covalent
covalent bond
PF3 is a molecular compound. It consists of a covalent bond between phosphorus and fluorine atoms.
In phosphorus trifluoride (PF3), the bond angle is approximately 97 degrees. This angle is slightly less than the ideal tetrahedral bond angle of 109.5 degrees due to the presence of a lone pair of electrons on the phosphorus atom, which repels the bonding pairs and causes a distortion in the molecular geometry. As a result, PF3 adopts a trigonal pyramidal shape.
The most idealized bond angle would be in CS2, which has a linear molecular geometry with a bond angle of 180 degrees. PF3, SBr2, and CHCl3 have trigonal pyramidal, angular, and tetrahedral geometries, respectively, which deviate from the ideal angles due to lone pair repulsions.
The chemical formula for phosphorus trifluoride is PF3.
PF5 :SP3d
The oxidation number of phosphorus (P) in PF3 is +3. This is because fluorine (F) has an oxidation number of -1, and the overall molecule PF3 has a total charge of 0.
Ax3e
tetrahedral
To find the number of molecules of PF3, we need to convert 150.0 grams of PF3 to moles, then use Avogadro's number (6.022 x 10^23 molecules/mol) to find the number of molecules. The molar mass of PF3 is approximately 87.97 g/mol. By dividing 150.0 g by the molar mass, we get the number of moles, which can be converted to molecules.
In PF3, the central phosphorus atom uses sp3 hybrid orbitals. In PF5, the central phosphorus atom uses sp3d hybrid orbitals.
PCl3 has more polar bonds than PF3 because chlorine is more electronegative than fluorine, resulting in greater electron density towards chlorine in PCl3.