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| Names | |||
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| IUPAC name
fluorosulfanyl thiohypofluorite
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| Other names
Difluorodisulfane[1]
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| Identifiers | |||
3D model (JSmol)
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PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |||
| S2F2 | |||
| Molar mass | 102.127 g/mol | ||
| Melting point | −133 °C (−207 °F; 140 K) | ||
| Boiling point | 15 °C (59 °F; 288 K) | ||
| Related compounds | |||
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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Disulfur difluoride is an inorganic compound with the chemical formula S2F2. It is a halide of sulfur.
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Transcription
Structure
Disulfur difluoride has a chain structure F−S−S−F. The angle between the Fa−S−S and S−S−Fb planes is 87.9°, while the angles of Fa−S−S and S−S−Fb are equivalent, and are equal to 108.3°. Both S−F bonds are equivalent and their length is 163.5 pm, while the length of the S−S bond is 189 pm. This structure is referred to as gauche, and is similar to H2O2.
There is a branched isomer of disulfur difluoride, thiothionyl fluoride, with the structure S=SF2.
Synthesis
Silver(II) fluoride can fluorinate sulfur in a strictly dry container at 125 °C (257 °F; 398 K), and the reaction produces FS−SF:[2]
Reactions
Disulfur difluoride undergoes intramolecular rearrangement in the presence of fluorides of alkali metals, yielding the isomer S=SF2:[3]
- FS−SF → S=SF2
- Decomposing to sulfur tetrafluoride and sulfur when heated to 180 °C:
- 2 S2F2 → SF4 + 3 S
- Reacting with sulfuric acid at 80 °C:
- S2F2 + 3 H2SO4 → 5 SO2 + 2 HF + 2 H2O
- Reacting with sodium hydroxide:
- Reacting with oxygen at high pressure, using nitrogen dioxide as a catalyst:
References
- ^ "Difluorodisulfane".
- ^ Davis, R.Wellington; Firth, Steven (1991). "The microwave spectrum of the chain isomer of disulfur difluoride: FS-SF". Journal of Molecular Spectroscopy. 145 (2): 225. doi:10.1016/0022-2852(91)90109-N.
- ^ Davis, R.Wellington (1986). "The microwave spectrum of the pyramidal isomer of disulfur difluoride: S=SF2". Journal of Molecular Spectroscopy. 116 (2): 371–383. doi:10.1016/0022-2852(86)90134-7.
- ^ Справочник химика / Редкол.: Никольский Б.П. и др.. — 3-е изд., испр. — Л.: Химия, 1971. — Т. 2. — 1168 с. (in Russian)
- ^ Химическая энциклопедия / Редкол.: Кнунянц И.Л. и др.. — М.: Советская энциклопедия, 1995. — Т. 4. — 639 с. — ISBN 978-5-85270-092-6 (in Russian)
- ^ Лидин Р.А. и др. Химические свойства неорганических веществ: Учеб. пособие для вузов. — 3-е изд., испр. — М.: Химия, 2000. — 480 с. — ISBN 978-5-7245-1163-6 (in Russian)
This page was last edited on 4 February 2024, at 20:20