Beryllium carbonate

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Beryllium carbonate
Identifiers
3D model (JSmol)
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 Toxic (T)

Irritant (Xi)
Dangerous for the environment (N)

Toxic TIrritant XiDangerous for the Environment (Nature) N
NFPA 704
Flammability code 0: Will not burn. E.g., waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
3
0
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 ☑Y☒N ?)
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. Toxic. It should be handled carefully since several related beryllium compounds are known carcinogens.

Natural occurrence[edit]

No purely beryllic carbonate is known to occur naturally. The only Be-rich carbonate mineral currently known is niveolanite.[6]

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
  6. ^ https://www.mindat.org/min-32289.html


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 Ce2(CO3)3 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
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