Chemistry:Disulfur dibromide
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 Sulfur, S; Bromine, Br
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| Names | |
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| IUPAC names
Disulfur dibromide
Dibromodisulfane | |
| Systematic IUPAC name
Bromosulfanyl thiohypobromite | |
| Identifiers | |
3D model (JSmol)
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| Properties | |
| S 2Br 2 | |
| Molar mass | 223.93 g·mol−1 |
| Appearance | Orange/yellow liquid |
| Density | 2.703 g/cm3 |
| Melting point | −46 °C (−51 °F; 227 K)[1] |
| Boiling point | 46–48 °C (115–118 °F; 319–321 K) (0.1 mmHg) |
| hydrolyzes | |
| Structure | |
| C2 | |
| 2 at sulfur atoms | |
| gauche | |
| Thermochemistry | |
Std molar
entropy (S |
350.52 J/(mol·K)[2] |
Std enthalpy of
formation (ΔfH⦵298) |
30.96 kJ/mol[2] |
| Hazards | |
| Safety data sheet | ICSC 1661 |
| GHS pictograms |   
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| GHS Signal word | Danger |
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Related
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Disulfur dibromide is the inorganic compound with the formula S
2Br
2. It is a yellow-brown liquid that fumes in air. It is prepared by direct combination of the elements and purified by vacuum distillation.[3] Higher yields can be obtained from disulfur dichloride and 50% aqueous hydrobromic acid, but the product must be promptly removed from water, lest it hydrolyze.[1] The compound has no particular application,[citation needed] unlike the related sulfur compound disulfur dichloride, although acidic alcoholysis is "an excellent synthesis of alkyl bromides."[1]
The molecular structure is Br–S–S–Br, akin to that of disulfur dichloride (S
2Cl
2). According to electron diffraction measurements, the angle between the Bra
–S–S and S–S–Brb
planes is 84° and the Br–S–S angle is 107°. The S–S distance is 198.0 pm, circa 5.0 pm shorter than for S
2Cl
2.[4]
References
- ↑ 1.0 1.1 1.2 Magee, Philip S. (1971). "The Sulfur–Bromine Bond". in Senning, Alexander. Sulfur in Organic and Inorganic Chemistry. 1. New York: Marcel Dekker. pp. 264–267. ISBN 0-8247-1615-9.
- ↑ 2.0 2.1 Thermodynamic Properties of Inorganic Materials · Pure Substances. Part 2 _ Compounds from BeBr_g to ZrCl2_g. Springer-Verlag Berlin Heidelberg. 1999. p. 99. ISBN 978-3-540-49411-9. https://materials.springer.com/bp/docs/978-3-540-49411-9.
- ↑ F. Fehér (1963). "Dibromodisulfane". in G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed.. 1. NY, NY: Academic Press. pp. 377–378.
- ↑ Zysman-Colman, Eli; Harpp, David (2004). "Comparison of the Structural Properties of Compounds Containing the XSSX Moiety (X = H, Me, R, Cl, Br, F, OR)". Journal of Sulfur Chemistry 25 (4): 291-316. doi:10.1080/17415990410001710163.
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