Eu2O3 Europium oxide

Europium oxide (EU2O3) nanorods have been prepared by the sonication of an aqueous solution of europium nitrate in the presence of ammonia. In this reaction, ammonium ions adsorbed on the Eu(OH)3 particles (formed due to the collapse of the bubbles) results in the formation of a monolayer which then fuse together by hydrogen bonding leading to the formation of nanorods [28]. 

Europium oxide interacts with stainless steel (grain boundary attack) above 500°C, to form europium silicate. No interaction occurs even at 1230°C when the silicon content of the steel is less than 58 ppm. Molybdenum or tungsten could be used as protective barriers, since these metals do not react with EU2O3 at elevated temperatures. ... 

In a similar work, ultrasound radiation was used to prepare EU2O3 doped in zir-conia and yttrium-stabilized zirconium (YSZ) nanoparticles [83]. Europium oxide was also coated sonochemically on the surface of submicron spherical zirconia and YSZ, which were fabricated by wet chemical methods. Time decay measurements of the doped and coated materials were conducted using a pulsed laser source. Lifetimes < 1.1 ms radiative lifetime of the Eu+ ions were detected for the doped and coated as-prepared materials. When the doped and coated samples were an-... 

EU2O3 Europium (III) oxide, 2 66 EuaHga Europium amalgam,... 

Several authors have obtained a yellowish product during the reduction of EU2O3 in silica tubes. This yellowish product is more likely to be europium silicate (see below) than a new form of oxide. 

Reduction of EU2O3 with lanthanum or europium, as well as carbon, affords the stablest M oxide ... 

EuO. — This lower oxide of europium was prepared by the reduction of EU2O3 with lanthanum metal at 1300 — 1500° C by Eick et al. [319]. EuO has a NaCl type structure with a = 5.1439 0.0005 A. Garton and Hukin [320] attempted the preparation of EuO by controlled oxidation of europium metal at 350° C with a stoichiometric addition of oxygen and obtained the oxide in fairly pure state. They also tried the thermal decomposition of EuCOs, Eu(HCOO)2 and Eu(0H)2. Only Eu(OH)2 proved to be advantegeous and gave a sample of EuO of reasonable purity. 

The decomposition of europium oxalate [82] occurred at a significantly lower temperature (520 K). Results were interpreted as indicating cation reduction to the divalent state. In vacuum, the products of decomposition were europium(II) carbonate and finely-divided carbon. In carbon dioxide at 593 K, europium(II) oxalate is stabilized. In an oxidizing atmosphere, europium is reoxidised and EU2O3 is formed at 663 K. A reaction mechanism was proposed in which carbon monoxide reacted with the oxalate ion to form carbon dioxide and 203. The reactions of ytterbium oxalate were similar. 

Precipitation as EUSO4 is the final step of separation. Calcination forms the oxide, the usual commercial form of europium, i.e.- EU2O3. 

Europium(III) oxide EU2O3 +10100 Iridium(III) chloride IrCl3 -14.4... 

In contrast, the divalent state is stabilized by the low electronegativity of the anions, with increasing stability as the anion electronegativity decreases. For instance, in the case of europium, for which the normal oxide is EU2O3, the corresponding EU2S3 sulfide does not exist. The normal sulfide is Eu(II)S, which is easily obtained by action of H2S on trivalent europium compounds (oxide, carbonate, etc). However the trivalence of europium is manifest in some chalcogenides, which may all be considered as ternary or quaternary compounds. 

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