Sodium peroxide

Names
IUPAC name

Sodium peroxide

Other names

Flocool
Solozone
Disodium peroxide

Identifiers

CAS Number

* 1313-60-6 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 14119 Y

EC Number |

* 215-209-4

PubChem CID

* 14803

RTECS number |

* WD3450000

UNII |

* 3GSN3JCJ5K Y

UN number | 1504

InChI

* InChI=1S/2Na.O2/c;;1-2/q2*+1;-2 N

Key: PFUVRDFDKPNGAV-UHFFFAOYSA-N N

SMILES

* [O-][O-].[Na+].[Na+]

Properties

Chemical formula

| Na2O2
Molar mass | 77.98 g/mol
Appearance  | yellow to white powder
Density | 2.805 g/cm3
Melting point |  460 °C (860 °F; 733 K) (decomposes)
Boiling point |  657 °C (1,215 °F; 930 K) (decomposes)

Solubility in water

| Reacts
Solubility | Soluble in acid
Insoluble in base
Reacts with ethanol

Magnetic susceptibility (χ)

| −28.10·10−6 cm3/mol
Structure

Crystal structure

| hexagonal
Thermochemistry

Heat capacity (C)

| 89.37 J/(mol·K)

Std molar
entropy (S ~~o~~ 298)

| 95 J/(mol·K)[1]

Std enthalpy of
formation (ΔfH⦵298)

| −515 kJ·mol−1[1]

Gibbs free energy (ΔfG˚)

| −446.9 kJ/mol
Hazards
Main hazards | Caustic, reacts with water and ethanol, oxidizer
Safety data sheet | External MSDS
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H271, 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)  |

~~W~~

Flash point | Non-flammable
Related compounds

Other cations

| Lithium peroxide
Potassium peroxide
Rubidium peroxide
Caesium peroxide

Related sodium oxides

| Sodium oxide
Sodium superoxide
Sodium ozonide

Related compounds

| Sodium hydroxide
Hydrogen 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

Sodium peroxide is an inorganic compound with the formula Na2O2. This yellowish solid is the product of sodium ignited in excess oxygen.[3] It is a strong base. This metal peroxide exists in several hydrates and peroxyhydrates including Na2O2·2H2O2·4H2O, Na2O2·2H2O, Na2O2·2H2O2, and Na2O2·8H2O.[4] The octahydrate, which is simple to prepare, is white, in contrast to the anhydrous material.[5]

## Contents

* 1 Properties
* 2 Preparation
* 3 Uses
* 4 References
* 5 External links

## Properties

Sodium peroxide crystallizes with hexagonal symmetry.[6] Upon heating, the hexagonal form undergoes a transition into a phase of unknown symmetry at 512 °C.[7] With further heating above the 657 °C boiling point, the compound decomposes to Na2O, releasing O2.[8]

2 Na2O2 → 2 Na2O + O2

## Preparation

Commercially, sodium peroxide is produced from the elements in a two-stage process. First sodium is oxidized to sodium oxide:[7][9]

4Na + O
2 → 2 Na

Subsequently, this oxide is treated with more oxygen:

2 Na
2O + O
2 → 2 Na

This was the method by which the substance was discovered in 1810 by Joseph Louis Gay-Lussac and Louis Jacques Thénard, as well as how it was for the first time commercially made by Hamilton Castner in the 1890s.[10]

It may also be produced by passing ozone gas over solid sodium iodide inside a platinum or palladium tube. The ozone oxidizes the sodium to form sodium peroxide. The iodine can be sublimed by mild heating. The platinum or palladium catalyzes the reaction and is not attacked by the sodium peroxide.

The octahydrate can be produced by treating sodium hydroxide with hydrogen peroxide.[5]

## Uses

Sodium peroxide hydrolyzes to give sodium hydroxide and hydrogen peroxide according to the reaction[9]

Na2O2 \+ 2 H2O → 2 NaOH + H2O2

Sodium peroxide was used to bleach wood pulp for the production of paper and textiles. Presently it is mainly used for specialized laboratory operations, e.g., the extraction of minerals from various ores. Sodium peroxide may go by the commercial names of Solozone[7] and Flocool.[8] In chemistry preparations, sodium peroxide is used as an oxidizing agent. It is also used as an oxygen source by reacting it with carbon dioxide to produce oxygen and sodium carbonate:

Na2O2 \+ CO2 → Na2CO3 \+ ​1⁄2 O2
Na2O2 \+ H2O + 2 CO2 → 2 NaHCO3 \+ ​1⁄2 O2

It is thus particularly useful in scuba gear, submarines, etc. Lithium peroxide and potassium superoxide have similar uses.

