Which of the following correctly describes the resonance structures of the nitrite ion, NO_2^-?

• A. NO_2^- has three resonance structures, each with a different atom carrying the negative charge.
• B. NO_2^- does not exhibit resonance because all bonds are equivalent.
• C. NO_2^- has two major resonance structures, each with one oxygen atom double-bonded to nitrogen and the other oxygen atom single-bonded with a negative charge.
• D. NO_2^- has only one resonance structure with both oxygen atoms single-bonded to nitrogen and each carrying a negative charge.

Answer: (C)

Verified step by step guidance

1. Recall that resonance structures are different Lewis structures for the same molecule that differ only in the placement of electrons, not atoms.
2. Draw the Lewis structure of the nitrite ion (NO_2^-), counting total valence electrons: nitrogen has 5, each oxygen has 6, and there is 1 extra electron due to the negative charge, totaling 18 electrons.
3. Arrange the atoms with nitrogen in the center bonded to two oxygen atoms, then distribute electrons to satisfy the octet rule, considering possible double bonds and formal charges.
4. Identify possible resonance structures by moving the double bond between nitrogen and one oxygen to the other oxygen, resulting in two major resonance forms where one oxygen is double-bonded and the other is single-bonded with a negative charge.
5. Evaluate the resonance structures by checking formal charges and bond equivalency; the correct description involves two major resonance structures with one oxygen double-bonded and the other single-bonded carrying the negative charge.