Chemistry:Sulfur tetrachloride
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| Names | |
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| IUPAC name
Sulfur(IV) chloride
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| Identifiers | |
3D model (JSmol)
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PubChem CID
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| Properties | |
| SCl4 | |
| Molar mass | 173.87 |
| Appearance | White powder |
| Melting point | −31 °C (−24 °F; 242 K) |
| Boiling point | −20 °C (−4 °F; 253 K) (decomposes) |
| soluble in water | |
| Hazards | |
| GHS pictograms |  
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| GHS Signal word | Danger |
| H314, H400 | |
| P260, P264, P273, P280, P301+330+331, P303+361+353, P304+340, P305+351+338, P310, P321, P363, P391, P405, P501 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Sulfur tetrachloride is an inorganic compound with chemical formula SCl4. It has only been obtained as an unstable pale yellow solid. The corresponding SF4 is a stable, useful reagent.
Preparation and structure
It is obtained by treating sulfur dichloride with chlorine at 193 K:
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[math]\displaystyle{ \begin{matrix}{}\\ \ce{{SCl2} + Cl2 -\gt [\text{193 K}] SCl4}\\{} \end{matrix} }[/math]
()
It melts with simultaneous decomposition above −20 °C.[1]
Its solid structure is uncertain. It is probably the salt SCl3+Cl−, since related salts are known with noncoordinating anions.[2][3] In contrast to this tetrachloride, SF4 is a neutral molecule.[4]
Reactions
It decomposes above −30 °C (242 K) to sulfur dichloride and chlorine.
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[math]\displaystyle{ \begin{matrix}{}\\ \ce{SCl4 -\gt [\text{-15 }^\circ \ce C] {SCl2} + Cl2}\\{} \end{matrix} }[/math]
()
It hydrolyzes readily:
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[math]\ce{ {SCl4} + H2O -> {SOCl2} + {2HCl} }[/math]
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Sulfur tetrachloride reacts with water, producing hydrogen chloride and sulfur dioxide through the hydrolysis process. Thionyl chloride is an implied intermediate.[5]
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[math]\ce{ {SCl4} + 2H2O -> {SO2} + {4HCl} }[/math]
()
- Oxidized by nitric acid:
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[math]\ce{ {SCl4} + {2HNO3} + 2H2O -> {H2SO4} + 2NO2 (^) + {4HCl} }[/math]
()
References
- ↑ Georg Brauer: Handbuch der Präparativen Anorganischen Chemie. (in German)
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ↑ Christian, Beverly H.; Collins, Michael J.; Gillespie, Ronald J.; Sawyer, Jeffery F. "Preparations, Raman spectra, and crystal structures of (SCl3)(SbCl6), (SeCl3)(SbCl6), (SBr1.2Cl1.8)(SbCl6), (TeCl3)(AlCl4) (triclinic modification), (TeCl3)(SbF6), (TeCl3)(AsF6), and (TeF3)2(SO4)" Inorganic Chemistry 1986, volume 25, 777-88. doi:10.1021/ic00226a012
- ↑ Goettel, J. T., Kostiuk, N. and Gerken, M. (2013), The Solid-State Structure of SF4: The Final Piece of the Puzzle . Angew. Chem. Int. Ed., 52: 8037–8040. doi:10.1002/anie.201302917
- ↑ Holleman-Wiberg, Lehrbuch der Anorganischen Chemie, 101. Auflage, de Gruyter Verlag 1995 ISBN:3-11-012641-9 (in German)
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