The chlorite ion, ClO2−, exhibits important atmospheric chemistry. Two distinct Lewis structures are proposed, each satisfying the molecular formula and charge.
Structure M: Cl is singly bonded to two O atoms; one O atom bears a full negative charge, and the overall ion charge resides entirely on oxygen. Chlorine possesses one lone pair.
Structure N: Cl forms one double bond (Cl=O) and one single bond (Cl−O) with the two oxygen atoms. In this representation, the negative charge is delocalized through resonance between the two O atoms.
(a) For Structure M, calculate the formal charge on every atom.
(b) For Structure N, calculate the formal charge on every atom.
(c) Evaluate which structure better represents the chlorite ion by discussing formal-charge minimization and the placement of negative charge on the more electronegative element.
(d) Predict whether the real chlorite ion is best described by a single dominant contributor or by resonance among multiple contributors, and justify your prediction.
(a) Calculate the formal charge on each atom in Structure M.
(b) Calculate the formal charge on each atom in Structure N.
(c) Determine which structure is more favorable, citing specific formal-charge considerations.
(d) Discuss whether the chlorite ion is best represented by a single Lewis contributor or by a resonance hybrid, providing justification.