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WHAT IS THE INTERMOLECULAR FORCE BETWEEN NF3 IN LIQUID STATE?
Every molecule has a london force (Induce dipole induce dipole force). In this molecule, the intermolecular force that hold these bonds together is dipole-diple interaction or dipolar interaction. There is no hydrogen bonding in here. If there is hydrogen bonding, H-atom must make bond with N,O,F. Therefore, intermolecular forces of NF3 is london force and dipole-diploe
What is the formula for NF3?
The chemical formula for nitrogen trifluoride is NF3. It consists of one nitrogen atom bonded to three fluorine atoms.
Which is the correct formula for nitrogen trifluoride out of NF NF2 NF3 N3F?
NF3 is the correct formula for nitrogen trifluoride.
What is the mass percent of nitrogen in NF3?
To find the mass percent of nitrogen in NF3, you need to calculate the molar mass of NF3 and then determine the mass of nitrogen in one mole of NF3. The molar mass of NF3 is 71.001 g/mol. The molar mass of nitrogen in NF3 is 14.007 g/mol. Therefore, the mass percent of nitrogen in NF3 is (14.007 g/mol / 71.001 g/mol) * 100% ≈ 19.76%.
What is the bond angle in NF3?
The bond angle in NF3 is approximately 107 degrees.
Is the correct formula for nitrogen trifluoride?
NF3
How many moles of NF3 are in 12g?
12 g NF3 equals 0,17 moles.
What is the name of the covalent compound of NF3?
The covalent compound of NF3 is called nitrogen trifluoride.
What is the hybridization of NF3?
The hybridization of NF3 is sp3. This means that the nitrogen atom in NF3 forms four equivalent sp3 hybrid orbitals when it bonds with the three fluorine atoms.
How many moles of NF3 are in 850.49 grams of nitrogen trifluoride?
To find the number of moles of NF3 in 850.49 grams, you first need to convert the mass to moles using the molar mass of NF3, which is 71.00 g/mol. Moles of NF3 = 850.49 g / 71.00 g/mol = 11.98 moles.
What is the attraction force for NF3?
The attraction forces in nitrogen trifluoride (NF3) primarily arise from dipole-dipole interactions due to its polar nature, as the molecule has a significant difference in electronegativity between nitrogen and fluorine. Additionally, London dispersion forces also contribute, though they are weaker in comparison. The overall attraction forces in NF3 are stronger than those in nonpolar molecules but weaker than those in ionic or hydrogen-bonding compounds. These intermolecular forces influence NF3's physical properties, such as boiling and melting points.
How do the bond angles in NF3 compare to those in NH3?
In NF3, the bond angles are larger than in NH3.
