Final answer:
In the liquid state, water experiences hydrogen bonds, carbon tetrabromide experiences dispersion forces, and dichloromethane primarily experiences dipole-dipole interactions.
Step-by-step explanation:
The predominant intermolecular force in the liquid state of water (H₂O), carbon tetrabromide (CBr₄), and dichloromethane (CH₂Cl₂) can be identified based on the molecular characteristics of each compound.
For water (H₂O), the hydrogen bonds are the strongest and most significant intermolecular force due to the oxygen atom's high electronegativity and the ability to form strong electrostatic attractions with hydrogen atoms of neighboring water molecules.
For carbon tetrabromide (CBr₄), dispersion forces, also known as London dispersion forces, are the dominant intermolecular force. Bromine atoms are large with many electrons, which leads to stronger temporary dipole-induced dipole attractions between the molecules.
Dichloromethane (CH₂Cl₂) primarily experiences dipole-dipole interactions because it is a polar molecule with a permanent dipole moment due to the electronegativity difference between the carbon-hydrogen and carbon-chlorine bonds, even though it can also exhibit some dispersion forces.