Which resonance structure is likely to contribute most to the correct structure of N_2O?

• A. N–N≡O with a positive formal charge on oxygen and a negative formal charge on the terminal nitrogen
• B. N–N–O with all atoms neutral and only single bonds
• C. N=N=O with a positive formal charge on the terminal nitrogen and a negative formal charge on oxygen
• D. N≡N–O with a positive formal charge on the central nitrogen and a negative formal charge on oxygen

Answer: (D)

Verified step by step guidance

1. Step 1: Understand that resonance structures are different Lewis structures for the same molecule that differ only in the placement of electrons, not atoms. The most significant resonance contributor is usually the one with the lowest formal charges and the most stable arrangement of charges.
2. Step 2: Calculate the formal charges for each atom in the given resonance structures using the formula: \(\text{Formal charge} = \text{Valence electrons} - \text{Nonbonding electrons} - \frac{1}{2} \times \text{Bonding electrons}\).
3. Step 3: Evaluate each resonance structure by checking the formal charges on atoms, aiming for structures where formal charges are minimized and negative charges reside on more electronegative atoms (like oxygen).
4. Step 4: Consider the bonding patterns and the octet rule for each atom. Structures that satisfy the octet rule for all atoms and have appropriate bond orders are generally more stable.
5. Step 5: Compare all resonance structures based on formal charges, octet fulfillment, and electronegativity considerations to determine which resonance structure contributes most to the actual electronic structure of N\(_2\)O.