Actinium – Element information, properties and uses


ACTINIUM, is a very rare radioactive element, atomic number 89. It occurs as one part in 7 billion in uranium minerals. A silvery white metal, it glows slightly in the dark. It oxidizes rapidly in moist air to form a coating of white actinium oxide. In compounds, actinium is colorless and trivalent. Actinium’s melting point is 1100° C; it has a face-centered cubic structure; and its Standard oxidation potential of about 2.6 volts indicates its highly electropositive character. Actinium was discovered in 1899 by Andre Debierne, a colleague of Marie Curie.


The only isotope of actinium with a long half-life (22 years) is \displaystyle A{{c}^{{227}}}, in the decay chain originating with \displaystyle {{U}^{{233}}}. isotopes with mass numbers from \displaystyle A{{c}^{{221}}} to \displaystyle A{{c}^{{230}}} are known. \displaystyle A{{c}^{{228}}}, which decays to \displaystyle T{{h}^{{228}}} by beta emission, often is used in tracer level studies of actinium chemistry.

Actinium is similar to yttrium and lanthanum in both electronic structure and chemistry. Because the crystal radius of \displaystyle A{{c}^{{+3}}} (1.11 Â) is slightly larger than that of \displaystyle L{{a}^{{+3}}} (1.06 A), \displaystyle A{{c}^{{+3}}} has greater basicity, causing differences in chemical properties sufficient to separate actinium from lanthanum and the lanthanide ions by ion exchange and solvent extraction techniques.

Cation exchange resins with nitric acid or citrate solutions separate actinium from \displaystyle R{{a}^{{+2}}}, \displaystyle T{{h}^{{+4}}}, \displaystyle L{{a}^{{+3}}}, and the trivalent lanthanides. Then oyltrifluoroacetone solutions in benzene separate actinium from these elements by solvent extraction. In aqueous solution \displaystyle A{{c}^{{+3}}} forms weak complex compounds with halides and nitrate and sulfate anions. It forms stronger complex compounds with organic anions such as acetate, glycolate, citrate, and ethylenediaminetetraacetate.

The fluoride, hydroxide, carbonate, phosphate, and oxalate compounds are insoluble and are used in purification. As a separation method, tracer concentrations of \displaystyle A{{c}^{{+3}}} are coprecipitated with lanthanum fluoride or oxalate. Iron hydroxide, aluminum hydroxide, barium sulfate, and zirconium iodate also may be used to coprecipitate tracer concentrations of \displaystyle A{{c}^{{+3}}} under proper conditions. Actinium is produced by the reduction of actinium fluoride or chloride with lithium or potassium vapor. It has no commercial uses.

Leave A Reply

This site uses Akismet to reduce spam. Learn how your comment data is processed.