What influences the pulling forces between polar molecules in Van Der Waals interactions?

The pulling forces between polar molecules in Van Der Waals interactions are primarily influenced by the polarity of the molecules involved. Polarity arises from the distribution of electronic charge across a molecule, due to differences in electronegativity between the atoms that make up the molecule. When a molecule is polar, it has a positive end and a negative end, which create dipole-dipole interactions with other polar molecules. These interactions are a key component of Van Der Waals forces, allowing polar molecules to attract one another.

The strength of these interactions depends on how polar the molecules are—greater differences in electronegativity and a more uneven distribution of charge will lead to stronger dipole-dipole interactions. Therefore, the correct influence on the pulling forces between polar molecules is their polarity, which governs the extent and nature of the attractive forces in Van Der Waals interactions.