Calculate the formal charges for each of the oxygen atoms within the nitrite ion, NO₂^–.

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

Answer: (A)

Verified step by step guidance

1. Identify the formula for calculating formal charge: \(\text{Formal Charge} = \text{Valence Electrons} - (\text{Nonbonding Electrons} + \frac{1}{2} \times \text{Bonding Electrons})\).
2. Determine the number of valence electrons for oxygen, which is 6.
3. For oxygen atom A (double bonded to nitrogen): Count the nonbonding electrons (lone pairs) and bonding electrons (shared in bonds). Here, oxygen A has 4 nonbonding electrons and shares 4 bonding electrons (double bond).
4. Calculate the formal charge for oxygen A using the formula: \(6 - (4 + \frac{1}{2} \times 4)\).
5. For oxygen atom B (single bonded to nitrogen): Count the nonbonding electrons (6 electrons) and bonding electrons (2 electrons from single bond). Calculate the formal charge for oxygen B: \(6 - (6 + \frac{1}{2} \times 2)\).