Question

Find the formal charge of \( O \), \( O \), \( O \), and \( N \) respectively.

• A. 0, +1, -1, +2
• B. -1, -1, 0, +1
• C. -1, 0, +2, +1
• D. +1, -1, 0, -1

Hint:

When calculating formal charges, keep track of the valence electrons, lone pairs, and bonds for each atom involved.

Answer 1

The Correct Option is C

To find the formal charges of the atoms in the given molecule, we need to use the formula for formal charge:

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

Let's analyze the Lewis structure in the image:

1. Oxygen (I):
   • Valence electrons = 6
   • Non-bonding electrons = 6
   • Bonding electrons = 2 (one single bond with N)
2. Oxygen (II):
   • Valence electrons = 6
   • Non-bonding electrons = 4
   • Bonding electrons = 4 (two bonds with N)
3. Oxygen (III):
   • Valence electrons = 6
   • Non-bonding electrons = 2
   • Bonding electrons = 6 (three bonds with N)
4. Nitrogen (N):
   • Valence electrons = 5
   • Non-bonding electrons = 0 (all are used in bonding)
   • Bonding electrons = 8 (one bond with O(I), two with O(II), three with O(III))

Thus, the formal charges are: -1, 0, +2, +1 for O, O, O, and N respectively.