Polonium

Polonium,  ₈₄Po

General properties
Name, symbol	polonium, Po
Pronunciation	/poʊˈloʊniəm/ po-LOH-nee-əm
Allotropes	α, β
Appearance	silvery
Polonium in the periodic table
Te ↑ Po ↓ Lv bismuth ← polonium → astatine
Atomic number (Z)	84
Group, block	group 16 (chalcogens), p-block
Period	period 6
Element category	post-transition metal, but this status is disputed
Standard atomic weight (Ar)	(209)
Electron configuration	[Xe] 4f^14 5d^10 6s^2 6p^4
per shell	2, 8, 18, 32, 18, 6
Physical properties
Phase	solid
Melting point	527 K ​(254 °C, ​489 °F)
Boiling point	1235 K ​(962 °C, ​1764 °F)
Density near r.t.	alpha: 9.196 g/cm^3 beta: 9.398 g/cm^3
Heat of fusion	ca. 13 kJ/mol
Heat of vaporization	102.91 kJ/mol
Molar heat capacity	26.4 J/(mol·K)
vapor pressure P (Pa) 1 10 100 1 k 10 k 100 k at T (K) (846) 1003 1236
Atomic properties
Oxidation states	6, 5,[1] 4, 2, −2 ​(an amphoteric oxide)
Electronegativity	Pauling scale: 2.0
Ionization energies	1st: 812.1 kJ/mol
Atomic radius	empirical: 168 pm
Covalent radius	140±4 pm
Van der Waals radius	197 pm
Miscellanea
Crystal structure	​cubic α-Po
Crystal structure	​rhombohedral β-Po
Thermal expansion	23.5 µm/(m·K) (at 25 °C)
Thermal conductivity	20 W/(m·K) (?)
Electrical resistivity	α: 0.40 µΩ·m (at 0 °C)
Magnetic ordering	nonmagnetic
CAS Number	7440-08-6
History
Naming	after Polonia, Latin for Poland, homeland of Marie Curie
Discovery	Pierre and Marie Curie (1898)
First isolation	Willy Marckwald (1902)
Most stable isotopes of polonium
iso NA half-life DM DE (MeV) DP ^208Po syn 2.898 y α 5.215 ^204Pb β^+ 1.401 ^208Bi ^209Po syn (125.2±3.3) y[2] α 4.979 ^205Pb β^+ 1.893 ^209Bi ^210Po trace 138.376 d α 5.307 ^206Pb

Polonium is a chemical element with symbol Po and atomic number 84. A rare and highly radioactive metal with no stable isotopes, polonium is chemically similar to selenium and tellurium, though it also shows resemblances to its horizontal neighbors thallium, lead, and bismuth due to its metallic character. Due to the short half-life of all its isotopes, its natural occurrence is limited to tiny traces of the fleeting polonium-210 (with a half-life of 138 days) in uranium ores, as it is the penultimate daughter of natural uranium-238. Though slightly longer-lived isotopes exist, they are much more difficult to produce. Today, polonium is more often produced in milligram quantities by the neutron irradiation of bismuth. Due to its intense radioactivity, which results in radiolysis of chemical bonds and immense radioactive self-heating, its chemistry has mostly been investigated on the trace scale only.

Polonium was discovered in 1898 by Marie and Pierre Curie, when it was chemically separated out of uranium ore and identified solely by its strong radioactivity: it was the first element to be so discovered. It was named after Marie Curie's homeland of Poland. Applications of polonium are sparse and dependent on its radioactivity: they include heaters in space probes, antistatic devices, and sources of neutrons and alpha particles. Its intense radioactivity makes it dangerously toxic to life.

