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Phosphorus trifluoride (formula P F 3), is a colorless and odorless gas.It is highly toxic and reacts slowly with water. Its main use is as a ligand in metal complexes.As a ligand, it parallels carbon monoxide in metal carbonyls, [1] and indeed its toxicity is due to its binding with the iron in blood hemoglobin in a similar way to carbon monoxide.
Phosphoryl fluoride (commonly called phosphorus oxyfluoride) is a compound with the chemical formula P O F 3. It is a colorless gas that hydrolyzes rapidly. It is a colorless gas that hydrolyzes rapidly.
Lower-period elements, however, may form hypervalent molecules, such as phosphorus pentafluoride or sulfur hexafluoride. [78] The reactivity of such species varies greatly—sulfur hexafluoride is inert, while chlorine trifluoride is extremely reactive—but there are some trends based on periodic table locations. Boron trifluoride is a planar ...
Phase behavior Triple point? K (? °C), ? Pa Critical point: 271 K (−2 °C), 42.7 atm Std enthalpy change of fusion, Δ fus H o? kJ/mol Std entropy change
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 ...
Phosphorus fluoride may refer to any of the following: Phosphorus trifluoride, PF 3; Phosphorus pentafluoride, PF 5; Diphosphorus tetrafluoride, [1] P 2 F 4; See phosphorus halides for a complete list of phosphorus halides.
The central phosphorus atom has sp 3 d hybridization, and the molecule has an asymmetric charge distribution. It appears as a colorless gas with a disagreeable odor, and it turns into a liquid at -8 °C. Phosphorus trifluorodichloride is formed by mixing phosphorus trifluoride with chlorine PF 3 + Cl 2 → PF 3 Cl 2 [2]
When comparing a polar and nonpolar molecule with similar molar masses, the polar molecule in general has a higher boiling point, because the dipole–dipole interaction between polar molecules results in stronger intermolecular attractions. One common form of polar interaction is the hydrogen bond, which is also