Europium | ||||||||||||||||||||||||||||||||||||||
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Pronunciation | /jʊəˈroʊpiəm/ | |||||||||||||||||||||||||||||||||||||
Appearance | silvery white, with a pale yellow tint; but rarely seen without oxide discoloration | |||||||||||||||||||||||||||||||||||||
Standard atomic weight Ar, std(Eu) | 151.964(1) | |||||||||||||||||||||||||||||||||||||
Europium in the periodic table | ||||||||||||||||||||||||||||||||||||||
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Atomic number (Z) | 63 | |||||||||||||||||||||||||||||||||||||
Group | group n/a | |||||||||||||||||||||||||||||||||||||
Period | period 6 | |||||||||||||||||||||||||||||||||||||
Block | f-block | |||||||||||||||||||||||||||||||||||||
Element category | lanthanide | |||||||||||||||||||||||||||||||||||||
Electron configuration | [Xe] 4f7 6s2 | |||||||||||||||||||||||||||||||||||||
Electrons per shell
| 2, 8, 18, 25, 8, 2 | |||||||||||||||||||||||||||||||||||||
Physical properties | ||||||||||||||||||||||||||||||||||||||
Phase at STP | solid | |||||||||||||||||||||||||||||||||||||
Melting point | 1099 K (826 °C, 1519 °F) | |||||||||||||||||||||||||||||||||||||
Boiling point | 1802 K (1529 °C, 2784 °F) | |||||||||||||||||||||||||||||||||||||
Density (near r.t.) | 5.264 g/cm3 | |||||||||||||||||||||||||||||||||||||
when liquid (at m.p.) | 5.13 g/cm3 | |||||||||||||||||||||||||||||||||||||
Heat of fusion | 9.21 kJ/mol | |||||||||||||||||||||||||||||||||||||
Heat of vaporization | 176 kJ/mol | |||||||||||||||||||||||||||||||||||||
Molar heat capacity | 27.66 J/(mol·K) | |||||||||||||||||||||||||||||||||||||
Vapor pressure
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Atomic properties | ||||||||||||||||||||||||||||||||||||||
Oxidation states | +1, +2, +3 (a mildly basic oxide) | |||||||||||||||||||||||||||||||||||||
Electronegativity | Pauling scale: 1.2 | |||||||||||||||||||||||||||||||||||||
Ionization energies |
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Atomic radius | empirical: 180 pm | |||||||||||||||||||||||||||||||||||||
Covalent radius | 198±6 pm | |||||||||||||||||||||||||||||||||||||
Spectral lines of europium | ||||||||||||||||||||||||||||||||||||||
Other properties | ||||||||||||||||||||||||||||||||||||||
Natural occurrence | primordial | |||||||||||||||||||||||||||||||||||||
Crystal structure | body-centered cubic (bcc) | |||||||||||||||||||||||||||||||||||||
Thermal expansion | poly: 35.0 µm/(m·K) (at r.t.) | |||||||||||||||||||||||||||||||||||||
Thermal conductivity | est. 13.9 W/(m·K) | |||||||||||||||||||||||||||||||||||||
Electrical resistivity | poly: 0.900 µΩ·m (at r.t.) | |||||||||||||||||||||||||||||||||||||
Magnetic ordering | paramagnetic | |||||||||||||||||||||||||||||||||||||
Magnetic susceptibility | +34,000.0·10−6 cm3/mol | |||||||||||||||||||||||||||||||||||||
Young's modulus | 18.2 GPa | |||||||||||||||||||||||||||||||||||||
Shear modulus | 7.9 GPa | |||||||||||||||||||||||||||||||||||||
Bulk modulus | 8.3 GPa | |||||||||||||||||||||||||||||||||||||
Poisson ratio | 0.152 | |||||||||||||||||||||||||||||||||||||
Vickers hardness | 165–200 MPa | |||||||||||||||||||||||||||||||||||||
CAS Number | 7440-53-1 | |||||||||||||||||||||||||||||||||||||
History | ||||||||||||||||||||||||||||||||||||||
Naming | after Europe | |||||||||||||||||||||||||||||||||||||
Discovery and first isolation | Eugène-Anatole Demarçay (1896, 1901) | |||||||||||||||||||||||||||||||||||||
Main isotopes of europium | ||||||||||||||||||||||||||||||||||||||
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Europium is a chemical element with the symbol Eu and atomic number 63. Europium is the most reactive lanthanide by far, having to be stored under an inert fluid to protect it from atmospheric oxygen or moisture. Europium is also the softest lanthanide, as it can be dented with a finger nail and easily cut with a knife. When oxidation is removed a shiny-white metal is visible. Europium was isolated in 1901 and is named after the continent of Europe. Being a typical member of the lanthanide series, europium usually assumes the oxidation state +3, but the oxidation state +2 is also common. All europium compounds with oxidation state +2 are slightly reducing. Europium has no significant biological role and is relatively non-toxic compared to other heavy metals. Most applications of europium exploit the phosphorescence of europium compounds. Europium is one of the rarest of rare earth elements on Earth and among the least abundant elements in the universe; only about 5×10−8% of all matter in the universe is europium.
