In the Lewis dot structure of the neutral compound N2O, which atom is the central atom, and what is its formal charge?

• A. Nitrogen (N) is the central atom with a formal charge of +1.
• B. Oxygen (O) is the central atom with a formal charge of -1.
• C. Oxygen (O) is the central atom with a formal charge of 0.
• D. Nitrogen (N) is the central atom with a formal charge of 0.

Answer: (A)

Verified step by step guidance

1. Identify the atoms present in N2O: two nitrogen (N) atoms and one oxygen (O) atom. Since oxygen is more electronegative and usually terminal, nitrogen is often the central atom in such molecules.
2. Draw possible Lewis structures by arranging the atoms with nitrogen in the center and oxygen at one end, then distribute the valence electrons to satisfy the octet rule for each atom.
3. Calculate the formal charge for each atom using the formula: \(\text{Formal Charge} = \text{Valence Electrons} - \text{Nonbonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons}\).
4. Compare the formal charges for each atom in the different Lewis structures to find the most stable arrangement, which usually has formal charges closest to zero and negative charges on the more electronegative atoms.
5. Conclude that the nitrogen atom in the center has a formal charge of +1, and the oxygen atom has a formal charge of -1, making this the most reasonable Lewis structure for N2O.