![]() Crystal structureĬaesium fluoride has the inverse halite structure, because caesium ions are larger than fluoride ions in the lithium, sodium, potassium, and rubidium halides, the cation is smaller than the anion. The low nucleophilicity of fluoride means it can be a useful base in organic chemistry. ![]() As with other soluble fluorides, CsF is moderately basic, because HF is a weak acid. Due to the strength of the Si– F bond, fluoride ion is useful for desilylation reactions (removal of Si groups) in organic chemistry caesium fluoride is an excellent source of anhydrous fluoride for such reactions ( vida infra). It therefore undergoes all of the usual reactions associated with soluble fluorides such as potassium fluoride, for example: Ģ CsF (aq) + CaCl 2 (aq) → 2 CsCl (aq) + CaF 2 ( s)īeing highly dissociated it is quite reactive as a fluoride source under anhydrous conditions too, and it will react with electron-deficient aryl chlorides to form aryl fluorides (halex reaction). ![]() Contact with acid should be avoided, as this forms highly toxic/corrosive hydrofluoric acid.Ĭaesium fluoride reacts usually as a source of fluoride ion, F. Like all soluble fluorides, it is mildly basic. It is therefore a useful, less hygroscopic alternative to tetra-n-butylammonium fluoride (TBAF) and TAS-fluoride (TASF) when anhydrous "naked" fluoride ion is needed. It is available in anhydrous form, and if water has been absorbed it is easy to dry by heating at 100 ° C for two hours in vacuo. It is more soluble and more readily dissociated than sodium fluoride or potassium fluoride. Sodium fluoride potassium fluoride rubidium fluorideĮxcept where noted otherwise, data are given for materials in their standard state (at 25 ☌, 100 kPa) Infobox disclaimer and referencesĬaesium fluoride ( cesium fluoride in North America), is an ionic compound usually found as a hygroscopic white solid. Caesium chloride caesium bromide caesium iodide
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