Which compound among the following has the highest dipole moment?

The dipole moment depends on the charge and distance between the central atom and side atoms. But the charge is more prominent than distance. It is determined as polar and non-polar molecules

It is used for covalent or ionic molecule

${\mathrm{\mu }}_{\mathrm{net}} = 0$ It is for non-polar molecule

${\mathrm{\mu }}_{\mathrm{net}} \ne 0$ It is for polar molecule

It can be determined by the geometry of the molecule. As, ammonia has trigonal pyramidal shape in which the dipole moment of lone pair balances the moment of bond pair.

In case of ${\mathrm{SO}}_2$, it have bent shape or V-shape has have net dipole moment towards oxygen atom side.

${\mathrm{N}}_2\mathrm{O}$ or ${\mathrm{CO}}_2$ both have the linear shape and so their moment is balanced and so net dipole moment is zero.

Hence, we can conclude that ${\mathrm{SO}}_2$ molecule has a maximum dipole moment.