Final answer:
CO₃²⁻ (carbonate ion), NO₃⁻ (nitrate ion), and O₃ (ozone) exhibit resonance as they have multiple valid resonance forms. Carbon dioxide (CO₂) does not show resonance as it has a fixed linear structure with two double bonds and no alternative electron distributions.
Step-by-step explanation:
The species among CO₂, CO₃²⁻, NO₃⁻, and O₃ that will exhibit resonance are CO₃²⁻, NO₃⁻, and O₃. Resonance is a concept where more than one valid Lewis structure can be drawn for a particular molecule or ion. In the cases of CO₃²⁻ (carbonate ion), NO₃⁻ (nitrate ion), and O₃ (ozone), there are multiple valid resonance forms that distribute the electrons differently between atoms while the arrangement of the atoms remains the same.
The carbonate ion (CO₃²⁻) has three resonance forms where the double bond can be placed between the carbon and any of the three oxygen atoms, resulting in a bond order of 1.33 for each C-O bond. The nitrate ion (NO₃⁻) also has three resonance structures with the double bond rotating between nitrogen and each of the three oxygen atoms.
Lastly, ozone (O₃) exhibits two resonance forms where the position of the double bond between the oxygen atoms changes. On the other hand, carbon dioxide (CO₂) has a linear structure with two equivalent carbon-oxygen double bonds and does not exhibit resonance as there is no alternative way to distribute the electrons while preserving the molecular structure.
Therefore, the correct answer is (d) CO₃²⁻, NO₃⁻, and O₃.