Pentafluoroselenium hypofluorite

Last updated
Pentafluoroselenium hypofluorite
Pentafluoroselenium hypofluorite.svg
Names
IUPAC name
Pentafluoro(fluorooxy)-λ6-selane
Identifiers
3D model (JSmol)
ChemSpider
PubChem CID
  • InChI=1S/F6OSe/c1-7-8(2,3,4,5)6
    Key: DOWDYMDJZSUENF-UHFFFAOYSA-N
  • InChI=1/F6OSe/c1-7-8(2,3,4,5)6
    Key: DOWDYMDJZSUENF-UHFFFAOYAU
  • F[Se](F)(F)(F)(F)OF
Properties
SeOF6
Molar mass 208.950
Appearancewhite solid [1]
Odor strong and irritating [2]
Melting point −54°C [2]
Boiling point −30°C [3]
decomposes
Related compounds
Other cations
Pentafluorosulfur hypofluorite
Pentafluorotellurium hypofluorite
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Pentafluoroselenium hypofluorite is a selenium compound with the chemical formula SeOF6. It was discovered at 1959. [4]

Contents

Preparation

Pentafluoroselenium hypofluorite can be produced from the reaction of selenium dioxide or selenium oxychloride with fluorine gas in the presence of silver difluoride catalyst. However, the reaction yield is low (14% [3] ), and it is hard to purify due to large amount of SeF6 byproduct. [4]

Pentafluoroselenium hypofluorite can also formed from selenium oxyfluoride and fluorine gas in the presence of potassium fluoride. [4] [5]

SeOF2 + KF → K+[SeOF3]− —F2→ K+[SeOF5]− —F2→ KF + SeOF6

The reaction of fluorine gas and Hg(OSeF5)2 produces SeOF6 in much higher yield and with less SeF6. [3]

Reactions

Pentafluoroselenium hypofluorite is reactive, but not as reactive as pentafluorosulfur hypofluorite. [3] It reacts with water to release oxygen gas. It reacts with potassium hydroxide too, forming potassium selenate, potassium fluoride, water and oxygen gas. [2] ：

2 SeOF6 + 16 KOH → 2 K2SeO4 + 12 KF + 8 H2O + O2↑

SeOF6 can also oxidize potassium iodide into iodine. [1] It explodes upon reacting with ethylene, and the reaction with perfluorocyclopentene produces F5SeOC5F9. [4] SeOF6 reacts with sulfur tetrafluoride to produce thionyl fluoride, thionyl tetrafluoride, sulfuryl fluoride, selenium hexafluoride and F5SOSeF5. [4] SeOF6 reacts very slowly with carbon monoxide, and produces F5SeOCFO at 65°C. [4] SeOF6 reacts with bromine to form BrOSeF5. [5]

Related Research Articles

<span class="mw-page-title-main">Nickel(II) fluoride</span> Chemical compound

Nickel(II) fluoride is the chemical compound with the formula NiF2. It is an ionic compound of nickel and fluorine and forms yellowish to green tetragonal crystals. Unlike many fluorides, NiF2 is stable in air.

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

Bromine pentafluoride, BrF5, is an interhalogen compound and a fluoride of bromine. It is a strong fluorinating agent.

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

Platinum hexafluoride is the chemical compound with the formula PtF6, and is one of seventeen known binary hexafluorides. It is a dark-red volatile solid that forms a red gas. The compound is a unique example of platinum in the +6 oxidation state. With only four d-electrons, it is paramagnetic with a triplet ground state. PtF6 is a strong fluorinating agent and one of the strongest oxidants, capable of oxidising xenon and O2. PtF6 is octahedral in both the solid state and in the gaseous state. The Pt-F bond lengths are 185 picometers.

