Polonium-210

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Polonium-210,  210Po
General
Name, symbolPolonium-210,210Po
Neutrons126
Protons84
Nuclide data
Natural abundanceTrace
Half-life138.376 d[1]
Parent isotopes210Bi (β)
Decay products206Pb
Isotope mass209.9828736[2] u
Spin0
Decay modes
Decay modeDecay energy (MeV)
Alpha decay5.40753[2]
Isotopes of polonium
Complete table of nuclides

Polonium-210 (210Po, Po-210, historically Radium F) is an isotope of polonium. It undergoes alpha decay to stable 206Pb with a half-life of 138.376 days, the longest of all naturally occurring polonium isotopes. First identified in 1898, and also marking the discovery of the element polonium, 210Po is generated in the decay chain of uranium-238 and radium-226. 210Po is a prominent contaminant in the environment, mostly affecting seafood and tobacco. It is also extremely toxic to humans as a result of its intense radioactivity.

History[edit]

The decay chain of uranium-238, known as the uranium series or radium series, of which polonium-210 is a member
Schematic of the final steps of the s-process. The red path represents the sequence of neutron captures; blue and cyan arrows represent beta decay, and the green arrow represents the alpha decay of 210Po. It is the short half-lives of 210Bi and 210Po that prevent the formation of heavier elements, instead resulting in a cycle of four neutron captures, two beta decays, and an alpha decay.

In 1898, Marie and Pierre Curie discovered a strongly radioactive substance in pitchblende and determined that it was a new element; it was one of the first radioactive elements discovered. Having identified it as such, they named the element polonium after Marie's home country, Poland. Willy Marckwald discovered a similar radioactive activity in 1902 and named it radio-tellurium, and at roughly the same time, Ernest Rutherford identified the same activity in his analysis of the uranium decay chain and named it radium F (originally radium E). By 1905, Rutherford concluded that all these observations were due to the same substance, 210Po. Further discoveries and the concept of isotopes, first proposed in 1913 by Frederick Soddy, firmly placed 210Po as the penultimate step in the uranium series.[3]

In 1943, 210Po was studied as a possible neutron initiator in nuclear weapons, as part of the Dayton Project. In subsequent decades, concerns for the safety of workers handling 210Po led to extensive studies on its health effects.[4]

210Po was used to kill Russian dissident and ex-FSB officer Alexander V. Litvinenko in 2006,[5][6] and was suspected as a possible cause of Yasser Arafat's death, following exhumation and analysis of his corpse in 2012–2013.[7]

Decay properties[edit]

210Po is an alpha emitter that has a half-life of 138.376 days; it decays directly to stable 206Pb. The majority of the time, 210Po decays by emission of an alpha particle only, not by emission of an alpha particle and a gamma ray; about one in 100,000 decays results in the emission of a gamma ray.[8] This low gamma ray production rate makes it more difficult to find and identify this isotope. Rather than gamma ray spectroscopy, alpha spectroscopy is the best method of measuring this isotope.

Owing to its much shorter half-life, a milligram of 210Po emits as many alpha particles per second as 5 grams of 226Ra.[9] A few curies of 210Po emit a blue glow caused by excitation of surrounding air.

210Po occurs in minute amounts in nature, where it is the penultimate isotope in the uranium series decay chain. It is generated via beta decay from 210Pb and 210Bi.

The astrophysical s-process is terminated by the decay of 210Po, as the neutron flux is insufficient to lead to further neutron captures in the short lifetime of 210Po. Instead, 210Po alpha decays to 206Pb, which then captures more neutrons to become 210Po and repeats the cycle, thus consuming the remaining neutrons. This results in a buildup of lead and bismuth, and ensures that heavier elements such as thorium and uranium are only produced in the much faster r-process.[10]

Production[edit]

Although 210Po occurs in trace amounts in nature, it is not abundant enough (0.1 ppb) for extraction from uranium ore to be feasible. Instead, most 210Po is produced synthetically, through neutron bombardment of 209Bi in a cyclotron. This process converts 209Bi to 210Bi, which beta decays to 210Po with a five day half-life. Through this method, approximately 8 grams of 210Po are produced in Russia and shipped to the United States every month for commercial applications.[4]

Applications[edit]

A single gram of 210Po generates 140 watts of power.[11] Because it emits many alpha particles, which are stopped within a very short distance in dense media and release their energy, 210Po has been used as a lightweight heat source to power thermoelectric cells in artificial satellites; for instance, a 210Po heat source was also in each of the Lunokhod rovers deployed on the surface of the Moon, to keep their internal components warm during the lunar nights.[12] Some anti-static brushes, used for neutralizing static electricity on materials like photographic film, contain a few microcuries of 210Po as a source of charged particles.[13] 210Po was also used in initiators for atomic bombs through the (α,n) reaction with beryllium.[14]

Hazards[edit]

210Po is extremely toxic; it and other polonium isotopes are some of the most radiotoxic substances to humans.[5][15] With one microgram being enough to kill the average adult, 210Po is 250,000 times more toxic than hydrogen cyanide by weight;[16] it is also thought that one gram of 210Po is enough to kill 50 million people and sicken another 50 million.[5] This is a consequence of its ionizing alpha radiation, as alpha particles are especially damaging to organic tissues inside the body. However, 210Po does not pose a threat outside the body, for alpha particles cannot penetrate human skin.[5]

The toxicity of 210Po stems entirely from its radioactivity. It is not chemically toxic in itself, but its solubility in aqueous solution as well as that of its salts poses a hazard because its spread throughout the body is facilitated in solution.[5] Intake of 210Po occurs primarily through contaminated air, food, or water, as well as through open wounds. Once inside the body, 210Po concentrates in soft tissues (especially in the reticuloendothelial system) and the bloodstream. Its biological half-life is approximately 50 days.[17]

