Question

Polarity in a molecule and hence the dipole moment depends primarily on electronegativity of the constituent atoms and shape of a molecule. Which of the following has the highest dipole moment?

• A. $HI$
• B. $C{O}_2$
• C. $S{O}_2$
• D. $H_{2}O$

Answer 1

The correct option is D $H_{2}O$

Dipole moment measures the polarity in a molecule and is indicated by $\mu$

Structure of each molecule and its dipole moment is given:

$\left(A\right)$ $C{O}_2$ ${\mu }_{net}=0$ $\mu =0$



$\left(B\right)$ $HI$ ${\mu }_{net}\ne 0$ $\mu =0.38D$



$\left(C\right)$ $H_{2}O$ $\mu \ne 0$ $\mu =1.84D$


$\left(D\right)$ $S{O}_2$ $\mu \ne 0$ $\mu =1.62D$

The electronegativity difference between $O$ and $H$ atoms is maximum. So, $H_{2}O$ will have the highest dipole moment $\left(\text{i.e.,}1.84D\right).$

Hence, $\left(C\right)$ is the correct option.