Sulfur dichloride
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Names | |||
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IUPAC name
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Other names
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Identifiers | |||
3D model (
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ChemSpider | |||
ECHA InfoCard
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100.031.014 | ||
EC Number |
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PubChem CID
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RTECS number
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UNII | |||
UN number | 1828 | ||
CompTox Dashboard (EPA)
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Properties | |||
SCl2 | |||
Molar mass | 102.96 g·mol−1 | ||
Appearance | Cherry-red liquid | ||
Odor | Pungent | ||
Density | 1.621 g/cm3 | ||
Melting point | −121.0 °C (−185.8 °F; 152.2 K) | ||
Boiling point | 59 °C (138 °F; 332 K) (decomposes) | ||
Insoluble, reacts slowly | |||
−49.4·10−6 cm3/mol | |||
Refractive index (nD)
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1.5570 | ||
Structure | |||
C2v | |||
Bent | |||
Hazards | |||
GHS labelling: | |||
Danger | |||
H314, H335, H400 | |||
P260, P261, P264, P271, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P312, P321, P363, P391, P403+P233, P405, P501 | |||
NFPA 704 (fire diamond) | |||
234 °C (453 °F; 507 K) | |||
Safety data sheet (SDS) | ICSC 1661 | ||
Related compounds | |||
Related
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Related compounds
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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 dichloride is the
organosulfur
compounds. It is a highly corrosive and toxic substance, and it reacts on contact with water to form chlorine-containing acids.
Chlorination of sulfur
SCl2 is produced by the chlorination of either elemental sulfur or disulfur dichloride.[1] The process occurs in a series of steps, some of which are:
- S8 + 4 Cl2 → 4 S2Cl2; ΔH = −58.2 kJ/mol
- S2Cl2 + Cl2 ↔ 2 SCl2; ΔH = −40.6 kJ/mol
The addition of
SCl4
, but this species is unstable at near room temperature. It is likely that several SnCl2 exist where n > 2.
ampules
which develop a slight positive pressure of chlorine, halting the decomposition.
Use of SCl2 in chemical synthesis
SCl2 is used in
thioether[2] A well tested method for the production of the mustard gas bis(2-chloroethyl)sulfide, is the addition of ethylene to sulfur dichloride:[3]
- SCl2 + 2 C2H4 → (ClC2H4)2S
SCl2 is also a precursor to several inorganic sulfur compounds. Treatment with fluoride salts gives SF4 via the decomposition of the intermediate sulfur difluoride. With H2S, SCl2 reacts to give "lower" sulfanes such as S3H2.
Reaction with ammonia affords sulfur nitrides related to S4N4. Treatment of SCl2 with primary amines gives sulfur diimides. One example is di-t-butylsulfurdiimide.[4]
Safety considerations
SCl2
]References
- ^ F. Fehér "Dichloromonosulfane" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 370.
- ^ Bishop, Roger (1992). "9-Thiabicyclo[3.3.1]nonane-2,6-dione". Organic Syntheses. 70: 120; Collected Volumes, vol. 9, p. 692.
- ISBN 0-471-95512-4.
- PMID 4962859.