All non-bonding electrons and nonzero formal charges should be included in the structure. What is the most stable resonance structure if oxygen is the central atom in the CON-ion? 120 H C CI :c=0N:

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
icon
Related questions
icon
Concept explainers
Question
**Title: Understanding Resonance Structures and Formal Charges**

**Introduction:**

In this section, we explore how to determine the most stable resonance structure for a given ion.

**Resonance Structures and Formal Charges:**

*Statement:*
"All non-bonding electrons and nonzero formal charges should be included in the structure."

*Question:*
"What is the most stable resonance structure if oxygen is the central atom in the CON⁻ ion?"

**Resonance Structure Diagram:**

The diagram presents a proposed Lewis structure for the CON⁻ ion:

- The ion is structured with oxygen (O) as the central atom.
- The carbon (C) atom is on the left and is bonded to oxygen with a triple bond.
- The nitrogen (N) atom is on the right and is bonded to oxygen with a single bond.

**Chemical Notation:**

- The carbon atom has two additional lone electrons indicated by a pair of dots on its left side, representing its lone pair.
- The oxygen atom has two single lone pairs indicated above and below it.
- The nitrogen atom has two lone pairs, similar to oxygen, indicated by dots on its top and bottom.

**Analysis:**

The resonant structure illustrates the distribution of electrons across the CON⁻ ion, taking into account formal charges and lone pairs. For accurate stability predictions, non-bonding electrons and formal charges are considered crucial. This resonance structure helps predict the behavior and reactivity of the molecule based on electron distribution.

**Conclusion:**

Understanding and drawing resonance structures with correct electron positioning and formal charges is essential in predicting molecular behavior and stability. By practicing these representations, students can better grasp molecular composition and its implications in chemical reactions.
Transcribed Image Text:**Title: Understanding Resonance Structures and Formal Charges** **Introduction:** In this section, we explore how to determine the most stable resonance structure for a given ion. **Resonance Structures and Formal Charges:** *Statement:* "All non-bonding electrons and nonzero formal charges should be included in the structure." *Question:* "What is the most stable resonance structure if oxygen is the central atom in the CON⁻ ion?" **Resonance Structure Diagram:** The diagram presents a proposed Lewis structure for the CON⁻ ion: - The ion is structured with oxygen (O) as the central atom. - The carbon (C) atom is on the left and is bonded to oxygen with a triple bond. - The nitrogen (N) atom is on the right and is bonded to oxygen with a single bond. **Chemical Notation:** - The carbon atom has two additional lone electrons indicated by a pair of dots on its left side, representing its lone pair. - The oxygen atom has two single lone pairs indicated above and below it. - The nitrogen atom has two lone pairs, similar to oxygen, indicated by dots on its top and bottom. **Analysis:** The resonant structure illustrates the distribution of electrons across the CON⁻ ion, taking into account formal charges and lone pairs. For accurate stability predictions, non-bonding electrons and formal charges are considered crucial. This resonance structure helps predict the behavior and reactivity of the molecule based on electron distribution. **Conclusion:** Understanding and drawing resonance structures with correct electron positioning and formal charges is essential in predicting molecular behavior and stability. By practicing these representations, students can better grasp molecular composition and its implications in chemical reactions.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

Blurred answer
Knowledge Booster
Theories of Bonding
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY