Lithium peroxide

__ Li+ __ O−

Names
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 | 45.881 g/mol
Appearance  | fine, white powder
Odor | odorless
Density | 2.31 g/cm3[1][2]
Melting point | Decomposes to Li2O at ~340°C [3]
Boiling point | NA

Solubility in water

| soluble
Structure

Crystal structure

| hexagonal
Thermochemistry

Std enthalpy of
formation (ΔfH⦵298)

| -13.82 kJ/g
Hazards
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H271, H272, H314, H318

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. It is a white, nonhygroscopic solid. Because of its high oxygen:mass and oxygen:volume ratios, the solid has been used to remove CO2 from the atmosphere in spacecraft.[4]

## Contents

* 1 Preparation
* 2 Uses
* 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 has also been described 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 an eclipsed "ethane-like" Li6O2 subunits with an O-O distance of around 1.5 Å.[6]

## Uses

It is used in air purifiers where weight is important, e.g., spacecraft to absorb carbon dioxide and release oxygen in the reaction:[4]

Li2O2 \+ CO2 → Li2CO3 \+ ​1⁄2 O2

It absorbs more CO2 than does the same weight of lithium hydroxide and offers the bonus of releasing oxygen.[7] Furthermore, unlike most other alkali metal peroxides, it is not hygroscopic.

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]

The successful combination of a lithium-air battery overlain with an air-permeable mesh solar cell was announced by The Ohio State University in 2014.[9] The combination of two functions in one device (a "solar battery") is expected to reduce costs significantly compared to separate devices and controllers as are currently employed.

## See also

* Lithium oxide

## 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.
9. ↑ [1] Patent-pending device invented at The Ohio State University: the world’s first solar battery.

## 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

* v
* t
* e

Oxygen compounds

* AgO
* Al2O3
* AmO2
* Am2O3
* As2O3
* As2O5
* Au2O3
* B2O3
* BaO
* BeO
* Bi2O3
* BiO2
* Bi2O5
* BrO2
* Br2O3
* Br2O5
* CO
* CO2
* C2O3
* CaO
* CaO2
* CdO
* CeO2
* Ce3O4
* Ce2O3
* ClO2
* Cl2O
* Cl2O3
* Cl2O4
* Cl2O6
* Cl2O7
* CoO
* Co2O3
* Co3O4
* CrO3
* Cr2O3
* Cr2O5
* Cr5O12
* CsO2
* Cs2O3
* CuO
* D2O
* Dy2O3
* Er2O3
* Eu2O3
* FeO
* Fe2O3
* Fe3O4
* Ga2O
* Ga2O3
* GeO
* GeO2
* H2O
* H218O
* H2O2
* HfO2
* HgO
* Hg2O
* Ho2O3
* I2O4
* I2O5
* I2O6
* I4O9
* In2O3
* IrO2
* KO2
* K2O2
* La2O3
* Li2O
* Li2O2
* Lu2O3
* MgO
* Mg2O3
* MnO
* MnO2
* Mn2O3
* Mn2O7
* MoO2
* MoO3
* Mo2O3
* NO
* NO2
* N2O
* N2O3
* N2O4
* N2O5
* NaO2
* Na2O
* Na2O2
* NbO
* NbO2
* Nd2O3
* OF2
* O2F2
* O3F2
* O4F2
* O2PtF6

Chemical formulas

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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
*[H318]: Causes serious 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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