Dipole moment depends on both bond polarity and molecular geometry. \(\text{CO}_2\) is linear — two equal and opposite C=O bond dipoles cancel → \(\mu = 0\). \(\text{CCl}_4\) is tetrahedral — four C–Cl dipoles cancel → \(\mu = 0\). \(\text{H}_2\text{O}\) is bent (V-shaped) with bond angle ~104.5° — the two O–H bond dipoles do NOT cancel, giving a net dipole moment of \(\mu \approx 1.85\) D, the highest among the options.