Beryllium carbonate
| Identifiers | |
|---|---|
13106-47-3  |
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| ChemSpider | 55490  |
| Jmol 3D model | Interactive image |
| PubChem | 61577 |
| RTECS number | DS2350000 |
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| Properties | |
| BeCO3 | |
| Melting point | 54 °C (129 °F; 327 K) |
| Boiling point | 100 °C (212 °F; 373 K) decomposes |
| 0.36 g/100 mL | |
| Thermochemistry | |
| 65 J/mol·K[1] | |
|
Std molar
entropy (S |
52 J/mol·K[1] |
|
Std enthalpy of
formation (ΔfH |
-1025 kJ/mol[1] |
|
Gibbs free energy (ΔfG˚)
|
-948 kJ/mol[1] |
| Vapor pressure | {{{value}}} |
|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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 verify (what is ?) |
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| Infobox references | |
Beryllium carbonate is a chemical compound with the chemical formula BeCO3.
Contents
Structures
There are three forms reported, anhydrous, a tetrahydrate and basic beryllium carbonate. The anhydrous form is reported to be unstable, decomposing to BeO and carbon dioxide, and requiring storage under CO2.[2] The tetrahydrate is said to be formed when CO2 is bubbled through a solution of Be(OH)2 and is also reported to be similarly unstable.[3]
Preparation
Basic beryllium carbonate is a mixed salt, which can be prepared by the reaction of beryllium sulfate and ammonium carbonate, and contains both carbonate and hydroxide ions, with formula Be2CO3(OH)2.[4] It is believed that in the older literature this is probably what was referred to as beryllium carbonate.[4]
Safety
It may cause irritation. It should be handled carefully since several related beryllium compounds are known carcinogens.
References
- ↑ 1.0 1.1 1.2 1.3 http://chemister.ru/Database/properties-en.php?dbid=1&id=4246
- ↑ Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
- ↑ David Anthony Everest, 1964, The Chemistry of Beryllium, Elsevier Pub. Co.
- ↑ 4.0 4.1 J.E. Macintyre, Dictionary of Inorganic Compounds 1992 CRC Press ISBN 0-412-30120-2
| H2CO3 | He | ||||||||||||||||
| Li2CO3 | BeCO3 | B | C | (NH4)2CO3, NH4HCO3 |
O | F | Ne | ||||||||||
| Na2CO3, NaHCO3, Na3H(CO3)2 |
MgCO3, Mg(HCO3)2 |
Al2(CO3)3 | Si | P | S | Cl | Ar | ||||||||||
| K2CO3, KHCO3 |
CaCO3, Ca(HCO3)2 |
Sc | Ti | V | Cr | MnCO3 | FeCO3 | CoCO3 | NiCO3 | CuCO3 | ZnCO3 | Ga | Ge | As | Se | Br | Kr |
| Rb2CO3 | SrCO3 | Y | Zr | Nb | Mo | Tc | Ru | Rh | Pd | Ag2CO3 | CdCO3 | In | Sn | Sb | Te | I | Xe |
| Cs2CO3, CsHCO3 |
BaCO3 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg | Tl2CO3 | PbCO3 | (BiO)2CO3 | Po | At | Rn | |
| Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Uut | Fl | Uup | Lv | Uus | Uuo | |
| ↓ | |||||||||||||||||
| La2(CO3)3 | Ce | Pr | Nd | Pm | Sm | Eu | Gd | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||
| Ac | Th | Pa | UO2CO3 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||
