Sulfur tetrafluoride

| Molecular geometry | |-

| NFPA-H = 3 | NFPA-F = 0 | NFPA-R = 2 | NFPA-S = W Selenium tetrafluoride Tellurium tetrafluoride Sulfur difluoride Disulfur decafluoride Sulfur hexafluoride Disulfur dibromide Sulfur trifluoride

Sulfur tetrafluoride is a chemical compound with the formula SF4. It is a colorless corrosive gas that releases dangerous hydrogen fluoride gas upon exposure to water or moisture. Sulfur tetrafluoride is a useful reagent for the preparation of organofluorine compounds, some of which are important in the pharmaceutical and specialty chemical industries.

Structure

Sulfur in SF4 is in the +4 oxidation state, with one lone pair of electrons. The atoms in SF4 are arranged in a see-saw shape, with the sulfur atom at the center. One of the three equatorial positions is occupied by a nonbonding lone pair of electrons. Consequently, the molecule has two distinct types of F ligands, two axial and two equatorial. The relevant bond distances are S–Fax = 164.3 pm and S–Feq = 154.2 pm. It is typical for the axial ligands in hypervalent molecules to be bonded less strongly.

The 19F NMR spectrum of SF4 reveals only one signal, which indicates that the axial and equatorial F atom positions rapidly interconvert via pseudorotation.

Synthesis and manufacture

At the laboratory scale, sulfur tetrafluoride is prepared from elemental sulfur and cobaltic fluoride :S + 4CoF3 → SF4 + 4CoF2

SF4 is industrially produced by the reaction of SCl2 and NaF with acetonitrile as a catalyst :3 SCl2 + 4 NaF → SF4 + S2Cl2 + 4 NaCl At higher temperatures (e.g. 225–450 °C), the solvent is superfluous. Moreover, sulfur dichloride may be replaced by elemental sulfur (S) and chlorine (Cl2).

A low-temperature (e.g. 20–86 °C) alternative to the chlorinative process above uses liquid bromine (Br2) as oxidant and solvent: :S(s) + 2 Br2(l; excess) + 4KF(s) → SF4↑ + 4 KBr(brom)

Use in synthesis of organofluorine compounds

Main article: Fluorination by sulfur tetrafluoride

In organic synthesis, SF4 is used to convert COH and C=O groups into CF and CF2 groups, respectively. The efficiency of these conversions are highly variable.

In the laboratory, the use of SF4 has been superseded by the safer and more easily handled diethylaminosulfur trifluoride, (C2H5)2NSF3, "DAST": This reagent is prepared from SF4: :

Other reactions

Sulfur chloride pentafluoride (), a useful source of the SF5 group, is prepared from SF4. : Hydrolysis of SF4 gives sulfur dioxide: :SF4 + 2 H2O → SO2 + 4 HF This reaction proceeds via the intermediacy of thionyl fluoride, which usually does not interfere with the use of SF4 as a reagent.

When amines are treated with SF4 and a base, aminosulfur difluorides result.

Toxicity

reacts inside the lungs with moisture, forming sulfur dioxide and hydrogen fluoride which forms highly toxic and corrosive hydrofluoric acid

References

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References

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