---
title: "Three possible resonance structures for the cyanate ion, \\(\\text{OCN}^-\\), are shown in the diagram below.  Based on formal charge principles and electronegativity, which of the following correctly identifies the structure that contributes most to the resonance hybrid of the cyanate ion and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/121438/"
date_modified: "2026-08-23T05:02:22+00:00"
---

# Three possible resonance structures for the cyanate ion, \(\text{OCN}^-\), are shown in the diagram below.

Based on formal charge principles and electronegativity, which of the following correctly identifies the structure that contributes most to the resonance hybrid of the cyanate ion and provides the correct justification?

Three possible resonance structures for the cyanate ion, \(\text{OCN}^-\), are shown in the diagram below.

Based on formal charge principles and electronegativity, which of the following correctly identifies the structure that contributes most to the resonance hybrid of the cyanate ion and provides the correct justification?

![Three resonance structures arranged horizontally from left to right in grayscale line-art format. Structure 1 on the left shows O double-bonded to C and C double-bonded to N. The O atom has 2 lone pairs (one top, one left; none below or right). The central C atom has no lone pairs. The N atom has 2 lone pairs (one top, one right; none below or left). The entire structure is enclosed in square brackets with a superscript '-' outside the top right, labeled 'Structure 1' underneath. Structure 2 in the middle shows O triple-bonded to C and C single-bonded to N. The O atom has 1 lone pair (left; none top, bottom, or right). The central C atom has no lone pairs. The N atom has 3 lone pairs (one top, one right, one bottom; none left). The structure is in square brackets with superscript '-', labeled 'Structure 2' underneath. Structure 3 on the right shows O single-bonded to C and C triple-bonded to N. The O atom has 3 lone pairs (one top, one left, one bottom; none right). The central C atom has no lone pairs. The N atom has 1 lone pair (right; none top, bottom, or left). The structure is in square brackets with superscript '-', labeled 'Structure 3' underneath. No other particles, labels, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787461341-7la9lv.jpg)

- **A.** Structure 1, because the two double bonds create a symmetrical electron distribution that minimizes electron-electron repulsions.
- **B.** Structure 2, because the triple bond between carbon and oxygen maximizes the overall bond energy of the ion.
- **C.** Structure 3, because the \(-1\) formal charge is located on the oxygen atom, which is more electronegative than nitrogen.
- **D.** Structure 3, because the central carbon atom has a formal charge of \(-1\), which is effectively stabilized by the adjacent triple bond.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121438/*