Polonium

Polonium
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84 bismuth ← polonium → astatine
Te
↑
Po
↓
Uuh
Periodic Table - Extended Periodic Table


General
Name, Symbol, Number polonium, Po, 84
Chemical series metalloids
Group, Period, Block 16, 6, p
Appearance silvery
Standard atomic weight (209)  g·mol−1
Electron configuration [Xe] 4f14 5d10 6s2 6p4
Electrons per shell 2, 8, 18, 32, 18, 6
Physical properties
Phase solid
Density (near r.t.) (alpha) 9.196  g·cm−3
Density (near r.t.) (beta) 9.398  g·cm−3
Melting point 527 K
(254 °C, 489 °F)
Boiling point 1235 K
(962 °C, 1764 °F)
Heat of fusion ca. 13  kJ·mol−1
Heat of vaporization 102.91  kJ·mol−1
Heat capacity (25 °C) 26.4  J·mol−1·K−1
Vapor pressure P(Pa) 1 10 100 1 k 10 k 100 k
at T(K) (846) 1003 1236

Atomic properties
Crystal structure cubic
Oxidation states 4, 2
(amphoteric oxide)
Electronegativity 2.0 (scale Pauling)
Ionization energies 1st: 812.1 kJ/mol
Atomic radius 190  pm
Atomic radius (calc.) 135  pm
Miscellaneous
Magnetic ordering nonmagnetic
Electrical resistivity (0 °C) (α) 0.40 µΩ·m
Thermal conductivity (300 K) ? 20  W·m−1·K−1
Thermal expansion (25 °C) 23.5  µm·m−1·K−1
CAS registry number 7440-08-6
Selected isotopes
Main article: Isotopes of polonium iso NA half-life DM DE (MeV) DP
208Po syn 2.898 y α 5.215 204Pb
ε, β+ 1.401 208Bi
209Po syn 103 y α 4.979 205Pb
ε, β+ 1.893 209Bi
210Po syn 138.376 d α 5.407 206Pb

References
Polonium (IPA: /pə(ʊ)ˈləʊniəm/) is a chemical element in the periodic table that has the symbol Po and atomic number 84. A rare and highly radioactive metalloid[1], polonium is chemically similar to tellurium and bismuth, and it occurs in uranium ores. Polonium has been studied for possible use in heating spacecraft. It is unstable; all isotopes of polonium are radioactive.

Contents [hide]
1 Applications
2 History
3 Occurrence
3.1 Synthesis by (n,γ) reaction
3.2 Synthesis by (p, n) and (p,2n) reactions
4 Isotopes
4.1 210Po
5 Chemical characteristics
6 Solid state form
7 Tests
7.1 Gamma counting
7.2 Alpha counting
8 Toxicity
8.1 Overview
8.2 Acute effects
8.3 Long term (chronic) effects
8.4 Regulatory exposure limits
8.5 Famous polonium poisoning cases
8.6 Treatment
9 See also
10 References
11 External links



[edit] Applications
When it is mixed or alloyed with beryllium, polonium can be a neutron source: beryllium releases a neutron upon absorption of an alpha particle that is supplied by 210Po. It has been used in this capacity as a neutron trigger or initiator for nuclear weapons. Other uses include

Devices that eliminate static charges in textile mills and other places.[2] However, beta particle sources are more commonly used and are less dangerous. A non-radioactive alternative is to use a high-voltage DC power supply to ionise air positively or negatively as required.[3]
210Po can be used as an atomic heat source to power radioisotope thermoelectric generators via thermoelectric materials.
Because of its very high toxicity, Polonium can be used as a poison (see, for example, Alexander Litvinenko poisoning).

[edit] History
Also called tentatively "Radium F", polonium was discovered by Marie Skłodowska-Curie and her husband Pierre Curie in 1898[4] and was later named after Marie Curie's native land of Poland (Latin: Polonia).[5][6] Poland at the time was under Russian, Prussian, and Austrian partition, and did not exist as an independent country. It was Curie's hope that naming the element after her native land would publicize its lack of independence. Polonium may be the first element named to highlight a political controversy.[7] Poland became an independent country again in 1918, following World War I.

