Sulfur chloride pentafluoride is an inorganic compound with the formula SF5Cl. It exists as a colorless gas at room temperature and is highly toxic, like most inorganic compounds containing the pentafluorosulfide (–SF5) functional group. The compound adopts an octahedral geometry with C
4v symmetry. Sulfur chloride pentafluoride is the only commercially available reagent for adding the –SF5 group to organic compounds.
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| Other names Pentafluorochlorosulfanyl | |||
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| ECHA InfoCard | 100.034.014 | ||
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| Properties | |||
Chemical formula | SF5Cl | ||
| Molar mass | 162.510 g/mol | ||
| Appearance | Colorless gas | ||
| Density | 6.642 g/dm3 | ||
| Melting point | −64 °C (−83 °F; 209 K) | ||
| Boiling point | −19 °C (−2 °F; 254 K) | ||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards | Toxic | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). (what is ?) Infobox references | |||
Reactivity
SF5Cl is highly reactive and toxic. In contrast, sulfur hexafluoride (SF6) is inert and nontoxic despite having a closely related chemical formula. This difference highlights the lability of the S–Cl bond in SF5Cl.
Under free-radical conditions, SF5Cl adds across double bonds. The following reaction occurs with propene:
- CH
3CH=CH
2 + SF
5Cl → CH3CHClCH2SF5
The addition reaction is catalyzed by (CH3CH2)3B at around −30 °C. SF5Br is used similarly.
SF5Cl is also a precursor to O(SF5)2 and F2NSF5 (from tetrafluorohydrazine).
Synthesis
Sulfur chloropentafluoride can be synthesized by several routes, starting from two lower sulfur fluorides, sulfur tetrafluoride and disulfur decafluoride:
- SF4 + Cl2 + CsF → SF5Cl + CsCl
- ClF + SF4 → SF5Cl
- S2F10 + Cl2 → 2 SF5Cl
The corresponding SF
5Br is prepared similarly from in-situ generated bromine monofluoride.
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