Characteristics

Isotopes

Polonium has 33 known isotopes, all of which are radioactive. They have atomic masses that range from 188 to 220 u. ²¹⁰Po (half-life 138.376 days) is the most widely available. The longer-lived ²⁰⁹Po (half-life 125.2 ± 3.3 years, longest-lived of all polonium isotopes)^[2] and ²⁰⁸Po (half-life 2.9 years) can be made through the alpha, proton, or deuteron bombardment of lead or bismuth in a cyclotron.^[3]

²¹⁰Po is an alpha emitter that has a half-life of 138.4 days; it decays directly to its stable daughter isotope, ²⁰⁶Pb. A milligram (5 curies) of ²¹⁰Po emits about as many alpha particles per second as 5 grams of ²²⁶Ra.^[4] A few curies (1 curie equals 37 gigabecquerels, 1 Ci = 37 GBq) of ²¹⁰Po emit a blue glow which is caused by ionisation of the surrounding air.

About one in 100,000 alpha emissions causes an excitation in the nucleus which then results in the emission of a gamma ray with a maximum energy of 803 keV.^[5][6]

Solid state form

The alpha form of solid polonium.

Polonium is a radioactive element that exists in two metallic allotropes. The alpha form is the only known example of a simple cubic crystal structure in a single atom basis, with an edge length of 335.2 picometers; the beta form is rhombohedral.^[7][8][9] The structure of polonium has been characterized by X-ray diffraction^[10][11] and electron diffraction.^[12]

²¹⁰Po (in common with ²³⁸Pu) has the ability to become airborne with ease: if a sample is heated in air to 55 °C (131 °F), 50% of it is vaporized in 45 hours to form diatomic Po₂ molecules, even though the melting point of polonium is 254 °C (489 °F) and its boiling point is 962 °C (1,764 °F).^[13][14][1] 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.

Chemistry

The chemistry of polonium is similar to that of tellurium, although it also shows some similarities to its neighbor bismuth due to its metallic character. Polonium dissolves readily in dilute acids, but is only slightly soluble in alkalis. Polonium solutions are first colored in pink by the Po²⁺ ions, but then rapidly become yellow because alpha radiation from polonium ionizes the solvent and converts Po²⁺ into Po⁴⁺. This process is accompanied by bubbling and emission of heat and light by glassware due to the absorbed alpha particles; as a result, polonium solutions are volatile and will evaporate within days unless sealed.^[15][16]

Compounds

Polonium has no common compounds, and almost all of its compounds are synthetically created; more than 50 of those are known.^[17] The most stable class of polonium compounds are polonides, which are prepared by direct reaction of two elements. Na₂Po has the antifluorite structure, the polonides of Ca, Ba, Hg, Pb and lanthanides form a NaCl lattice, BePo and CdPo have the wurtzite and MgPo the nickel arsenide structure. Most polonides decompose upon heating to about 600 °C, except for HgPo that decomposes at ~300 °C and the lanthanide polonides, which do not decompose but melt at temperatures above 1000 °C. For example, PrPo melts at 1250 °C and TmPo at 2200 °C.^[18] PbPo is one of the very few naturally occurring polonium compounds, as polonium alpha decays to form lead.^[19]

Polonium hydride (PoH
2) is a volatile liquid at room temperature prone to dissociation; it is thermally unstable.^[18] Water is the only other known hydrogen chalcogenide which is a liquid at room temperature; however this is due to hydrogen bonding. The two oxides PoO₂ and PoO₃ are the products of oxidation of polonium.^[20]

Halides of the structure PoX₂, PoX₄ and PoF₆ are known. They are soluble in the corresponding hydrogen halides, i.e., PoCl_X in HCl, PoBr_X in HBr and PoI₄ in HI.^[21] Polonium dihalides are formed by direct reaction of the elements or by reduction of PoCl₄ with SO₂ and with PoBr₄ with H₂S at room temperature. Tetrahalides can be obtained by reacting polonium dioxide with HCl, HBr or HI.^[22]

Other polonium compounds include potassium polonite as a polonite, polonate, acetate, bromate, carbonate, citrate, chromate, cyanide, formate, (II) and (IV) hydroxides, nitrate, selenate, selenite, monosulfide, sulfate, disulfate and sulfite.^[21][23]

Polonium compounds^[22][24]