This element was the first one discovered by the Curies while they were investigating the cause of pitchblende radioactivity. The pitchblende, after removal of the radioactive elements uranium and thorium, was more radioactive than both the uranium and thorium put together. This spurred the Curies on to find additional radioactive elements. The Curies first separated out polonium from the pitchblende, and then within a few years, also isolated radium.


[edit] Occurrence
Polonium is a very rare element in nature because of the short half-life of all its isotopes. It is found in uranium ores at about 100 micrograms per metric ton (1 part in 1010), which is approximately 0.2% of the abundance of radium. The amounts in the Earth's crust are not harmful. Polonium has been found in tobacco smoke from tobacco leaves grown with phosphate fertilizers.[8][9]


[edit] Synthesis by (n,γ) reaction
In 1934 an experiment showed that when natural 209Bi is bombarded with neutrons, 210Bi is created, which then decays to 210Po via β decay. Polonium may now be made in milligram amounts in this procedure which uses high neutron fluxes found in nuclear reactors. Only about 100 grams are produced each year, practically all of it in Russia, making polonium exceedingly rare.[10] [11]


[edit] Synthesis by (p, n) and (p,2n) reactions
It has been found that the longer lived isotopes of polonium can be formed by proton bombardment of bismuth using a cyclotron. Other more neutron rich isotopes can be formed by the irradiation of platinum with carbon nuclei.[12]


[edit] Isotopes
Polonium has 25 known isotopes, all of which are radioactive. They have atomic masses that range from 194u to 218u. 210Po is the most widely available. 209Po (half-life 103 years) and 208Po (half-life 2.9 years) can be made through the alpha, proton, or deuteron bombardment of lead or bismuth in a cyclotron.


[edit] 210Po
210Po is an alpha emitter that has a half-life of 138.376 days; it decays directly to its daughter isotope 206Pb. A milligram of 210Po emits as many alpha particles per second as 4.215 grams of 226Ra. A few curies (1 curie equals 37 gigabecquerels) of 210Po emit a blue glow which is caused by excitation of surrounding air. A single gram of 210Po generates 140 watts of power.[13] 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, 210Po heat source was also used in each of the Lunokhod rovers deployed on the surface of the Moon, to keep their internal components warm during the lunar nights.[14] Some anti-static brushes contain up to 500 microcuries of 210Po as a source of charged particles for neutralizing static electricity in materials like photographic film.[15]

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.[16] 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.


[edit] Chemical characteristics
The chemistry of polonium is similar to that of tellurium and bismuth. Polonium dissolves readily in dilute acids, but is only slightly soluble in alkalis. The hydrogen compound PoH2 is liquid at room temperature (M.P. -36.1°C to B.P. 35.3°C). Halides of the structure PoX2, PoX4 and PoX6 are known. The two oxides PoO2 and PoO3 are the products of oxidation of polonium.[17]

210Po (in common with 238Pu) has the ability to become airborne with ease: if a sample is heated in air to 328 K (55°C, 131°F), 50% of it is vaporized in 45 hours, even though the melting point of polonium is 527 K (254°C, 489°F) and its boiling point is 1235 K (962°C, 1763°F).[18] More than one hypothesis exists for how polonium does this; one suggestion is that small clusters of polonium atoms are spalled off by the alpha decay.

It has been reported that some microbes can methylate polonium by the action of methylcobalamin.[19][20]This is similar to the way in which mercury, selenium and tellurium are methylated in living things to create organometallic compounds. As a result when considering the biochemistry of polonium one should consider the possibility that the polonium will follow the same biochemical pathways as selenium and tellurium.


The alpha form of solid polonium.
[edit] Solid state form
The alpha form of solid polonium has a simple cubic crystal structure with an edge length of 3.352 Å.