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">Hydrogen fluoride</span> Chemical compound

Hydrogen fluoride (fluorane) is an inorganic compound with chemical formula HF. It is a very poisonous, colorless gas or liquid that dissolves in water to yield an aqueous solution termed hydrofluoric acid. It is the principal industrial source of fluorine, often in the form of hydrofluoric acid, and is an important feedstock in the preparation of many important compounds including pharmaceuticals and polymers, e.g. polytetrafluoroethylene (PTFE). HF is also widely used in the petrochemical industry as a component of superacids. Due to strong and extensive hydrogen bonding, it boils at near room temperature, much higher than other hydrogen halides.

<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:

<span class="mw-page-title-main">Manganese(IV) fluoride</span> Chemical compound

Manganese tetrafluoride, MnF4, is the highest fluoride of manganese. It is a powerful oxidizing agent and is used as a means of purifying elemental fluorine.

Arsenic trifluoride is a chemical compound of arsenic and fluorine with the chemical formula AsF3. It is a colorless liquid which reacts readily with water.

Dinitrogen difluoride is a chemical compound with the formula N2F2. It is a gas at room temperature, and was first identified in 1952 as the thermal decomposition product of the fluorine azide. It has the structure F−N=N−F and exists in both cis and trans isomers, as typical for diimides.

<span class="mw-page-title-main">Palladium(II) fluoride</span> Chemical compound

Palladium(II) fluoride, also known as palladium difluoride, is the chemical compound of palladium and fluorine with the formula PdF2.

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

Thionyl tetrafluoride, also known as sulfur tetrafluoride oxide, is an inorganic compound with the formula SOF4. It is a colorless gas.

<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.

Chromium pentafluoride is the inorganic compound with the chemical formula CrF5. It is a red volatile solid that melts at 34 °C. It is the highest known chromium fluoride, since the hypothetical chromium hexafluoride has not yet been synthesized.

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.

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

Platinum tetrafluoride is the inorganic compound with the chemical formula PtF
4. In the solid state, the compound features platinum(IV) in octahedral coordination geometry.

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">Terbium(IV) fluoride</span> Chemical compound

Terbium(IV) fluoride is an inorganic compound with a chemical formula TbF4. It is a white solid that is a strong oxidizer. It is also a strong fluorinating agent, emitting relatively pure atomic fluorine when heated, rather than the mixture of fluoride vapors emitted from cobalt(III) fluoride or cerium(IV) fluoride.

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

Seleninyl fluoride is an oxyfluoride of selenium with the chemical formula SeOF2.

References

  1. 1 2 Holloway, John H.; Laycock, David (1983). "Preparations and Reactions of Inorganic Main-Group Oxide Fluorides". Advances in Inorganic Chemistry. Vol. 27. Elsevier. pp. 157–195. doi:10.1016/s0898-8838(08)60107-5. ISBN   978-0-12-023627-5. ISSN   0898-8838.
  2. 1 2 3 Mitra, Grihapati; Cady, George H. (1959). "Preparation and Properties of Pentafluoroselenium Hypofluorite (F5SeOF) and Bis-(pentafluoroselenium) Peroxide (F5SeOOSeF5)". Journal of the American Chemical Society. 81 (11). American Chemical Society (ACS): 2646–2648. doi:10.1021/ja01520a012. ISSN   0002-7863.
  3. 1 2 3 4 Shreeve, Jean'Ne M. (1983). "Fluorinated Hypofluorites and Hypochlorites". Advances in Inorganic Chemistry. Vol. 26. Elsevier. pp. 119–168. doi:10.1016/s0898-8838(08)60092-6. ISBN   978-0-12-023626-8. ISSN   0898-8838.
  4. 1 2 3 4 5 6 James Everett Smith, George H. Cady (June 1970). "Reactions of fluoroxypentafluoroselenium". Inorganic Chemistry. 9 (6): 1442–1445. doi:10.1021/ic50088a029. ISSN   0020-1669 . Retrieved 2022-02-02.
  5. 1 2 Seppelt, Konrad (1973). "Halogenderivate der Pentafluoroorthoselensäure". Chemische Berichte. 106 (1). Wiley: 157–164. doi:10.1002/cber.19731060119. ISSN   0009-2940.
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.