Hydrogen astatide

Hydrogen astatide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
532398
Properties
HAt
Conjugate acid Astatonium
Conjugate base Astatide
Related compounds
Other anions
 Hydrogen bromide

Hydrogen chloride
Hydrogen fluoride
Hydrogen iodide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Hydrogen astatide, also known as astatine hydride, astatane, or astidohydrogen, is a chemical compound with the chemical formula HAt, consisting of an astatine atom covalently bonded to a hydrogen atom.[1] It thus is a hydrogen halide.

This chemical compound can dissolve in water to form hydroastatic acid, which exhibits properties very similar to the other four binary acids, and is in fact the strongest among them. However, it is limited in use due to its ready decomposition into elemental hydrogen and astatine,[2] as well as the short half-life of the various isotopes of astatine. Because the atoms have a nearly equal electronegativity, and as the At+ ion has been observed,[3] dissociation could easily result in the hydrogen carrying the negative charge. Thus, a hydrogen astatide sample can undergo the following reaction:

2 HAt → H+ + At− + H− + At+ → H2 + At2

This results in elemental hydrogen gas and astatine precipitate. Further, a trend for hydrogen halides, or HX, is that enthalpy of formation becomes less negative, i.e., decreases in magnitude but increases in absolute terms, as the halide becomes larger. Whereas hydroiodic acid solutions are stable, the hydronium-astatide solution is clearly less stable than the water-hydrogen-astatine system. Finally, radiolysis from astatine nuclei could sever the H-At bonds.

Additionally, astatine has no stable isotopes. The most stable is astatine-210, which has a half-life of approximately 8.1 hours, making its chemical compounds especially difficult to work with,[4] as the astatine will quickly decay into other elements.

References

  1. ↑ PubChem, "astatane - Compound Summary", accessed July 3, 2009.
  2. ↑ Fairbrother, Peter, "Re: Is hydroastatic acid possible?", accessed July 3, 2009.
  3. ↑ Advances in Inorganic Chemistry, Volume 6 by Emeleus, p.219, Academic Press, 1964 ISBN 0-12-023606-0
  4. ↑ Gagnon, Steve, "It's Elemental", accessed July 3, 2009.
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