Lithium carbonate
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| Names | |
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| IUPAC name
Lithium carbonate
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| Other names
Dilithium carbonate, Carbolith, Cibalith-S, Duralith, Eskalith, Lithane, Lithizine, Lithobid, Lithonate, Lithotabs Priadel, Zabuyelite
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.008.239 |
| KEGG | |
PubChem CID
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| RTECS number |
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| UNII | |
CompTox Dashboard (EPA)
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| Properties | |
| Li2CO3 | |
| Molar mass | 73.891 g/mol |
| Appearance | Odorless white powder |
| Density | 2.11 g/cm3 |
| Melting point | 723 °C |
| Boiling point | 1310 °C decomp. |
| 15.4 g/L (0 °C) 13.2 g/L (20 °C) 7.2 g/L (100 °C) | |
| Solubility | insoluble in acetone and ethanol |
Refractive index (nD)
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1.428 [1] |
| Thermochemistry | |
Heat capacity (C)
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1.341 J/(g·K) |
Std enthalpy of
formation (ΔfH⦵298) |
-16.46 kJ/g |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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irritant |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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525 mg/kg |
| Related compounds | |
Other cations
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Sodium carbonate Potassium carbonate Rubidium carbonate Caesium carbonate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Lithium carbonate is a chemical compound of lithium, carbon, and oxygen with the formula Li2CO3. This colorless salt is widely used in the processing of metal oxides and has received attention for its use in psychiatry. It is found in nature as the rare mineral zabuyelite.[2]
Properties
Like almost all other lithium compounds, Li2CO3 is polymeric. It is relatively covalent and this is shown by its small solubility. The isolation of lithium from aqueous extracts of its ores capitalizes on this low solubility. Its apparent solubility increases tenfold under a mild pressure of carbon dioxide; this effect is due to the formation of the metastable bicarbonate:
- Li2CO3 + CO2 + H2O → 2 LiHCO3
Applications
Lithium carbonate is an important industrial chemical. It forms low-melting fluxes with silica and other materials. Glasses derived from lithium carbonate are useful in ovenware. Lithium carbonate is a common ingredient in both low-fire and high-fire ceramic glaze. Its alkaline properties are conducive to changing the state of metal oxide colorants in glaze particularly red iron oxide (Fe2O3). Cement sets more rapidly when prepared with lithium carbonate, and is useful for tile adhesives. When added to aluminium trifluoride, it forms LiF which gives a superior electrolyte for the processing of aluminium.[3] Lithium carbonate is used as an active material of carbon dioxide sensors.[4] It is also used in the manufacture of most lithium-ion battery cathodes, which are made of lithium cobalt oxide.
Medical uses
In 1843, lithium carbonate was used as a new solvent for stones in the bladder. In 1859, some doctors recommended a therapy with lithium salts for a number of ailments including gout, urinary calculi, rheumatism, mania, depression and headache. In 1949, Cade discovered the anti-manic effects of lithium ions. This knowledge led lithium, specifically lithium carbonate to be used to treat mania associated with bipolar disorder.
Lithium carbonate is used to treat mania, the elevated phase of bipolar disorder. Lithium ions interfere with chemical reactions (sodium pump) that relay and amplify messages carried to the cells of the brain.[5] In mania there is an observed irregular increase in protein kinase C (PKC) activity within the brain. A recent study has shown that lithium carbonate and sodium valproate, another drug traditionally used to treat the disorder, act in the brain by inhibiting PKC’s activity and help to create other compounds that also inhibit the PKC.[6] Additionally, daily doses of lithium have been found to delay progression of amyotrophic lateral sclerosis (ALS) in an Italian study of 44 people with the disorder. No other treatment to date has shown such a dramatic effect on ALS.[7] Despite these findings, a great deal remains unknown regarding lithium's mood controlling properties.
Recently, topical lithium has been utilized in dermatological disorders, such as herpes viral infections. It is hoped that lithium will be used in the future as an anti-inflammatory, antiviral, anti-fungal, and anti-tumor agent. Lithium salts when used at low doses do not cause addiction, but do have a number of risks and side effects associated with their use, especially at higher doses. Lithium intoxication affects the central nervous system and renal system and is potentially lethal.[8]
Pyrotechnics
Lithium carbonate is found in fireworks, because lithium imparts a deep red to flames.
References
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
- ^ David Barthelmy. "Zabuyelite Mineral Data". Mineralogy Database. Retrieved 2010-02-07.
- ^ Ulrich Wietelmann, Richard J. Bauer "Lithium and Lithium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH: Weinheim.
- ^ Technical Information for Carbon Dioxide Sensors
- ^ Medical use
- ^ Yildiz, A; Guleryuz, S; Ankerst, DP; Ongür, D; Renshaw, PF (2008). "Protein kinase C inhibition in the treatment of mania: a double-blind, placebo-controlled trial of tamoxifen". Archives of general psychiatry. 65 (3): 255–63. doi:10.1001/archgenpsychiatry.2007.43. PMID 18316672.
- ^ MDA Research|Lithium Slows ALS Progression In Study
- ^ Simard, M; Gumbiner, B; Lee, A; Lewis, H; Norman, D (1989). "Lithium carbonate intoxication. A case report and review of the literature" (PDF). Archives of internal medicine. 149 (1): 36–46. doi:10.1001/archinte.149.1.36. PMID 2492186.
For more information
- Official FDA information published by Drugs.com