Sodium peroxide was once used on a large scale for the production of sodium perborate, but alternative routes to that cleaning agent have been developed.[4]

## References

1. ↑ 1.0 1.1 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed.. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
2. ↑ "Hazard Rating Information for NFPA Fire Diamonds". http://www.nmsu.edu/safety/programs/chem_safety/NFPA-ratingS-Z.htm.
3. ↑ 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.
4. ↑ 4.0 4.1 Jakob, Harald; Leininger, Stefan; Lehmann, Thomas; Jacobi, Sylvia; Gutewort, Sven (2007). "Peroxo Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a19_177.pub2. ISBN 978-3-527-30673-2.
5. ↑ 5.0 5.1 Penneman, R. A.; Toy, A. D. F. (1950). "Sodium Peroxide 8-Hydrate". Inorganic Syntheses. 3. pp. 1–4. doi:10.1002/9780470132340.ch1.
6. ↑ Tallman, R. L.; Margrave, J. L.; Bailey, S. W. (1957). "The Crystal Structure Of Sodium Peroxide". J. Am. Chem. Soc. 79 (11): 2979–80. doi:10.1021/ja01568a087. Bibcode: 1957JAChS..79.2979T.
7. ↑ 7.0 7.1 7.2 Macintyre, J. E., ed. Dictionary of Inorganic Compounds, Chapman & Hall: 1992.
8. ↑ 8.0 8.1 Lewis, R. J. Sax's Dangerous Properties of Industrial Materials, 10th ed., John Wiley & Sons, Inc.: 2000.
9. ↑ 9.0 9.1 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.
10. ↑ (in en) Bulletin of Pharmacy. 1895. https://books.google.com/books?id=SoJNAAAAMAAJ&pg=PA356.

## External links

* International Chemical Safety Card 1606

* v
* t
* e

Sodium compounds

* NaAlO2
* NaBH4
* NaBH3(CN)
* NaBO2
* NaBiO3
* NaBr
* NaBrO
* NaBrO3
* NaCH3COO
* NaC6H5CO2
* NaC6H4(OH)CO2
* NaCN
* NaCl
* NaClO
* NaClO2
* NaClO3
* NaClO4
* NaF
* Na2FeO4
* NaH
* NaHCO3
* NaH2PO4
* NaHSO3
* NaHSO4
* NaI
* NaIO3
* NaIO4
* Na5IO6
* NaMnO4
* NaN3
* NaNH2
* NaNO2
* NaNO3
* NaOCN
* NaO2
* NaO3
* NaOH
* NaPO2H2
* NaReO4
* NaSCN
* NaSH
* NaTcO4
* NaVO3
* Na2CO3
* Na2C2O4
* Na2CrO4
* Na2Cr2O7
* Na2GeO3
* Na2MnO4
* Na3MnO4
* Na2MoO4
* Na2MoS4
* Na2N2O2
* Na2O
* Na2O2
* Na2O(UO3)2
* Na2PO3F
* Na2S
* Na2SO3
* Na2SO4
* Na2S2O3
* Na2S2O4
* Na2S2O5
* Na2S2O6
* Na2S2O7
* Na2S2O8
* Na2S4O6
* Na2Se
* Na2SeO3
* Na2SeO4
* Na2SiO3
* Na2Si2O5
* Na4SiO4
* Na2Te
* Na2TeO3
* Na2TeO4
* Na2Po
* Na2Ti3O7
* Na2U2O7
* Na2WO4
* Na2Zn(OH)4
* Na3N
* Na3P
* Na3PO4
* Na3VO4
* Na4Fe(CN)6
* Na4P3O7
* Na5P3O10

Chemical formulas

Template:Peroxides

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*[CID]: Compound ID
*[H271]: May cause fire or explosion: strong 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
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*[P303+361+353]: IF ON SKIN (or hair): Remove/Take off immediately all contaminated clothing. Rinse skin with water/shower
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