Chemistry:Sodium superoxide
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| Names | |
|---|---|
| IUPAC name
sodium superoxide
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| Other names
sodium superoxide
sodium dioxide | |
| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
PubChem CID
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| RTECS number |
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| UNII | |
| UN number | 2547 |
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| Properties | |
| 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 |
| Decomposes | |
| Basicity (pKb) | N/A |
| Structure | |
| cubic | |
| Thermochemistry | |
Heat capacity (C)
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72.1 J/mol K |
Std molar
entropy (S |
115.9 J/mol K |
Std enthalpy of
formation (ΔfH⦵298) |
−260.2 kJ/mol |
Gibbs free energy (ΔfG˚)
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−218.4 kJ/mol |
| Hazards | |
| GHS pictograms |  
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| GHS Signal word | Danger |
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| NFPA 704 (fire diamond) | |
| Flash point | Non flammable |
| Related compounds | |
Other anions
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sodium oxide sodium peroxide |
Other cations
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Lithium superoxide Potassium superoxide Rubidium superoxide Caesium superoxide |
Except where otherwise noted, 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.[1] This yellow-orange solid is a salt of the superoxide anion. It is an intermediate in the oxidation of sodium by oxygen.
Preparation
NaO2 is prepared by treating sodium peroxide with oxygen at high pressures:[2]
- Na2O2 + O2 → 2 NaO2
It can also be prepared by careful oxygenation of a solution of sodium in cryogenic liquid ammonia:
- Na(in NH3) + O2 → NaO2
Although the existence of a sodium oxide higher than peroxide was speculated since 19th century, it was not until 1948 when American chemists were able to definitely synthesize it by the latter method.[3]
Properties
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.[4] It crystallizes in the NaCl motif.
References
- ↑ Hayyan, Maan; Hashim, Mohd Ali; AlNashef, Inas M. (2016-02-15). "Superoxide Ion: Generation and Chemical Implications". Chemical Reviews (American Chemical Society (ACS)) 116 (5): 3029–3085. doi:10.1021/acs.chemrev.5b00407. ISSN 0009-2665. PMID 26875845.
- ↑ Stephen E. Stephanou, Edgar J. Seyb Jr., Jacob Kleinberg "Sodium Superoxide" Inorganic Syntheses 1953; Vol. 4, 82-85.
- ↑ Schechter, William H.; Sisler, Harry H.; Kleinberg, Jacob (January 1948). "The Absorption of Oxygen by Sodium in Liquid Ammonia: Evidence for the Existence of Sodium Superoxide" (in en). Journal of the American Chemical Society 70 (1): 267–269. doi:10.1021/ja01181a083. ISSN 0002-7863. https://pubs.acs.org/doi/abs/10.1021/ja01181a083.
- ↑ Sasol Encyclopaedia of Science and Technology , G.C. Gerrans, P. Hartmann-Petersen , p.243 "sodium oxides" , google books link
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