In the environment, 210Po can accumulate in seafood.[18] It has been detected in various organisms in the Baltic Sea, where it can propagate in, and thus contaminate, the food chain.[15] 210Po is also known to contaminate vegetation, primarily originating from the decay of atmospheric radon-222 and absorption from soil.[19]

In particular, 210Po attaches to, and concentrates in, tobacco leaves.[4][17] Elevated concentrations of 210Po in tobacco were documented as early as 1964, and cigarette smokers were thus found to be exposed to considerably greater doses of radiation from 210Po and its parent 210Pb.[19] Heavy smokers may be exposed to the same amount of radiation (estimates vary from 100 µSv[15] to 160 mSv[20] per year) as individuals in Poland were from Chernobyl fallout traveling from Ukraine.[15] As a result, 210Po is most dangerous when inhaled from cigarette smoke, providing further evidence for a link between smoking and lung cancer.[21]

See also[edit]

References[edit]

  1. ^ Audi, Georges; Kondev, Filip G.; Wang, Meng; Huang, Wen Jia; Naimi, Sarah (2017), "The NUBASE2016 evaluation of nuclear properties" (PDF), Chinese Physics C, 41 (3): 030001–1—030001–138, Bibcode:2017ChPhC..41c0001A, doi:10.1088/1674-1137/41/3/030001
  2. ^ a b Wang, Meng; Audi, Georges; Kondev, Filip G.; Huang, Wen Jian; Naimi, Sarah; Xu, Xing (2017), "The AME2016 atomic mass evaluation (II). Tables, graphs, and references" (PDF), Chinese Physics C, 41 (3): 030003–1—030003–442, doi:10.1088/1674-1137/41/3/030003
  3. ^ Thoennessen, M. (2016). The Discovery of Isotopes: A Complete Compilation. Springer. pp. 6–8. doi:10.1007/978-3-319-31763-2. ISBN 978-3-319-31761-8. LCCN 2016935977.
  4. ^ a b c Roessler, G. (2007). "Why 210Po?" (PDF). Health Physics News. Vol. 35 no. 2. Health Physics Society.
  5. ^ a b c d e McFee, R.B.; Leikin, J.B. (2009). "Death by polonium-210: lessons learned from the murder of former Soviet spy Alexander Litvinenko". Seminars in Diagnostic Pathology. 26 (1): 61–67. doi:10.1053/j.semdp.2008.12.003. PMID 19292030.
  6. ^ Cowell, Alan (November 24, 2006). "Radiation Poisoning Killed Ex-Russian Spy". The New York Times.
  7. ^ "Arafat's death: what is Polonium-210?". Al Jazeera. July 10, 2012.
  8. ^ 210PO A DECAY Archived February 24, 2015, at the Wayback Machine
  9. ^ C. R. Hammond. "The Elements" (PDF). Fermi National Accelerator Laboratory. pp. 4–22.
  10. ^ Burbidge, E. M.; Burbidge, G. R.; Fowler, W. A.; Hoyle, F. (1957). "Synthesis of the Elements in Stars". Reviews of Modern Physics. 29 (4): 547–650. Bibcode:1957RvMP...29..547B. doi:10.1103/RevModPhys.29.547.
  11. ^ "Polonium" (PDF). Argonne National Laboratory. Archived from the original (PDF) on 2012-03-10.
  12. ^ Andrew Wilson, Solar System Log, (London: Jane's Publishing Company Ltd, 1987), p. 64.
  13. ^ "Staticmaster Alpha Ionizing Brush". Company 7.
  14. ^ Lillian Hoddeson; Paul W. Henriksen; Roger A. Meade (12 February 2004). Critical Assembly: A Technical History of Los Alamos During the Oppenheimer Years, 1943-1945. Cambridge University Press. ISBN 978-0-521-54117-6.
  15. ^ a b c d Skwarzec, B.; Strumińska, D.I.; Boryło, A. (2006). "Radionuclides of iron (55Fe), nickel (63Ni), polonium (210Po), uranium (234U, 235U, 238U), and plutonium (238Pu, 239+240Pu, 241Pu) in Poland and Baltic Sea environment" (PDF). Nukleonika. 51: S45–S51.
  16. ^ Ahmed, M.F.; Alam, L.; Mohamed, C.A.R.; Mokhtar, M.B.; Ta, G.C. (2018). "Health risk of polonium-210 ingestion via drinking water: An experience of Malaysia". International Journal of Environmental Research and Public Health. 15: 2056–1—2056–19. doi:10.3390/ijerph15102056.
  17. ^ a b Frequently asked questions about polonium-210 (PDF) (Report). Centers for Disease Control and Prevention. Retrieved 19 June 2019.
  18. ^ Richter, F.; Wagmann, M.; Zehringer, M. (2012). "Polonium – on the Trace of a Powerful Alpha Nuclide in the Environment". CHIMIA International Journal for Chemistry. 66 (3): 131. doi:10.2533/chimia.2012.131.
  19. ^ a b Persson, B.R.R.; Holm, E. (2009). Polonium-210 and Lead-210 in the Terrestrial environment: A historical review. International Topical Conference on Po and Radioactive Pb Isotopes. Seville, Spain.
  20. ^ "F. Typical Sources of Radiation Exposure". National Institute of Health. Archived from the original on 2013-06-13. Retrieved 2019-06-20.
  21. ^ Radford, Edward P.; Hunt, Vilma R. (1964). "Polonium-210: A Volatile Radioelement in Cigarettes". Science. 143 (3603): 247–249. doi:10.1126/science.143.3603.247. JSTOR 1712451.