(c) What would you predict for the lengths of the bonds in NO₂^- relative to N¬O single bonds and double bonds?

Verified step by step guidance

1. Understand the structure of the NO2- ion: The NO2- ion is known as the nitrite ion. It consists of one nitrogen atom bonded to two oxygen atoms, with a negative charge distributed across the molecule.
2. Consider resonance structures: NO2- has resonance structures, which means the negative charge and the bonding electrons are delocalized over the molecule. This results in bond lengths that are intermediate between a single and a double bond.
3. Compare bond types: A single N-O bond is typically longer than a double N-O bond due to the difference in electron sharing and bond strength. Double bonds involve more electron sharing, leading to shorter bond lengths.
4. Predict bond lengths in NO2-: Due to resonance, the N-O bonds in NO2- are neither purely single nor purely double bonds. They are expected to be shorter than a typical N-O single bond but longer than a typical N-O double bond.
5. Conclude with bond order: The bond order in NO2- is approximately 1.5, indicating that the bond lengths are intermediate between single and double bonds, reflecting the partial double bond character due to resonance.