Question

Angular shape of ozone molecule consist of:

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

Hint:

Even though the true structure of ozone is a resonance hybrid where both O-O bond lengths are equal, the total count of localized $\sigma$ and $\pi$ bonds in its valid Lewis representations remains 2 $\sigma$ bonds and 1 $\pi$ bond.

Answer 1

The Correct Option is D

Step 1: Understanding the Concept:
The ozone molecule (\( \text{O}_3 \)) consists of three oxygen atoms.
To understand its bonding scheme and geometry, we look at its chemical structure and localized resonance forms.

Step 2: Key Formula or Approach:
An ozone molecule has a central oxygen atom bonded to two terminal oxygen atoms.
The molecule has a bent or angular geometry due to the presence of a lone pair on the central oxygen atom.

Step 3: Detailed Explanation:
In the basic Lewis structure of ozone, the central oxygen atom forms a single covalent bond with one terminal oxygen atom and a double covalent bond with the other terminal oxygen atom.
- A single bond contains exactly $1$ $\sigma$ (sigma) bond.
- A double bond contains exactly $1$ $\sigma$ (sigma) bond and $1$ $\pi$ (pi) bond.
Summing up the localized bonds in the framework:
\[ \text{Total } \sigma \text{ bonds} = 1 + 1 = 2 \]
\[ \text{Total } \pi \text{ bonds} = 1 \]
Thus, the angular skeletal structure of ozone is composed of 2 sigma ($\sigma$) and 1 pi ($\pi$) bonds.

Step 4: Final Answer:
The angular shape of an ozone molecule consists of 2 sigma and 1 pi-bonds.