Actinium

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Actinium is a radioactive chemical element with symbol Ac (not to be confused with the abbreviation for an acetyl group) and has the atomic number 89, which was discovered in 1899. It was the first non-primordial radioactive element to be isolated. Polonium, radium and radon were observed before actinium, but they were not isolated until 1902. Actinium gave the name to the actinide series, a group of 15 similar elements between actinium and lawrencium in the periodic table.

A soft, silvery-white radioactive metal, actinium reacts rapidly with oxygen and moisture in air forming a white coating of actinium oxide that prevents further oxidation. As with most lanthanides and actinides, actinium assumes oxidation state +3 in nearly all its chemical compounds. Actinium is found only in traces in uranium ores as the isotope ²²⁷Ac, which decays with a half-life of 21.772 years, predominantly emitting beta particles. One tonne of uranium ore contains about 0.2 milligrams of actinium. The close similarity of physical and chemical properties of actinium and lanthanum makes separation of actinium from the ore impractical. Instead, the element is prepared, in milligram amounts, by the neutron irradiation of ²²⁶Template:Radium in a nuclear reactor. Owing to its scarcity, high price and radioactivity, actinium has no significant industrial use. Its current applications include a neutron source and an agent for radiation therapy targeting cancer cells in the body.

History

André-Louis Debierne, a French chemist, announced the discovery of a new element in 1899. He separated it from pitchblende residues left by Marie and Pierre Curie after they had extracted radium. In 1899, Debierne described the substance as similar to titanium<ref>Template:Cite journal</ref> and (in 1900) as similar to thorium.<ref>Template:Cite journal</ref> Friedrich Oskar Giesel independently discovered actinium in 1902<ref>Template:Cite journal</ref> as a substance being similar to lanthanum and called it "emanium" in 1904.<ref>Template:Cite journal</ref> After a comparison of the substances half-lives determined by Debierne<ref>Template:Cite journal</ref>, Hariett Brooks in 1904, and Otto Hahn and Otto Sackur in 1905, Debierne's chosen name for the new element was retained because it had seniority.<ref>Template:Cite journal</ref><ref>Template:Cite journal</ref>

Articles published in the 1970s<ref>Template:Cite journal</ref> and later<ref name="Adloff">Template:Cite journal</ref> suggest that Debierne's results published in 1904 conflict with those reported in 1899 and 1900. This has led some authors to advocate that Giesel alone should be credited with the discovery.<ref>Template:Cite journal</ref> A less confrontational vision of scientific discovery is proposed by Adloff<ref name="Adloff" /> He suggests that hindsight criticism of the early publications should be mitigated by the nascent state of radiochemistry, highlights the prudence of Debierne's claims in the original papers, and notes that nobody can contend that Debierne's substance did not contain actinium. Debierne, who is now considered by the vast majority of historians as the discoverer, lost interest in the element and left the topic. Giesel, on the other hand, can rightfully be credited with the first preparation of radiochemically pure actinium and with the identification of its atomic number 89.

The name actinium originates from the Ancient Greek aktis, aktinos (ακτίς, ακτίνος), meaning beam or ray.<ref name=CRC/> Its symbol Ac is also used in abbreviations of other compounds that have nothing to do with actinium, such as acetyl, acetate<ref>Template:Cite book</ref> and sometimes acetaldehyde.<ref>Template:Cite book</ref>

Properties

Actinium is a soft, silvery-white,<ref name="blueglow"/><ref name=brit>Actinium, in Encyclopædia Britannica, 15th edition, 1995, p. 70</ref> radioactive, metallic element. Its estimated shear modulus is similar to that of lead.<ref>Frederick Seitz, David Turnbull Solid state physics: advances in research and applications, Academic Press, 1964 ISBN 0-12-607716-9 pp. 289–291</ref> Owing to its strong radioactivity, actinium glows in the dark with a pale blue light, which originates from the surrounding air ionized by the emitted energetic particles.<ref>Template:Cite book</ref> Actinium has similar chemical properties as lanthanum and other lanthanides, and therefore these elements are difficult to separate when extracting from uranium ores. Solvent extraction and ion chromatography are commonly used for the separation.<ref>Template:Cite journal</ref>

The first element of the actinides, actinium gave the group its name, much as lanthanum had done for the lanthanides. The group of elements is more diverse than the lanthanides and therefore it was not until 1945 that Glenn T. Seaborg proposed the most significant change to Mendeleev's periodic table, by introducing the actinides.<ref>Template:Cite journal</ref>

Actinium reacts rapidly with oxygen and moisture in air forming a white coating of actinium oxide that prevents further oxidation.<ref name="blueglow">Template:Cite journal</ref> As with most lanthanides and actinides, actinium exists in the oxidation state +3, and the Ac³⁺ ions are colorless in solutions.<ref name=bse/> The oxidation state +3 originates from the 6d¹7s² electronic configuration of actinium, that is it easily donates 3 electrons assuming a stable closed-shell structure of the noble gas radon.<ref name=brit/> The oxidation state +2 is only known for actinium dihydride (AcH₂).

