Difference between revisions of "Actinium fluoride"
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| − | '''Actinium fluoride''', AcF<sub>3</sub>, is the only known binary [[fluoride]] of [[actinium]]. It has been prepared (on a 10-µg scale) by the reaction of [[actinium hydroxide]] with [[hydrofluoric acid]], and will also precipitate out when soluble actinium salts are treated with fluoride ions.<ref name=" | + | '''Actinium fluoride''', AcF<sub>3</sub>, is the only known binary [[fluoride]] of [[actinium]]. It has been prepared (on a 10-µg scale) by the reaction of [[actinium hydroxide]] with [[hydrofluoric acid]], and will also precipitate out when soluble actinium salts are treated with fluoride ions.<ref name="Fried"/><ref name="K&M"/> It reacts with [[ammonia]] and [[water]] vapour at 900–1000 °C to give the [[Actinium oxofluoride|oxofluoride]].<ref name="Fried"/><ref name="K&M"/> |
==Notes and references== | ==Notes and references== | ||
Revision as of 11:51, 9 January 2011
| Actinium fluoride | |
|---|---|
| Other names | Actinium(III) fluoride Actinium trifluoride |
| Identifiers | |
| Standard InChI | InChI=1S/Ac.3FH/h;3*1H/q+3;;;/p-3 |
| Standard InChIKey | HPPLGHKTZRXLTB-UHFFFAOYSA-K |
| CAS number | [] |
| Properties[1] | |
| Chemical formula | AcF3 |
| Molar mass | 284.02 g mol−1 [note 1] |
| Appearance | white solid |
| Density | 7.88 g cm−3 |
| Solubility in water | insoluble |
| Structure[5] | |
| Crystal structure | Lanthanum trifluoride |
| Lattice constant | a = 741(1) pm, c = 753(2) pm |
| Related compounds | |
| Other anions | Actinium chloride Actinium bromide Actinium iodide |
| Other cations | Scandium fluoride Yttrium fluoride Lanthanum fluoride |
| Other compounds | Actinium oxofluoride |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Actinium fluoride, AcF3, is the only known binary fluoride of actinium. It has been prepared (on a 10-µg scale) by the reaction of actinium hydroxide with hydrofluoric acid, and will also precipitate out when soluble actinium salts are treated with fluoride ions.[4][5] It reacts with ammonia and water vapour at 900–1000 °C to give the oxofluoride.[4][5]
Notes and references
Notes
- ↑ The molar mass is based on actinium-227 (t½ = 21.772(3) a; Ar = 227.027 7521(26)),[2] the most commonly encountered isotope of actinium and the one used in the original chemical studies.[3][4]
References
- ↑ CRC Handbook of Chemistry and Physics, 62nd ed.; Weast, Robert C., Ed.; CRC Press: Boca Raton, FL, 1981; p B-73. ISBN 0-8493-0462-8.
- ↑ Audi, G.; Bersillon, O.; Blachot, J.; Wapstra, A. H. The NUBASE evaluation of nuclear and decay properties. Nucl. Phys. A 2003, 729, 3–128. doi:10.1016/j.nuclphysa.2003.11.001, <http://amdc.in2p3.fr/nubase/Nubase2003.pdf>.
- ↑ Hagemann, French The Isolation of Actinium. J. Am. Chem. Soc. 1950, 72 (2), 768–71. DOI: 10.1021/ja01158a033.
- ↑ 4.0 4.1 4.2 Fried, Sherman; Hagemann, French; Zachariasen, W. H. The Preparation and Identification of Some Pure Actinium Compounds. J. Am. Chem. Soc. 1950, 72 (2), 771–75. DOI: 10.1021/ja01158a034.
- ↑ 5.0 5.1 5.2 Kirby, H. W.; Morss, L. R. Actinium. In The Chemistry of the Actinide and Transactinide Elements, 3rd ed.; Morss, Lester R.; Edelstein, Norman M.; Fuger, Jean, Eds.; Springer: Dordrecht, the Netherlands, 2006; Vol. 1, Chapter 2, pp 18–51. doi:10.1007/1-4020-3598-5_2, <http://radchem.nevada.edu/classes/rdch710/files/actinium.pdf>.
External links
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