Which of the following species requires a resonance hybrid...

Which of the following species requires a resonance hybrid for its Lewis structure: (a) $\mathrm{CO}_{2},$ (b) $\mathrm{OCl}^{-}$ (c) $\mathrm{CO}_{3}^{2-},$ or $(\mathrm{d}) \mathrm{OH}^{-} ?$ Explain.

Key Concepts

Formal Charge

Formal charge is a concept used to assign charges to individual atoms in a molecule based on the difference between the number of valence electrons in the free atom and those assigned in the Lewis structure. Assessing formal charge across multiple resonance forms helps in determining the most stable electron configuration for a molecule or ion.

Delocalization of Electrons

Delocalization of electrons refers to the phenomenon where electrons are spread over several atoms instead of being confined between two atoms. This spread helps stabilize molecules by reducing charge concentration and is a key reason why resonance hybrids are used in describing certain chemical species.

Resonance Hybrid

A resonance hybrid represents the true electronic structure of a molecule or ion when multiple viable Lewis structures (resonance forms) exist. It indicates that the electron density is delocalized over two or more atoms rather than being fixed in a single location, which provides extra stability to the species.

Lewis Structure

A Lewis structure is a diagram that shows the arrangement of electrons in a molecule, including bonding pairs and lone pairs. It is a critical tool for predicting the molecular shape, reactivity, and distribution of electrons, and it sometimes requires multiple representations to fully depict delocalized electron systems.

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