Which of the following statements correctly describes the Lewis dot structure for the neutral dinitrogen monoxide (N2O) molecule?

• A. The central atom is nitrogen, with a triple bond to one nitrogen and a single bond to oxygen.
• B. The molecule has a linear structure with all atoms connected by single bonds.
• C. The central atom is oxygen, with single bonds to each nitrogen atom.
• D. The two nitrogen atoms are bonded to each other by a single bond, and both are singly bonded to oxygen.

Answer: (A)

Verified step by step guidance

1. Step 1: Identify the total number of valence electrons in the N2O molecule. Nitrogen has 5 valence electrons and oxygen has 6 valence electrons. Since there are two nitrogen atoms and one oxygen atom, calculate the total valence electrons as: \$2 \times 5 + 6 = 16$ electrons.
2. Step 2: Determine the central atom. In N2O, nitrogen is less electronegative than oxygen, so nitrogen is typically the central atom. This means the structure will have nitrogen in the center bonded to the other nitrogen and oxygen atoms.
3. Step 3: Arrange the atoms linearly as N–N–O or N–O–N and try to distribute the 16 valence electrons to satisfy the octet rule for each atom. Consider multiple bonding possibilities (single, double, triple bonds) to achieve full octets.
4. Step 4: Evaluate bonding patterns. A common and stable Lewis structure for N2O has the central nitrogen atom forming a triple bond with one nitrogen atom and a single bond with the oxygen atom. This arrangement satisfies the octet rule and accounts for all valence electrons.
5. Step 5: Confirm the molecular geometry. The Lewis structure with the central nitrogen atom triple bonded to nitrogen and single bonded to oxygen results in a linear molecule, consistent with experimental observations.