The beta form of polonium is rhombohedral; it has been reported in the chemical literature, along with the alpha form, several times. A picture of it is present on the web.[21]

Two papers report X-ray diffraction experiments on polonium metal.[22][23] The first report of the crystal structure of polonium was done using electron diffraction.[24]


[edit] Tests

Intensity against photon energy for three isotopes



[edit] Gamma counting
By means of radiometric methods such as gamma spectroscopy (or a method using a chemical separation followed by an activity measurement with a non-energy-dispersive counter), it is possible to measure the concentrations of radioisotopes and to distinguish one from another. In practice, background noise would be present and depending on the detector, the line width would be larger which would make it harder to identify and measure the isotope. In biological/medical work it is common to use the natural 40K present in all tissues/body fluids as a check of the equipment and as an internal standard.


Intensity against alpha energy for four isotopes, note that the line width is narrow and the fine details can be seen
Intensity against alpha energy for four isotopes, note that the line width is wide and some of the fine details can not be seen. This is for liquid scintillation counting where random effects cause a variation in the number of visible photons generated per alpha decay
[edit] Alpha counting
The best way to test for (and measure) many alpha emitters is to use alpha-particle spectroscopy as it is common to place a drop of the test solution on a metal disk which is then dried out to give a uniform coating on the disk. This is then used as the test sample. If the thickness of the layer formed on the disk is too thick then the lines of the spectrum are broadened, this is because some of the energy of the alpha particles is lost during their movement through the layer of active material. An alternative method is to use internal liquid scintillation where the sample is mixed with a scintillation cocktail. When the light emitted is then counted, some machines will record the amount of light energy per radioactive decay event. Due to the imperfections of the liquid scintillation method (such as a failure for all the photons to be detected, cloudy or coloured samples can be difficult to count) and the fact that random quenching can reduce the number of photons generated per radioactive decay it is possible to get a broadening of the alpha spectra obtained through liquid scintillation. It is likely that these liquid scintillation spectra will be subject to a Gaussian broadening rather than the distortion exhibited when the layer of active material on a disk is too thick.

A third energy dispersive method for counting alpha particles is to use a semiconductor detector.

From left to right the peaks are due to 209Po, 210Po, 239Pu and 241Am. The fact that isotopes such as 239Pu and 241Am have more than one alpha line indicates that the nucleus has the ability to be in different discrete energy levels (like a molecule can).


[edit] Toxicity

[edit] Overview
By mass, polonium is around 250 billion times more toxic than hydrogen cyanide (the oral LD50 for 210Po is about 50 ng (see below) compared to about 250 mg for hydrogen cyanide[25]). The main hazard is its intense radioactivity (as an alpha emitter), which makes it very difficult to handle safely - one gram of Po will self-heat to a temperature of around 500°C. Even in microgram amounts, handling 210Po is extremely dangerous, requiring specialized equipment and strict handling procedures. Alpha particles emitted by polonium will damage organic tissue easily if polonium is ingested, inhaled, or absorbed (though they do not penetrate the epidermis and hence are not hazardous if the polonium is outside the body).


[edit] Acute effects
The median lethal dose (LD50) for acute radiation exposure is generally about 4.5 Sv.[26] The committed effective dose equivalent 210Po is 0.51 µSv/Bq if ingested, and 2.5 µSv/Bq if inhaled.[27] Since 210Po has an activity of 166 TBq per gram[27] (1 gram produces 166×1012 decays per second), a fatal 4-Sv dose can be caused by ingesting 8.8 MBq (238 microcurie), about 50 nanograms (ng), or inhaling 1.8 MBq (48 microcurie), about 10 ng. One gram of 210Po could thus in theory poison 100 million people of whom 50 million would die. The actual toxicity of 210Po is lower than these estimates, because radiation exposure that is spread out over several weeks (the biological half-life of polonium in humans is 30 to 50 days[28]) is somewhat less damaging than an instantaneous dose. It has been estimated that a minimal lethal dose of 210Po for an 80 kg person is 4 millicuries, or 0.89 micrograms, still an extremely small amount. [29]


[edit] Long term (chronic) effects
In addition to the acute effects, radiation exposure (both internal and external) carries a long-term risk of death from cancer of 5–10% per Sv.[26] The general population is exposed to small amounts of polonium as a radon daughter in indoor air; the isotopes 214Po and 218Po are thought to cause the majority[30] of the estimated 15,000-22,000 lung cancer deaths in the US every year that have been attributed to indoor radon.[31] Tobacco smoking causes significant additional exposure to Po.


