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| Names | |
|---|---|
| IUPAC name Lithium peroxide | |
| Other names Dilithium peroxide Lithium(I) peroxide | |
| Identifiers | |
3D model (JSmol) | |
| ChemSpider |
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| ECHA InfoCard | 100.031.585 |
| UNII | |
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| Properties | |
| Li2O2 | |
| Molar mass | 45.885 g/mol |
| Appearance | fine, white powder |
| Odor | odorless |
| Density | 2.32 g/cm3[1][2] |
| Melting point | Decomposes toLi2O at ~450°C but melts at 197°C[3] |
| Boiling point | NA |
| soluble[vague] | |
| Structure | |
| hexagonal | |
| Thermochemistry | |
Std enthalpy of formation(ΔfH⦵298) | −13.83 kJ/g |
| Hazards | |
| GHS labelling: | |
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| Danger | |
| H271,H272,H314 | |
| P210,P220,P221,P260,P264,P280,P283,P301+P330+P331,P303+P361+P353,P304+P340,P305+P351+P338,P306+P360,P310,P321,P363,P370+P378,P371+P380+P375,P405,P501 | |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Othercations | Sodium peroxide Potassium peroxide Rubidium peroxide Caesium peroxide |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Lithium peroxide is theinorganic compound with theformulaLi2O2. Lithium peroxide is a white solid, and unlike most other alkali metal peroxides, it isnonhygroscopic. Because of its high oxygen:mass and oxygen:volume ratios, the solid has been used to remove CO2 from and release O2 to the atmosphere inspacecraft.[4]
It is prepared by the reaction ofhydrogen peroxide andlithium hydroxide. This reaction initially produces lithiumhydroperoxide:[4][5]
This lithium hydroperoxide may exist as lithium peroxide monoperoxohydrate trihydrate (Li2O2·H2O2·3H2O).Dehydration of this material gives the anhydrous peroxide salt:
Li2O2 decomposes at about 450 °C to givelithium oxide:
The structure of solid Li2O2 has been determined byX-ray crystallography anddensity functional theory. The solid features eclipsed "ethane-like" Li6O2 subunits with an O-O distance of around 1.5 Å.[6]
It is used in air purifiers where weight is important, e.g., spacecraft or other sealed spaces and apparatuses to absorb carbon dioxide and release oxygen in the reaction:[4]
Li2O2 + CO2 → Li2CO3 +1⁄2 O2
Similar to the reaction of lithium hydroxide with carbon dioxide to release 1 Li2CO3 and 1 H2O, lithium peroxide has high absorption capacity and absorbs more CO2 than does the same weight of lithium hydroxide and offers the bonus of releasing oxygen instead of water.[7]
Lithium peroxide can also act as a catalyst for polymerization of styrene to polystyrene. The polymerization of styrene to polystyrene typically involves the use of radical initiators via the free radical chain mechanism but lithium peroxide can also initiate radical polymerization reactions under certain conditions, although not as widely used.
The reversible lithium peroxide reaction is the basis for a prototypelithium–air battery. Using oxygen from the atmosphere allows the battery to eliminate storage of oxygen for its reaction, saving battery weight and size.[8]
