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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(II) halides may be prepared by passing an electric discharge through a mixture of the trihalide vapour and hydrogen gas. [ citation needed ] The relatively stable P 2 I 4 is known to have a trans , bent configuration similar to hydrazine and finds some uses in organic syntheses, the others are of purely academic interest at the ...
Phosphoryl chloride (commonly called phosphorus oxychloride) is a colourless liquid with the formula P O Cl 3. It hydrolyses in moist air releasing phosphoric acid and fumes of hydrogen chloride . It is manufactured industrially on a large scale from phosphorus trichloride and oxygen or phosphorus pentoxide . [ 4 ]
In chemistry, a trigonal bipyramid formation is a molecular geometry with one atom at the center and 5 more atoms at the corners of a triangular bipyramid. [1] This is one geometry for which the bond angles surrounding the central atom are not identical (see also pentagonal bipyramid), because there is no geometrical arrangement with five terminal atoms in equivalent positions.
This triphenylphosphine dichloride Ph 3 PCl 2 is related to phosphorus pentachloride PCl 5. Treatment of this species with hydroxylamine in the presence of Ph 3 P results in replacement of the two single P–Cl bonds in Ph 3 PCl 2 by one double P=N bond: 2 Ph 3 PCl 2 + NH 2 OH·HCl + Ph 3 P → [(Ph 3 P) 2 N]Cl + 4HCl + Ph 3 PO ...
In the case of phosphorus pentachloride (PCl 5), the example shown on the right, the central phosphorus atom is bonded to five chlorine atoms. In the traditional Lewis view, this violates the octet rule as the five phosphorus-chlorine bonds would result in a net ten electrons around the phosphorus atom.
Si-F bonds and Si-H bonds both increase in length upon pentacoordination and related effects are seen in phosphorus species, but to a lesser degree. The reason for the greater magnitude in bond length change for silicon species over phosphorus species is the increased effective nuclear charge at phosphorus.
Phosphorus has a valence 3 in phosphine (PH 3) and a valence of 5 in phosphorus pentachloride (PCl 5), which shows that an element may exhibit more than one valence. The structural formula of a compound represents the connectivity of the atoms, with lines drawn between two atoms to represent bonds. [1]