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8 P 2 O 3 ⇌ P 4 + 6 P 2 O 4. In addition, phosphorus trioxide can be converted into phosphorus tetroxide by controlled oxidation with oxygen in carbon tetrachloride solution. [4] [5] [6] Careful reduction of phosphorus pentoxide with red phosphorus at 450-525 °C also produces phosphorus tetroxide.
Phosphorus pentoxide (phosphorus(V) oxide, phosphoric anhydride), P 2 O 5; Phosphorus trioxide (phosphorus(III) oxide, phosphorous anhydride), P 2 O 3; Phosphorus tetroxide, P 2 O 4; Several other, less common, oxides of phosphorus, including P 4 O 7, P 4 O 9, and P 2 O 6; Gases: Phosphorus monoxide, PO; Phosphorus dioxide, PO 2
Phosphorus pentoxide crystallizes in at least four forms or polymorphs.The most familiar one, a metastable form [1] (shown in the figure), comprises molecules of P 4 O 10.Weak van der Waals forces hold these molecules together in a hexagonal lattice (However, in spite of the high symmetry of the molecules, the crystal packing is not a close packing [2]).
A phosphoryl group is a trivalent >P(=O)− group, consisting of a phosphorus atom (symbol P) and an oxygen atom (symbol O), where the three free valencies are on the phosphorus atom. While commonly depicted as possessing a double bond (P=O) the bonding is in fact non-classical. [1]
Phosphine oxide is the inorganic compound with the formula H 3 PO. Although stable as a dilute gas, liquid or solid samples are unstable. Unlike many other compounds of the type PO x H y, H 3 PO is rarely discussed and is not even mentioned in major sources on main group chemistry.
Solid HP(O)(OH) 2 has tetrahedral geometry about the central phosphorus atom, with a P−H bond of 132 pm, one P=O double bond of 148 pm and two longer P−OH single bonds of 154 pm. In common with other phosphorus oxides with P−H bonds (e.g. hypophosphorous acid and dialkyl phosphites ), [ 2 ] it exists in equilibrium with an extremely minor ...
6 P 2 Mo 18 O 62). Oxygen can form oxides with heavier noble gases xenon and radon, although this needs indirect methods. Even though no oxides of krypton are known, oxygen is able to form covalent bonds with krypton in an unstable compound Kr(OTeF 5) 2. One unexpected oxygen compound is dioxygenyl hexafluoroplatinate, O + 2 PtF −
P 4 O 6 reacts with ozone at 195 K to give the unstable compound P 4 O 18. [3] P 4 O 18 decomposes above 238 K in solution with the release of O 2 gas. Decomposition of dry P 4 O 18 is explosive. In a disproportionation reaction, P 4 O 6 is converted into the mixed P(III)P(V) species P 4 O 8 when heated in a sealed tube at 710 K, with the side ...