Beryllium carbonate

From Wikipedia, the free encyclopedia
Jump to: navigation, search
Beryllium carbonate
Identifiers
3D model (Jmol)
ChemSpider
ECHA InfoCard 100.032.740
RTECS number DS2350000
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]
52 J/mol·K[1]
-1025 kJ/mol[1]
-948 kJ/mol[1]
Hazards
Main hazards Irritant (Xi)
Lethal dose or concentration (LD, LC):
150 mg/kg (guinea pig)
US health exposure limits (NIOSH):
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]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
Infobox references

Beryllium carbonate is a chemical compound with the chemical formula BeCO3.

Structures[edit]

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.[3] 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.[4]

Preparation[edit]

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.[5] It is believed that in the older literature this is probably what was referred to as beryllium carbonate.[5]

Safety[edit]

It may cause irritation. It should be handled carefully since several related beryllium compounds are known carcinogens.

References[edit]

  1. ^ a b c d http://chemister.ru/Database/properties-en.php?dbid=1&id=4246
  2. ^ a b c "NIOSH Pocket Guide to Chemical Hazards #0054". National Institute for Occupational Safety and Health (NIOSH). 
  3. ^ Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
  4. ^ David Anthony Everest, 1964, The Chemistry of Beryllium, Elsevier Pub. Co.
  5. ^ a b J.E. Macintyre, Dictionary of Inorganic Compounds 1992 CRC Press ISBN 0-412-30120-2


Carbonates
H2CO3 He
Li2CO3,
LiHCO3
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 Nh Fl Mc Lv Ts Og
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