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What is the oxidation number of p in pf3?
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.
What is the polarity of PF3?
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.
What type of hybrid orbital is PF3 and PF5?
PF5 :SP3d
What is the hybridization of the P atom in PF3?
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.
What are the bond angles of PF3Br2?
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..
What is the oxidation number of p in pf3?
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.
Is p-F non polar?
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.
What is the polarity of PF3?
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.
How many lone pairs of electrons are on the P atom in PF3?
There are 1
What mass of F2 is needed to produce 120g of PF3 if the reaction is 78.1?
To determine the mass of F2 needed to produce 120 g of PF3, we first need to calculate the molar mass of PF3, which is approximately 88 g/mol (phosphorus = 31 g/mol, fluorine = 19 g/mol × 3). The balanced chemical reaction for producing PF3 from P and F2 is: P + 3F2 → PF3. Since the molar ratio of PF3 to F2 is 1:3, we need 3 moles of F2 for every mole of PF3 produced. Therefore, for 120 g of PF3, which is about 1.36 moles (120 g / 88 g/mol), we would require approximately 4.08 moles of F2, or about 164 g (4.08 moles × 38 g/mol for F2).
P4 plus 6F2 yields 4PF3 What mass of F2 is needed to produce 186 g of PF3 if the reaction has a 76.5 percent yield?
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.
What type of hybrid orbital is PF3 and PF5?
PF5 :SP3d
What mass of F2 is needed to produce 120g of PF3 if the reaction is 78.1 yield?
To find the mass of F2 needed to produce 120 g of PF3 at a yield of 78.1%, we first calculate the theoretical mass of PF3 that would require 100% yield. The molar mass of PF3 is approximately 88 g/mol. Therefore, the theoretical mass of PF3 produced from 120 g at 78.1% yield is ( 120 , \text{g} / 0.781 = 153.5 , \text{g} ). Assuming the reaction is balanced as ( P + \frac{3}{2} F_2 \rightarrow PF_3 ), we can then determine that the stoichiometry requires 1 mole of F2 for every mole of PF3. Hence, the mass of F2 needed is calculated using the molar mass of F2 (approximately 38 g/mol), resulting in approximately 60 g of F2 needed to produce the required PF3.
What is the hybridization of the P atom in PF3?
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.
What are the bond angles of PF3Br2?
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..
Is P - F polar?
P-F is Polar
P-q and q-p are logically equivalent prove?
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
