---
title: "A student compares the following Lewis structures for nitrous oxide, \\(\\text{N}_2\\text{O}\\), which has the atom connectivity \\(\\text{N}-\\text{N}-\\text{O}\\).  Structure I: \\(\\text{N}\\equiv\\text{N}-\\text{O}\\), with one lone pair on the terminal nitrogen atom, no lone pairs on the central nitrogen atom, and three lone pairs on the oxygen atom.  Structure II: \\(\\text{N}=\\text{N}=\\text{O}\\), with two lone pairs on the terminal nitrogen atom, no lone pairs on the central nitrogen atom, and two lone pairs on the oxygen atom.  Each structure uses 16 valence electrons and gives every atom an octet. Which statement correctly identifies the favored Lewis structure and justifies the choice using formal charges?"
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date_modified: "2026-08-19T12:40:09+00:00"
---

# A student compares the following Lewis structures for nitrous oxide, \(\text{N}_2\text{O}\), which has the atom connectivity \(\text{N}-\text{N}-\text{O}\).

Structure I: \(\text{N}\equiv\text{N}-\text{O}\), with one lone pair on the terminal nitrogen atom, no lone pairs on the central nitrogen atom, and three lone pairs on the oxygen atom.

Structure II: \(\text{N}=\text{N}=\text{O}\), with two lone pairs on the terminal nitrogen atom, no lone pairs on the central nitrogen atom, and two lone pairs on the oxygen atom.

Each structure uses 16 valence electrons and gives every atom an octet. Which statement correctly identifies the favored Lewis structure and justifies the choice using formal charges?

A student compares the following Lewis structures for nitrous oxide, \(\text{N}_2\text{O}\), which has the atom connectivity \(\text{N}-\text{N}-\text{O}\).

Structure I: \(\text{N}\equiv\text{N}-\text{O}\), with one lone pair on the terminal nitrogen atom, no lone pairs on the central nitrogen atom, and three lone pairs on the oxygen atom.

Structure II: \(\text{N}=\text{N}=\text{O}\), with two lone pairs on the terminal nitrogen atom, no lone pairs on the central nitrogen atom, and two lone pairs on the oxygen atom.

Each structure uses 16 valence electrons and gives every atom an octet. Which statement correctly identifies the favored Lewis structure and justifies the choice using formal charges?

- **A.** Structure II is favored. Its formal charges on the terminal nitrogen, central nitrogen, and oxygen atoms are \(-1\), \(+1\), and \(0\), respectively, because avoiding a negative formal charge on oxygen produces the more favorable structure.
- **B.** Structure II is favored. Its formal charges on the terminal nitrogen, central nitrogen, and oxygen atoms are all \(0\), so it is favored because it has no charge separation.
- **C.** Structure I is favored. Its formal charges on the terminal nitrogen, central nitrogen, and oxygen atoms are \(0\), \(+1\), and \(-1\), respectively, because a structure containing a triple bond is always favored over one containing two double bonds.
- **D.** Structure I is favored. Its formal charges on the terminal nitrogen, central nitrogen, and oxygen atoms are \(0\), \(+1\), and \(-1\), respectively, because the negative formal charge is located on the more electronegative atom.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119403/*