Radon difluoride (RnF
2) is a compound of radon, a radioactive noble gas. Radon reacts readily with fluorine to form a solid compound, but this decomposes on attempted vaporization and its exact composition is uncertain.[1][2] Calculations suggest that it may be ionic,[3] unlike all other known binary noble gas compounds. The usefulness of radon compounds is limited because of the radioactivity of radon. The longest-lived isotope, radon-222, has a half-life of only 3.82 days, which decays by α-emission to yield polonium-218.[4]
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| Names | |
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| IUPAC name
Radon difluoride
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| Other names
Radon(II) fluoride
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
CompTox Dashboard (EPA)
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| Properties | |
| RnF2 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Preparation
editWhen radon is heated to 400 °C with fluorine, radon difluoride is formed.[1]
Reactions
editRadon difluoride can be reduced to radon and hydrogen fluoride when heated with hydrogen gas at 500 °C.[1]
References
edit- ^ a b c Fields, Paul R.; Stein, Lawrence; Zirin, Moshe H. (1962). "Radon Fluoride". Journal of the American Chemical Society. 84 (21): 4164–4165. doi:10.1021/ja00880a048.
- ^ Stein, Lawrence (1970). "Ionic Radon Solution". Science. 168 (3929): 362–4. Bibcode:1970Sci...168..362S. doi:10.1126/science.168.3929.362. PMID 17809133. S2CID 31959268.
- ^ Pitzer, Kenneth S. (1975). "Fluorides of radon and element 118". J. Chem. Soc., Chem. Commun. (18): 760b–761. doi:10.1039/C3975000760b.
- ^ Stein, Lawrence (1987). "Chemical Properties of Radon". Radon and its Decay Products. ACS Symposium Series. Vol. 331. pp. 240–251. doi:10.1021/bk-1987-0331.ch018. ISBN 978-0-8412-1015-8.
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