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|Section2= |Section3= |Section4= |Section7= |Section8= }} Phosphorus pentachloride is the chemical compound with the formula PCl5. It is one of the most important phosphorus chlorides, others being PCl3 and POCl3. PCl5 finds use as a chlorinating reagent. It is a colourless, water- and moisture-sensitive solid, although commercial samples can be yellowish and contaminated with hydrogen chloride. ==Structure== The structures for the phosphorus chlorides are invariably consistent with VSEPR theory. The structure of PCl5 depends on its environment. Gaseous and molten PCl5 is a neutral molecule with trigonal bipyramidal (''D''3h) symmetry. The hypervalent nature of this species (as well as for PCl, see below) can be explained with the inclusion of non-bonding MOs (Molecular orbital theory) or resonance (Valence bond theory). This trigonal bipyramidal structure persists in non-polar solvents, such as CS2 and CCl4. In the solid state PCl5 is ionic, formulated PClPCl. In solutions of polar solvents, PCl5 undergoes "autoionization". Dilute solutions dissociate according to the following equilibrium: :PCl5 ()Cl− At higher concentrations, a second equilibrium becomes more prevalent: :2 PCl5 ()() The cation PCl and the anion PCl are tetrahedral and octahedral, respectively. At one time, PCl5 in solution was thought to form a dimeric structure, P2Cl10, but this suggestion is not supported by Raman spectroscopic measurements. 抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』 ■ウィキペディアで「Phosphorus pentachloride」の詳細全文を読む スポンサード リンク
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