Caesium fluoride (cesium fluoride in American English) is an inorganic compound with the formula CsF. A hygroscopic white salt, caesium fluoride is used in the synthesis of organic compounds as a source of the fluoride anion. The compound is noteworthy from the pedagogical perspective as caesium also has the highest electropositivity of all commonly available elements and fluorine has the highest electronegativity.
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| IUPAC name Caesium fluoride | |
| Other names Cesium fluoride | |
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| ECHA InfoCard | 100.033.156 |
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| Properties | |
| CsF | |
| Molar mass | 151.903 g/mol |
| Appearance | white crystalline solid |
| Density | 4.64 g/cm3 |
| Melting point | 703 °C (1,297 °F; 976 K) |
| Boiling point | 1,251 °C (2,284 °F; 1,524 K) (2,284 °F; 1,524 K) |
| 573.0 g/100 mL (25 °C) | |
| Solubility | Insoluble in acetone, diethyl ether, pyridine and ethanol 191 g/100 mL in methanol. |
| Basicity (pKb) | −744 kJ/mol |
| −44.5·10−6 cm3/mol | |
Refractive index (nD) | 1.477 |
| Structure | |
| cubic, cF8 | |
| Fm3m, No. 225 | |
a = 0.6008 nm | |
Lattice volume (V) | 0.2169 nm3 |
Formula units (Z) | 4 |
| Octahedral | |
Dipole moment | 7.9 D |
| Thermochemistry | |
Heat capacity (C) | 51.1 J/mol·K |
Std molar entropy (S⦵298) | 92.8 J/mol·K |
Std enthalpy of formation (ΔfH⦵298) | −553.5 kJ/mol |
Gibbs free energy (ΔfG⦵) | −525.5 kJ/mol |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards | toxic |
| GHS labelling: | |
Signal word | Danger |
| H301, H311, H315, H318, H331, H361f | |
| P201, P202, P260, P261, P264, P270, P271, P280, P281, P301+P310, P301+P330+P331, P302+P352, P303+P361+P353, P304+P340, P305+P351+P338, P308+P313, P310, P311, P312, P321, P322, P330, P332+P313, P361, P362, P363, P403+P233, P405, P501 | |
| NFPA 704 (fire diamond) | 3 0 0 |
| Flash point | Non-flammable |
| Safety data sheet (SDS) | External MSDS |
| Related compounds | |
Other anions | Caesium chloride Caesium bromide Caesium iodide Caesium astatide |
Other cations | Lithium fluoride Sodium fluoride Potassium fluoride Rubidium fluoride Francium fluoride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references | |
Synthesis and properties
Caesium fluoride can be prepared by the reaction of caesium hydroxide (CsOH) with hydrofluoric acid (HF) and the resulting salt can then be purified by recrystallization. The reaction is shown below:
- CsOH + HF → CsF + H2O
Using the same reaction, another way to create caesium fluoride is to treat caesium carbonate (Cs2CO3) with hydrofluoric acid and again, the resulting salt can then be purified by recrystallization. The reaction is shown below:
- Cs2CO3 + 2 HF → 2 CsF + H2O + CO2
CsF is more soluble than sodium fluoride or potassium fluoride in organic solvents. It is available in its anhydrous form, and if water has been absorbed, it is easy to dry by heating at 100 °C for two hours in vacuo. CsF reaches a vapor pressure of 1 kilopascal at 825 °C, 10 kPa at 999 °C, and 100 kPa at 1249 °C.
Structure
Caesium fluoride has the halite structure, which means that the Cs+ and F− pack in a cubic closest packed array as do Na+ and Cl− in sodium chloride. Unlike sodium chloride, caesium fluoride's anion is smaller than its cation, so it is the anion size that sterically inhibits larger coordination numbers than six under normally encountered conditions. A larger halide ion would allow for the eight-coordination seen in other caesium halide crystals.
Applications in organic synthesis
Being highly dissociated, CsF is a more reactive source of fluoride than related alkali metal salts. CsF is an alternative to tetra-n-butylammonium fluoride (TBAF) and TAS-fluoride (TASF).
As a base
As with other soluble fluorides, CsF is moderately basic, because HF is a weak acid. The low nucleophilicity of fluoride means it can be a useful base in organic chemistry. CsF gives higher yields in Knoevenagel condensation reactions than KF or NaF.
Formation of Cs-F bonds
Caesium fluoride serves as a source of fluoride in organofluorine chemistry. Similarly to potassium fluoride, CsF reacts with hexafluoroacetone to form a stable perfluoroalkoxide salt. It will convert electron-deficient aryl chlorides to aryl fluorides (Halex process), although potassium fluoride is more commonly used.
Deprotection agent
Due to the strength of the Si–F bond, fluoride is useful for desilylation reactions, i.e., cleavage of Si-O bonds in organic synthesis. CsF is commonly used for such reactions. Solutions of caesium fluoride in THF or DMF attack a wide variety of organosilicon compounds to produce an organosilicon fluoride and a carbanion, which can then react with electrophiles, for example:
Precautions
Like other soluble fluorides, CsF is moderately toxic. Contact with acid should be avoided, as this forms highly toxic/corrosive hydrofluoric acid. The caesium ion (Cs+) and caesium chloride are generally not considered toxic.
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