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

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Solution

The dipole moment is the product of the magnitude of the positive or negative charge (q) & the distance (d) between the charges,i.e
$μ = q \times d .$
The SI unit is coulomb meter. The molecule with symmetrical & linear geometries has zero dipole moment because they are the vector in nature & the dipole of different bonds cancels with one another.
$C O_{2}$ is symmetrical & has dipole moment 0.Therefore it will have a linear shape with a bond angle 180°.
So, Resultant μ = 0 D
$H_{2} O$ is an unsymmetrical molecule & bent geometries, the geometries have a specific dipole moment (1.84D) because the bond polarities do not cancel each other. Therefore $H_{2} O$ will have a bent structure with bond angle 104°.

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