Question

The formal charge on central oxygen atom in ozone is

• A. +1
• B. -1
• C. 0
• D. +2

Answer 1

The Correct Option is A

In ozone (O\(_3\)), the central oxygen atom is bonded to two oxygen atoms. The structure of ozone involves resonance, with one structure showing a double bond between the central oxygen and one oxygen atom and a single bond between the central oxygen and the other oxygen atom. To calculate the formal charge on the central oxygen, we use the formal charge formula: \[ \text{Formal charge} = V - (N + \frac{B}{2}) \] where: 
\( V \) is the number of valence electrons of the atom.
\( N \) is the number of non-bonding electrons on the atom.
\( B \) is the number of electrons shared in bonds with adjacent atoms. For the central oxygen in ozone:
Valence electrons of oxygen = 6 (since oxygen is in group 16).
The central oxygen has one lone pair (2 electrons) and is involved in two bonds, each with 2 electrons (totaling 4 electrons in bonds). So the formal charge is: \[ \text{Formal charge} = 6 - (2 + \frac{6}{2}) = 6 - (2 + 3) = 6 - 5 = +1 \] Thus, the formal charge on the central oxygen atom is +1.

The correct option is (A): +1