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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.
No trifluoride is soluble in water, but several are soluble in other solvents. [57] The tetrafluorides show a mixture of ionic and covalent bonding. Zirconium, hafnium, plus many of the actinides form tetrafluorides with an ionic structure that puts the metal cation in an 8-coordinate square antiprism. [58] [59] Melting points are around 1000 ...
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
Hexafluorophosphoric acid (HPF 6) is derived from phosphorus pentafluoride and hydrogen fluoride. Its conjugate base, hexafluorophosphate (PF 6 – ), is a useful non-coordinating anion . It is often used in lithium-ion batteries , where besides providing good ionic conductivity for the liquid electrolyte, it also passivates positive aluminium ...
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
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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.