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Barium peroxide

Barium dioxide | (anhydrous) | (octahydrate) Colorless solid (octahydrate) | (anhydrous) | (octahydrate) | (20 C) (anhydrous) | (octahydrate) | NFPA-H = 3 | NFPA-F = 0 | NFPA-R = 2 | NFPA-S = ox

Barium peroxide is an inorganic compound with the formula . 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.

Structure

Barium peroxide consists of barium cations and peroxide anions . The solid is isomorphous to calcium carbide, .

Preparation and use

Barium peroxide arises by the reversible reaction of with barium oxide. The peroxide forms around 500 C and oxygen is released above 820 C. : This reaction is the basis for the now-obsolete Brin process for separating oxygen from the atmosphere. Other oxides, e.g. and SrO, behave similarly.

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

:

The insoluble barium sulfate is filtered from the mixture.

Footnotes

References

  1. (January 2013). "Accommodation of Excess Oxygen in Group II Monoxides". Journal of the American Ceramic Society.
  2. (2002). "Structure and Properties of Mechanically Activated Barium Peroxide". Inorganic Materials.
  3. (2001). "Inorganic chemistry". Academic Press; De Gruyter.
  4. Harald Jakob. "Peroxo Compounds, Inorganic".
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barium-compounds peroxides pyrotechnic-oxidizers pyrotechnic-colorants oxidizing-agents
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