Calcium peroxide
Calcium peroxide or calcium dioxide is the inorganic compound with the formula CaO2. It is the peroxide (O22−) salt of Ca2+. Commercial samples can be yellowish, but the pure compound is white. It is almost insoluble in water.[2]
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| Identifiers | |
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CAS Number |
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3D model (JSmol) |
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.013.764 |
| EC Number |
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| E number | E930 (glazing agents, ...) |
Gmelin Reference |
674257 |
| KEGG | |
PubChem CID |
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| RTECS number |
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| UNII | |
| UN number | 1457 |
CompTox Dashboard (EPA) |
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InChI
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SMILES
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| Properties | |
Chemical formula |
CaO2 |
| Molar mass | 72.0768 g/mol |
| Appearance | white or yellowish powder |
| Odor | odorless |
| Density | 2.91 g/cm3 |
| Melting point | ~ 355 °C (671 °F; 628 K) (decomposes) |
Solubility in water |
decomposes |
| Acidity (pKa) | 12.5 |
Magnetic susceptibility (χ) |
-23.8·10−6 cm3/mol |
Refractive index (nD) |
1.895 |
| Structure | |
Crystal structure |
Orthorhombic[1] |
Space group |
Pna21 |
Coordination geometry |
8[1] |
| Hazards | |
| GHS pictograms |   |
| GHS Signal word | Warning |
GHS hazard statements |
H272, H315, H319, H335 |
GHS precautionary statements |
P210, P220, P221, P261, P264, P271, P280, P302+352, P304+340, P305+351+338, P312, P321, P332+313, P337+313, P362, P370+378, P403+233, P405, P501 |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose) |
>5000 mg/kg (oral, rat) >10000 mg/kg (dermal, rat) |
| Related compounds | |
Other anions |
Calcium oxide |
Other cations |
Strontium peroxide Barium peroxide Sodium peroxide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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| Infobox references | |
Structure and stability
As a solid, it is relatively stable against decomposition. In contact with water however it hydrolyzes with release of oxygen. Upon treatment with acid, it forms hydrogen peroxide.
Preparation
Calcium peroxide is produced by combining calcium salts and hydrogen peroxide:
- Ca(OH)2 + H2O2 → CaO2 + 2 H2O
The octahydrate precipitates upon the reaction of calcium hydroxide with dilute hydrogen peroxide. Upon heating it dehydrates.
Applications
It is mainly used as an oxidant to enhance the extraction of precious metals from their ores. In its second main application, it is used as a food additive under the E number E930 it is used as flour bleaching agent and improving agent.[2]
In agriculture it is used in the presowing treatments of rice seed. Also, calcium peroxide has found use in the aquaculture to oxygenate and disinfect water. In the ecological restoration industry it is used in the treatment of soils. Calcium peroxide is used in a similar manner to magnesium peroxide for environmental restoration programs. It is used to restore soil and groundwater contaminated with petroleum by the process of enhanced in-situ bioremediation.
It is also used for curing polythioether polymers by oxidising terminal thiol groups to disulphide bridges.
References
- Zhao, X.; Nguyen, M.C.; Wang, C.Z.; Ho, K.M. (2013). "Structures and stabilities of alkaline earth metal peroxides XO2 (X = Ca, Be, Mg) studied by a genetic algorithm" (PDF). RSC Advances. doi:10.1039/C3RA43617A.
- 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.CS1 maint: multiple names: authors list (link)