* Molecular Geometry: PCl₃ has a trigonal pyramidal shape due to the lone pair of electrons on the phosphorus atom. This asymmetric shape leads to a permanent dipole moment.
* Polarity: The electronegativity difference between phosphorus and chlorine creates a polar bond, resulting in a net dipole moment for the entire molecule.
Other forces present but weaker:
* London Dispersion Forces: While weaker, London dispersion forces are always present between molecules due to temporary fluctuations in electron distribution.
* Hydrogen Bonding: PCl₃ does not exhibit hydrogen bonding because it lacks a hydrogen atom bonded to a highly electronegative atom like oxygen or nitrogen.
In summary: While London dispersion forces are present, the dominant intermolecular force in PCl₃ is dipole-dipole interaction due to its permanent dipole moment.