Chemical compounds

Only a limited number of actinium compounds are known including AcF₃, AcCl₃, AcBr₃, AcOF, AcOCl, AcOBr, Ac₂S₃, Ac₂O₃ and AcPO₄. Except for AcPO₄, they are all similar to the corresponding lanthanum compounds and contain actinium in the oxidation state +3.<ref name=bse/><ref>Template:Cite journal</ref> In particular, the lattice constants of the analogous lanthanum and actinium compounds differ by only a few percent.<ref name=j2/>

Here a, b and c are lattice constants, No is space group number and Z is the number of formula units per unit cell. Density was not measured directly but calculated from the lattice parameters.

Oxides

Actinium oxide (Ac₂O₃) can be obtained by heating the hydroxide at 500 °C or the oxalate at 1100 °C, in vacuum. It crystal lattice is isotypic with the oxides of most trivalent rare-earth metals.<ref name=j2/>

Halides

Actinium trifluoride can be produced either in solution or in solid reaction. The former reaction is carried out at room temperature, by adding hydrofluoric acid to a solution containing actinium ions. In the latter method, actinium metal is treated with hydrogen fluoride vapors at 700 °C in an all-platinum setup. Treating actinium trifluoride with ammonium hydroxide at 900–1000 °C yields oxyfluoride AcOF. Whereas lanthanum oxyfluoride can be easily obtained by burning lanthanum trifluoride in air at 800 °C for an hour, similar treatment of actinium trifluoride yields no AcOF and only results in melting of the initial product.<ref name=j2/><ref name=m87>Meyer, pp. 87–88</ref>

AcF₃ + 2 NH₃ + H₂O → AcOF + 2 NH₄F

Actinium trichloride is obtained by reacting actinium hydroxide or oxalate with carbon tetrachloride vapors at temperatures above 960 °C. Similar to oxyfluoride, actinium oxychloride can be prepared by hydrolyzing actinium trichloride with ammonium hydroxide at 1000 °C. However, in contrast to the oxyfluoride, the oxychloride could well be synthesized by igniting a solution of actinium trichloride in hydrochloric acid with ammonia.<ref name=j2/>

Reaction of aluminium bromide and actinium oxide yields actinium tribromide:

Ac₂O₃ + 2 AlBr₃ → 2 AcBr₃ + Al₂O₃

and treating it with ammonium hydroxide at 500 °C results in the oxybromide AcOBr.<ref name=j2/>

Other compounds

Actinium hydride was obtained by reduction of actinium trichloride with potassium at 300 °C, and its structure was deduced by analogy with the corresponding LaH₂ hydride. The source of hydrogen in the reaction was uncertain.<ref>Meyer, p. 43</ref>

Mixing monosodium phosphate (NaH₂PO₄) with a solution of actinium in hydrochloric acid yields white-colored actinium phosphate hemihydrate (AcPO₄·0.5H₂O), and heating actinium oxalate with hydrogen sulfide vapors at 1400 °C for a few minutes results in a black actinium sulfide Ac₂S₃. It may possibly be produced by acting with a mixture of hydrogen sulfide and carbon disulfide on actinium oxide at 1000 °C.<ref name=j2/>

Isotopes

Template:Main Naturally occurring actinium is composed of one radioactive isotope; Template:Chem. Thirty-six radioisotopes have been identified, the most stable being Template:Chem with a half-life of 21.772 years, Template:Chem with a half-life of 10.0 days and Template:Chem with a half-life of 29.37 hours. All remaining radioactive isotopes have half-lives that are less than 10 hours and the majority of them have half-lives shorter than one minute. The shortest-lived known isotope of actinium is Template:Chem (half-life of 69 nanoseconds) which decays through alpha decay and electron capture. Actinium also has two meta states.<ref name ="nubas">Template:Cite journal</ref>

Purified Template:Chem comes into equilibrium with its decay products at the end of 185 days. It decays according to its 21.773-year half-life emitting mostly beta (98.8%) and some alpha particles (1.2%);<ref name=bse>Actinium, Great Soviet Encyclopedia (in Russian)</ref> the successive decay products are part of the actinium series. Owing to the low available amounts, low energy of its beta particles (46 keV) and low intensity of alpha radiation, Template:Chem is difficult to detect directly by its emission and it is therefore traced via its decay products.<ref name=bse/> The isotopes of actinium range in atomic weight from 206 u (Template:Chem) to 236 u (Template:Chem).<ref name ="nubas"/>

Occurrence and synthesis

Actinium is found only in traces in uranium ores as ²²⁷Ac – one tonne of ore contains about 0.2 milligrams of actinium.<ref name=j1>Template:Cite journal</ref><ref name=g946>Template:Greenwood&Earnshaw2nd</ref> The actinium isotope ²²⁷Ac is a transient member of the actinium series decay chain, which begins with the parent isotope ²³⁵U (or ²³⁹Pu) and ends with the stable lead isotope ²⁰⁷Pb. Another actinium isotope (²²⁵Ac) is transiently present in the neptunium series decay chain, beginning with ²³⁷Np (or ²³³U) and ending with thallium (²⁰⁵Tl) and near-stable bismuth (²⁰⁹Bi).

The low natural concentration, and the close similarity of physical and chemical properties to those of lanthanum and other lanthanides, which are always abundant in actinium-bearing ores, render separation of actinium from the ore impractical, and complete separation was never achieved.<ref name=j2>Template:Cite journal</ref> Instead, actinium is prepared, in milligram amounts, by the neutron irradiation of ²²⁶Template:Radium in a nuclear reactor.<ref name=g946/><ref>Template:Cite book</ref>

Failed to parse (Cannot write to or create math temp directory): \mathrm{^{226}_{\ 88}Ra\ +\ ^{1}_{0}n\ \longrightarrow \ ^{227}_{\ 88}Ra\ \xrightarrow[42.2 \ min]{\beta^-} \ ^{227}_{\ 89}Ac}

The reaction yield is about 2% of the radium weight. ²²⁷Ac can further capture neutrons resulting in small amounts of ²²⁸Ac. After the synthesis, actinium is separated from radium and from the products of decay and nuclear fusion, such as thorium, polonium, lead and bismuth. The extraction can be performed with thenoyltrifluoroacetone-benzene solution from an aqueous solution of the radiation products, and the selectivity to a certain element is achieved by adjusting the pH (to about 6.0 for actinium).<ref name=j1/> An alternative procedure is anion exchange with an appropriate resin in nitric acid, which can result in a separation factor of 1,000,000 for radium and actinium vs. thorium in a two-stage process. Actinium can then be separated from radium, with a ratio of about 100, using a low cross-linking cation exchange resin and nitric acid as eluant.<ref name=sep/>

²²⁵Ac was first produced artificially at the Institute for Transuranium Elements (ITU) in Germany using a cyclotron and at St George Hospital in Sydney using a linac in 2000.<ref>Template:Cite journal</ref> This rare isotope has potential applications in radiation therapy and is most efficiently produced by bombarding a radium-226 target with 20–30 MeV deuterium ions. This reaction also yields ²²⁶Ac which however decays with a half-life of 29 hours and thus does not contaminate ²²⁵Ac.<ref>Russell, Pamela J.; Jackson, Paul and Kingsley, Elizabeth Anne Prostate cancer methods and protocols, Humana Press, 2003, ISBN 0-89603-978-1, p. 336</ref>

Actinium metal has been prepared by the reduction of actinium fluoride with lithium vapor in vacuum at a temperature between 1100 and 1300 °C. Higher temperatures resulted in evaporation of the product and lower ones lead to an incomplete transformation. Lithium was chosen among other alkali metals because its fluoride is most volatile.<ref name=CRC>Hammond, C. R. The Elements in Template:RubberBible86th</ref><ref name="blueglow"/>

Applications

Owing to its scarcity, high price and radioactivity, actinium currently has no significant industrial use.<ref name=CRC/>

²²⁷Ac is highly radioactive and was therefore studied for use as an active element of radioisotope thermoelectric generators, for example in spacecraft. The oxide of ²²⁷Ac pressed with beryllium is also an efficient neutron source with the activity exceeding that of the standard americium-beryllium and radium-beryllium pairs.<ref name=b1>Russell, Alan M. and Lee, Kok Loong Structure-property relations in nonferrous metals, Wiley, 2005, ISBN 0-471-64952-X, pp. 470–471</ref> In all those applications, ²²⁷Ac (a beta source) is merely a progenitor which generates alpha-emitting isotopes upon its decay. Beryllium captures alpha particles and emits neutrons owing to its large cross-section for the (α,n) nuclear reaction:

