Question

Which of the following statement is not correct about the structures of ozone and sulphur dioxide?

• A. Both have angular shape
• B. Both have resonance structures
• C. Both have same hybridization
• D. Both have same bond angles

Hint:

Ozone and sulphur dioxide are both bent molecules with resonance, but their bond angles are not exactly equal.

Answer 1

The Correct Option is D

Step 1: Compare ozone and sulphur dioxide.
We must find the statement that is NOT correct about $O_3$ and $SO_2$. So we test each claim about their shape, resonance, hybridization, and bond angle.
Step 2: Check the shape.
Both molecules have a lone pair on the central atom, which bends them. So both are angular (bent). That statement is correct.
Step 3: Check resonance.
Both $O_3$ and $SO_2$ have two equivalent resonance structures where the double bond shifts side to side. So both show resonance. That statement is correct.
Step 4: Check hybridization.
The central atom in each is $sp^2$ hybridized (three electron regions). So both have the same hybridization. That statement is correct.
Step 5: Check the bond angles.
The angle in $O_3$ is about $117^\circ$, while in $SO_2$ it is about $119^\circ$. These are not the same. So the claim that they have the same bond angle is wrong.
Step 6: State the incorrect statement.
The statement that is not correct is \[ \boxed{\text{Both have same bond angles}} \]