Lithium peroxide

__ Li+ __ O−

Names
IUPAC name

Lithium peroxide

Other names

Dilithium peroxide
Lithium(I) peroxide

Identifiers

CAS Number

* 12031-80-0 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 23787 Y

PubChem CID

* 25489

UNII |

* 9ANX556R5F Y

InChI

* InChI=1S/2Li.O2/c;;1-2/q2*+1;-2 Y

Key: HPGPEWYJWRWDTP-UHFFFAOYSA-N Y

* InChI=1/2Li.O2/c;;1-2/q2*+1;-2

Key: HPGPEWYJWRWDTP-UHFFFAOYAV

SMILES

* [Li+].[Li+].[O-][O-]

Properties

Chemical formula

| Li2O2
Molar mass | 45.885 g/mol
Appearance  | fine, white powder
Odor | odorless
Density | 2.32 g/cm3[1][2]
Melting point | Decomposes to Li2O at ~450°C but melts at 197°C[3]
Boiling point | NA
Structure

Crystal structure

| hexagonal
Thermochemistry

Std enthalpy of
formation (ΔfH⦵298)

| −13.83 kJ/g
Hazards
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H271, H272, H314

GHS precautionary statements

| P210, P220, P221, P260, P264, P280, P283, P301+330+331, P303+361+353, P304+340, P305+351+338, P306+360, P310, P321, P363, P370+378, P371+380+375, P405, P501
NFPA 704 (fire diamond)  |

Related compounds

Other cations

| Sodium peroxide
Potassium peroxide
Rubidium peroxide
Caesium peroxide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

Tracking categories (test):

* SizeSet

Lithium peroxide is the inorganic compound with the formula Li2O2. Lithium peroxide is a white solid, and unlike most other alkali metal peroxides, it is nonhygroscopic. 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 in spacecraft.[4]

## Contents

* 1 Preparation
* 2 Uses
* 2.1 Air purification
* 2.2 Styrene polymerization
* 2.3 Lithium-air battery
* 3 See also
* 4 References
* 5 External links

## Preparation

It is prepared by the reaction of hydrogen peroxide and lithium hydroxide. This reaction initially produces lithium hydroperoxide:[4][5]

LiOH + H2O2 → LiOOH + H2O

This lithium hydroperoxide may exist as lithium peroxide monoperoxohydrate trihydrate (Li2O2·H2O2·3H2O). Dehydration of this material gives the anhydrous peroxide salt:

2 LiOOH → Li2O2 \+ H2O2

Li2O2 decomposes at about 450 °C to give lithium oxide:

2 Li2O2 → 2 Li2O + O2

The structure of solid Li2O2 has been determined by X-ray crystallography and density functional theory. The solid features eclipsed "ethane-like" Li6O2 subunits with an O-O distance of around 1.5 Å.[6]

## Uses

### Air purification

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]

### Styrene polymerization

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.

### Lithium-air battery

The reversible lithium peroxide reaction is the basis for a prototype lithium–air battery. Using oxygen from the atmosphere allows the battery to eliminate storage of oxygen for its reaction, saving battery weight and size.[8]

