Barium peroxide

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Barium peroxide

  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 Edit this at Wikidata
EC Number
  • 215-128-4
RTECS number
  • CR0175000
UNII
UN number 1449
  • 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 (anhydrous)
313.45 g/mol (octahydrate)
Appearance Grey-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:
GHS03: OxidizingGHS07: Exclamation mark
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 four-colored diamondHealth 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).
checkY verify (what is checkY☒N ?)

Barium peroxide is 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]

Structure

Barium peroxide consists of barium

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. ^
    doi:10.1111/j.1551-2916.2012.05452.x
  2. doi:10.1023/A:1015105922260
    .
  3. ^
    ISBN 978-3527306732
    .
  4. ISBN 0-12-352651-5
    .

See also

External links

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