Astatine

85 polonium ← astatine → radon I ↑ At ↓ (Uus) periodic table
General
Name, Symbol, Number	astatine, At, 85
Chemical series	halogens
Group, Period, Block	17, 6, p
Appearance	metallic (presumed)
Atomic mass	(210) g/mol
Electron configuration	[Xe] 4f14 5d10 6s2 6p5
Electrons per shell	2, 8, 18, 32, 18, 7
Physical properties
Phase	solid
Melting point	575 K (302 °C, 576 °F)
Boiling point	? 610 K (? 337 °C, ? 639 °F)
Heat of vaporization	ca. 40 kJ/mol
Vapor pressure P/Pa 1 10 100 1 k 10 k 100 k at T/K 361 392 429 475 531 607
Atomic properties
Crystal structure	no data
Oxidation states	±1, 3, 5, 7
Electronegativity	2.2 (Pauling scale)
Ionization energies	1st: (est.) 920 kJ/mol
Miscellaneous
Magnetic ordering	no data
Thermal conductivity	(300 K) 1.7 W/(m·K)
CAS registry number	7440-68-8
Notable isotopes
Main article: Isotopes of astatine iso NA half-life DM DE (MeV) DP 210At 100% 8.1 h ε, β+ 3.981 210Po α 5.631 206Bi

Astatine (chemical symbol At, atomic number 85) is the rarest naturally occurring chemical element. It is a member of the halogen family of elements and is the heaviest halogen. Its chemical properties appear to resemble those of iodine. All its isotopes are radioactive, and a few of them are produced by the natural radioactive decay of uranium-235 and uranium-238. Various compounds of astatine have been prepared in minute amounts, and the possibility of their use for nuclear medicine is being studied.

Occurrence and production

The total amount of astatine in the Earth's crust has been estimated to be less than one ounce (28 grams) at any given time—corresponding to no more than one teaspoonful in volume. It is produced in nature by the radioactive decay of uranium and thorium, and it is therefore present in trace amounts in minerals of these elements.

Astatine can be artificially produced by bombarding bismuth with energetic alpha particles. This method generates the relatively long-lived isotopes ²⁰⁹At, ²¹⁰At, and ²¹¹At. These isotopes can then be separated from the bismuth by a process of distillation, which involves heating the mixture in the presence of air, and condensing the vapors in a separate container.

History

The name astatine was derived from the Greek word αστατος (astatos), meaning "unsteady." Long before it was discovered, Dmitri Mendeleev had predicted its existence based on his analysis of the periodic table. He called it "eka-iodine."

This element was discovered in 1940 by Dale R. Corson, K. R. MacKenzie, and Emilio Segrè at the University of California, Berkeley. They found it during experiments in which they subjected bismuth to a barrage of alpha particles. An earlier name for the element was alabamine (Ab).

Notable characteristics

In the periodic table, astatine is located in group 17 (former group 7A), the halogen family, below iodine. In addition, it lies in period six, between polonium and radon.

According to experiments done with a mass spectrometer, the chemical properties of this highly radioactive element probably resemble those of the other halogens, especially iodine. (Like iodine, it would be expected to accumulate in the thyroid gland.) Yet astatine is thought to be more metallic than iodine and is classified as a metalloid. Researchers at the Brookhaven National Laboratory have been able to study elementary reactions that involve astatine, but chemical research into this element is limited by its extreme rarity, which is a result of its extremely short half-life.

Isotopes

Astatine has many known isotopes, all of which are radioactive. Their mass numbers range from 191 to 223. There exist also 23 metastable excited states. Among the various known isotopes, the longest-lived member is ²¹⁰At, which has a half-life of 8.1 hours; the shortest-lived member is ²¹³At, which has a half-life of 125 nanoseconds.

Compounds

Multiple compounds of astatine have been synthesized in microscopic amounts and studied as intensively as possible before their inevitable radioactive disintegration. These compounds are primarily of theoretical interest. They are, however, also being studied for their potential use in nuclear medicine.

See also

• Chemical element
• Halogen
• Iodine
• Periodic table

References

ISBN links support NWE through referral fees

• Astatine Los Alamos National Laboratory. Retrieved October 3, 2007.
• Cotton, F. Albert, and Geoffrey Wilkinson. Advanced Inorganic Chemistry, 4th ed. New York: Wiley, 1980. ISBN 0-471-02775-8
• Chang, Raymond. Chemistry, ninth ed. New York: McGraw-Hill Science/Engineering/Math, 2006. ISBN 0073221031
• Greenwood, N.N., and A. Earnshaw. Chemistry of the Elements, 2nd Edition. Oxford, U.K.; Burlington, Massachusetts: Butterworth-Heinemann, Elsevier Science, 1998. ISBN 0750633654 Online Version Retrieved October 3, 2007.

External links

All links retrieved August 18, 2023.

• WebElements.com - Astatine

Credits

New World Encyclopedia writers and editors rewrote and completed the Wikipedia article in accordance with New World Encyclopedia standards. This article abides by terms of the Creative Commons CC-by-sa 3.0 License (CC-by-sa), which may be used and disseminated with proper attribution. Credit is due under the terms of this license that can reference both the New World Encyclopedia contributors and the selfless volunteer contributors of the Wikimedia Foundation. To cite this article click here for a list of acceptable citing formats.The history of earlier contributions by wikipedians is accessible to researchers here:

• Astatine  ^history

The history of this article since it was imported to New World Encyclopedia:

• History of "Astatine"

Note: Some restrictions may apply to use of individual images which are separately licensed.