Caesium carbonate

Caesium carbonate

Caesium, Cs   Carbon, C   Oxygen, O
Names
Preferred IUPAC name Dicaesium carbonate
Other names Caesium carbonate Cesium carbonate
Identifiers
CAS Number	534-17-8 Y
3D model (JSmol)	Interactive image
ChemSpider	10339 Y
ECHA InfoCard	100.007.812
EC Number	208-591-9
PubChem CID	10796
UNII	QQI20A14P4 Y
CompTox Dashboard (EPA)	DTXSID0052178
InChI InChI=1S/CH2O3.2Cs/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2 Y Key: FJDQFPXHSGXQBY-UHFFFAOYSA-L Y InChI=1/CH2O3.2Cs/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2 Key: FJDQFPXHSGXQBY-NUQVWONBAO
SMILES [Cs+].[Cs+].[O-]C([O-])=O
Properties
Chemical formula	Cs2CO3
Molar mass	325.819 g·mol−1
Appearance	white powder
Density	4.072 g/cm3
Melting point	610 °C (1,130 °F; 883 K) (decomposes)
Solubility in water	2605 g/L (15 °C)
Solubility in ethanol	110 g/L
Solubility in dimethylformamide	119.6 g/L
Solubility in dimethyl sulfoxide	361.7 g/L
Solubility in sulfolane	394.2 g/L
Solubility in methylpyrrolidone	723.3 g/L
Magnetic susceptibility (χ)	−103.6·10−6 cm3/mol
Hazards
Flash point	Non-flammable
Related compounds
Other anions	Caesium bicarbonate
Other cations	Lithium carbonate Sodium carbonate Potassium carbonate Rubidium carbonate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y verify (what is YN ?) Infobox references

Caesium carbonate oder cesium carbonate is a chemical compound with the chemical formula Cs₂CO₃. It is white crystalline solid. Caesium carbonate has a high solubility in polar solvents such as water, ethanol and DMF. Its solubility is higher in organic solvents compared to other carbonates like potassium carbonate and sodium carbonate, although it remains quite insoluble in other organic solvents such as toluene, p-xylene, and chlorobenzene. This compound is used in organic synthesis as a base. It also appears to have applications in energy conversion.

Preparation

Caesium carbonate can be prepared by thermal decomposition of caesium oxalate. Upon heating, caesium oxalate is converted to caesium carbonate with emission of carbon monoxide.

Cs₂C₂O₄ → Cs₂CO₃ + CO

It can also be synthesized by reacting caesium hydroxide with carbon dioxide.

2 CsOH + CO₂ → Cs₂CO₃ + H₂O

Chemical reactions

Caesium carbonate facilitates the N-alkylation of compounds such as sulfonamides, amines, β-lactams, indoles, heterocyclic compounds, N-substituted aromatic imides, phthalimides, and other similar compounds. Research on these compounds has focused on their synthesis and biological activity. In the presence of sodium tetrachloroaurate (Na[AuCl₄]), caesium carbonate is very efficient mechanism for aerobic oxidation of different kinds of alcohols into ketones and aldehydes at room temperature without additional polymeric compounds. There is no acid formation produced when primary alcohols are used. The process of selective oxidation of alcohols to carbonyls had been quite difficult due to the nucleophilic character of the carbonyl intermediate. In the past Cr(VI) and Mn(VII) reagents have been used to oxidize alcohols, however, these reagents are toxic and comparatively expensive. Caesium carbonate can also be used in Suzuki, Heck, and Sonogashira synthesis reactions. Caesium carbonate produces carbonylation of alcohols and carbamination of amines more efficiently than some of the mechanisms that have been introduced in the past. Caesium carbonate can be used for sensitive synthesis when a balanced strong base is needed.

For energy conversion

Relatively effective polymer solar cells are built by thermal annealing of caesium carbonate. Caesium carbonate increases the energy effectiveness of the power conversion of solar cells and enhances the life times of the equipment. The studies done on UPS and XPS reveal that the system will do less work due to the thermal annealing of the Cs₂CO₃ layer. Caesium carbonate breaks down into Cs₂O and Cs₂O₂ by thermal evaporation. It was suggested that, when Cs₂O combines with Cs₂O₂ they produce n-type dopes that supplies additional conducting electrons to the host devices. This produces a highly efficient inverted cell that can be used to further improve the efficiency of polymer solar cells or to design adequate multijunction photovoltaic cells. The nanostructure layers of Cs₂CO₃ can be used as cathodes for organic electronic materials due to its capacity to increase the kinetic energy of the electrons. The nanostructure layers of caesium carbonate had been probed for various fields using different techniques. The fields include such as photovoltaic studies, current-voltage measurements, UV photoelectron spectroscopy, X-ray photoelectron spectroscopy, and impedance spectroscopy. The n-type semiconductor produced by thermal evaporation of Cs₂CO₃ reacts intensively with metals like Al, and Ca in the cathode. This reaction will cut down the work the cathode metals. Polymer solar cells based on solution process are under extensive studies due to their advantage in producing low cost solar cells. Lithium fluoride has been used to raise the power conversion efficiency of polymer solar cells. However, it requires high temperatures (> 500 degree), and high vacuum states raise the cost of production. The devices with Cs₂CO₃ layers have produced equivalent power conversion efficiency compared with the devices that use lithium fluoride. Placing a Cs₂CO₃ layer in between the cathode and the light-emitting polymer improves the efficiency of the white OLED.

Further reading

• Crich, David; Banerjee, Abhisek (2006). "Expedient Synthesis of syn-β-Hydroxy-α-amino acid derivatives: Phenylalanine, Tyrosine, Histidine and Tryptophan". J. Org. Chem. 71 (18): 7106–9. doi:10.1021/jo061159i. PMC 2621330. PMID 16930077.
• Gerard, Dijkstra; Wim H. Kruizinga; Richard M. Kellogg (1987). "An Assessment of the Causes of the "Cesium Effect"". J. Org. Chem. 52 (19): 4230. doi:10.1021/jo00228a015.

External links

• Preparations from Organic Syntheses in which caesium carbonate appears
• Caesium carbonate factsheet from Chemetall GmbH
• Material Safety Data Sheet Cesium Carbonate, 99.5%