Sodium peroxide

Sodium peroxide
Sodium peroxide
Names
IUPAC name
Sodium peroxide
Other names
Flocool
Solozone
Disodium peroxide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.013.828 Edit this at Wikidata
EC Number
  • 215-209-4
RTECS number
  • WD3450000
UNII
UN number 1504
  • InChI=1S/2Na.O2/c;;1-2/q2*+1;-2 ☒N
    Key: PFUVRDFDKPNGAV-UHFFFAOYSA-N ☒N
  • [O-][O-].[Na+].[Na+]
Properties
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)
Reacts
Solubility Soluble in acid
Insoluble in base
Reacts with ethanol
−28.10·10−6 cm3/mol
Structure
hexagonal
Thermochemistry
89.37 J/(mol·K)
95 J/(mol·K)[1]
−515 kJ·mol−1[1]
−446.9 kJ/mol
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 caustic
GHS labelling:
GHS03: OxidizingGHS05: Corrosive
Danger
H271, 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)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard W+OX: Reacts with water in an unusual or dangerous manner AND is oxidizer
3
0
2
W
OX
Flash point Non-flammable
Safety data sheet (SDS) External MSDS
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).
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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]

  1. ^ a b 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". Archived from the original on 2004-09-04.
  3. ^ Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 98. ISBN 978-0-08-022057-4.
  4. ^ Harald Jakob, Stefan Leininger, Thomas Lehmann, Sylvia Jacobi, Sven Gutewort. "Peroxo Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry, 2007, Wiley-VCH, Weinheim. doi:10.1002/14356007.a19_177.pub2.
  5. ^ Cite error: The named reference IS was invoked but never defined (see the help page).