Intermolecular Forces for NF3

In this video we’ll identify the intermolecular forces for NF3 (Nitrogen trifluoride). Using a flowchart to guide us, we find that NF3 is a polar molecule. It also has the Fluorine atoms bonded to a Nitrogen atom. Therefore NF3 the main intermolecular force is s Dipole-Dipole. There are also London Dispersion Forces present. In determining the intermolecular forces present for NF3 we follow these steps: - Determine if there are ions present. Since NF3 is a molecule and there is no + or – sign after the Nitrogen trifluoride can say that it is not an ion. - Next, based on its Lewis Structure, we determine if NF3 is polar or non-polar. Since there is difference in electronegativity between the atom F and N atoms, and the molecule is asymmetrical, NF3 is considered to be a polar molecule. Since we have a difference in electronegativity and the F is bonded to a N atom the main intermolecular force Dipole-Dipole. Useful Resources: