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.
The structure of sodium oxide has been determined by X-ray crystallography. Most 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.[3][4]
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]
Burning sodium in air produces a mixture of Na2O and sodium peroxide (Na2O2).
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.
ApplicationsEdit
GlassmakingEdit
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:
Na2CO3 → Na2O + CO2
Na2O + SiO2 → Na2SiO3
Na2CO3 + SiO2 → Na2SiO3 + CO2
A typical manufactured glass contains around 15% sodium oxide, 70% silica (silicon dioxide), and 9% lime (calcium oxide). The sodium carbonate "soda" serves as a flux to lower the temperature at which the silica mixture melts. Such soda-lime glass has a much lower melting temperature than pure silica and has slightly higher elasticity. These changes arise because the Na2[SiO2]x[SiO3]-based material is somewhat more flexible.
ReactionsEdit
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").
ReferencesEdit
^ abZumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN978-0-618-94690-7.
^Zintl, E.; Harder, A.; Dauth B. (1934). "Gitterstruktur der oxyde, sulfide, selenide und telluride des lithiums, natriums und kaliums". Zeitschrift für Elektrochemie und Angewandte Physikalische Chemie. 40 (8): 588–93. doi:10.1002/bbpc.19340400811. S2CID 94213844.
^Wells, A. F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press ISBN0-19-855370-6
^ abE. Dönges (1963). "Sodium Oxide (IV)". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 1pages=975-6. NY,NY: Academic Press.
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October 20, 2023
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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 Sodium oxide Sodium oxide Sodium oxideNamesIUPAC name Sodium oxideOther names SodaDisodium oxideSodium oxidosodiumNatrium oxide historic IdentifiersCAS Number 1313 59 3 Y3D model JSmol Interactive imageECHA InfoCard 100 013 827EC Number 215 208 9PubChem CID 73971UNII 3075U8R23D YUN number 1825CompTox Dashboard EPA DTXSID0049781InChI InChI 1S 2Na O q2 1 2SMILES O 2 Na Na PropertiesChemical formula Na 2OMolar mass 61 979 g mol 1Appearance white solidDensity 2 27 g cm3Melting point 1 132 C 2 070 F 1 405 K Boiling point 1 950 C 3 540 F 2 220 K sublimatesSublimationconditions sublimates at 1275 CSolubility in water Reacts to form NaOHSolubility Reacts with ethanolMagnetic susceptibility x 19 8 10 6 cm3 molStructureCrystal structure Antifluorite face centered cubic cF12Space group Fm3m No 225Coordination geometry Tetrahedral Na cubic O2 ThermochemistryHeat capacity C 72 95 J mol K Std molarentropy S 298 73 J mol K 1 Std enthalpy offormation DfH 298 416 kJ mol 1 Gibbs free energy DfG 377 1 kJ molHazardsOccupational safety and health OHS OSH Main hazards corrosive reacts violently with waterGHS labelling Pictograms 2 Hazard statements H314Precautionary statements P260 P264 P280 P301 P330 P331 P303 P361 P353 P304 P340 P305 P351 P338 P310 P321 P363 P405 P501NFPA 704 fire diamond 301WFlash point nonflammableSafety data sheet SDS ICSC 1653Related compoundsOther anions Sodium sulfideSodium selenideSodium tellurideSodium polonideOther cations Lithium oxidePotassium oxideRubidium oxideCaesium oxideRelated sodium oxides Sodium peroxideSodium superoxideSodium ozonideRelated compounds Sodium hydroxideExcept where otherwise noted data are given for materials in their standard state at 25 C 77 F 100 kPa Y verify what is Y N Infobox references Contents 1 Structure 2 Preparation 3 Applications 3 1 Glassmaking 4 Reactions 5 ReferencesStructure EditThe structure of sodium oxide has been determined by X ray crystallography Most 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 3 4 Preparation EditSodium oxide is produced by the reaction of sodium with sodium hydroxide sodium peroxide or sodium nitrite 5 2 NaOH 2 Na 2 Na2O H2To 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 N2Burning sodium in air produces a mixture of Na2O and sodium peroxide Na2O2 A third much less known method involves heating sodium metal with iron III oxide rust 6 Na Fe2O3 3 Na2O 2 Fethe reaction should be done in an inert atmosphere to avoid the reaction of sodium with the air instead Applications EditGlassmaking Edit 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 Na2CO3 Na2O CO2 Na2O SiO2 Na2SiO3 Na2CO3 SiO2 Na2SiO3 CO2A typical manufactured glass contains around 15 sodium oxide 70 silica silicon dioxide and 9 lime calcium oxide The sodium carbonate soda serves as a flux to lower the temperature at which the silica mixture melts Such soda lime glass has a much lower melting temperature than pure silica and has slightly higher elasticity These changes arise because the Na2 SiO2 x SiO3 based material is somewhat more flexible Reactions EditSodium oxide reacts readily and irreversibly with water to give sodium hydroxide Na2O H2O 2 NaOHBecause of this reaction sodium oxide is sometimes referred to as the base anhydride of sodium hydroxide more archaically anhydride of caustic soda References Edit a b Zumdahl Steven S 2009 Chemical Principles 6th Ed Houghton Mifflin Company p A23 ISBN 978 0 618 94690 7 Sigma Aldrich Co Sodium oxide Retrieved on 2014 05 25 Zintl E Harder A Dauth B 1934 Gitterstruktur der oxyde sulfide selenide und telluride des lithiums natriums und kaliums Zeitschrift fur Elektrochemie und Angewandte Physikalische Chemie 40 8 588 93 doi 10 1002 bbpc 19340400811 S2CID 94213844 Wells A F 1984 Structural Inorganic Chemistry Oxford Clarendon Press ISBN 0 19 855370 6 Greenwood Norman N Earnshaw Alan 1997 Chemistry of the Elements 2nd ed Butterworth Heinemann ISBN 978 0 08 037941 8 a b E Donges 1963 Sodium Oxide IV In G Brauer ed Handbook of Preparative Inorganic Chemistry 2nd Ed Vol 1pages 975 6 NY NY Academic Press nbsp Wikimedia Commons has media related to Sodium oxide Retrieved from https en wikipedia org w index php title Sodium oxide amp oldid 1171900015, wikipedia, wiki, book, books, library,
