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Phosphorus pentachloride is the chemical compound with the formula PCl 5. It is one of the most important phosphorus chlorides/oxychlorides, others being PCl 3 and POCl 3. PCl 5 finds use as a chlorinating reagent. It is a colourless, water-sensitive solid, although commercial samples can be yellowish and contaminated with hydrogen chloride.
Phosphorus pentachloride, phosphorus pentabromide, and phosphorus heptabromide are ionic in the solid and liquid states; PCl 5 is formulated as PCl 4 + PCl 6 –, but in contrast, PBr 5 is formulated as PBr 4 + Br −, and PBr 7 is formulated as PBr 4 + Br 3 −. They are widely used as chlorinating and brominating agents in organic chemistry.
A pentachloride is a compound or ion that contains five chlorine atoms or ions. Common pentachlorides include: Antimony pentachloride, SbCl 5; Arsenic pentachloride, AsCl 5; Molybdenum pentachloride, MoCl 5; Niobium pentachloride, NbCl 5; Phosphorus pentachloride, PCl 5; Protactinium pentachloride, PaCl 5; Osmium pentachloride, OsCl 5; Rhenium ...
The reaction of phosphorus pentachloride (PCl 5) with phosphorus pentoxide (P 4 O 10). 6 PCl 5 + P 4 O 10 → 10 POCl 3. The reaction can be simplified by chlorinating a mixture of PCl 3 and P 4 O 10, generating the PCl 5 in situ. The reaction of phosphorus pentachloride with boric acid or oxalic acid: [12] 3 PCl 5 + 2 B(OH) 3 → 3 POCl 3 + B ...
Phosphorus pentachloride (PCl 5), sulfur hexafluoride (SF 6), chlorine trifluoride (ClF 3), the chlorite (ClO − 2) ion in chlorous acid and the triiodide (I − 3) ion are examples of hypervalent molecules.
PCl 5 is a colourless solid which has an ionic formulation of PCl 4 + PCl 6 −, but adopts the trigonal bipyramidal geometry when molten or in the vapour phase. [17] PBr 5 is an unstable solid formulated as PBr 4 + Br − and PI 5 is not known. [17] The pentachloride and pentafluoride are Lewis acids.
Solid phosphorus pentachloride is an ionic compound, formulated PCl + 4 PCl − 6, that is, a salt containing the tetrachlorophosphonium cation. [7] [8] Dilute solutions dissociate according to the following equilibrium: PCl 5 ⇌ PCl + 4 + Cl −
The tetrahedral intermediate collapses, ejecting chloride ion as the leaving group and forming oxonium species 3. Deprotonation gives the mixed anhydride, 4, and an equivalent of HCl. Alcohols and amines react with acid halides to produce esters and amides, respectively, in a reaction formally known as the Schotten-Baumann reaction. [19]