Europium (pronEng|jʊˈroʊpiəm) is a
chemical elementwith the symbol Eu and atomic number63. It was named after the continent Europe.
Europium is the most reactive of the
rare earth elements; it rapidly oxidizes in air, and resembles calciumin its reaction with water; deliveries of the metal element in solid form, even when coated with a protective layer of mineral oil, are rarely shiny. Europium ignites in air at about 150 °C to 180 °C. It is about as hard as lead and quite ductile.
There are many commercial applications for europium metal, although it has been used to dope some types of
glassto make lasers, as well as for screening for Down syndromeand some other genetic diseases. Due to its amazing ability to absorb neutrons, it is also being studied for use in nuclear reactors. Europium oxide (Eu2O3) is widely used as a red phosphorin television sets and fluorescent lamps, and as an activator for yttrium-based phosphors. Whereas trivalent europium gives red phosphors, divalent europium gives blue phosphors. The two europium phosphor classes, combined with the yellow/green terbium phosphors give "white" light, the color temperature of which can be varied by altering the proportion or specific composition of the individual phosphors. This is the phosphor system typically encountered in the helical fluorescent lightbulbs. Combining the same three classes is one way to make trichromatic systems in TV and computer screens. It is also being used as an agent for the manufacture of fluorescent glass. Europium fluorescence is used to interrogate biomolecular interactions in drug-discovery screens. It is also used in the anti-counterfeiting phosphors in Eurobanknotes. [ Europium and the Euro [http://www.smarterscience.com/eurosandeuropium.html] ]
Europium is commonly included in trace element studies in
geochemistryand petrologyto understand the processes that form igneous rocks(rocks that cooled from magmaor lava). The nature of the europium anomalyfound is used to help reconstruct the relationships within a suite of igneous rocks.
Europium was first found by
Paul Émile Lecoq de Boisbaudranin 1890, who obtained basic fraction from samarium- gadoliniumconcentrates which had spectral lines not accounted for by samariumor gadolinium; however, the discovery of europium is generally credited to French chemist Eugène-Anatole Demarçay, who suspected samples of the recently discovered element samariumwere contaminated with an unknown element in 1896 and who was able to isolate europium in 1901.When the europium-doped yttrium orthovanadate red phosphor was discovered in the early 1960s, and understood to be about to cause a revolution in the color television industry, there was a mad scramble for the limited supply of europium on hand among the monazite processors. (Typical europium content in monazite was about 0.05%.) Luckily, Molycorp, with its bastnäsitedeposit at Mountain Pass, California, whose lanthanides had an unusually "rich" europium content of 0.1%, was about to come on-line and provide sufficient europium to sustain the industry. Prior to europium, the color-TV red phosphor was very weak, and the other phosphor colors had to be muted, to maintain color balance. With the brilliant red europium phosphor, it was no longer necessary to mute the other colors, and a much brighter color TV picture was the result. Europium has continued in use in the TV industry ever since, and, of course, also in computer monitors. Californian bastnäsite now faces stiff competition from Bayan Obo, China, with an even "richer" europium content of 0.2%.Frank Spedding, celebrated for his development of the ion-exchange technology that revolutionized the rare earth industry in the mid-1950s once related the story of how, in the 1930s, he was lecturing on the rare earths when an elderly gentleman approached him with an offer of a gift of several pounds of europium oxide. This was an unheard-of quantity at the time, and Spedding did not take the man seriously. However, a package duly arrived in the mail, containing several pounds of genuine europium oxide. The elderly gentleman had turned out to be the Dr. McCoy who had developed a famous method of europium purification involving redox chemistry.
Europium is never found in nature as a free element; however, there are many minerals containing europium, with the most important sources being
bastnäsiteand monazite. Europium has also been identified in the spectra of the sun and certain stars. Depletion or enrichment of europium in minerals relative to other rare earth elements is known as the europium anomaly.
Divalent europium in small amounts happens to be the activator of the bright blue fluorescence of some samples of the mineral fluorite (calcium difluoride). The most outstanding examples of this originated around
Weardale, and adjacent parts of northern England, and indeed it was this fluorite that gave its name to the phenomenon of fluorescence, although it was not until much later that europium was discovered or determined to be the cause.
Europium compounds include:
Fluorides: EuF2 EuF3
Chlorides: EuCl2 EuCl3
Bromides: EuBr2 EuBr3
Iodides: EuI2 EuI3
Oxides: EuO Eu2O3 Eu3O4
* Tellurides: EuTe
Nitrides: EuNEuropium(II) compounds tend to predominate, in contrast to most lanthanides: (which generally form compounds with an oxidation state of +3). Europium(II) chemistry is very similar to barium(II) chemistry, as they have similar ionic radii. Divalent europium is a mild reducing agent, such that under atmospheric conditions, it is the trivalent form that predominates. Under anaerobic, and particularly under geothermal conditions, the divalent form is sufficiently stable such that it tends to be incorporated into minerals of calcium and the other alkaline earths. This is the cause of the "negative europium anomaly", that depletes europium from being incorporated into the most usual light lanthanide minerals such as monazite, relative to the chondritic abundance. Bastnäsite tends to show less of a negative europium anomaly than monazite does, and hence is the major source of europium today.The accessible divalency of europium has always made it one of the easiest lanthanides to extract and purify, even when present, as it usually is, in low concentration. "See also ."