Characteristics
Physical properties
Europium is a ductile metal with a hardness similar to that of lead. It crystallizes in a body-centered cubic lattice. Some properties of europium are strongly influenced by its half-filled electron shell. Europium has the second lowest melting point and the lowest density of all lanthanides.
Europium becomes a superconductor when it is cooled below 1.8 K and compressed to above 80 GPa. This occurs because europium is divalent in the metallic state, and is converted into the trivalent state by the applied pressure. In the divalent state, the strong local magnetic moment (J = 7/2) suppresses the superconductivity, which is induced by eliminating this local moment (J = 0 in Eu3+).
Chemical properties
Europium is the most reactive rare-earth element. It rapidly oxidizes in air, so that bulk oxidation of a centimeter-sized sample occurs within several days. Its reactivity with water is comparable to that of calcium, and the reaction is
- 2 Eu + 6 H2O → 2 Eu(OH)3 + 3 H2
Because of the high reactivity, samples of solid europium rarely have
the shiny appearance of the fresh metal, even when coated with a
protective layer of mineral oil. Europium ignites in air at 150 to
180 °C to form europium(III) oxide:
- 4 Eu + 3 O2 → 2 Eu2O3
Europium dissolves readily in dilute sulfuric acid to form pale pink solutions of the hydrated Eu(III), which exist as a nonahydrate:
- 2 Eu + 3 H2SO4 + 18 H2O →
- 2 [Eu(H2O)9]3+ + 3 SO2−
4 + 3 H2
Eu(II) vs. Eu(III)
Although usually trivalent, europium readily forms divalent compounds. This behavior is unusual for most lanthanides, which almost exclusively form compounds with an oxidation state of +3. The +2 state has an electron configuration 4f7 because the half-filled f-shell provides more stability. In terms of size and coordination number, europium(II) and barium(II) are similar. The sulfates of both barium and europium(II) are also highly insoluble in water.
Divalent europium is a mild reducing agent, oxidizing in air to form
Eu(III) compounds. In anaerobic, and particularly geothermal conditions,
the divalent form is sufficiently stable that it tends to be
incorporated into minerals of calcium and the other alkaline earths.
This ion-exchange process is the basis of the "negative europium anomaly", the low europium content in many lanthanide minerals such as monazite, relative to the chondritic
abundance. Bastnäsite tends to show less of a negative europium anomaly
than does monazite, and hence is the major source of europium today.
The development of easy methods to separate divalent europium from the
other (trivalent) lanthanides made europium accessible even when present
in low concentration, as it usually is.
Isotopes
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 decay with a half-life of 5+11
−3×1018 years, giving about 1 alpha decay per two minutes in every kilogram of natural europium. This value is in reasonable agreement with theoretical predictions. Besides the natural radioisotope 151Eu, 35 artificial radioisotopes have been characterized, the most stable being 150Eu with a half-life of 36.9 years, 152Eu with a half-life of 13.516 years, and 154Eu with a half-life of 8.593 years. All the remaining radioactive isotopes have half-lives shorter than 4.7612 years, and the majority of these have half-lives shorter than 12.2 seconds. This element also has 8 meta states, with the most stable being 150mEu (t1/2=12.8 hours), 152m1Eu (t1/2=9.3116 hours) and 152m2Eu (t1/2=96 minutes).
