Final answer:
The attraction among water molecules is stronger than the attraction among carbon dioxide molecules due to the ability of water to form strong hydrogen bonds, whereas carbon dioxide can only exhibit weaker dispersion forces. Therefore correct option is B
Step-by-step explanation:
The attraction among water molecules is stronger than the attraction among carbon dioxide molecules. This is because water molecules are capable of forming strong hydrogen bonds due to the presence of a highly electronegative oxygen atom that creates a strong dipole. In contrast, carbon dioxide molecules are nonpolar and can only exhibit weaker dispersion forces.
Ionic bonds, such as those found between sodium and chloride ions, are generally very strong due to the electrostatic attraction between oppositely charged ions. However, when comparing to the interactions within a polyatomic ion or diatomic molecule, we have to consider the type of forces present. Polyatomic ions are held together by strong covalent bonds, and similarly, diatomic molecules may also be held together by covalent bonds.
However, the interactions between separate carbon dioxide molecules are comparatively weaker than those among water molecules. Carbon dioxide molecules interact through London dispersion forces, which are temporary and fluctuate due to the movement of electrons. These forces are significantly weaker compared to the hydrogen bonds that are prevalent in water.