Question

Phosphorus trichloride (pcl3) and ammonia (nh3) are both polar molecules. First, use what you have learned from our lessons to thoroughly explain the types of van der waals forces present in each substance. Then identify and discuss a type of van der waals force that exists in ammonia but not in phosphorus trichloride. How do you know?

Answer 1

Phosphorus trichloride and ammonia are both polar molecules with dipole-dipole forces and London dispersion forces. Ammonia also has hydrogen bonding, which is absent in phosphorus trichloride.

Step-by-step explanation:

Phosphorus trichloride (PCl3) and ammonia (NH3) are both polar molecules due to the presence of polar bonds within the molecules. In PCl3, there are three polar P-Cl bonds, and in NH3, there is a polar N-H bond.

The types of van der Waals forces present in both substances are dipole-dipole forces and London dispersion forces.

One type of van der Waals force that exists in ammonia but not in phosphorus trichloride is hydrogen bonding. Hydrogen bonding occurs between a hydrogen atom bonded to an electronegative atom (in this case, nitrogen) and another electronegative atom (such as oxygen or nitrogen) in a neighboring molecule. This type of bonding is stronger than ordinary dipole-dipole attractions and contributes to the higher boiling point of ammonia compared to phosphorus trichloride.