![]() | |
![]() | |
![]() | |
Names | |
---|---|
IUPAC name Beryllium bromide | |
Identifiers | |
3D model (JSmol) | |
ChemSpider | |
ECHA InfoCard | 100.029.196 |
EC Number |
|
PubChem CID | |
UNII | |
CompTox Dashboard (EPA) | |
| |
| |
Properties | |
Be Br2 | |
Molar mass | 168.820 g/mol |
Appearance | colorless white crystals |
Density | 3.465 g/cm3 (20 °C) |
Melting point | 508 °C (946 °F; 781 K)sublimes at 473 °C (883 °F; 746 K) |
Boiling point | 520 °C (968 °F; 793 K) [1] |
Highly [1] | |
Solubility | soluble in ethanol, diethyl ether, pyridine insoluble in benzene |
Structure | |
Orthorhombic | |
Thermochemistry | |
Heat capacity (C) | 0.4111 J/g K |
Std molar entropy (S⦵298) | 9.5395 J/K |
Std enthalpy of formation (ΔfH⦵298) | −2.094 kJ/g |
Hazards | |
Occupational safety and health (OHS/OSH): | |
Main hazards | see Berylliosis |
GHS labelling: | |
![]() ![]() ![]() | |
Danger | |
H301, H315, H317, H319, H330, H335, H350i, H372, H411 | |
P260, P301+P310, P304+P340, P305+P351+P338, P320, P330, P405, P501 | |
NFPA 704 (fire diamond) | |
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] |
Related compounds | |
Other anions | Beryllium fluoride Beryllium chloride Beryllium iodide |
Other cations | Magnesium bromide Calcium bromide Strontium bromide Barium bromide Radium bromide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). |
Beryllium bromide is the chemical compound with the formula BeBr2. It is very hygroscopic and dissolves well in water. The Be2+ cation, which is relevant to BeBr2, is characterized by the highest known charge density (Z/r = 6.45), making it one of the hardest cations and a very strong Lewis acid. [3]
It can be prepared by reacting beryllium metal with elemental bromine at temperatures of 500 °C to 700 °C: [1]
When the oxidation is conducted on an ether suspension, one obtains colorless dietherate: [4]
The same dietherate is obtained by suspending beryllium dibromide in diethyl ether: [5]
This ether ligand can be displaced by other Lewis bases.is ether ligand can be displaced by other Lewis bases.
Beryllium bromide hydrolyzes slowly in water: BeBr2 + 2 H2O → 2 HBr + Be(OH)2
Two forms (polymorphs) of BeBr2 are known. Both structures consist of tetrahedral Be2+ centers interconnected by doubly bridging bromide ligands. One form consist of edge-sharing polytetrahedra. The other form resembles zinc iodide with interconnected adamantane-like cages. [6] [7]
Beryllium compounds are toxic if inhaled or ingested.