−3×1018 years, giving about 1 alpha decay per two minutes in every kilogram of natural europium. This value is in reasonable agreement with theoretical predictions. Besides the natural radioisotope 151Eu, 35 artificial radioisotopes have been characterized, the most stable being 150Eu with a half-life of 36.9 years, 152Eu with a half-life of 13.516 years, and 154Eu with a half-life of 8.593 years. All the remaining radioactive isotopes have half-lives shorter than 4.7612 years, and the majority of these have half-lives shorter than 12.2 seconds. This element also has 8 meta states, with the most stable being 150mEu (t1/2=12.8 hours), 152m1Eu (t1/2=9.3116 hours) and 152m2Eu (t1/2=96 minutes).
The primary decay mode for isotopes lighter than 153Eu is electron capture, and the primary mode for heavier isotopes 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.
As with other lanthanides, many isotopes of europium, especially those that have odd mass numbers or are neutron-poor like. 152Eu, have high cross sections for neutron capture, often high enough to be neutron poisons.
151Eu is the beta decay product of samarium-151, but since this has a long decay half-life and short mean time to neutron absorption, most 151Sm instead ends up as 152Sm.
152Eu (half-life 13.516 years) and 154Eu (half-life 8.593 years) cannot be beta decay products because 152Sm and 154Sm are non-radioactive, but 154Eu is the only long-lived "shielded" nuclide, other than 134Cs, to have a fission yield of more than 2.5 parts per million fissions. A larger amount of 154Eu is produced by neutron activation of a significant portion of the non-radioactive 153Eu; however, much of this is further converted to 155Eu.
155Eu (half-life 4.7612 years) has a fission yield of 330 parts per million (ppm) for uranium-235 and thermal neutrons; most of it is transmuted to non-radioactive and nonabsorptive gadolinium-156 by the end of fuel burnup.
Overall, europium is overshadowed by caesium-137 and strontium-90 as a radiation hazard, and by samarium and others as a neutron poison.
Occurrence
Europium is not found in nature as a free element. Many minerals contain europium, with the most important sources being bastnäsite, monazite, xenotime and loparite-(Ce).
No europium-dominant minerals are known yet, despite a single find of a
tiny possible Eu–O or Eu–O–C system phase in the Moon's regolith.
Depletion or enrichment of europium in minerals relative to other rare-earth elements is known as the europium anomaly. Europium is commonly included in trace element studies in geochemistry and petrology to understand the processes that form igneous rocks (rocks that cooled from magma or lava). The nature of the europium anomaly found helps reconstruct the relationships within a suite of igneous rocks. The average crustal abundance of europium is 2-2.2 ppm.
Divalent europium (Eu2+) in small amounts is the activator of the bright blue fluorescence of some samples of the mineral fluorite (CaF2). The reduction from Eu3+ to Eu2+ is induced by irradiation with energetic particles. The most outstanding examples of this originated around Weardale and adjacent parts of northern England; it was the fluorite found here that fluorescence was named after in 1852, although it was not until much later that europium was determined to be the cause.
In astrophysics, the signature of europium in stellar spectra can be used to classify stars
and inform theories of how or where a particular star was born. For
instance, astronomers recently identified higher-than-expected levels of
europium within the star J1124+4535, hypothesizing that this star originated in a dwarf galaxy that collided with the Milky Way billions of years ago.
