Sodium superoxide

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Sodium superoxide
Identifiers
CAS number 12034-12-7 YesY
PubChem 61542
RTECS number WE2860010
Jmol-3D images Image 1
Properties
Molecular formula NaO2
Molar mass 54.9886 g/mol
Appearance Yellow to orange crystalline solid
Density 2.2 g/cm3
Melting point 551.7 °C (1,025.1 °F; 824.9 K)
Boiling point Decomposes
Solubility in water Decomposes
Basicity (pKb) N/A
Structure
Crystal structure cubic
Thermochemistry
Specific
heat capacity
C
72.1 J/mol K
Std molar
entropy
So298
115.9 J/mol K
Std enthalpy of
formation
ΔfHo298
-260.2 kJ/mol
Gibbs free energy ΔG -218.4 kJ/mol
Hazards
EU classification Corrosive
R-phrases R35
S-phrases S1/2, S26, S37/39, S45
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazard OX: Oxidizer. E.g., potassium perchlorateNFPA 704 four-colored diamond
Flash point Non flammable
Related compounds
Other anions sodium oxide
sodium peroxide
Other cations potassium superoxide
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Sodium superoxide is the inorganic compound with the formula NaO2. This yellow-orange solid is a salt of the superoxide anion. It is an intermediate in the oxidation of sodium by oxygen.

Preparation[edit]

NaO2 is prepared by treating sodium peroxide with oxygen at high pressures:[1]

Na2O2 + O2 → 2 NaO2

It can also be prepared by careful oxygenation of a solution of sodium in ammonia:

Na(in NH3) + O2 → NaO2

Properties[edit]

The product is paramagnetic, as expected for a salt of the O
2
anion. It hydrolyses readily to give a mixture of sodium hydroxide, oxygen and hydrogen peroxide.[2] It crystallizes in the NaCl motif.[citation needed]

References[edit]

  1. ^ Stephen E. Stephanou, Edgar J. Seyb Jr., Jacob Kleinberg "Sodium Superoxide" Inorganic Syntheses 1953; Vol. 4, 82-85.
  2. ^ Sasol Encyclopaedia of Science and Technology , G.C. Gerrans, P. Hartmann-Petersen , p.243 "sodium oxides" , google books link