Thionyl tetrafluoride

Last updated
Thionyl tetrafluoride
Sulfur oxytetrafluoride.png
Ball-and-stick model of thionyl tetrafluoride Thionyl-tetrafluoride-3D-balls.png
Ball-and-stick model of thionyl tetrafluoride
Space-filling model of thionyl tetrafluoride Thionyl-tetrafluoride-3D-SF.png
Space-filling model of thionyl tetrafluoride
Names
IUPAC name
Thionyl tetrafluoride
Identifiers
3D model (JSmol)
ChemSpider
PubChem CID
  • InChI=1S/F4OS/c1-6(2,3,4)5 X mark.svgN
    Key: DUGWRBKBGKTKOX-UHFFFAOYSA-N X mark.svgN
  • O=S(F)(F)(F)F
Properties
SOF4
Appearancecolorless gas
Density 1.653−0.0036T (°C) liquid [1]
Melting point −99.6 °C (−147.3 °F; 173.6 K)
Boiling point −49 °C (−56 °F; 224 K) 5090 cal/mol heat of vapourisation [1]
reaction in water
log P 7.2349−859.58/T−26275/T² [1]
Structure
distorted trigonal bipyramid
Hazards
GHS labelling:
GHS-pictogram-acid.svg GHS-pictogram-skull.svg
Danger
H300, H310, H314, H330
P260, P262, P264, P270, P271, P280, P284, P301+P310, P301+P330+P331, P302+P350, P303+P361+P353, P304+P340, P305+P351+P338, P310, P320, P321, P322, P330, P361, P363, P403+P233, P405, P501
Related compounds
Related oxohalides
 Thionyl fluoride
Selenyl tetrafluoride
Related compounds
 Phosphoryl trifluoride
pentafluorosulfur hypofluorite
sulfuryl fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

Thionyl tetrafluoride, also known as sulfur tetrafluoride oxide, is an inorganic compound with the formula S O F 4. It is a colorless gas.

Contents

The shape of the molecule is a distorted trigonal bipyramid, with the oxygen found on the equator. The atoms on the equator have shorter bond lengths than the fluorine atoms on the axis. The sulfur oxygen bond is 1.409Å. A S−F bond on the axis has length 1.596Å and the S−F bond on the equator has length 1.539Å. The angle between the equatorial fluorine atoms is 112.8°. The angle between axial fluorine and oxygen is 97.7°. The angle between oxygen and equatorial fluorine is 123.6° and between axial and equatorial fluorine is 85.7°. [2] The fluorine atoms only produce one NMR line, probably because they exchange positions. [1] It is isoelectronic with phosphorus pentafluoride.

Formation

Thionyl fluoride reacting with fluorine gas can produce thionyl tetrafluoride. [1] This was how the gas was first discovered by Moissan and Lebeau in 1902. They identified the formula by the pressure changes resulting from the reaction. Silver fluoride and platinum are capable of catalyzing the reaction.

It can also be formed the reaction of silver difluoride with thionyl fluoride at 392 °F (200 °C), [3] or by electrolyzing hydrogen fluoride with a solution of sulfur dioxide, which also made oxygen difluoride and sulfuryl fluoride. Thionyl chloride or thionyl fluoride electrolyzed with hydrogen fluoride produced even more of the gas. [4]

Reactions

Thionyl tetrafluoride reacts with water to make hydrofluoric acid, sulfurofluoridic acid, and sulfuryl difluoride. Mercury can strip off fluoride to make thionyl fluoride and mercurous fluoride. Strong bases result in formation of fluoride and fluorosulfate ions. [1]

Reactions with the strong Lewis acids, such as AsF5 and SbF5, result in the formation SOF3+ cation and the corresponding salts SOF3[AsF6] and SOF3[SbF6], respectively. [5]

Click chemistry

Thionyl tetrafluoride can be used in click chemistry through reactions with primary amines known as sulfur(VI) fluoride exchange (SuFEx). [6] This kind of reaction was the first "click" reaction to generate a three-dimensional core.

Related Research Articles

<span class="mw-page-title-main">Oxygen difluoride</span> Chemical compound

Oxygen difluoride is a chemical compound with the formula OF2. As predicted by VSEPR theory, the molecule adopts a bent molecular geometry. It is a strong oxidizer and has attracted attention in rocketry for this reason. With a boiling point of −144.75 °C, OF2 is the most volatile (isolable) triatomic compound. The compound is one of many known oxygen fluorides.

