1,4-Oxathiane
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Names | |
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Preferred IUPAC name
1,4-Oxathiane | |
Other names
1,4-Thioxane;p-Thioxane; 1-Oxa-4-thiacyclohexane
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Identifiers | |
3D model (JSmol)
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ECHA InfoCard | 100.036.454 |
EC Number |
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PubChemCID
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UNII | |
CompTox Dashboard(EPA)
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Properties | |
C4H8OS | |
Molar mass | 104.17g·mol−1 |
Melting point | −17 °C (1 °F; 256 K) |
Boiling point | 147.0 °C (296.6 °F; 420.1 K) |
Hazards | |
GHSlabelling: | |
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Warning | |
H226,H315,H319,H335 | |
P210,P233,P240,P241,P242,P243,P261,P264,P271,P280,P302+P352,P303+P361+P353,P304+P340,P305+P351+P338,P312,P321,P332+P313,P337+P313,P362,P370+P378,P403+P233,P403+P235,P405,P501 | |
Lethal doseor concentration (LD, LC): | |
LD50(median dose)
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2830 mg/kg oral rat |
Related compounds | |
Related compounds
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1,4-dioxane |
Except where otherwise noted, data are given for materials in theirstandard state(at 25 °C [77 °F], 100 kPa).
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1,4-Oxathianeis aheterocyclic compoundcontaining oneoxygenatom and onesulfuratom at opposite corners of asaturatedsix-membered ring. Bysystematic numbering,the oxygen atom is position number 1, sulfur is number 4, and positions 2, 3, 5, and 6 arecarbonatoms.
Production
[edit]1,4-Oxathiane can be produced from low cost ingredients by heatingethylene glycolorethylene oxidewithhydrogen sulfide.Alternate ways are to dehydrate bis(hydroxy ethyl) sulfide by heating withpotassium hydrogen sulfate.These reactions also form 1,4-dithianeas abyproduct.[1]
The original 1912 preparation of 1,4-oxathiane involved iodoethyl ether with potassium sulfide in alcohol. A similar method used 2-chloroethyl ether.[1]
Reactions
[edit]The sulfur atom in 1,4-oxathiane can undergo reaction as other substituted sulfides can. It can be oxidised to asulfoxidewithcalcium hypochloriteorsodium periodate,[2]or continuing to asulfone.
It can react with ammonia to form diimines.[3]
With elementalchlorinebelow 0 °C, 3-chloro-1,4-oxathiane is formed. Above 0 °C, 2,3-dichloro-1,4-oxathiane results and further chlorination yields 2,3,5,6-tetrachloro-1,4-oxathiane.[1]
Withhydrofluoric acid,1,4-oxathiane is undergoeselectrophilic fluorinationto yield perfluoro-1,4-oxathiane: all eight hydrogen atoms are replaced with fluorinesubstituents,and also four fluorine atoms are attached to the sulfur atom.[1]
With elementalbrominein ether, an oxathianium salt is formed. In this an extra bromine atom bonds to the sulfur atom which gets a positive charge. To balance this, a bromide ion forms to make up a salt. Similarly iodine in acetic acid reacts to make 4-iodo-1,4-oxathianium iodide. Heating 1,4-oxathiane withethyl iodideyields 4-ethyl-1,4-oxathianium iodide.[1]
References
[edit]- ^abcdeBreslow, David S.;Skolnik, Herman (2009).Multi-Sulfur and Sulfur and Oxygen Five- and Six-Membered Heterocycles.John Wiley & Sons. pp. 823–828.ISBN978-0-470-18833-0.
- ^Yamamoto, ed. (2004). "Product Subclass 8: Aluminum Oxide (Alumina)".Category 1, Organometallics.doi:10.1055/sos-SD-007-00192.ISBN9783131122117.
- ^Kambe, ed. (2008). "Product Subclass 2: Cyclic Dialkyl Sulfones and Derivatives".Category 5, Compounds with One Saturated Carbon Heteroatom Bond.doi:10.1055/sos-SD-039-00922.ISBN9783131189219.