Naturally occurring europium is composed of 2
isotopes, 151Eu and 153Eu, with 153Eu being the most abundant (52.2% natural abundance). While 153Eu is stable, 151Eu was recently found to be unstable to alpha decaywith half-lifeof yr [Search for α decay of natural Europium, P. Belli, R. Bernabei, F. Cappell, R. Cerulli, C.J. Dai, F.A. Danevich, A. d'Angelo, A. Incicchitti, V.V. Kobychev, S.S. Nagorny, S. Nisi, F. Nozzoli, D. Prosperi, V.I. Tretyak, and S.S. Yurchenko, Nucl. Phys. A 789, 15 (2007) doi|10.1016/j.nuclphysa.2007.03.001] , in reasonable agreement with theoretical predictions. Besides natural radioisotope 151Eu, 35 artificial radioisotopes have been characterized, with the most stable being 150Eu with a half-lifeof 36.9 years, 152Eu with a half-life of 13.516 years, and 154Eu with a half-life of 8.593 years. All of the remaining radioactiveisotopes have half-lives that are less than 4.7612 years, and the majority of these have half-lives that are less than 12.2 seconds. This element also has 8 meta states, with the most stable being 150mEu (t½ 12.8 hours), 152m1Eu (t½ 9.3116 hours) and 152m2Eu (t½ 96 minutes).
decay modebefore the most abundant stable isotope, 153Eu, is electron capture, and the primary mode after is beta minus decay. The primary decay products before 153Eu are isotopes of samarium(Sm) and the primary products after are isotopes of gadolinium(Gd).
Europium as a nuclear fission product
Europium is produced by nuclear fission, but the
fission product yields of europium isotopes are low near the top of the mass range for fission products.
Like other lanthanides, many isotopes, especially isotopes with odd mass numbers and neutron-poor isotopes like 152Eu, have high
cross sections for neutron capture, often high enough to be neutron poisons.
151Eu is the
beta decayproduct of Sm-151, but since this has a long decay half-life and short mean time to neutron absorption, most 151Sm instead winds up as 152Sm.
152Eu (half-life 13.516 years) and 154Eu (halflife 8.593 years) cannot be beta decay products because 152Sm and 154Sm are nonradioactive, but 154Eu is the only long-lived "shielded"
nuclide, other than 134Cs, to have a fission yield of more than 2.5 parts per millionfissions. [ORNL Table of the Nuclides] A larger amount of 154Eu will be produced by neutron activationof a significant portion of the nonradioactive153Eu; however, much of this will be further converted to 155Eu.
155Eu (halflife 4.7612 years) has a fission yield of 330 ppm for
U-235and thermal neutrons. Most will be transmuted to nonradioactive and nonabsorptive Gadolinium-156 by the end of fuel burnup.
Overall, europium is overshadowed by
Cs-137and Sr-90as a radiation hazard, and by samariumand others as a neutron poison.
The toxicity of europium compounds has not been fully investigated, but there are no clear indications that europium is highly toxic compared to other heavy metals. The metal dust presents a fire and explosion hazard. Europium has no known biological role.
Isolation of Europium
Europium metal is available commercially, so it is not normally necessary to make it in the laboratory — which is just as well, as it is difficult to isolate as the pure metal. This is largely because of the way it is found in nature, wherein the lanthanoids are found in a number of minerals. The most important are
xenotime, monazite, and bastnäsite. The first two are orthophosphate minerals LnPO4 (Ln denotes a mixture of all the lanthanoids except promethiumwhich is vanishingly rare due to being radioactive) and the third is a fluoride carbonate LnCO3F. Lanthanoids with even atomic numbers are more common. The most common lanthanoids in these minerals are, in order, cerium, lanthanum, neodymium, and praseodymium. Monazite also contains thoriumand yttrium, which makes handling difficult since thorium and its decomposition products are radioactive.
For many purposes it is not particularly necessary to separate the metals, but if separation into individual metals is required, the process is complex. Initially, the metals are extracted as salts from the ores by extraction with
sulfuric acid(H2SO4), hydrochloric acid(HCl), and sodium hydroxide(NaOH). Modern purification techniques for these lanthanoid salt mixtures are ingenious and involve selective complexationtechniques, solvent extractions, and ion exchange chromatography.
Pure europium is available through the electrolysis of a mixture of molten EuCl3 and NaCl (or CaCl2) in a graphite cell which acts as cathode, using graphite as anode. The other product is
* [http://periodic.lanl.gov/elements/63.html Los Alamos National Laboratory – Europium]
* [http://www.webelements.com/webelements/elements/text/Eu/index.html WebElements.com – Europium]
* [http://education.jlab.org/itselemental/ele063.html It's Elemental – Europium]
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