Sodium oxide
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Names | |||
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IUPAC name
Sodium oxide
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Other names
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Identifiers | |||
3D model (
JSmol ) |
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ECHA InfoCard
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100.013.827 | ||
EC Number |
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PubChem CID
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UNII | |||
UN number | 1825 | ||
CompTox Dashboard (EPA)
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Properties | |||
Na2O | |||
Molar mass | 61.979 g·mol−1 | ||
Appearance | white solid | ||
Density | 2.27 g/cm3 | ||
Melting point | 1,132 °C (2,070 °F; 1,405 K) | ||
Boiling point | 1,950 °C (3,540 °F; 2,220 K) sublimates | ||
sublimates at 1275 °C | |||
Reacts to form NaOH | |||
Solubility | Reacts with ethanol | ||
−19.8·10−6 cm3/mol | |||
Structure | |||
Antifluorite (face centered cubic), cF12
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Fm3m, No. 225 | |||
Tetrahedral (Na+); cubic (O2−) | |||
Thermochemistry | |||
Heat capacity (C)
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72.95 J/(mol·K) | ||
Std molar
entropy (S⦵298) |
73 J/(mol·K)[1] | ||
Std enthalpy of (ΔfH⦵298)formation |
−416 kJ/mol[1] | ||
Gibbs free energy (ΔfG⦵)
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−377.1 kJ/mol | ||
Hazards | |||
Occupational safety and health (OHS/OSH): | |||
Main hazards
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corrosive, reacts violently with water | ||
GHS labelling: | |||
[2] | |||
H314 | |||
P260, P264, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P405, P501 | |||
NFPA 704 (fire diamond) | |||
Flash point | nonflammable | ||
Safety data sheet (SDS) | ICSC 1653 | ||
Related compounds | |||
Other anions
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Other cations
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Related compounds
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Sodium hydroxide | ||
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 oxide is a chemical compound with the formula Na2O. It is used in ceramics and glasses. It is a white solid but the compound is rarely encountered. Instead "sodium oxide" is used to describe components of various materials such as glasses and fertilizers which contain oxides that include sodium and other elements.
Structure
The structure of sodium oxide has been determined by
Preparation
Sodium oxide is produced by the reaction of sodium with sodium hydroxide, sodium peroxide, or sodium nitrite:[5]
- 2 NaOH + 2 Na → 2 Na2O + H2
To the extent that NaOH is contaminated with water, correspondingly greater amounts of sodium are employed. Excess sodium is distilled from the crude product.[6]
A second method involves heating a mixture of sodium azide and sodium nitrate:[6]
- 5 NaN3 + NaNO3 → 3 Na2O + 8 N2
Burning sodium in
A third much less known method involves heating sodium metal with iron(III) oxide (rust):
- 6 Na + Fe2O3 → 3 Na2O + 2 Fe
the reaction should be done in an inert atmosphere to avoid the reaction of sodium with the air instead.
Applications
Glassmaking
Glasses are often described in terms of their sodium oxide content although they do not really contain Na2O. Furthermore, such glasses are not made from sodium oxide, but the equivalent of Na2O is added in the form of "soda" (sodium carbonate), which loses carbon dioxide at high temperatures:
A typical manufactured
Reactions
Sodium oxide reacts readily and irreversibly with water to give sodium hydroxide:
- Na2O + H2O → 2 NaOH
Because of this reaction, sodium oxide is sometimes referred to as the base anhydride of sodium hydroxide (more archaically, "anhydride of caustic soda").
References
- ^ ISBN 978-0-618-94690-7.
- ^ Sigma-Aldrich Co., Sodium oxide. Retrieved on 2014-05-25.
- S2CID 94213844.
- ISBN 0-19-855370-6
- ISBN 978-0-08-037941-8.
- ^ a b E. Dönges (1963). "Sodium Oxide (IV)". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 1pages=975-6. NY, NY: Academic Press.