## See also

* Lithium oxide
* Lithium monoxide anion

## References

1. ↑ "Physical Constants of Inorganic Compounds," in CRC Handbook of Chemistry and Physics, 91st Edition (Internet Version 2011), W. M. Haynes, ed., CRC Press/Taylor and Francis, Boca Raton, Florida. (pp: 4-72).
2. ↑ Speight, James G. (2005). Lange's Handbook of Chemistry (16th Edition). (pp: 1.40). McGraw-Hill. Online version available at: http://www.knovel.com/web/portal/browse/display?_EXT_KNOVEL_DISPLAY_bookid=1347&VerticalID=0
3. ↑ Phys.Chem.Chem.Phys.,2013,15, 11025. doi:10.1039/c3cp51056e
4. ↑ 4.0 4.1 4.2 Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 98. ISBN 978-0-08-022057-4. https://books.google.com/books?id=OezvAAAAMAAJ&q=0-08-022057-6&dq=0-08-022057-6&source=bl&ots=m4tIRxdwSk&sig=XQTTjw5EN9n5z62JB3d0vaUEn0Y&hl=en&sa=X&ei=UoAWUN7-EM6ziQfyxIDoCQ&ved=0CD8Q6AEwBA.
5. ↑ E. Dönges "Lithium and Sodium Peroxides" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 979.
6. ↑ L. G. Cota and P. de la Mora "On the structure of lithium peroxide, Li2O2" Acta Crystallogr. 2005, vol. B61, pages 133-136. doi:10.1107/S0108768105003629
7. ↑ Ulrich Wietelmann, Richard J. Bauer "Lithium and Lithium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH: Weinheim. doi:10.1002/14356007.a15_393.pub2
8. ↑ Girishkumar, G.; B. McCloskey; AC Luntz; S. Swanson; W. Wilcke (July 2, 2010). "Lithium- air battery: Promise and challenges". The Journal of Physical Chemistry Letters 1 (14): 2193–2203. doi:10.1021/jz1005384.

## External links

* WebElements entry

* v
* t
* e

Lithium compounds

Inorganic|

* LiAlCl4
* LiAlH4
* LiAlO2
* LiBF4
* LiBH4
* LiBO2
* LiB3O5
* Li2B4O7
* LiBr
* Li2CO3
* Li2C2
* LiCl
* LiClO
* LiClO3
* LiClO4
* LiCoO2
* LiF
* LiH
* LiI
* LiIO3
* Li2IrO3
* Li2MoO4
* LiNH2
* Li2NH
* LiN3
* Li3N
* LiNO2
* LiNO3
* LiNbO3
* LiOH
* LiO2
* Li2O
* Li2O2
* LiPF6
* Li2PtO3
* Li2Po
* Li2RuO3
* Li2S
* Li2SO3
* Li2SO4
* Li3H(CO3)2
* Li2SiO3
* LiTaO3
* Li2TiO3

Organic|

* 12-hydroxystearate
* acetate
* aspartate
* citrate
* diisopropylamide
* orotate
* succinate
* stearate
* organolithiums

Minerals|

* Amblygonite
* Elbaite
* Eucryptite
* Jadarite
* Lepidolite
* Lithiophilite
* Petalite
* Pezzottaite
* Saliotite
* Spodumene
* Sugilite
* Tourmaline
* Zabuyelite
* Zinnwaldite

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*[CID]: Compound ID
*[H271]: May cause fire or explosion: strong oxidizer
*[H272]: May intensify fire: oxidizer
*[H314]: Causes severe skin burns and eye damage
*[P210]: Keep away from heat/sparks/open flames/hot surfaces – No smoking
*[P220]: Keep/Store away from clothing/…/combustible materials
*[P221]: Take any precaution to avoid mixing with combustibles
*[P260]: Do not breathe dust/fume/gas/mist/vapours/spray
*[P264]: Wash … thoroughly after handling
*[P280]: Wear protective gloves/protective clothing/eye protection/face protection
*[P283]: Wear fire/flame resistant/retardant clothing
*[P301+330+331]: IF SWALLOWED: Rinse mouth. Do NOT induce vomiting
*[P303+361+353]: IF ON SKIN (or hair): Remove/Take off immediately all contaminated clothing. Rinse skin with water/shower
*[P304+340]: IF INHALED: Remove victim to fresh air and keep at rest in a position comfortable for breathing
*[P305+351+338]: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do – continue rinsing
*[P306+360]: IF ON CLOTHING: Rinse immediately contaminated clothing and skin with plenty of water before removing clothes
*[P310]: Immediately call a POISON CENTER or doctor/physician
*[P321]: Specific treatment (see … on this label)
*[P363]: Wash contaminated clothing before reuse
*[P370+378]: In case of fire: Use … for extinction
*[P371+380+375]: In case of major fire and large quantities: Evacuate area. Fight fire remotely due to the risk of explosion
*[P405]: Store locked up
*[P501]: Dispose of contents/container to …
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