Final answer:
In liquid water, hydrogen bonding is the predominant intermolecular force due to its polar nature and ability to form strong dipole-dipole interactions. Carbon tetrachloride exhibits London dispersion forces as it is nonpolar, while methyl chloride exhibits dipole-dipole interactions due to its permanent dipole moment.
Step-by-step explanation:
The predominant intermolecular force in liquid water (H₂O) is hydrogen bonding. This is because water has a hydrogen atom bonded to a highly electronegative oxygen atom, allowing for strong dipole-dipole interactions that we recognize as hydrogen bonds. In contrast, the main intermolecular force in carbon tetrachloride (CCl₄) is London dispersion forces, as it is a nonpolar molecule, and the instantaneous dipoles within the molecule result in these temporary attractive forces. Methyl chloride (CH₃Cl) exhibits dipole-dipole interactions due to the permanent dipole created by the difference in electronegativity between the carbon atom and the chlorine atom. However, these forces are not as strong as hydrogen bonding.