Sulfur tetrachloride
From Wikipedia the free encyclopedia
 | |
| Names | |
|---|---|
| IUPAC name Sulfur(IV) chloride | |
| Identifiers | |
3D model (JSmol) | |
| ECHA InfoCard | 100.149.178 |
PubChem CID | |
CompTox Dashboard (EPA) | |
| |
| |
| 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 labelling: | |
  | |
| Danger | |
| H314, H400 | |
| P260, P264, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, 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). | |
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[edit]
It is obtained by treating sulfur dichloride with chlorine at 193 K:
-
(1)
![{\displaystyle {\begin{matrix}{}\\{\ce {{SCl2}+Cl2->[{\text{193 K}}]SCl4}}\\{}\end{matrix}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/a9def2efb84134526c63d5304a080329bfcf89b9)
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[edit]
It decomposes above −30 °C (242 K) to sulfur dichloride and chlorine.
-
(2)
![{\displaystyle {\begin{matrix}{}\\{\ce {SCl4->[{\text{-15 }}^{\circ }{\ce {C}}]{SCl2}+Cl2}}\\{}\end{matrix}}}](https://wikimedia.org/api/rest_v1/media/math/render/svg/502e8c19766026db1f83a732e9e7a102a8ebc2c1)
It hydrolyzes readily:
-
(3)
Sulfur tetrachloride reacts with water, producing hydrogen chloride and sulfur dioxide through the hydrolysis process. Thionyl chloride is an implied intermediate.[5]
-
(4)
- Oxidized by nitric acid:
-
(5)
References[edit]
- ^ 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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