Three nonequivalent resonance structures for the chlorate ion are shown here. Assign formal charges to all atoms in the resonance structures and identify the more likely resonance structure.
\underset{A}{\left[\begin{matrix} :\overset{..}{\underset{|}{O}:} \\ :\overset{..}{\underset{..}{O}}- \underset{..}{Cl}- \overset{..}{\underset{..}{O}}: \end{matrix} \right]^{-} }\longleftrightarrow \underset{B}{\left[\begin{matrix} :\underset{||}{O}: \\ :\overset{..}{\underset{..}{O}}-\underset{..}{Cl}=\overset{..}{\underset{..}{O}} \end{matrix} \right]^{-} } \longleftrightarrow\underset{C}{ \left[\begin{matrix} :\underset{||}{O}: \\ \overset{..}{\underset{..}{O}}= \underset{..}{Cl}=\overset{..}{\underset{..}{O}} \end{matrix} \right]^{-} }You are asked to use formal charge to identify the most likely resonance structure of those given for a polyatomic ion.
You are given three valid resonance structures.
Formal charges:
Structure B is the most likely resonance structure. The formal charges in B are close to zero, and the highly electronegative oxygen atom carries a −1 formal charge. Structure A is unlikely because of the large positive formal charge on chlorine. Structure C is unlikely because the least electronegative element in the ion (chlorine) has a negative formal charge while the most electronegative element in the ion (oxygen) has a formal charge of zero.