To determine the correct Lewis structure for O₃ (ozone), we need to follow the steps for drawing Lewis structures:

• Step 1: Calculate total valence electrons.
  Each oxygen atom has 6 valence electrons. For O₃, total valence electrons = $3\times 6=18$.
• Step 2: Draw a skeletal structure.
  The three oxygen atoms are connected in a bent arrangement. Let's label them O₁ - O₂ - O₃, where O₂ is the central atom.
• Step 3: Place two electrons between each bonded atom.
  O₁ - O₂ - O₃. This uses $2\times 2=4$ electrons. Remaining electrons = $18-4=14$.
• Step 4: Distribute remaining electrons as lone pairs to terminal atoms first to satisfy octets.
  O₁ needs 6 more electrons (3 lone pairs) to complete its octet. O₃ needs 6 more electrons (3 lone pairs) to complete its octet. This uses $6+6=12$ electrons. Remaining electrons = $14-12=2$.
• Step 5: Place any remaining electrons on the central atom.
  The 2 remaining electrons are placed on the central O₂ atom as one lone pair.
• Step 6: Check octets and form multiple bonds if necessary.
  At this point:
  • O₁ has 2 (bond) + 6 (lone pair) = 8 electrons (octet satisfied).
  • O₂ has 2 (bond) + 2 (bond) + 2 (lone pair) = 6 electrons (octet NOT satisfied).
  • O₃ has 2 (bond) + 6 (lone pair) = 8 electrons (octet satisfied).
  To satisfy the octet of the central O₂ atom, one lone pair from either O₁ or O₃ must be converted into a double bond with O₂. Let's take a lone pair from O₁.
• Step 7: Final Lewis Structure (Resonance).
  This leads to two resonance structures for O₃:
  
  Structure 1: O₁=O₂-O₃
  O₁: 2 lone pairs, 1 double bond (8 electrons)
  O₂: 1 lone pair, 1 double bond, 1 single bond (8 electrons)
  O₃: 3 lone pairs, 1 single bond (8 electrons)
  
  Structure 2: O₁-O₂=O₃
  O₁: 3 lone pairs, 1 single bond (8 electrons)
  O₂: 1 lone pair, 1 double bond, 1 single bond (8 electrons)
  O₃: 2 lone pairs, 1 double bond (8 electrons)
  
  Both resonance structures are valid. The actual structure is a resonance hybrid of these two.

Option Analysis:

• A) This structure shows a triple bond and a single bond. The central oxygen would have 10 electrons (octet violation). Also, the total valence electrons are incorrect.
• B) This structure shows two double bonds. The central oxygen would have 8 electrons, but the terminal oxygens would have 6 electrons each (octet violation).
• C) This option correctly depicts one of the resonance structures of O₃, with a double bond on one side and a single bond on the other, and all atoms satisfying the octet rule. The central oxygen has one lone pair. This matches our derived structure.
• D) This structure shows two single bonds and two lone pairs on the central oxygen, meaning the central oxygen has only 6 electrons (octet violation).

Correct Answer: (C)