgY
  • 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 (anhydrous)
313.45 g/mol (octahydrate)
AppearanceGrey-white crystalline solid (anhydrous)
Colorless solid (octahydrate)
Odor Odorless
Density 5.68 g/cm3 (anhydrous)
2.292 g/cm3 (octahydrate)
Melting point 450 °C (842 °F; 723 K)
Boiling point 800 °C (1,470 °F; 1,070 K) (decomposes to BaO & O2. [1] )
0.091 g/(100 mL) (20 °C) (anhydrous)
0.168 g/cm3 (octahydrate)
Solubility dissolves with decomposition in acid
−40.6·10−6 cm3/mol
Structure
Tetragonal [2]
D174h, I4/mmm, tI6
6
Hazards
GHS labelling:
GHS-pictogram-rondflam.svg GHS-pictogram-exclam.svg
Warning
H272, H302, H332
P210, P220, P221, P261, P264, P270, P271, P280, P301+P312, P304+P312, P304+P340, P312, P330, P370+P378, P501
NFPA 704 (fire diamond)
NFPA 704.svgHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
3
0
2
OX
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Yes check.svgY  verify  (what is  Yes check.svgYX mark.svgN ?)

Barium peroxide is an inorganic compound with the formula Ba O 2. This white solid (gray when impure) is one of the most common inorganic peroxides, and it was the first peroxide compound discovered. Being an oxidizer and giving a vivid green colour upon ignition (as do all barium compounds), it finds some use in fireworks; historically, it was also used as a precursor for hydrogen peroxide. [3]

Contents

Structure

Barium peroxide consists of barium cations Ba2+ and peroxide anions O2−2. The solid is isomorphous to calcium carbide, CaC2.

Preparation and use

Barium peroxide arises by the reversible reaction of O2 with barium oxide. The peroxide forms around 500 °C and oxygen is released above 820 °C. [1]

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 and SrO, behave similarly. [4]

In another obsolete application, barium peroxide was once used to produce hydrogen peroxide via its reaction with sulfuric acid: [3]

BaO2 + H2SO4 → H2O2 + BaSO4

The insoluble barium sulfate is filtered from the mixture.

Footnotes

  1. 1 2 Accommodation of Excess Oxygen in Group II Monoxides - S.C. Middleburgh, R.W. Grimes and K.P.D. Lagerlof Journal of the American Ceramic Society 2013, Volume 96, pages 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.
  3. 1 2 Harald Jakob; Stefan Leininger; Thomas Lehmann; Sylvia Jacobi; Sven Gutewort. "Peroxo Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry . Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_177.pub2. ISBN   978-3-527-30673-2.
  4. ↑ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN   0-12-352651-5.

See also

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