Given the structure of $O_3$ (ozone) as $O=O-O$, which of the following is a correct resonance structure?

• A. $O-O-O$
• B. $O\equiv O-O$
• C. $O-O=O$
• D. $O=O=O$

Answer: (C)

Verified step by step guidance

1. Step 1: Understand the structure of ozone (O\_3). Ozone is a molecule with three oxygen atoms connected in a bent shape, and it exhibits resonance, meaning the actual structure is a hybrid of multiple Lewis structures.
2. Step 2: Recall that in resonance structures, the total number of valence electrons and the overall charge must remain the same. For ozone, there are 18 valence electrons (6 from each oxygen atom).
3. Step 3: Draw possible Lewis structures by arranging single and double bonds between the oxygen atoms, ensuring that each oxygen has a complete octet and the total electrons count is correct. Also, assign formal charges to check the stability of each resonance form.
4. Step 4: Evaluate the given options by checking if they satisfy the octet rule, have reasonable formal charges (preferably zero or minimal charges), and maintain the total number of electrons. Structures with two double bonds or all single bonds usually violate these rules or have unfavorable charges.
5. Step 5: Identify the correct resonance structure as the one where one oxygen-oxygen bond is a double bond, the other is a single bond, and the formal charges are minimized, matching the known resonance contributors of ozone.