Which set of formal charges correctly corresponds to the three major resonance forms of $N_{2}O$ (nitrous oxide), written as $N-N-O$?

• A. Form 1: $N$ (left) = 0, $N$ (center) = $+1$, $O$ = $-1$; Form 2: $N$ (left) = $-1$, $N$ (center) = $+1$, $O$ = 0; Form 3: $N$ (left) = 0, $N$ (center) = 0, $O$ = 0
• B. Form 1: $N$ (left) = 0, $N$ (center) = 0, $O$ = 0; Form 2: $N$ (left) = $+1$, $N$ (center) = $-1$, $O$ = 0; Form 3: $N$ (left) = 0, $N$ (center) = $+1$, $O$ = $-1$
• C. Form 1: $N$ (left) = $+1$, $N$ (center) = 0, $O$ = $-1$; Form 2: $N$ (left) = 0, $N$ (center) = $-1$, $O$ = $+1$; Form 3: $N$ (left) = $-1$, $N$ (center) = 0, $O$ = $+1$
• D. Form 1: $N$ (left) = 0, $N$ (center) = $+1$, $O$ = $-1$; Form 2: $N$ (left) = $-1$, $N$ (center) = $+1$, $O$ = 0; Form 3: $N$ (left) = 0, $N$ (center) = 0, $O$ = 0

Answer: (A)

Verified step by step guidance

1. Step 1: Draw the Lewis structure of nitrous oxide (N\_2O) with the atoms arranged as N - N - O, and count the total number of valence electrons. Nitrogen has 5 valence electrons and oxygen has 6, so total electrons = 5 + 5 + 6 = 16 electrons.
2. Step 2: Draw the three major resonance structures by distributing the electrons to satisfy the octet rule as much as possible, while varying the placement of double and triple bonds and lone pairs between the atoms.
3. Step 3: For each resonance structure, calculate the formal charge on each atom using the formula: \(\text{Formal Charge} = \text{Valence Electrons} - (\text{Nonbonding Electrons} + \frac{1}{2} \times \text{Bonding Electrons})\).
4. Step 4: Assign the formal charges to the left nitrogen, center nitrogen, and oxygen atoms in each resonance form based on your calculations from Step 3.
5. Step 5: Compare the formal charges across the resonance forms to identify the set that matches the given correct answer: Form 1 with left N = 0, center N = +1, O = -1; Form 2 with left N = -1, center N = +1, O = 0; and Form 3 with all atoms having formal charge 0.