S[tex]O_{2}[/tex] has a larger dipole moment than S[tex]O_{3}[/tex].
Both have δ+ S and δ- O atoms. S[tex]O_{2}[/tex] is bent leading to the dipole shown.
S[tex]O_{3}[/tex] is trigonal planar so that the individual dipoles on the S-O bonds cancel and the molecule has no dipole moment.
What is dipole moment in chemistry and its application?
If +q amount positive charge separated by −q amount of negative charge by the bond distance l, then dipole moment (μ) of polar molecule = q × l. Perfectly non-polar molecules like hydrogen, oxygen, and nitrogen have zero dipole moment. The polar molecules like water, ammonia, and methane have positive values.
Why is dipole moment important?
The significance/applications of dipole moment are as follows: Dipole moment is useful in finding the polar nature of the chemical bond: As the magnitude of dipole moment increases, the polar nature of the bond increases. Molecules with zero dipole moment are non-polar in nature.
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