Final answer:
The correct statement is that the polarity of a molecule is dependent on its 3-D structure. This determines if a molecule has a dipole moment, resulting in a polar or nonpolar characteristic. Other statements regarding molecular interactions and solubility are incorrect.
Step-by-step explanation:
The statement that is correct among the options given is, C. The polarity of a molecule is dependent on its 3-D structure. This is because the molecular structure and the polarity of each of its bonds determine if the molecule as a whole will have a net dipole moment, resulting in a polar or nonpolar molecule. Asymmetrical molecules with polar bonds typically have a dipole moment, while in symmetrical molecules, the bond moments may cancel out, leading to no net dipole moment and a nonpolar molecule.
It is worth noting that, contrary to statement A, high molecular dipole moments are characteristic of polar molecules, not nonpolar ones. Statement B is incorrect because polar solutes tend to be more soluble in polar solvents. Regarding statement D, not all polar molecules are capable of hydrogen bonding; only those with hydrogen atoms bonded to highly electronegative atoms, such as oxygen, nitrogen, or fluorine. Finally, statement E is also incorrect as, in general, dipole-dipole interactions are stronger than London dispersion forces, particularly in small polar molecules.