Jump to content

Europium(III) acetate

From Wikipedia, the free encyclopedia
Europium(III) acetate
Names
Other names
Europium acetate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.013.337 Edit this at Wikidata
EC Number
  • 214-670-9
  • InChI=1S/3C2H4O2.Eu/c3*1-2(3)4;/h3*1H3,(H,3,4);/q;;;+3/p-3
    Key: LNYNHRRKSYMFHF-UHFFFAOYSA-K
  • CC(=O)[O-].CC(=O)[O-].CC(=O)[O-].[Eu+3]
Properties
Eu(CH3COO)3
Molar mass 329,092 g/mol (anhydrous) 341,059 g/mol (monohydrate)
Appearance white solid
soluble in water
Related compounds
Other anions
 Europium(III) oxide
Europium(III) hydroxide
Europium(III) carbonate
Other cations
 Samarium(III) acetate
Gadolinium(III) acetate
Related compounds
 Europium(II) acetate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Europium(III) acetate is an inorganic salt of europium and acetic acid with the chemical formula of Eu(CH3COO)3. In this compound, europium exhibits the +3 oxidation state. It can exist in the anhydrous form, sesquihydrate[a][1] and tetrahydrate.[2] Its hydrate molecule is a dimer.[3][4]

Preparation

[edit]

Europium acetate can be obtained by stirring reaction of acetic acid and europium oxide under heating, and then diluting with water and crystallizing:[5]

Eu2O3 + 6 CH3COOH → 2 Eu(CH3COO)3 + 3 H2O

Europium can also directly participate in the reaction:[1]

2 Eu + 6 CH3COOH → 2 Eu(CH3COO)3 + 3 H2↑

Properties

[edit]

Physical properties

[edit]
Structure of europium acetate

The anhydrous europium acetate crystallizes monoclinically in the space group C2/c (space group no. 15) with the lattice parameters a = 1126.0(3), b = 2900.5(6), c = 799.1( 2) pm and β = 132.03(2)° with four formula units per unit cell.[1] The sesquihydrate crystallizes monoclinically in the space group Cc (No. 9) with the lattice parameters a = 1608.7(2), b = 1665.6(2), c = 839.1(1) pm and β = 115.75( 9)° with four formula units per unit cell.[1] The heat capacity at 280 K is 803±16 J/(mol∙K).[6]

Chemical properties

[edit]

Europium acetate can be dissolved in water, acidified with acetic acid, and the compound of divalent europium [Eu(CH3COO)2(CH3COOH)(H2O)2] can be obtained by electrochemical reduction.[7]

Europium acetate can be crystallized in excess glacial acetic acid to give the salt [Eu(H(CH3COO)2)3](H2O).[1]

Decomposition

[edit]

Europium acetate can be decomposed by heating, and the hydrate first loses water to obtain anhydrous, and then passes through basic acetate EuOCH3COO, basic carbonate Eu2O2CO3, and finally obtains europium oxide.[8] The tetrahydrate of europium acetate decomposes in air over 6 stages to europium oxide.[8][9]

Stage 1 at 135 °C:

Eu(CH3COO)3·4H2O → Eu(CH3COO)3·H2O + 3H2O

Stage 2 at 170 °C:

Eu(CH3COO)3·3H2O → Eu(CH3COO)3·0.5 H2O + 0.5 H2O

Stage 3 at 210 °C:

Eu(CH3COO)3·0.5H2O → Eu(CH3COO)3 + 0.5 H2O

Stage 4 at 310 °C:

Eu(CH3COO)3 → EuO(CH3COO) + C3H6O + CO2

Stage 5 at 390 °C:

2EuO(CH3COO) → Eu2O2[CO3] + C3H6O

Stage 6 at 670 °C:

Eu2O2[CO3] → Eu2O3 + CO2

Notes

[edit]
  1. ^ Note: The sesquihydrate of europium(III) acetate has the structure [Eu2(CH3COO)6(H2O)](H2O)2.

References

[edit]
  1. ^ a b c d e Sonia Gomez Torres, Ingo Pantenburg, Gerd Meyer (2006). "Direct Oxidation of Europium Metal with Acetic Acid: Anhydrous Europium(III) Acetate, Eu(OAc)3, its Sesqui-hydrate, Eu(OAc)3(H2O)1.5, and the "Hydrogendiacetate", [Eu(H(OAc)2)3](H2O)". Zeitschrift für anorganische und allgemeine Chemie. 632 (12–13): 1989–1994. doi:10.1002/zaac.200600154. ISSN 1521-3749. Retrieved 2019-02-01.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  2. ^ Herbert N. McCoy (1939-09-01). "The Salts of Europium". Journal of the American Chemical Society. 61 (9): 2455–2456. Bibcode:1939JAChS..61.2455M. doi:10.1021/ja01878a055. ISSN 0002-7863. Retrieved 2019-02-01.
  3. ^ P. Starynowicz (1995-12-01). "Structure and spectroscopy of diaqua(μ3-acetato)(acetato-O)(acetic acid-O)europium(II), [Eu(OAc)2(AcOH)(H2O)2]". Polyhedron. 14 (23): 3573–3577. doi:10.1016/0277-5387(95)00174-Q. ISSN 0277-5387. Retrieved 2019-02-01.
  4. ^ Cameron J. Kepert, Lu Wei-Min, Peter C. Junk, Brian W. Skelton, Allan H. White (1999). "Structural Systematics of Rare Earth Complexes. X ('Maximally') Hydrated Rare Earth Acetates". Australian Journal of Chemistry. 52 (6): 437. doi:10.1071/CH98041. ISSN 0004-9425. Retrieved 2020-01-18.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  5. ^ Tang, Huian; Liu, Yanzhi; Zhao, Aiping. A preparation method of europium acetate [Patent]. CN104387254A. 2015.
  6. ^ Dobrokhotova, Zh. V.; Fomina, I. G.; Kiskin, M. A.; Bykov, M. A.; Belov, G. V.; Novotortsev, V. M. (2006), "The thermodynamic properties of rare-earth metal binuclear acetates and pivalates", Russian Journal of Physical Chemistry (in German), vol. 80, no. 3, pp. 323-329, Bibcode:2006RJPCA..80..323D, doi:10.1134/S0036024406030034, ISSN 0036-0244, S2CID 97590163{{citation}}: CS1 maint: multiple names: authors list (link)
  7. ^ P. Starynowicz (1995-12-01). "Structure and spectroscopy of diaqua(μ3-acetato)(acetato-O)(acetic acid-O)europium(II), [Eu(OAc)2(AcOH)(H2O)2]". Polyhedron. 14 (23): 3573–3577. doi:10.1016/0277-5387(95)00174-Q. ISSN 0277-5387. Retrieved 2019-02-01.
  8. ^ a b Ogawa M, Manabe K. Thermal Decomposition of Europium (III) Acetate Tetrahydrate Archived 2019-02-01 at the Wayback Machine（酢酸ユウロピウム(III)4水和物の熱分解）. Journal of the Ceramic Society of Japan, 1988, 96(1117): 890-893.
  9. ^ Balboul, Basma A. A.; Zaki, Mohamed I (2011), "Thermal decomposition course of Eu(CH3COO)3·4H2O and the reactivity at the gas/solid interface thus established", Journal of Analytical and Applied Pyrolysis (in German), vol. 92, no. 1, pp. 137-142, doi:10.1016/j.jaap.2011.05.004{{citation}}: CS1 maint: multiple names: authors list (link)
Retrieved from "https://en.wikipedia.org/w/index.php?title=Europium(III)_acetate&oldid=1264702187"