Final answer:
The cohesive behavior between water molecules is due to Hydrogen bonds (answer C), a type of dipole-dipole interaction, where the partially positive hydrogen of one water molecule is attracted to the partially negative oxygen of a nearby water molecule.
Step-by-step explanation:
The characteristic of the molecular structure of water that allows for cohesive behavior between water molecules is C) Hydrogen bonds. These bonds are a type of weak dipole-dipole interaction. In water, the hydrogen atoms are bound to a highly electronegative oxygen atom resulting in polar covalent bonds within the molecule. This polarity leads to a significant molecular dipole in each water molecule, where the hydrogen has a partial positive charge, and the oxygen has a partial negative charge.
Consequently, the partially positive hydrogen of one water molecule feels an attraction to the partially negative oxygen of another water molecule, leading to the formation of a hydrogen bond. These hydrogen bonds are relatively weak compared to covalent and ionic bonds, but they are strong enough to give rise to the unique properties of water, such as its high surface tension, its ability to dissolve various substances, and its role as an essential ingredient for life. When considering the options in the question, hydrogen bonds are the only ones that correctly describe the intermolecular forces between two different water molecules.