<span class="mw-page-title-main">Trigonal bipyramidal molecular geometry</span> Molecular structure with atoms at the center and vertices of a triangular bipyramid

In chemistry, a trigonal bipyramid formation is a molecular geometry with one atom at the center and 5 more atoms at the corners of a triangular bipyramid. This is one geometry for which the bond angles surrounding the central atom are not identical, because there is no geometrical arrangement with five terminal atoms in equivalent positions. Examples of this molecular geometry are phosphorus pentafluoride, and phosphorus pentachloride in the gas phase.

Antimony pentafluoride is the inorganic compound with the formula SbF5. This colourless, viscous liquid is a strong Lewis acid and a component of the superacid fluoroantimonic acid, formed upon mixing liquid HF with liquid SbF5 in 1:1 ratio. It is notable for its strong Lewis acidity and the ability to react with almost all known compounds.

<span class="mw-page-title-main">Xenon difluoride</span> Chemical compound

Xenon difluoride is a powerful fluorinating agent with the chemical formula XeF
2, and one of the most stable xenon compounds. Like most covalent inorganic fluorides it is moisture-sensitive. It decomposes on contact with water vapor, but is otherwise stable in storage. Xenon difluoride is a dense, colourless crystalline solid.

<span class="mw-page-title-main">Sulfur tetrafluoride</span> Chemical compound

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.

<span class="mw-page-title-main">Selenium tetrafluoride</span> Chemical compound

Selenium tetrafluoride (SeF4) is an inorganic compound. It is a colourless liquid that reacts readily with water. It can be used as a fluorinating reagent in organic syntheses (fluorination of alcohols, carboxylic acids or carbonyl compounds) and has advantages over sulfur tetrafluoride in that milder conditions can be employed and it is a liquid rather than a gas.

<span class="mw-page-title-main">Xenon oxytetrafluoride</span> Chemical compound

Xenon oxytetrafluoride is an inorganic chemical compound. It is an unstable colorless liquid with a melting point of −46.2 °C that can be synthesized by partial hydrolysis of XeF
6, or the reaction of XeF
6 with silica or NaNO
3:

<span class="mw-page-title-main">Dioxygenyl</span> Chemical compound

The dioxygenyl ion, O+
2, is a rarely-encountered oxycation in which both oxygen atoms have a formal oxidation state of +⁠1/2⁠. It is formally derived from oxygen by the removal of an electron:

Arsenic pentafluoride is a chemical compound of arsenic and fluorine. It is a toxic, colorless gas. The oxidation state of arsenic is +5.

<span class="mw-page-title-main">Selenoyl fluoride</span> Chemical compound

Selenoyl fluoride, selenoyl difluoride, selenium oxyfluoride, or selenium dioxydifluoride is a chemical compound with the formula SeO2F2.

<span class="mw-page-title-main">Germanium tetrafluoride</span> Chemical compound

Germanium tetrafluoride (GeF4) is a chemical compound of germanium and fluorine. It is a colorless gas.

In chemistry, molecular oxohalides (oxyhalides) are a group of chemical compounds in which both oxygen and halogen atoms are attached to another chemical element A in a single molecule. They have the general formula AOmXn, where X is a halogen. Known oxohalides have fluorine (F), chlorine (Cl), bromine (Br), and/or iodine (I) in their molecules. The element A may be a main group element, a transition element, a rare earth element or an actinide. The term oxohalide, or oxyhalide, may also refer to minerals and other crystalline substances with the same overall chemical formula, but having an ionic structure.

<span class="mw-page-title-main">Thiophosphoryl fluoride</span> Chemical compound

Thiophosphoryl fluoride is an inorganic molecular gas with formula PSF3 containing phosphorus, sulfur and fluorine. It spontaneously ignites in air and burns with a cool flame. The discoverers were able to have flames around their hands without discomfort, and called it "probably one of the coldest flames known". The gas was discovered in 1888.

Fluorine forms a great variety of chemical compounds, within which it always adopts an oxidation state of −1. With other atoms, fluorine forms either polar covalent bonds or ionic bonds. Most frequently, covalent bonds involving fluorine atoms are single bonds, although at least two examples of a higher order bond exist. Fluoride may act as a bridging ligand between two metals in some complex molecules. Molecules containing fluorine may also exhibit hydrogen bonding. Fluorine's chemistry includes inorganic compounds formed with hydrogen, metals, nonmetals, and even noble gases; as well as a diverse set of organic compounds. For many elements the highest known oxidation state can be achieved in a fluoride. For some elements this is achieved exclusively in a fluoride, for others exclusively in an oxide; and for still others the highest oxidation states of oxides and fluorides are always equal.

