Beryllium nitrate
| Names | |
|---|---|
| Systematic IUPAC name
Beryllium nitrate | |
| Other names
Beryllium dinitrate
| |
| Identifiers | |
| |
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.033.678 |
| EC Number |
|
PubChem CID
|
|
| UNII |
|
| UN number | 2464 |
CompTox Dashboard (EPA)
|
|
| |
| |
| Properties | |
| Be(NO3)2 | |
| Molar mass | 133.021982 g/mol |
| Appearance | white solid |
| Odor | odorless |
| Density | 1.56 g/cm3 |
| Melting point | 60.5 °C (140.9 °F; 333.6 K) |
| Boiling point | 142 °C (288 °F; 415 K) (decomposes) |
| 166 g/100 mL | |
| Thermochemistry | |
Std enthalpy of
formation (ΔfH⦵298) |
-700.4 kJ/mol |
| Hazards | |
| 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)[1] |
REL (Recommended)
|
Ca C 0.0005 mg/m3 (as Be)[1] |
IDLH (Immediate danger)
|
Ca [4 mg/m3 (as Be)][1] |
| Related compounds | |
Other cations
|
Magnesium nitrate Calcium nitrate Strontium nitrate Barium nitrate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Beryllium nitrate is an inorganic compound with the idealized chemical formula Be(NO3)2. The formula suggests a salt, but, as for many beryllium compounds, the compound is highly covalent. Little of its chemistry is well known. "When added to water, brown fumes are evolved; when hydrolyzed in sodium hydroxide solution, both nitrate and nitrite ions are produced."[2]
6_ICD_Code59272.png)
Synthesis and reactions
[edit]The straw-colored adduct Be(NO3)2(N2O4) forms upon treatment of beryllium chloride with dinitrogen tetroxide:
- BeCl2 + 3 N2O4 → Be(NO3)2(N2O4) + 2 NOCl
Upon heating, this adduct loses N2O4 and produces colorless Be(NO3)2. Further heating of Be(NO3)2 induces conversion to basic beryllium nitrate, which adopts a structure akin to that for basic beryllium acetate.[4]
Unlike the basic acetate, with its six lipophilic methyl groups, the basic nitrate is insoluble in most solvents.
References
[edit]- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0054". National Institute for Occupational Safety and Health (NIOSH).
- ^ Addison, C.C.; Logan, N. (1964). Anhydrous Metal Nitrates. Advances in Inorganic Chemistry and Radiochemistry. Vol. 6. pp. 71–142. doi:10.1016/S0065-2792(08)60225-3. ISBN 9780120236060.
- ^ Haley, M. J.; Wallwork, S. C.; Duffin, B.; Logan, N.; Addison, C. C. (1997). "Hexa-μ-nitrato-μ4-oxo-tetraberyllium". Acta Crystallographica Section C Crystal Structure Communications. 53 (7): 829–830. doi:10.1107/S010827019700303X.
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 122. ISBN 978-0-08-037941-8.
 | This inorganic compound–related article is a stub. You can help Wikipedia by expanding it. |