---
title: "Three candidate Lewis electron-dot structures for the dinitrogen monoxide molecule, \\(\\text{N}_2\\text{O}\\), are shown below.  Which of the following identifies the structure that contributes most to the actual electron distribution in \\(\\text{N}_2\\text{O}\\) and provides the correct justification?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/119582/"
date_modified: "2026-08-21T06:54:02+00:00"
---

# Three candidate Lewis electron-dot structures for the dinitrogen monoxide molecule, \(\text{N}_2\text{O}\), are shown below.

Which of the following identifies the structure that contributes most to the actual electron distribution in \(\text{N}_2\text{O}\) and provides the correct justification?

Three candidate Lewis electron-dot structures for the dinitrogen monoxide molecule, \(\text{N}_2\text{O}\), are shown below.

Which of the following identifies the structure that contributes most to the actual electron distribution in \(\text{N}_2\text{O}\) and provides the correct justification?

![Three distinct Lewis electron-dot diagrams labeled Structure 1, Structure 2, and Structure 3 are arranged horizontally in a single row from left to right. Structure 1 on the left shows three linear atoms: a left terminal N, a central N, and a right terminal O. The left N is connected to the central N by a triple bond (three parallel horizontal lines) and has exactly one lone pair (two dots to its left). The central N has zero lone pairs. The central N is connected to the right O by a single bond (one horizontal line). The right O has exactly three lone pairs: two dots above, two dots below, and two dots to its right. Structure 2 in the center shows three linear atoms: a left terminal N, a central N, and a right terminal O. The left N is connected to the central N by a double bond (two parallel horizontal lines) and has exactly two lone pairs (two dots above, two dots to the left; no dots below). The central N has zero lone pairs. The central N is connected to the right O by a double bond (two parallel horizontal lines). The right O has exactly two lone pairs (two dots above, two dots to the right; no dots below). Structure 3 on the right shows three linear atoms: a left terminal N, a central N, and a right terminal O. The left N is connected to the central N by a single bond (one horizontal line) and has exactly three lone pairs: two dots above, two dots below, and two dots to its left. The central N has zero lone pairs. The central N is connected to the right O by a triple bond (three parallel horizontal lines). The right O has exactly one lone pair (two dots to its right). All text and symbols are black on a white background. No other particles, labels, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787295242-scYMpT.jpg)

- **A.** Structure 2, because having two double bonds distributes electron density symmetrically across the molecule.
- **B.** Structure 2, because placing a formal charge of \(0\) on the oxygen atom results in a more stable, uncharged oxygen center.
- **C.** Structure 1, because the nitrogen-nitrogen triple bond has a higher bond energy than a double bond, resulting in the lowest potential energy.
- **D.** Structure 1, because the formal charges on all atoms are minimized and the negative formal charge resides on the more electronegative oxygen atom.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119582/*