[edit] Regulatory exposure limits
The maximum allowable body burden for ingested 210Po is only 1,100 Bq (0.03 microcurie), which is equivalent to a particle weighing only 6.8 picograms. The maximum permissible workplace concentration of airborne 210Po is about 10 Bq/m3 (3 × 10-10 µCi/cm3).[32] The target organs for polonium in humans are the spleen and liver.[33] As the spleen (150 g) and the liver (1.3 to 3 kg) are much smaller than the rest of the body, if the polonium is concentrated in these vital organs, it is a greater threat to life than the dose which would be suffered (on average) by the whole body if it were spread evenly throughout the body, in the same way as caesium or tritium (as T2O).

210Po is widely used in industry, and readily available with little regulation or restriction. In the US, a tracking system run by the Nuclear Regulatory Commission will be implemented in 2007 to register purchases of more than 16 curies of polonium 210 (enough to make up 5,000 lethal doses). The IAEA "is said to be considering tighter regulations... There is talk that it might tighten the polonium reporting requirement by a factor of 10, to 1.6 curies."[34]


[edit] Famous polonium poisoning cases
Notably, the alleged murder of Alexander Litvinenko, a Russian dissident, in 2006 was announced as due to 210Po poisoning [35] (see Alexander Litvinenko poisoning). According to Nick Priest, a radiation expert speaking on Sky News on December 2, Litvinenko was probably the first person ever to die of the acute α-radiation effects of 210Po.

It has also been suggested that Irène Joliot-Curie was the first person ever to die from the radiation effects of polonium (due to a single intake) in 1956.[36] She was accidentally exposed to polonium in 1946 when a sealed capsule of the element exploded on her laboratory bench. A decade later, on 17 March 1956, she died in Paris from leukemia which may or may not have been caused by that exposure.

According to the book The Bomb in the Basement, several death cases in Israel during 1957-1969 were caused by 210Po.[37] A leak was discovered at a Weizmann Institute laboratory in 1957. Traces of 210Po were found on the hands of Prof. Dror Sadeh, a physicist who researched radioactive materials. Medical tests indicated no harm, but the tests did not include bone marrow. Sadeh died prematurely from cancer. One of his students died of leukemia, and two colleagues died after a few years, both from cancer. The issue was investigated secretly, and there was never any formal admission that a connection between the leak and the deaths had existed.


[edit] Treatment
It has been suggested that chelation agents such as British Anti-Lewisite (dimercaprol) can be used to decontaminate humans.[38][39] In one experiment, rats were given a fatal dose of 1.45 MBq/kg (8.7 ng/kg) of 210Po; all untreated rats were dead after 44 days, but 90% of the rats treated with the chelation agent HOEtTTC remained alive after 5 months.[40]


[edit] See also
Isotopes of polonium
Polonium - Radon Decay Chain [4]
The entry for polonium at fictional applications of real materials
Polonium halo

