The formal charge of P is 0 and the formal charge of F is 0.
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.
PF3 is nonpolar because it has a trigonal pyramidal molecular geometry with three identical bonds and a lone pair on the central phosphorus atom. The dipole moments of the three P-F bonds cancel each other out, resulting in a molecule with no net dipole moment.
PF5 :SP3d
The phosphorus atom in PF3 is sp3 hybridized. It forms three sigma bonds with the three fluorine atoms using three of its four sp3 hybridized orbitals. The remaining sp3 hybrid orbital contains a lone pair of electrons on the phosphorus atom.
The central atom of a phosphorus pentafluoride molecule is the phosphorus atom. Five fluorine atoms are directly bonded to it and there is no lone pairs located in the central atom. Having a trigonal bipyramidal shape, every bond angle in the equatorial plane is equal to 120 degrees and every bond angle in axial plane is equal to 90 degrees..
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.
Yes, PF3 is a nonpolar molecule. The molecule has a trigonal pyramidal shape with the fluorine atoms positioned symmetrically around the phosphorus atom, resulting in a net dipole moment of zero.
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PF3 is nonpolar because it has a trigonal pyramidal molecular geometry with three identical bonds and a lone pair on the central phosphorus atom. The dipole moments of the three P-F bonds cancel each other out, resulting in a molecule with no net dipole moment.
First, calculate the molar mass of PF3: P = 30.97 g/mol, F = 19.00 g/mol, so PF3 = 30.97 + (3 * 19.00) = 88.97 g/mol. Given that the reaction is 76.5% yield, the actual mass of PF3 produced is 186 g / 0.765 = 242.75 g. From the balanced equation, 6 moles of F2 are needed to produce 4 moles of PF3. Therefore, the molar ratio is 6:4. Calculate the moles of PF3 produced and then find the moles of F2 needed. Finally, convert moles of F2 to grams.
PF5 :SP3d
The phosphorus atom in PF3 is sp3 hybridized. It forms three sigma bonds with the three fluorine atoms using three of its four sp3 hybridized orbitals. The remaining sp3 hybrid orbital contains a lone pair of electrons on the phosphorus atom.
The central atom of a phosphorus pentafluoride molecule is the phosphorus atom. Five fluorine atoms are directly bonded to it and there is no lone pairs located in the central atom. Having a trigonal bipyramidal shape, every bond angle in the equatorial plane is equal to 120 degrees and every bond angle in axial plane is equal to 90 degrees..
P-F is Polar
p --> q and q --> p are not equivalent p --> q and q --> (not)p are equivalent The truth table shows this. pq p --> q q -->(not)p f f t t f t t t t f f f t t t t
p > q~qTherefore, ~p| p | q | p > q | ~q | ~p || t | t | t | f | f || t | f | t | t | f || f | t | t | f | t || f | f | t | t | t |
P Q (/P or /Q) T T F T F T F T T F F T