Formula	Color	m.p. (°C)	Sublimation temp. (°C)	Symmetry	Pearson symbol	Space group	No	a (pm)	b(pm)	c(pm)	Z	ρ (g/cm^3)	ref
PoO2	pale yellow	500 (dec.)	885	fcc	cF12	Fm3m	225	563.7	563.7	563.7	4	8.94	[25]
PoCl2	dark ruby red	355	130	orthorhombic	oP3	Pmmm	47	367	435	450	1	6.47	[26]
PoBr2	purple-brown	270 (dec.)											[27]
PoCl4	yellow	300	200	monoclinic									[26]
PoBr4	red	330 (dec.)		fcc	cF100	Fm3m	225	560	560	560	4		[27]
PoI4	black												[28]

Oxides PoO PoO2 PoO3

Hydrides PoH2

Halides PoX2 (except PoF2) PoX4 PoF6 PoBr2Cl2 (salmon pink)

History

Also tentatively called "radium F", polonium was discovered by Marie and Pierre Curie in 1898,^[29] and was named after Marie Curie's native land of Poland (Latin: Polonia).^[30][31] Poland at the time was under Russian, German, and Austro-Hungarian 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.^[32] Polonium may be the first element named to highlight a political controversy.^[32]

This element was the first one discovered by the Curies while they were investigating the cause of pitchblende radioactivity. Pitchblende, after removal of the radioactive elements uranium and thorium, was more radioactive than the uranium and thorium combined. This spurred the Curies to search for additional radioactive elements. They first separated out polonium from pitchblende in July 1898, and five months later, also isolated radium.^[15][29][33]

In the United States, polonium was produced as part of the Manhattan Project's Dayton Project during World War II. It was a critical part of the implosion-type nuclear weapon design used in the Fat Man bomb on Nagasaki in 1945. Polonium and beryllium were the key ingredients of the 'urchin' detonator at the center of the bomb's spherical plutonium pit.^[34] The urchin ignited the nuclear chain reaction at the moment of prompt-criticality to ensure the bomb did not fizzle.^[34]

Much of the basic physics of polonium was classified until after the war. The fact that it was used as an initiator was classified until the 1960s.^[35]

The Atomic Energy Commission and the Manhattan Project funded human experiments using polonium on five people at the University of Rochester between 1943 and 1947. The people were administered between 9 and 22 microcuries (330 and 810 kBq) of polonium to study its excretion.^[36][37][38]

Occurrence and production

Polonium is a very rare element in nature because of the short half-life of all its isotopes. ²¹⁰Po, ²¹⁴Po, and ²¹⁸Po appear in the decay chain of ²³⁸U; thus polonium can be found in uranium ores at about 0.1 mg per metric ton (1 part in 10¹⁰),^[39][40] 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.^[41][42][43]

Because it is present in such small concentrations, isolation of polonium from natural sources is a very tedious process. The largest batch of the element ever extracted, performed in the first half of the 20th century, contained only 40 Ci (1.5 TBq) (9 mg) of polonium-210 and was obtained by processing 37 tonnes of residues from radium production.^[44] Polonium is now obtained by irradiating bismuth with high-energy neutrons or protons.^[15][45]

In 1934, an experiment showed that when natural ²⁰⁹Bi is bombarded with neutrons, ²¹⁰Bi is created, which then decays to ²¹⁰Po via beta-minus decay. The final purification is done pyrochemically followed by liquid-liquid extraction techniques.^[46] Polonium may now be made in milligram amounts in this procedure which uses high neutron fluxes found in nuclear reactors.^[45] Only about 100 grams are produced each year, practically all of it in Russia, making polonium exceedingly rare.^[47][48]

This process can cause problems in lead-bismuth based liquid metal cooled nuclear reactors such as those used in the Soviet Navy's K-27. Measures must be taken in these reactors to deal with the unwanted possibility of ²¹⁰Po being released from the coolant.^[49][50]

The longer-lived isotopes of polonium, ²⁰⁸Po and ²⁰⁹Po, can be formed by proton or deuteron bombardment of bismuth using a cyclotron. Other more proton-rich and more unstable isotopes can be formed by the irradiation of platinum with carbon nuclei.^[51]

Applications

Polonium-based sources of alpha particles were produced in the former Soviet Union.^[52] Such sources were applied for measuring the thickness of industrial coatings via attenuation of alpha radiation.^[53]

