Show all possible resonance structures for each of the...

Show all possible resonance structures for each of the following molecules or ions:
(a) Nitrate ion, $\mathrm{NO}_{3}^{-}$
(b) Nitrous oxide (laughing gas), $\mathrm{N}_{2} \mathrm{O}$ (where the bonding is in the order $\mathrm{N}-\mathrm{N}-\mathrm{O})$

Key Concepts

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule, including bonding and non-bonding electrons. They are the starting point for developing resonance structures by showing all possible electron arrangements that satisfy the octet (or duet) rule.

Formal Charge Distribution

Formal charge is a bookkeeping tool used to assign charge values to atoms within a molecule based on their electron configuration relative to a neutral state. It helps determine the most plausible resonance forms by minimizing charge separation and ensuring the overall charge of the species remains correct.

Bond Order

Bond order denotes the number of chemical bonds between a pair of atoms and provides insight into bond stability and strength. In resonance hybrids, effective bond orders are often fractional because the bonding electrons are distributed over multiple resonance forms, which is critical to understanding the true electronic structure.

Resonance Structures

Resonance structures are different Lewis structures for the same molecule or ion that depict the delocalization of electrons. They illustrate how electron density is distributed across atoms and bonds and contribute to a resonance hybrid that better represents the actual structure of the molecule.

Electron Delocalization

Electron delocalization occurs when electrons are not confined to a single bond or pair of atoms, but are spread out over two or more atoms. This concept explains the stabilization of structures such as the nitrate ion where the negative charge is shared over multiple oxygen atoms.

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