Question

The correct formal charges on oxygen atoms numbered \(2,1\) and \(3\), respectively, are:

• A. \(-1,0,+1\)
• B. \(0,0,0\)
• C. \(0,+1,-1\)
• D. \(+1,0,-1\)

Hint:

In ozone, the central oxygen generally has \(+1\) formal charge and the single bonded terminal oxygen has \(-1\) formal charge.

Answer 1

The Correct Option is C

To determine the formal charges on the oxygen atoms numbered \(2, 1,\) and \(3\), we use the formula for calculating formal charge:

\(\text{Formal Charge} = \text{Valence Electrons} - (\text{Non-bonding Electrons} + \frac{1}{2}\text{Bonding Electrons})\)

 

Here is the step-by-step calculation for each oxygen atom:

1. Oxygen 2:
   - Valence electrons = 6 (for oxygen)
   - Non-bonding electrons = 4
   - Bonding electrons = 4 (2 bonds, each contributing 2 electrons)
   \(\text{Formal Charge} = 6 - (4 + \frac{4}{2}) = 6 - 6 = 0\)
2. Oxygen 1:
   - Valence electrons = 6
   - Non-bonding electrons = 2
   - Bonding electrons = 6 (3 bonds, each contributing 2 electrons)
   \(\text{Formal Charge} = 6 - (2 + \frac{6}{2}) = 6 - 5 = +1\)
3. Oxygen 3:
   - Valence electrons = 6
   - Non-bonding electrons = 6
   - Bonding electrons = 2 (1 bond, contributing 2 electrons)
   \(\text{Formal Charge} = 6 - (6 + \frac{2}{2}) = 6 - 7 = -1\)

Thus, the formal charges on the oxygen atoms numbered \(2, 1,\) and \(3\) are \(0, +1, -1\), respectively.