Diphosphorus tetrafluoride
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Names | |||
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IUPAC name
difluorophosphanyl(difluoro)phosphane
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Other names
tetrafluorodiphosphine; phosphorus difluoride
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Identifiers | |||
3D model (JSmol)
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ChemSpider | |||
PubChem CID
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CompTox Dashboard (EPA)
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Properties | |||
F4P2 | |||
Molar mass | 137.941136648 g·mol−1 | ||
Melting point | −86.5 °C (−123.7 °F; 186.7 K) | ||
Boiling point | −6.2 °C (20.8 °F; 266.9 K) | ||
Related compounds | |||
Other anions
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Diphosphorus tetrachloride Diphosphorus tetraiodide | ||
Other cations
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dinitrogen tetrafluoride | ||
Related Binary Phosphorus halides
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phosphorus trifluoride phosphorus pentafluoride | ||
Related compounds
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diphosphane diphosphines | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |||
Infobox references | |||
Diphosphorus tetrafluoride is a gaseous compound of phosphorus and fluorine with formula P2F4. Two fluorine atoms are connected to each phosphorus atom, and there is a bond between the two phosphorus atoms. Phosphorus can be considered to have oxidation state +2, as indicated by the name phosphorus difluoride.[1]
Production[]
When it was discovered in 1966 by , and at the , they allowed to react with mercury at room temperature.[2]
2PF2I +2Hg → P2F4 + Hg2I2
Properties[]
The P-P bond in diphosphorus tetrafluoride is much stronger than the corresponding N-N bond in dinitrogen tetrafluoride which easily breaks into nitrogen difluoride.[2]
The infrared spectrum has absorption at 842 cm−1, 830 cm−1, 820 cm−1, and weaker at 408 cm−1 and 356 cm−1.[2]
The molecule has C2h symmetry.[3]
Reactions[]
Under ultraviolet light diphosphorus tetrafluoride reacts with alkynes connected to trifluoromethyl groups to add difluorophosphino (-PF2) groups on each side of a double bond. Other kinds of alkynes produced polymers with this treatment.[4] With alkenes, similarly bis(difluorophosphino) is added across the double bond.[5]
Diphosphorus tetrafluoride reacts with diborane to yield another gas P2F4•BH3 which does not condense above −85°C. This decomposes to yet another gas PF3•BH3 and a polymer with formula PF.[6]
Diphosphorus tetrafluoride reacts with oxygen to yield diphosphorus tetrafluoride oxide, which has one oxygen atom inserted between the two phosphorus atoms. PF2OPF2[2] This also is a gas with boiling point around −18°C. It is also produced in the reaction with water. 2P2F2 + H2O →2PHF2 + F2POPF2.[7]
References[]
- ^ Toy, Arthur D. F. (2016). The Chemistry of Phosphorus: Pergamon Texts in Inorganic Chemistry. Elsevier. p. 418. ISBN 978-1-4831-3959-3.
- ^ a b c d Lustig, Max; Ruff, John K.; Colburn, Charles B. (August 1966). "Diphosphorus Tetrafluoride and Diphosphorus Oxytetrafluoride". Journal of the American Chemical Society. 88 (16): 3875. doi:10.1021/ja00968a046.
- ^ Rhee, Kee H.; Snider, A.Monroe; Miller, Foil A. (June 1973). "Infrared and Raman spectra and structure of P2F4". Spectrochimica Acta Part A: Molecular Spectroscopy. 29 (6): 1029–1035. Bibcode:1973AcSpA..29.1029R. doi:10.1016/0584-8539(73)80142-4.
- ^ Morse, J.G.; Mielcarek, J.J. (July 1988). "Photoreactions of tetrafluorodiphosphine with alkynes". Journal of Fluorine Chemistry. 40 (1): 41–49. doi:10.1016/S0022-1139(00)81060-X.
- ^ Morse, Joseph G.; Morse, Karen W. (March 1975). "Photoreactions of tetrafluorodiphosphine with nonsubstituted olefins and perfluoroolefins". Inorganic Chemistry. 14 (3): 565–569. doi:10.1021/ic50145a024.
- ^ Morse, Karen W.; Parry, Robert W. (January 1967). "The Basic Properties of Tetrafluorodiphosphine. The Synthesis of Tetrafluorodiphosphine Borane". Journal of the American Chemical Society. 89 (1): 172–173. doi:10.1021/ja00977a049.
- ^ Rudolph, R. W.; Taylor, R. C.; Parry, R. W. (August 1966). "Fluorophosphine Ligands. III. Syntheses Involving PF I. The Preparation and Characterization of μ-Oxo-bisdifluorophosphine, Cyanodifluorophosphine, and Tetrafluorodiphosphine". Journal of the American Chemical Society. 88 (16): 3729–3734. doi:10.1021/ja00968a010. PMID 5916370.
- Phosphorus halides
- Fluorine compounds