Difference between revisions of "Hydrogen polonide"
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| − | '''Hydrogen polonide''', H<sub>2</sub>Po, is the heaviest of the [[chalcogen]] [[hydride]]s. It has been prepared in trace quantities by the reduction of [[polonium]] with [[magnesium]] in dilute [[hydrochloric acid]].<ref>{{citation | title = Über Poloniumwasserstoff. II. Mitteilung | first1 = Fritz | last1 = Paneth | first2 = Adolf | last2 = Johannsen | journal = Ber. Dtsch. Chem. Ges. | volume = 55 | issue = 8 | pages = 2622–37 | doi = 10.1002/cber.19220550836}}.</ref> Its physical properties are unknown but, by comparison with other chalcogen hydrides, it is expected to be a volatile liquid at room temperature.<ref>{{Greenwood&Earnshaw1st|page=900}}.</ref> It is thought to be implicated in the bio-volatization of polonium, leading to a relative excess of polonium in the atmosphere compared with open ocean waters.<ref>{{citation | title = Bio-volatilization of polonium: Results from laboratory analyses | journal = Aquat. Geochem. | volume = 1 | issue = 2 | year = 1995 | doi = 10.1007/BF00702890 | pages = 175–88 | first1 = N. | last1 = Hussain | first2 = T. G. | last2 = Ferdelman | first3 = T. M. | last3 = Church | first4 = George W. | last4 = Luther III}}.</ref> | + | {{chembox |
| + | | Section1 = {{Chembox Identifiers | ||
| + | | CASNo = 31060-73-8 | ||
| + | }} | ||
| + | | Section2 = {{Chembox Properties | ||
| + | | Formula = H<sub>2</sub>Po | ||
| + | | MolarMass = 212.00 g mol<sup>−1</sup> | ||
| + | }} | ||
| + | }} | ||
| + | '''Hydrogen polonide''', H<sub>2</sub>Po, is the heaviest of the [[chalcogen]] [[hydride]]s. It has been prepared in trace quantities by the reduction of [[polonium]] with [[magnesium]] in dilute [[hydrochloric acid]].<ref>{{citation | title = Über Poloniumwasserstoff. II. Mitteilung | first1 = Fritz | last1 = Paneth | first2 = Adolf | last2 = Johannsen | journal = Ber. Dtsch. Chem. Ges. | volume = 55 | issue = 8 | pages = 2622–37 | doi = 10.1002/cber.19220550836}}.</ref> Its physical properties are unknown but, by comparison with other chalcogen hydrides, it is expected to be a volatile liquid at room temperature.<ref>{{Greenwood&Earnshaw1st|page=900}}.</ref><ref>{{citation | first = K. W. | last = Bagnall | title = The Chemistry of Polonium | journal = Adv. Inorg. Chem. Radiochem. | year = 1962 | volume = 4 | pages = 197–229 | url = http://books.google.de/books?&lr=&id=8qePsa3V8GQC&oi=fnd&pg=PA197#v=onepage&q&f=false}}.</ref> It is thought to be implicated in the bio-volatization of polonium, leading to a relative excess of polonium in the atmosphere compared with open ocean waters.<ref>{{citation | title = Bio-volatilization of polonium: Results from laboratory analyses | journal = Aquat. Geochem. | volume = 1 | issue = 2 | year = 1995 | doi = 10.1007/BF00702890 | pages = 175–88 | first1 = N. | last1 = Hussain | first2 = T. G. | last2 = Ferdelman | first3 = T. M. | last3 = Church | first4 = George W. | last4 = Luther III}}.</ref> | ||
==References== | ==References== | ||
Latest revision as of 00:45, 27 May 2010
| Hydrogen polonide | |
|---|---|
| Identifiers | |
| CAS number | [] |
| Properties | |
| Chemical formula | H2Po |
| Molar mass | 212.00 g mol−1 |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Hydrogen polonide, H2Po, is the heaviest of the chalcogen hydrides. It has been prepared in trace quantities by the reduction of polonium with magnesium in dilute hydrochloric acid.[1] Its physical properties are unknown but, by comparison with other chalcogen hydrides, it is expected to be a volatile liquid at room temperature.[2][3] It is thought to be implicated in the bio-volatization of polonium, leading to a relative excess of polonium in the atmosphere compared with open ocean waters.[4]
References
- ↑ Paneth, Fritz; Johannsen, Adolf Über Poloniumwasserstoff. II. Mitteilung. Ber. Dtsch. Chem. Ges., 55 (8), 2622–37. DOI: 10.1002/cber.19220550836.
- ↑ Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; p 900. ISBN 0-08-022057-6.
- ↑ Bagnall, K. W. The Chemistry of Polonium. Adv. Inorg. Chem. Radiochem. 1962, 4, 197–229, <http://books.google.de/books?&lr=&id=8qePsa3V8GQC&oi=fnd&pg=PA197#v=onepage&q&f=false>.
- ↑ Hussain, N.; Ferdelman, T. G.; Church, T. M.; Luther III, George W. Bio-volatilization of polonium: Results from laboratory analyses. Aquat. Geochem. 1995, 1 (2), 175–88. DOI: 10.1007/BF00702890.
External links
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See also the corresponding article on Wikipedia. |
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