Which of the following molecules contains delocalized electrons due to resonance?

• A. Ammonia (NH_3)
• B. Ozone (O_3)
• C. Carbon dioxide (CO_2)
• D. Methane (CH_4)

Answer: (C)

Verified step by step guidance

1. Understand the concept of resonance: Resonance occurs when a molecule can be represented by two or more valid Lewis structures that differ only in the placement of electrons, particularly pi electrons or lone pairs, leading to delocalized electrons over multiple atoms.
2. Analyze each molecule's Lewis structure to identify if resonance is possible:
3. For Ammonia (NH_3), draw the Lewis structure showing nitrogen bonded to three hydrogens with a lone pair on nitrogen. Since there are no multiple bonds or alternative electron placements, resonance is not present.
4. For Ozone (O_3), draw the Lewis structures showing the arrangement of three oxygen atoms with alternating single and double bonds and lone pairs. Multiple valid resonance structures exist where the double bond shifts between different oxygen atoms, indicating delocalized electrons.
5. For Carbon dioxide (CO_2) and Methane (CH_4), draw their Lewis structures. Both have fixed double or single bonds without alternative resonance forms, so no delocalized electrons due to resonance are present.