Final answer:
Force C, which represents hydrogen bonding, is stronger than Force D, which represents van der Waals forces. This conclusion is based on the general strength hierarchy of intermolecular forces, where hydrogen bonds are stronger than both London dispersion forces and dipole-dipole interactions that make up van der Waals forces.
Step-by-step explanation:
To compare the relative strength of force C and force D, we need to identify and understand the nature of these forces. According to the options provided:
- Hydrogen bonding is generally stronger than other forms of dipole-dipole interactions and is specifically known for its strong attractive forces between molecules where hydrogen is bonded to a highly electronegative atom.
- Van der Waals forces include dipole-dipole interactions and London dispersion forces, both of which are generally weaker than hydrogen bonds.
When comparing these forces, hydrogen bonding (Force C) is indeed stronger than van der Waals forces (Force D), which can be either London dispersion forces or dipole-dipole interactions. Therefore, the correct comparison is option (a) where Force C is stronger than Force D.