| Sodium oxide | |
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| IUPAC name |
Sodium oxide
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| Other names | Disodium oxide |
| Identifiers | |
| CAS number | 1313-59-3  |
| PubChem | 73971 |
| UN number | 1825 |
| Properties | |
| Molecular formula | Na2O |
| Molar mass | 61.9789 g/mol |
| Appearance | White solid |
| Density | 2.27 g/cm3 |
| Melting point |
1132°C |
| Boiling point |
1950 °C decomposes |
| Solubility in water | reacts violently to form NaOH |
| Structure | |
| Crystal structure | Antifluorite (face centered cubic), cF12 |
| Space group | Fm3m, No. 225 |
| Coordination geometry |
Tetrahedral (Na+); cubic (O2–) |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
−414.2 kJ/mol |
| Standard molar entropy S |
75.1 J mol−1 K−1 |
| Hazards | |
| MSDS | ICSC 1653 |
| EU Index | Not listed |
| Main hazards | Corrosive, reacts violently with water |
| Flash point | Non-flammable |
| Related compounds | |
| Other anions | Sodium sulfide Sodium selenide Sodium telluride |
| Other cations | Lithium oxide Potassium oxide Rubidium oxide Caesium oxide |
| Related sodium oxides | Sodium peroxide Sodium superoxide |
| Related compounds | Sodium hydroxide |
| (what is this?) (verify) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| Infobox references | |
Sodium oxide (SOX) is a chemical compound with the formula Na2O. It is used in ceramics and glasses. Treatment with water affords sodium hydroxide.
- Na2O + H2O → 2 NaOH
The alkali metal oxides M2O (M = Li, Na, K, Rb) crystallise in the antifluorite structure. In this motif the positions of the anions and cations are reversed relative to their positions in CaF2, with sodium ions tetrahedrally coordinated to 4 oxide ions and oxide cubically coordinated to 8 sodium ions.[1][2]
Contents |
Applications
Glass making
In the typical application, glass contains around 15% sodium oxide, the other components being silica (silicon dioxide) and lime (calcium oxide) at around 70% and 9%, respectively. The soda serves as a flux to lower the temperature at which the silica melts. Soda glass has a lower melting temperature vs pure silica, and has improved mechanical properties due to its slight increases in elasticity. These changes arise because the silicon dioxide and soda react to form sodium silicates of the general formula Na2[SiO2]x[SIO3].
Other
Na2O forms when sodium is treated with oxygen.
- 4 Na + O2 → 2 Na2O
Burning sodium in air will produce Na2O and about 20% sodium peroxide Na2O2.
- 6 Na + 2 O2 → 2 Na2O + Na2O2
Pure Na2O can be prepared by reaction of liquid sodium with NaNO3.
- 10 Na + 2 NaNO3 → 6 Na2O + N2
Sodium Oxide is also used in street lights and highway lights. Owners of highways and streets have been asked to use Na2O lights because of their high brightness.[citation needed]
References
- ^ Zintl, E.; Harder, A.; Dauth B. (1934), "Gitterstruktur der oxyde, sulfide, selenide und telluride des lithiums, natriums und kaliums", Z. Elektrochem. Angew. Phys. Chem. 40: 588–93
- ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
External links
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