Beryllium sulfate
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.033.478 Edit this at Wikidata
EC Number
  • 236-842-2
RTECS number
  • DS4800000
UNII
  • InChI=1S/Be.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 checkY
    Key: KQHXBDOEECKORE-UHFFFAOYSA-L checkY
  • InChI=1/Be.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2
    Key: KQHXBDOEECKORE-NUQVWONBAA
  • [Be+2].[O-]S([O-])(=O)=O
Properties[1]
BeSO4
Molar mass 105.075 g/mol (anhydrous)
177.136 g/mol (tetrahydrate)
Appearance white solid
Odor odorless
Density 2.44 g/cm3 (anhydrous)
1.71 g/cm3 (tetrahydrate)
Melting point 110 °C (230 °F; 383 K) (tetrahydrate, −2H2O)
400 °C (dihydrate, dehydr.)
550–600 decomposes
Boiling point 2,500 °C (4,530 °F; 2,770 K) (anhydrate)
580 °C (tetrahydrate)
36.2 g/100 mL (0 °C)
40.0 g/100 mL (20 °C)
54.3 g/100 mL (60 °C)
Solubility insoluble in alcohol
1.4374 (tetrahydrate)
Thermochemistry
90 J/mol K
-1197 kJ/mol
-1088 kJ/mol
Hazards
GHS labelling:
Acute Tox. 2 Carc. 1B Aquatic Chronic 2
Danger
H301, H315, H317, H319, H330, H335, H350, H372, H411
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
82 mg/kg (rat, oral)
80 mg/kg (mouse, oral)[3]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 0.002 mg/m3
C 0.005 mg/m3 (30 minutes), with a maximum peak of 0.025 mg/m3 (as Be)[2]
REL (Recommended)
 Ca C 0.0005 mg/m3 (as Be)[2]
IDLH (Immediate danger)
 Ca [4 mg/m3 (as Be)][2]
Safety data sheet (SDS) ICSC 1351
Related compounds
Other cations
 Magnesium sulfate
Calcium sulfate
Strontium sulfate
Barium sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Beryllium sulfate normally encountered as the tetrahydrate, [Be(H2O)4]SO4 is a white crystalline solid. It was first isolated in 1815 by Jons Jakob Berzelius.[4] Beryllium sulfate may be prepared by treating an aqueous solution of many beryllium salts with sulfuric acid, followed by evaporation of the solution and crystallization. The hydrated product may be converted to anhydrous salt by heating at 400 °C.[5]

Structure

According to X-ray crystallography the tetrahydrate contains a tetrahedral Be(OH2)42+ unit and sulfate anions. The small size of the Be2+ cation determines the number of water molecules that can be coordinated.[6] In contrast, the analogous magnesium salt, MgSO4·6H2O contains an octahedral Mg(OH2)62+ unit.[7] The existence of the tetrahedral [Be(OH2)4]2+ ion in aqueous solutions of beryllium nitrate and beryllium chloride has been confirmed by vibrational spectroscopy, as indicated by the totally symmetric BeO4 mode attt 531 cm−1. This band is absent in beryllium sulfate, and the sulfate modes are perturbed. The data support the existence of Be(OH2)3OSO3.[8]

The anhydrous compound has a structure similar to that of boron phosphate. The structure contains alternating tetrahedrally coordinated Be and S and each oxygen is 2 coordinate (Be-O-S). The Be-O distance is 156 pm and the S-O distance is 150 pm.[9]

A mixture of beryllium and radium sulfate was used as the neutron source in the discovery of nuclear fission.

References

  1. ^ Weast, Robert C., ed. (1981). CRC Handbook of Chemistry and Physics (62nd ed.). Boca Raton, FL: CRC Press. p. B-82. ISBN 0-8493-0462-8..
  2. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0054". National Institute for Occupational Safety and Health (NIOSH).
  3. ^ "Beryllium compounds (as Be)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  4. ^ Lathrop Parsons, Charles (1909), The Chemistry and Literature of Beryllium, London, pp. 29–33, ISBN 9780559264160((citation)): CS1 maint: location missing publisher (link).
  5. ^ Patnaik, Pradyot (2002), Handbook of Inorganic Chemicals, McGraw-Hill, ISBN 0-07-049439-8.
  6. ^ Kellersohn, T.; Delaplane, R. G.; Olovsson, I. (1994). "The synergetic effect in beryllium sulfate tetrahydrate – an experimental electron-density study". Acta Crystallographica Section B: Structural Science. 50 (3): 316–326. doi:10.1107/S010876819400039X.
  7. ^ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
  8. ^ Rudolph, Wolfram W.; Fischer, Dieter; Irmer, Gert; Pye, Cory C. (2009). "Hydration of Beryllium(II) in Aqueous Solutions of Common Inorganic Salts. A Combined Vibrational Spectroscopic and ab initio Molecular Orbital Study". Dalton Transactions (33): 6513–6527. doi:10.1039/B902481F. PMID 19672497.
  9. ^ Grund, Alfred (1955). "Die Kristallstruktur von BeSO4". Tschermaks Mineralogische und Petrographische Mitteilungen. 5 (3): 227–230. Bibcode:1955MinPe...5..227G. doi:10.1007/BF01191066. ISSN 0041-3763.

External links

Beryllium compounds
Compounds containing the sulfate group (SO2−4)
Authority control databases: National
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