Because of intense alpha radiation, a one-gram sample of ²¹⁰Po will spontaneously heat up to above 500 °C (932 °F) generating about 140 watts of power. Therefore, ²¹⁰Po is used as an atomic heat source to power radioisotope thermoelectric generators via thermoelectric materials.^{[4][15][54][55]} For instance, ²¹⁰Po heat sources were used in the Lunokhod 1 (1970) and Lunokhod 2 (1973) Moon rovers to keep their internal components warm during the lunar nights, as well as the Kosmos 84 and 90 satellites (1965).^[52][56]

The alpha particles emitted by polonium can be converted to neutrons using beryllium oxide, at a rate of 93 neutrons per million alpha particles.^[54] Thus Po-BeO mixtures or alloys are used as a neutron source, for example in a neutron trigger or initiator for nuclear weapons^[15][57] and for inspections of oil wells. About 1500 sources of this type, with an individual activity of 1,850 Ci (68 TBq), have been used annually in the Soviet Union.^[58]

Polonium was also part of brushes or more complex tools that eliminate static charges in photographic plates, textile mills, paper rolls, sheet plastics, and on substrates (such as automotive) prior to the application of coatings.^[59] Alpha particles emitted by polonium ionize air molecules that neutralize charges on the nearby surfaces.^[60][61] Some anti-static brushes contain up to 500 microcuries (20 MBq) of ²¹⁰Po as a source of charged particles for neutralizing static electricity.^[62] In USA, the devices with no more than 500 µCi (19 MBq) of (sealed) ²¹⁰Po per unit can be bought in any amount under a "general license",^[63] which means that a buyer need not be registered by any authorities. Polonium needs to be replaced in these devices nearly every year because of its short half-life; it is also highly radioactive and therefore has been mostly replaced by less dangerous beta particle sources.^[4]

Tiny amounts of ²¹⁰Po are sometimes used in the laboratory and for teaching purposes—typically of the order of 4–40 kBq (0.11–1.08 µCi), in the form of sealed sources, with the polonium deposited on a substrate or in a resin or polymer matrix—are often exempt from licensing by the NRC and similar authorities as they are not considered hazardous. Small amounts of ²¹⁰Po are manufactured for sale to the public in the United States as 'needle sources' for laboratory experimentation, and are retailed by scientific supply companies. The polonium is a layer of plating which in turn is plated with a material such as gold, which allows the alpha radiation (used in experiments such as cloud chambers) to pass while preventing the polonium from being released and presenting a toxic hazard. According to United Nuclear, they typically sell between four and eight such sources per year.^[64][65]

Biology and toxicity

Overview

Polonium is highly dangerous and has no biological role.^[15] By mass, polonium-210 is around 250,000 times more toxic than hydrogen cyanide (the LD₅₀ for ²¹⁰Po is less than 1 microgram for an average adult (see below) compared with about 250 milligrams for hydrogen cyanide^[66]). The main hazard is its intense radioactivity (as an alpha emitter), which makes it very difficult to handle safely. Even in microgram amounts, handling ²¹⁰Po is extremely dangerous, requiring specialized equipment (a negative pressure alpha glove box equipped with high performance filters), adequate monitoring, and strict handling procedures to avoid any contamination. Alpha particles emitted by polonium will damage organic tissue easily if polonium is ingested, inhaled, or absorbed, although they do not penetrate the epidermis and hence are not hazardous as long as the alpha particles remain outside the body. Wearing chemically resistant and intact gloves is a mandatory precaution to avoid transcutaneous diffusion of polonium directly through the skin. Polonium delivered in concentrated nitric acid can easily diffuse through inadequate gloves (e.g., latex gloves) or the acid may damage the gloves.^[67]

It has been reported that some microbes can methylate polonium by the action of methylcobalamin.^[68][69] This is similar to the way in which mercury, selenium and tellurium are methylated in living things to create organometallic compounds. Studies investigating the metabolism of polonium-210 in rats have shown that only 0.002 to 0.009% of polonium-210 ingested is excreted as volatile polonium-210.^[70]

