Chemistry:Radium carbonate
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| Names | |||
|---|---|---|---|
| IUPAC name
Radium carbonate
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| Identifiers | |||
3D model (JSmol)
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| Properties | |||
| RaCO 3[2] | |||
| Molar mass | 286.0089 g/mol[3] | ||
| Appearance | white powder[2] | ||
| 0.05 g/L (25 °C)[4] | |||
Solubility product (Ksp)
|
10−7.5±0.1 (25 °C)[4] | ||
| Hazards | |||
| Main hazards | radioactive | ||
| Related compounds | |||
Other cations
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |||
| Infobox references | |||
Radium carbonate is a chemical compound of radium, carbon, and oxygen, having the chemical formula RaCO
3. It is the radium salt of carbonic acid. It contains radium cations (Ra2+) and carbonate anions (CO2−
3). This salt is a highly radioactive, amorphous,[4] white powder that has potential applications in medicine.[5][2] It is notable for forming disordered crystals at room temperature and for being approximately 10 times more soluble than its lighter congener barium carbonate.[4] Radium carbonate is one of a few radium compounds which has significantly different properties from corresponding barium compounds. Moreover, radium is the only alkaline-earth metal which forms disordered crystals in its carbonate phase. Even though radium carbonate has very low solubility in water, it is soluble in dilute mineral acids and concentrated ammonium carbonate.[6]
Preparation
Radium carbonate can be produced by dissolving radium sulfate at elevated temperatures in concentrated sodium carbonate and subsequent removal of supernatant:[7]
- RaSO
4(s) → Ra2+ + SO2−
4 - Ra2+ + CO2−
3 → RaCO
3(s)
Because of the very low solubility of RaCO
3, it will form a white precipitate.
Reactions
Radium carbonate can be used to produce radium nitrate and other radium salts:
- RaCO
3 + 2 HNO
3 → Ra(NO
3)
2 + H
2O + CO
2
References
- ↑ "Radium carbonate - Hazardous Agents | Haz-Map". https://haz-map.com/Agents/1813?referer=BrowseByAlphabet&return_url=%2FAgents%2F(BrowseByAlphabet)%2FR.
- ↑ 2.0 2.1 2.2 "Radium carbonate | Article about radium carbonate by The Free Dictionary". https://encyclopedia2.thefreedictionary.com/radium+carbonate.Template:Reliable?
- ↑ "RADIUM CARBONATE - (7116-98-5) - Physical Properties • Chemical Properties • Solubility • Uses/Function • Reactions • Thermochemistry". http://chemistry-reference.com/q_compounds.asp?CAS=7116-98-5&language=en.
- ↑ 4.0 4.1 4.2 4.3 Matyskin, Artem V.; Ebin, Burçak; Allard, Stefan; Torapava, Natallia; Eriksson, Lars; Persson, Ingmar; Brown, Paul L.; Ekberg, Christian (July 21, 2023). "Disordered Crystal Structure and Anomalously High Solubility of Radium Carbonate". Inorganic Chemistry 62 (30): 12038–12049. doi:10.1021/acs.inorgchem.3c01513. PMID 37477287.
- ↑ Westrøm, Sara; Malenge, Marion; Jorstad, Ida Sofie; Napoli, Elisa; Bruland, Øyvind S.; Bønsdorff, Tina B.; Larsen, Roy H. (17 January 2018). "Ra-224 labeling of calcium carbonate microparticles for internal α-therapy: Preparation, stability, and biodistribution in mice". Journal of Labelled Compounds and Radiopharmaceuticals 61 (6): 472–486. doi:10.1002/jlcr.3610. PMID 29380410.
- ↑ Salutsky, M.; Kirby, H. (1964). The Radiochemistry of Radium. doi:10.2172/4560824. https://www.osti.gov/servlets/purl/4560824/. Retrieved 2021-01-08.
- ↑ Matyskin, Artem V.; Ebin, Burçak; Tyumentsev, Mikhail; Allard, Stefan; Skarnemark, Gunnar; Ramebäck, Henrik; Ekberg, Christian (5 July 2016). "Disassembly of old radium sources and conversion of radium sulfate into radium carbonate for subsequent dissolution in acid". Journal of Radioanalytical and Nuclear Chemistry 310 (2): 589–595. doi:10.1007/s10967-016-4927-x. Bibcode: 2016JRNC..310..589M. https://link.springer.com/article/10.1007/s10967-016-4927-x.
| 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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