Question

Angular shape of ozone molecule consists of

• A. 1 sigma and 2 pi-bonds
• B. 2 sigma and 2 pi-bonds
• C. 1 sigma and 1 pi-bond
• D. 2 sigma and 1 pi-bond

Hint:

For molecules like ozone with resonance structures, count sigma bonds individually but pi bonds collectively based on resonance. Always consider delocalization in calculating actual bond characteristics.

Answer 1

The Correct Option is D

Step 1: Understanding the structure of ozone (\( O_3 \))
Ozone is a triatomic molecule consisting of three oxygen atoms.
Its structure is angular (bent) and not linear due to the presence of lone pairs on the central oxygen atom. 
Step 2: Bonding in Ozone
Ozone has a resonance structure between \( O=O-O \) and \( O-O=O \).
The actual structure is a resonance hybrid where the double bond character is delocalized between the two bonds.
This means that one pi bond is delocalized over two oxygen atoms, and both O–O bonds have bond orders between a single and a double bond (about 1.5 each). 
Step 3: Sigma and Pi Bond Count
Each O–O bond contains one sigma bond. There are 2 O–O bonds.
One pi bond is delocalized over these two bonds. So, total = 2 sigma bonds and 1 pi bond. \[ \text{Total bonding} = 2\sigma + 1\pi \] Hence, the correct answer is option (4).