Difluoroamino sulfur pentafluoride is a gaseous chemical compound of fluorine, sulfur, and nitrogen. It is unusual in having a hexa-coordinated sulfur atom with a link to nitrogen. Other names for this substance include difluoro(pentafluorosulfur)amine, pentafluorosulfanyldifluoramine, and pentafluorosulfanyl N,N-difluoramine.

<span class="mw-page-title-main">Difluorodisulfanedifluoride</span> Chemical compound

1,1,1,2-tetrafluorodisulfane, also known as 1,2-difluorodisulfane 1,1-difluoride or just difluorodisulfanedifluoride (FSSF3) is an unstable molecular compound of fluorine and sulfur. The molecule has a pair of sulfur atoms, with one fluorine atom on one sulfur, and three fluorine atoms on the other. It has the uncommon property that all the bond lengths are different. The bond strength is not correlated with bond length but is inversely correlated with the force constant (Badger's rule). The molecule can be considered as sulfur tetrafluoride in which a sulfur atom is inserted into a S-F bond.

Pentafluorosulfur hypofluorite is an oxyfluoride of sulfur in the +6 oxidation state, with a fluorine atom attached to oxygen. The formula is SOF6. In standard conditions it is a gas.

<span class="mw-page-title-main">Chlorine trifluoride oxide</span> Chemical compound

Chlorine oxide trifluoride or chlorine trifluoride oxide is a corrosive liquid molecular compound with formula ClOF3. It was developed secretly as a rocket fuel oxidiser.

<span class="mw-page-title-main">Molybdenum oxytetrafluoride</span> Chemical compound

Molybdenum oxytetrafluoride is the inorganic compound with the formula MoOF4. It is a white, diamagnetic solid. According to X-ray crystallography, it is a coordination polymer consisting of a linear chain of alternating Mo and F atoms. Each Mo center is octahedral, the coordination sphere being defined by oxide, three terminal fluorides, and two bridging fluorides. In contrast to this motif, tungsten oxytetrafluoride crystallizes as a tetramer, again with bridging fluoride ligands.

Pentafluoroselenium hypofluorite is a selenium compound with the chemical formula SeOF6. It was discovered at 1959.

References

  1. 1 2 3 4 5 6 Harry Julius Emeléus and A.G. Sharpe Advances in Inorganic Chemistry Volume 2 Academic Press 1960 page 117
  2. ↑ Hedberg, Lise; Hedberg, Kenneth (March 1982). "Thionyl tetrafluoride. Reanalysis of the molecular structure and resolution of the multiple model problem". The Journal of Physical Chemistry. 86 (5): 598–602. doi:10.1021/j100394a004.
  3. ↑ Dudley, F. B. (1956). "Pentafluorosulfur Hypofluorite and Thionyl Tetrafluoride". Journal of the American Chemical Society. 78 (8): 1553–1557. doi:10.1021/ja01589a013.
  4. ↑ Nagase, Shunji; Abe, Takashi; Baba, Hajime (1 July 1969). "Fluorination of Inorganic Sulfur Compounds". Bulletin of the Chemical Society of Japan. 42 (7): 2062–2064. doi:10.1246/bcsj.42.2062.
  5. ↑ Brownstein, M.; Dean, P. A. W.; Gillespie, R. J. (1970-01-01). "The trifluorosulphur(VI) oxide cation, SOF3+". Journal of the Chemical Society D: Chemical Communications (1): 9–9. doi:10.1039/C29700000009. ISSN   0577-6171.
  6. ↑ Li, Suhua; Wu, Peng; Moses, John E.; Sharpless, K. Barry (2017-02-01). "Multidimensional SuFEx Click Chemistry: Sequential Sulfur(VI) Fluoride Exchange Connections of Diverse Modules Launched From An SOF4 Hub". Angewandte Chemie International Edition. 56 (11): 2903–2908. doi:10.1002/anie.201611048. ISSN   1521-3773. PMC   5434761 . PMID   28165188.
This page is based on this Wikipedia article
Text is available under the CC BY-SA 4.0 license; additional terms may apply.
Images, videos and audio are available under their respective licenses.