Beryllium perchlorate

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Beryllium perchlorate
Names
Other names
  • Beryllium diperchlorate
Identifiers
3D model (JSmol)
ChemSpider
UNII
  • InChI=1S/Be.2ClHO4/c;2*2-1(3,4)5/h;2*(H,2,3,4,5)/q+2;;/p-2
    Key: MVTQSBYPNJATTN-UHFFFAOYSA-L
  • tetrahydrate: InChI=1S/Be.2ClHO4.4H2O/c;2*2-1(3,4)5;;;;/h;2*(H,2,3,4,5);4*1H2/q+2;;;;;;/p-2
    Key: TYWIVKBGKVAEHJ-UHFFFAOYSA-L
  • [Be+2].[O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O
  • tetrahydrate: [Be+2].O.O.O.O.[O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O
Properties
Be(ClO4)2
Molar mass 279.975 g/mol
Appearance White solid
Melting point 140 °C (284 °F; 413 K) (decomposition, tetrahydrate)
198 g/100 mL (25 °C, tetrahydrate)
Solubility Soluble in acetone
Structure
Tetrahederal (Be)
Related compounds
Other cations
 Magnesium perchlorate
Calcium perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Beryllium perchlorate is an inorganic chemical compound with the formula Be(ClO4)2·nH2O, where n is 2 or 4. All forms are white, hygroscopic, and water-soluble solids.

Synthesis and reactions

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Beryllium perchlorate tetrahydrate, Be(ClO4)2·4H2O, is produced from the reaction of beryllium oxide and concentrated perchloric acid followed by the evaporation of the solution:[1][2][3]

BeO + 2 HClO4 → Be(ClO4)2 + H2O

The dihydrate can be similarly prepared by the reaction of beryllium chloride and hydronium perchlorate at 60 °C.[4]

Heating of the tetrahydrate does not produce the anhydrous form; it instead decomposes at 140 °C, producing an unidentified basic beryllium perchlorate, and if this compound is heated to 260 °C, it decomposes to beryllium oxide. Similarly, if the dihydrate is heated to 200 °C, it decomposes to basic beryllium perchlorate (Be4O(ClO4)6), which then decomposes at 270 °C to BeO.[5]

The tetrahydrate and dihydrate dissolves in water to form the [Be(H2O)4]2+ ion, which then partially hydrolyzes to the trimeric ion [Be3(OH)3(H2O)6]3+. They also dissolve in acetone which then can react with triphenylphosphine oxide to form Be(OPPh3)4(ClO4)2.[3][6]

Structure

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The structure of the dihydrate, which was probed by IR spectroscopy, consists of discreet [Be(H2O)4]2+ and [Be(ClO4)4]2– ions.[4]

References

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  1. ^ J. Marignac, Ann. Chim., 4, 45 (1873)
  2. ^ Ohtaki, Hitoshi (1967). "Ionic equilibriums in mixed solvents. I. Hydrolysis of beryllium ion in a 0.2 mole fraction dioxane-water mixture containing 3M lithium chlorate as an ionic medium". Inorganic Chemistry. 6 (4): 808–813. doi:10.1021/ic50050a033. ISSN 0020-1669. Retrieved 2025-05-21.
  3. ^ a b Kakihana, Hidetake; Maeda, Masunobu (1970-01-01). "The Hydrolysis of the Beryllium Ion in Heavy Water". Bulletin of the Chemical Society of Japan. 43 (1): 109–113. doi:10.1246/bcsj.43.109. ISSN 0009-2673.
  4. ^ a b L. B. Serezhkina; Z. L. Grigorovich; V. H. Serezhkin; N. S. Tamm; A. V. Novoselova (1973). "Beryllium perchlorate dihydrate". Dokl. Akad. Nauk SSSR. 211 (3): 552–553.
  5. ^ L. G. Berezkina; S. L. Borisova; N. S. Tamm; A. V. Novoselova (1975). "Thermal decomposition of beryllium perchlorate tetrahydrate". Dokl. Akad. Nauk SSSR. 225 (3): 571–573.
  6. ^ Cecconi, Franco; A. Ghilardi, Carlo; Midollini, Stefano; Orlandini, Annabella (2000). "Beryllium complexes with mono- and tripodal- phosphinoxide ligands. X-ray crystal structure of [{N(CH2PPh2O)3}Be(OH2)](ClO4)2". Inorganic Chemistry Communications. 3 (7): 350–353. doi:10.1016/S1387-7003(00)00092-7. Retrieved 2025-05-21.