Production
Europium is associated with the other rare-earth elements
and is, therefore, mined together with them. Separation of the
rare-earth elements occurs during later processing. Rare-earth elements
are found in the minerals bastnäsite, loparite-(Ce), xenotime, and monazite in mineable quantities. Bastnäsite is a group of related fluorocarbonates, Ln(CO3)(F,OH). Monazite is a group of related of orthophosphate minerals LnPO
4 (Ln denotes a mixture of all the lanthanides except promethium), loparite-(Ce) is an oxide, and xenotime is an orthophosphate (Y,Yb,Er,...)PO4. Monazite also contains thorium and yttrium, which complicates handling because thorium and its decay products are radioactive. For the extraction from the ore and the isolation of individual lanthanides, several methods have been developed. The choice of method is based on the concentration and composition of the ore and on the distribution of the individual lanthanides in the resulting concentrate. Roasting the ore, followed by acidic and basic leaching, is used mostly to produce a concentrate of lanthanides. If cerium is the dominant lanthanide, then it is converted from cerium(III) to cerium(IV) and then precipitated. Further separation by solvent extractions or ion exchange chromatography yields a fraction which is enriched in europium. This fraction is reduced with zinc, zinc/amalgam, electrolysis or other methods converting the europium(III) to europium(II). Europium(II) reacts in a way similar to that of alkaline earth metals and therefore it can be precipitated as a carbonate or co-precipitated with barium sulfate.[35] Europium metal is available through the electrolysis of a mixture of molten EuCl3 and NaCl (or CaCl2) in a graphite cell, which serves as cathode, using graphite as anode. The other product is chlorine gas.
4 (Ln denotes a mixture of all the lanthanides except promethium), loparite-(Ce) is an oxide, and xenotime is an orthophosphate (Y,Yb,Er,...)PO4. Monazite also contains thorium and yttrium, which complicates handling because thorium and its decay products are radioactive. For the extraction from the ore and the isolation of individual lanthanides, several methods have been developed. The choice of method is based on the concentration and composition of the ore and on the distribution of the individual lanthanides in the resulting concentrate. Roasting the ore, followed by acidic and basic leaching, is used mostly to produce a concentrate of lanthanides. If cerium is the dominant lanthanide, then it is converted from cerium(III) to cerium(IV) and then precipitated. Further separation by solvent extractions or ion exchange chromatography yields a fraction which is enriched in europium. This fraction is reduced with zinc, zinc/amalgam, electrolysis or other methods converting the europium(III) to europium(II). Europium(II) reacts in a way similar to that of alkaline earth metals and therefore it can be precipitated as a carbonate or co-precipitated with barium sulfate.[35] Europium metal is available through the electrolysis of a mixture of molten EuCl3 and NaCl (or CaCl2) in a graphite cell, which serves as cathode, using graphite as anode. The other product is chlorine gas.
A few large deposits produce or produced a significant amount of the world production. The Bayan Obo
iron ore deposit contains significant amounts of bastnäsite and
monazite and is, with an estimated 36 million tonnes of rare-earth
element oxides, the largest known deposit.
The mining operations at the Bayan Obo deposit made China the largest
supplier of rare-earth elements in the 1990s. Only 0.2% of the
rare-earth element content is europium. The second large source for
rare-earth elements between 1965 and its closure in the late 1990s was
the Mountain Pass rare earth mine.
The bastnäsite mined there is especially rich in the light rare-earth
elements (La-Gd, Sc, and Y) and contains only 0.1% of europium. Another
large source for rare-earth elements is the loparite found on the Kola
peninsula. It contains besides niobium, tantalum and titanium up to 30%
rare-earth elements and is the largest source for these elements in
Russia.
Compounds
Europium compounds tend to exist trivalent oxidation state under most
conditions. Commonly these compounds feature Eu(III) bound by 6–9
oxygenic ligands, typically water. These compounds, the chlorides,
sulfates, nitrates, are soluble in water or polar organic solvent.
Lipophilic europium complexes often feature acetylacetonate-like
ligands, e.g., Eufod.
Halides
Europium metal reacts with all the halogens:
- 2 Eu + 3 X2 → 2 EuX3 (X = F, Cl, Br, I)
This route gives white europium(III) fluoride (EuF3), yellow europium(III) chloride (EuCl3), gray europium(III) bromide (EuBr3), and colorless europium(III) iodide (EuI3). Europium also forms the corresponding dihalides: yellow-green europium(II) fluoride (EuF2), colorless europium(II) chloride (EuCl2), colorless europium(II) bromide (EuBr2), and green europium(II) iodide (EuI2).