Acute effects

The median lethal dose (LD₅₀) for acute radiation exposure is generally about 4.5 Sv.^[71] The committed effective dose equivalent ²¹⁰Po is 0.51 µSv/Bq if ingested, and 2.5 µSv/Bq if inhaled.^[72] So a fatal 4.5 Sv dose can be caused by ingesting 8.8 MBq (240 µCi), about 50 nanograms (ng), or inhaling 1.8 MBq (49 µCi), about 10 ng. One gram of ²¹⁰Po could thus in theory poison 20 million people of whom 10 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^[73]) is somewhat less damaging than an instantaneous dose. It has been estimated that a median lethal dose of ²¹⁰Po is 15 megabecquerels (0.41 mCi), or 0.089 micrograms, still an extremely small amount.^[74][75] For comparison, one grain of table salt is about 0.06 mg = 60 μg.

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.^[71] 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^[76] of the estimated 15,000–22,000 lung cancer deaths in the US every year that have been attributed to indoor radon.^[77] Tobacco smoking causes additional exposure to polonium.^[78]

Regulatory exposure limits and handling

The maximum allowable body burden for ingested ²¹⁰Po is only 1.1 kBq (30 nCi), which is equivalent to a particle massing only 6.8 picograms. The maximum permissible workplace concentration of airborne ²¹⁰Po is about 10 Bq/m³ (3×10⁻¹⁰ µCi/cm³).^[79] The target organs for polonium in humans are the spleen and liver.^[80] 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 was implemented in 2007 to register purchases of more than 16 curies (590 GBq) 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 (59 GBq)."^[81] As of 2013, this is still the only alpha emitting byproduct material available, as a NRC Exempt Quantity, which may be held without a radioactive material license.

Polonium and its compounds must be handled in a glove box, which is further enclosed in another box, maintained at a slightly higher pressure than the glove box to prevent the radioactive materials from leaking out. Gloves made of natural rubber do not provide sufficient protection against the radiation from polonium; surgical gloves are necessary. Neoprene gloves shield radiation from polonium better than natural rubber.^[82]

Well-known poisoning cases

20th century

Polonium was administered to humans for experimental purposes from 1943 to 1947; it was injected into four hospitalised patients, and orally given to a fifth. Studies such as this were funded by the Manhattan Project and the AEC, and conducted at the University of Rochester. The objective was to obtain data on human excretion of polonium to correlate with more extensive data from rats. Patients selected as subjects were chosen because experimenters wanted persons who had not been exposed to polonium either through work or accident. All subjects had incurable diseases. Excretion of polonium was followed, and an autopsy was conducted at that time on the deceased patient to determine which organs absorbed the polonium. Patients' ages ranged from 'early thirties' to 'early forties.' The experiments were described in Chapter 3 of Biological Studies with Polonium, Radium, and Plutonium, National Nuclear Energy Series, Volume VI-3, McGraw-Hill, New York, 1950. Not specified is the isotope under study, but at the time polonium-210 was the most readily available polonium isotope. The DoE factsheet submitted for this experiment reported no follow up on these subjects.^[83]

It has also been suggested that Irène Joliot-Curie was the first person to die from the radiation effects of polonium. She was accidentally exposed to polonium in 1946 when a sealed capsule of the element exploded on her laboratory bench. In 1956, she died from leukemia.^[84]

According to the 2008 book The Bomb in the Basement, several deaths in Israel during 1957–1969 were caused by ²¹⁰Po.^[85] A leak was discovered at a Weizmann Institute laboratory in 1957. Traces of ²¹⁰Po were found on the hands of professor Dror Sadeh, a physicist who researched radioactive materials. Medical tests indicated no harm, but the tests did not include bone marrow. Sadeh died 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.^[86]

21st century

The cause of death in the 2006 murder of the Russian KGB agent who defected to the British MI6 intelligence agency, Alexander Litvinenko was determined to be ²¹⁰Po poisoning.^[87][88] According to Prof. Nick Priest of Middlesex University, an environmental toxicologist and radiation expert, speaking on Sky News on December 3, 2006, Litvinenko was probably the first person to die of the acute α-radiation effects of ²¹⁰Po.^[89]

