Chlorine dioxide, ClO₂(g), is an industrial bleaching agent that contains an odd number of valence electrons.
(a) Calculate the total number of valence electrons that must be represented in a Lewis diagram for ClO₂.
(b) Draw a single, most reasonable Lewis structure for ClO₂ that includes the unpaired electron and shows any expanded octet if present.
(c) The measured O–Cl–O bond angle in ClO₂ is 118°. Relate this angle to the electron-domain geometry predicted by a Lewis diagram and explain why it deviates from the idealized value.
(d) Discuss how the placement of the unpaired electron and the ability of chlorine to exceed an octet influence the formal charge distribution in your structure from part (b).