Failed to parse (Cannot write to or create math temp directory): \mathrm{^{9}_{4}Be\ +\ ^{4}_{2}He\ \longrightarrow \ ^{12}_{\ 6}C\ +\ ^{1}_{0}n\ +\ \gamma}

The ²²⁷AcBe neutron sources can be applied in a neutron probe – a standard device for measuring the quantity of water present in soil, as well as moisture/density for quality control in highway construction.<ref>Majumdar, D. K. Irrigation Water Management: Principles and Practice, 2004 ISBN 81-203-1729-7 p. 108</ref><ref>Chandrasekharan, H. and Gupta, Navindu Fundamentals of Nuclear Science – Application in Agriculture, 2006 ISBN 81-7211-200-9 pp. 202 ff</ref> Such probes are also used in well logging applications, in neutron radiography, tomography and other radiochemical investigations.<ref>Template:Cite journal</ref>

²²⁵Ac is applied in medicine to produce ²¹³Template:Bismuth in a reusable generator<ref name=sep>Template:Cite journal</ref> or can be used alone as an agent for radiation therapy, in particular targeted alpha therapy (TAT). This isotope has a half-life of 10 days that makes it much more suitable for radiation therapy than ²¹³Bi (half-life 46 minutes). Not only ²²⁵Ac itself, but also its decay products emit alpha particles which kill cancer cells in the body. The major difficulty with application of ²²⁵Ac was that intravenous injection of simple actinium complexes resulted in their accumulation in the bones and liver for a period of tens of years. As a result, after the cancer cells were quickly killed by alpha particles from ²²⁵Ac, the radiation from the actinium and its decay products might induce new mutations. To solve this problem, ²²⁵Ac was bound to a chelating agent, such as citrate, ethylenediaminetetraacetic acid (EDTA) or diethylene triamine pentaacetic acid (DTPA). This reduced actinium accumulation in the bones, but the excretion from the body remained slow. Much better results were obtained with such chelating agents as HEHA<ref>Template:Cite journal</ref> or DOTA (1,4,7,10-tetraazacyclododecane-1,4,7,10-tetraacetic acid) coupled to trastuzumab, a monoclonal antibody that interferes with the HER2/neu receptor. The latter delivery combination was tested on mice and proved to be effective against leukemia, lymphoma, breast, ovarian, neuroblastoma and prostate cancers.<ref>Template:Cite journal</ref><ref>Template:Cite journal</ref><ref>Template:Cite journal</ref>

The medium half-life of ²²⁷Ac (21.77 years) makes it very convenient radioactive isotope in modeling the slow vertical mixing of oceanic waters. The associated processes cannot be studied with the required accuracy by direct measurements of current velocities (of the order 50 meters per year). However, evaluation of the concentration depth-profiles for different isotopes allows estimating the mixing rates. The physics behind this method is as follows: oceanic waters contain homogeneously dispersed ²³⁵U. Its decay product, ²³¹Pa, gradually precipitates to the bottom, so that its concentration first increases with depth and then stays nearly constant. ²³¹Pa decays to ²²⁷Ac; however, the concentration of the latter isotope does not follow the ²³¹Pa depth profile, but instead increases toward the sea bottom. This occurs because of the mixing processes which raise some additional ²²⁷Ac from the sea bottom. Thus analysis of both ²³¹Pa and ²²⁷Ac depth profiles allows to model the mixing behavior.<ref>Template:Cite journal</ref><ref>Template:Cite journal</ref>

Precautions

²²⁷Ac is highly radioactive and experiments with it are carried out in a specially designed laboratory equipped with a glove box and radiation shielding. When actinium trichloride is administered intravenously to rats, about 33% of actinium is deposited into the bones and 50% into the liver. Its toxicity is comparable to, but slightly lower than that of americium and plutonium.<ref>Template:Cite journal</ref>

See also

• Actinium series

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References

Template:Reflist

Bibliography

• Meyer, Gerd and Morss, Lester R. Synthesis of lanthanide and actinide compounds, Springer, 1991, ISBN 0-7923-1018-7

External links

• NLM Hazardous Substances Databank – Actinium, Radioactive
• Actinium in Template:Cite book

Template:Compact periodic table Template:Use dmy datesTemplate:Link GA Template:Link FA

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