Which compound among the following has the hi | vedclass

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(B) The dipole moment $(\mu)$ is a vector quantity that depends on the polarity of bonds and the geometry of the molecule.
$CO_2$ and $N_2O$ are line

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$SO_2$

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(B) The dipole moment $(\mu)$ is a vector quantity that depends on the polarity of bonds and the geometry of the molecule.
$CO_2$ and $N_2O$ are linear molecules with symmetric charge distribution,resulting in a net dipole moment of $\mu = 0 \ D$.
$NH_3$ has a trigonal pyramidal geometry with a lone pair on the nitrogen atom. The dipole moments of the $N-H$ bonds and the lone pair reinforce each other,giving it a dipole moment of approximately $1.47 \ D$.
$SO_2$ has a bent ($V$-shaped) geometry due to the presence of a lone pair on the sulfur atom. The bond dipoles of the $S=O$ bonds do not cancel out,resulting in a net dipole moment of approximately $1.63 \ D$.
Comparing the values,$SO_2$ has the highest dipole moment among the given options.

Which compound among the following has the highest dipole moment?

Similar Questions

Which of the following is non-polar?

Assertion : Molecules of larger size have higher polarizability.
Reason : Polarizability is observed only in those molecules which have a permanent dipole moment.

The correct order of dipole moment for the following molecules is:

Which of the following is a polar compound?

Which among the following molecules is non-polar?

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