Beryllium bromide
From Infogalactic: the planetary knowledge core
 |
|
| Names | |
|---|---|
| IUPAC name
Beryllium bromide
|
|
| Identifiers | |
7787-46-4  |
|
| ChemSpider | 74208  |
| Jmol 3D model | Interactive image |
| PubChem | 82230 |
|
|
|
|
| Properties | |
| BeBr2 | |
| 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 | |
| 0.4111 J/g K | |
|
Std molar
entropy (S |
9.5395 J/K |
|
Std enthalpy of
formation (ΔfH |
-2.094 kJ/g |
| Vapor pressure | {{{value}}} |
| 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).
|
|
 verify (what is ?) |
|
| Infobox references | |
Beryllium bromide is the chemical compound with the formula BeBr2. It is very hygroscopic and dissolves well in water. The compound is a polymer with tetrahedral Be centres.[2]
Preparation and reactions
It can be prepared by reacting beryllium metal with elemental bromine at temperatures of 500 °C to 700 °C:[1]
- Be + Br2 → BeBr2
Beryllium bromide is also formed when treating beryllium oxide with hydrobromic acid:
- BeO + 2 HBr → BeBr2 + H2O
It hydrolizes slowly in water: BeBr2 + 2 H2O → 2 HBr + Be(OH)2
Safety
Beryllium compounds are toxic if inhaled or ingested.
References
- ↑ 1.0 1.1 1.2 Lua error in package.lua at line 80: module 'strict' not found.
- ↑ Crystal modifications of Beryllium dihalides BeCl2, BeBr2, and BeI2 Troyanov, S. I. Zhurnal Neorganicheskoi Khimii (2000), 45(10), 1619-1624.
<templatestyles src="Asbox/styles.css"></templatestyles>
 |
This inorganic compound–related article is a stub. You can help Wikipedia by expanding it. |
