Although both $CO_{2}$ and $H_{2}O$ are triatomic molecules,the shape of $H_{2}O$ molecule is bent while that of $CO_{2}$ is linear. Explain this on the basis of dipole moment.

(N/A) According to experimental results,the dipole moment of carbon dioxide $(CO_{2})$ is zero. This is possible only if the molecule is linear,so that the dipole moments of the two $C=O$ bonds are equal in magnitude and opposite in direction,thereby nullifying each other. Resultant $\mu = 0 \, D$.
On the other hand,$H_{2}O$ has a dipole moment of $1.84 \, D$. This non-zero value indicates that the $H_{2}O$ molecule is bent. In this structure,the dipole moments of the two $O-H$ bonds do not cancel each other out,and the presence of lone pairs on the oxygen atom further contributes to the net dipole moment.