Abnormally high concentrations of ²¹⁰Po were detected in July 2012 in clothes and personal belongings of the Palestinian leader Yasser Arafat, a heavy smoker, who died on 11 November 2004 of uncertain causes. The spokesman for the Institut de Radiophysique in Lausanne, Switzerland, where those items were analyzed, stressed that the "clinical symptoms described in Arafat's medical reports were not consistent with polonium-210 and that conclusions could not be drawn as to whether the Palestinian leader was poisoned or not", and that "the only way to confirm the findings would be to exhume Arafat's body to test it for polonium-210".^[90] On 27 November 2012 Arafat's body was exhumed and samples were taken for separate analysis by experts from France, Switzerland and Russia.^[91] On 12 October 2013, The Lancet published the group's finding that high levels of the element were found in Arafat's blood, urine, and in saliva stains on his clothes and toothbrush.^[92] The French tests later found some polonium but stated it was from "natural environmental origin".^[93] Following later Russian tests, Vladimir Uiba, the head of the Russian Federal Medical and Biological Agency, stated in December 2013 that Arafat died of natural causes, and they had no plans to conduct further tests.^[93]

Treatment

It has been suggested that chelation agents such as British Anti-Lewisite (dimercaprol) can be used to decontaminate humans.^[94] 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.^[95]

Detection in biological specimens

Polonium-210 may be quantified in biological specimens by alpha particle spectrometry to confirm a diagnosis of poisoning in hospitalized patients or to provide evidence in a medicolegal death investigation. The baseline urinary excretion of polonium-210 in healthy persons due to routine exposure to environmental sources is normally in a range of 5–15 mBq/day. Levels in excess of 30 mBq/day are suggestive of excessive exposure to the radionuclide.^[96]

Occurrence in humans and the biosphere

Polonium-210 is widespread in the biosphere, including in human tissues, because of its position in the uranium-238 decay chain. Natural uranium-238 in the Earth's crust decays through a series of solid radioactive intermediates including radium-226 to the radioactive gas radon-222, some of which, during its 3.8-day half-life, diffuses into the atmosphere. There it decays through several more steps to polonium-210, much of which, during its 138-day half-life, is washed back down to the Earth's surface, thus entering the biosphere, before finally decaying to stable lead-206.^[97][98][99]

As early as the 1920s Antoine Lacassagne, using polonium provided by his colleague Marie Curie, showed that the element has a very specific pattern of uptake in rabbit tissues, with high concentrations particularly in liver, kidney and testes.^[100] More recent evidence suggests that this behavior results from polonium substituting for sulfur in sulfur-containing amino-acids or related molecules^[101] and that similar patterns of distribution occur in human tissues.^[102] Polonium is indeed an element naturally present in all humans, contributing appreciably to natural background dose, with wide geographical and cultural variations, and particularly high levels in arctic residents, for example.^[103]

Tobacco

Polonium-210 in tobacco contributes to many of the cases of lung cancer worldwide. Most of this polonium is derived from lead-210 deposited on tobacco leaves from the atmosphere; the lead-210 is a product of radon-222 gas, much of which appears to originate from the decay of radium-226 from fertilizers applied to the tobacco soils.^{[43][104][105][106][107]}

The presence of polonium in tobacco smoke has been known since the early 1960s.^[108][109] Some of the world's biggest tobacco firms researched ways to remove the substance—to no avail—over a 40-year period. The results were never published.^[43]

Food

Polonium is also found in the food chain, especially in seafood.^[110][111]

See also

• Decay chain
• Polonium halo

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Bibliography

• Bagnall, K. W. (1962). "The Chemistry of Polonium". Advances in Inorganic Chemistry and Radiochemistry. 4. New York: Academic Press. pp. 197–226. doi:10.1016/S0065-2792(08)60268-X. ISBN 0-12-023604-4. Retrieved June 14, 2012.
• Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth–Heinemann. ISBN 0080379419.

External links

• Chemistry in its element podcast (MP3) from the Royal Society of Chemistry's Chemistry World: Polonium
• Polonium at The Periodic Table of Videos (University of Nottingham)