[edit] References
^ http://www.chemicalelements.com/groups/metalloids.html
^ http://news.bbc.co.uk/1/hi/england/1868414.stm
^ http://www.thermo.com/eThermo/CMA/PDFs/Articles/articlesFile_16929.pdf
^ Curie P., Curie M. (1898). ".". Comptes Rendus 126: 1101.
^ Pfützner M. (1999). "Borders of the Nuclear World --- 100 Years After Discovery of Polonium". Acta Physica Polonica B 30: 1197.
^ Adloff J. P. (681-688). "The centennial of the 1903 Nobel Prize for physics". Radichimica Acta 91: 2003. DOI:10.1524/ract.91.12.681.23428.
^ Kabzinska K. (1998). "Chemical and Polish aspects of polonium and radium discovery". Przemysl Chemiczny 77: 104-107.
^ Kilthau, Gustave F.. "Cancer risk in relation to radioactivity in tobacco". Radiologic Technology 67: 217-222.
^ Alpha Radioactivity (210 Polonium) and Tobacco Smoke
^ http://www.rsc.org/chemistryworld/News/2006/November/27110601.asp RSC Chemistry World Q&A
^ http://www.sptimesrussia.com/index.php?action_id=2&story_id=20100
^ Atterling, H., Forsling, W. (1959). "Light Polonium Isotopes from Carbon Ion Bombardments of Platinum". Arkiv for Fysik 15 (1): 81-88.
^ Polonium, Argonne National Laboratory
^ Andrew Wilson, Solar System Log, (London: Jane's Publishing Company Ltd, 1987), p. 64.
^ http://www.amstat.com/solutions/staticmaster.html
^ http://atom.kaeri.re.kr/cgi-bin/decay?Po-210%20A
^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
^ Bogdan Wąs, Ryszard Misiak, Mirosław Bartyzel, Barbara Petelenz (2006). "Thermochromatographic Separation of 206,208Po from a Bismuth Target Bombardet with Protons". Nukleonica 51 (Suppl. 2): s3-s5.
^ Momoshima N., Song L.X., Osaki S.,Maeda Y., (2001). "Formation and emission of volatile polonium compound by microbial activity and polonium methylation with methylcobalamin.". Environ Sci Technol 35 (15): 2956-2960. DOI:S0013-936X(00)01730-2 10.1021/es001730+ S0013-936X(00)01730-2.
^ Momoshima N., Song L.X., Osaki S.,Maeda Y., (2002). "Biologically induced Po emission from fresh water". J Environ Radioact. 63 (2): 187-197. DOI:10.1016/S0265-931X(02)00028-0.
^ http://cst-www.nrl.navy.mil/lattice/struk/a_i.html
^ R.J. Desando and R.C Lange, Journal of Inorganic and Nuclear Chemistry, 1966, 28, 1837-1846.
^ W.H Beamer and C.R. Maxwell, Journal of Chemical Physics, 1946, 14, 569-569.
^ M.A. Rollier, S.B. Hendricks and L.R. Maxwell, Journal of Chemical Physics, 1936, 4, 648-652.
^ Hydrogen cyanide msds
^ a b http://www.pnl.gov/main/publications/external/technical_reports/PNNL-14424.pdf
^ a b Nuclide Safety Data Sheet: Polonium–210
^ Effective half-life of polonium in the human
^ http://nuclearweaponarchive.org/News/PoloniumPoison.html
^ National Academy of Sciences 1988 report Health Risks of Radon and Other Internally Deposited Alpha-Emitters: BEIR IV, page 5
^ National Academy of Sciences 1999 report Health Effects Of Exposure To Indoor Radon
^ Nuclear Regulatory Commission limits for 210Po
^ http://www.pilgrimwatch.org/health1.html
^ Peter D. Zimmerman (2006). The Smoky Bomb Threat. The New York Times. Retrieved on 2006-12-19.
^ "The mystery of Litvinenko's death", BBC News, 24 November 2006.
^ Innocent chemical a killer - The Daily Telegraph (of Australia), December 4, 2006 [1]
^ Karpin, Michael (2006). The bomb in the basement: How Israel went nuclear and what that means for the world. Simon and Schuster. ISBN 0743265947.
^ [2]9 also see NRCP Report No. 65: Management of Persons Accidentally Contaminated With Radionuclides
^ [3]
^ Rencováa J., Svoboda V., Holuša R., Volf V., Jones M. M., Singh P. K. (1997). "Reduction of subacute lethal radiotoxicity of polonium-210 in rats by chelating agents". International Journal of Radiation Biology 72 (3): 247 - 249. DOI:10.1080/095530097143338.

[edit] External links
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WebElements.com – Polonium
History of Polonium
Los Alamos National Laboratory – Polonium
NLM Hazardous Substances Databank – Polonium, Radioactive
The Human Plutonium Injection Experiments (Polonium experiments - pg20)
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Categories: Chemical elements | Metalloids | Chalcogens | Carcinogens