Question

What is $\text{O}-\text{O}$ bond length in resonance hybrid of ozone?

• A. 131 pm
• B. 121 pm
• C. 128 pm
• D. 148 pm

Hint:

For ozone ($\text{O}_3$), remember that its bond length (128 pm) lies perfectly intermediate between the regular $\text{O}-\text{O}$ single bond (148 pm) and the $\text{O}=\text{O}$ double bond in molecular oxygen (121 pm).

Answer 1

The Correct Option is C

Step 1: Understanding the Question:
The question requires us to recall the experimental oxygen-oxygen bond length present in the resonance hybrid structure of an ozone ($\text{O}_3$) molecule.

Step 2: Detailed Explanation:
The ozone molecule is a resonance hybrid represented primarily by two canonical contributing structures. In these individual contributing structures, one oxygen-oxygen bond is a single bond (typical length around 148 pm) and the other is a double bond (typical length around 121 pm).
\includegraphics[width=0.5\linewidth]{images/4sol.png}
Due to the delocalization of $\pi$-electrons, both bonds in the actual resonance hybrid become completely equivalent, each possessing a bond order of 1.5. Consequently, the experimental bond length is intermediate between a single and a double bond, precisely measuring 128 pm for both bonds.

Step 3: Final Answer:
The $\text{O}-\text{O}$ bond length in the resonance hybrid of ozone is 128 pm, which corresponds to option (C).