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| Names | |
|---|---|
| IUPAC name
Sulfur(IV) chloride
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| Identifiers | |
3D model (JSmol)
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| ECHA InfoCard | 100.149.178 |
PubChem CID
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CompTox Dashboard (EPA)
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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 labelling: | |
 
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| 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).
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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.
YouTube Encyclopedic
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SCl4 Lewis Structure: How to Draw the Lewis Structure for Sulfur Tetrachloride
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Sulfur Monochloride (Disulfur Dichloride)
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Sulfur Hexafluoride - Deep Voice Gas
Transcription
This is the SCl4 Lewis structure: sulfur tetrachloride. Sulfur has 6 valence electrons. Chlorine has 7, but there are four Chlorines; so 6 plus 28 is 34 total valence electrons. Sulfur is the least electronegative, we'll put that at the center, and then we'll put the Chlorines around the outside. There are four Chlorines. We have a total of 34 valence electrons. We'll put a pair between the Sulfur and the Chlorines to form chemical bonds. We've used eight. Then we'll go around the outer atoms: 10, 12, and 32. So at this point in the Lewis structure for SCl4, we've used 32 out of the 34 valence electrons. Since Sulfur's in period 3 on the periodic table, it can have more than eight valence electrons. So we'll just take those last two electrons and put them right there. So now we've used all 34 valence electrons. The octets are satisfied for the Chlorines; and Sulfur has ten valence electrons around it, but that's OK because it's in period 3. If you'll check the formal charges on each of the atoms, you'll find that the formal charges are zero. So this is the best Lewis structure for SCl4. This is Dr. B., thanks for watching.
Preparation and structure
It is obtained by treating sulfur dichloride with chlorine at 193 K:
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(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
It decomposes above −30 °C (242 K) to sulfur dichloride and chlorine.
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(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:
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(3)
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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(4)
- Oxidized by nitric acid:
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(5)
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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This page was last edited on 7 May 2023, at 21:46