Chalcogenides and pnictides
Europium
forms stable compounds with all of the chalcogens, but the heavier
chalcogens (S, Se, and Te) stabilize the lower oxidation state. Three oxides are known: europium(II) oxide (EuO), europium(III) oxide (Eu2O3), and the mixed-valence oxide Eu3O4, consisting of both Eu(II) and Eu(III).
Otherwise, the main chalcogenides are europium(II) sulfide
(EuS), europium(II) selenide (EuSe) and europium(II) telluride (EuTe):
all three of these are black solids. EuS is prepared by sulfiding the
oxide at temperatures sufficiently high to decompose the Eu2O3:
- Eu2O3 + 3 H2S → 2 EuS + 3 H2O + S
The main nitride is europium(III) nitride (EuN).
History
Although
europium is present in most of the minerals containing the other rare
elements, due to the difficulties in separating the elements it was not
until the late 1800s that the element was isolated. William Crookes observed the phosphorescent spectra of the rare elements including those eventually assigned to europium.
Europium was first found in 1892 by Paul Émile Lecoq de Boisbaudran, who obtained basic fractions from samarium-gadolinium concentrates which had spectral lines not accounted for by samarium or gadolinium. However, the discovery of europium is generally credited to French chemist Eugène-Anatole Demarçay,
who suspected samples of the recently discovered element samarium were
contaminated with an unknown element in 1896 and who was able to isolate
it in 1901; he then named it europium.
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
scramble for the limited supply of europium on hand among the monazite
processors, as the typical europium content in monazite is about 0.05%. However, the Molycorp bastnäsite deposit at the Mountain Pass rare earth mine, California,
whose lanthanides had an unusually high 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 to be in use in the TV industry ever since as
well as 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
he was lecturing on the rare earths in the 1930s, 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 Herbert Newby McCoy, who had developed a famous method of europium purification involving redox chemistry.
Applications
Relative to most other elements, commercial applications for europium
are few and rather specialized. Almost invariably, its phosphorescence
is exploited, either in the +2 or +3 oxidation state.
It is a dopant in some types of glass in lasers and other optoelectronic devices. Europium oxide (Eu2O3) is widely used as a red phosphor in television sets and fluorescent lamps, and as an activator for yttrium-based phosphors. Color TV screens contain between 0.5 and 1 g of europium oxide. Whereas trivalent europium gives red phosphors,
the luminescence of divalent europium depends strongly on the
composition of the host structure. UV to deep red luminescence can be
achieved. The two classes of europium-based phosphor (red and blue), 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 phosphor system is typically encountered in
helical fluorescent light bulbs. Combining the same three classes is one
way to make trichromatic systems in TV and computer screens, but as an additive, it can be particularly effective in improving the intensity of red phosphor. Europium is also used in the manufacture of fluorescent glass, increasing the general efficiency of fluorescent lamps. One of the more common persistent after-glow phosphors besides copper-doped zinc sulfide is europium-doped strontium aluminate.
Europium fluorescence is used to interrogate biomolecular interactions
in drug-discovery screens. It is also used in the anti-counterfeiting
phosphors in euro banknotes.
An application that has almost fallen out of use with the
introduction of affordable superconducting magnets is the use of
europium complexes, such as Eu(fod)3, as shift reagents in NMR spectroscopy. Chiral shift reagents, such as Eu(hfc)3, are still used to determine enantiomeric purity.
A recent (2015) application of europium is in quantum memory
chips which can reliably store information for days at a time; these
could allow sensitive quantum data to be stored to a hard disk-like
device and shipped around.
Precautions
Hazards | |
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GHS pictograms | |
GHS signal word | Danger |
H250 | |
P222, P231, P422 | |
NFPA 704 |
There are no clear indications that europium is particularly toxic compared to other heavy metals. Europium chloride, nitrate and oxide have been tested for toxicity: europium chloride shows an acute intraperitoneal LD50 toxicity of 550 mg/kg and the acute oral LD50 toxicity is 5000 mg/kg. Europium nitrate shows a slightly higher intraperitoneal LD50 toxicity of 320 mg/kg, while the oral toxicity is above 5000 mg/kg. The metal dust presents a fire and explosion hazard.