Question
Although both $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}$ are triatomic molecules, the shape of $\mathrm{H}_2 \mathrm{O}$ molecule is bent while that of $\mathrm{CO}_2$ is linear. Explain this on the basis of dipole moment.
✓
Answer
According to experimental results, the dipole moment of carbon dioxide is zero. This is possible only if the molecule is linear so that the dipole moments of $\mathrm{C}-\mathrm{O}$ bonds are equal and opposite to nullify each other.
Resultant μ = 0 D
$\mathrm{H}_2 \mathrm{O}$, on the other hand, has a dipole moment value of 1.84 D (though it is a triatomic molecule as $\mathrm{CO}_2$ ). The value of the dipole moment suggests that the structure of $\mathrm{H}_2 \mathrm{O}$ molecule is bent where the dipole moment of $\mathrm{O}-\mathrm{H}$ bonds are unequal.
Resultant μ = 0 D
$\mathrm{H}_2 \mathrm{O}$, on the other hand, has a dipole moment value of 1.84 D (though it is a triatomic molecule as $\mathrm{CO}_2$ ). The value of the dipole moment suggests that the structure of $\mathrm{H}_2 \mathrm{O}$ molecule is bent where the dipole moment of $\mathrm{O}-\mathrm{H}$ bonds are unequal.
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