**Title: Drawing Lewis Structures for the Azide Ion, N₃⁻****Objective:** Learn how to draw the Lewis structure for the most stable azide ion, \(\text{N}_3^-\), including the representation of lone pairs.**Instructions:**1. **Understanding the Structure:** - The azide ion \(\text{N}_3^-\) consists of three nitrogen atoms. - It is important to distribute electrons to satisfy the octet rule for each nitrogen atom while considering formal charges.2. **Drawing the Lewis Structure:** - Start by connecting the three nitrogen atoms linearly. - Place a negative charge on the structure to represent the extra electron in the azide ion.3. **Including Lone Pairs:** - Assign lone pairs on the outer nitrogen atoms to complete their octets. - Ensure the formal charge distribution is as close to zero as possible, favoring a negative charge on the more electronegative atoms when needed.4. **Tools and Tips:** - Use the "Draw" tool to structure the bonds between nitrogen atoms. - The "Rings" feature is not required in this linear structure. - Check your work using the formal charge formula: Formal Charge = (Valence electrons) - (Non-bonding electrons) - 0.5*(Bonding electrons).5. **Example Lewis Structure:** - Represent the bonds as lines and lone pairs as dots around the nitrogen atoms. Common valid structures for \(\text{N}_3^-\) might show two N-N bonds with lone pairs completing the octets.**Reference:**- This exercise is adapted from McQuarrie, Rock, and Gallogly's "General Chemistry," 4th edition. This activity helps you understand the basics of drawing Lewis structures for polyatomic ions, especially those with multiple resonance forms like the azide ion.

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Draw the Lewis structure for the most stable azide ion, N,. Include lone pairs.

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...

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Question

**Title: Drawing Lewis Structures for the Azide Ion, N₃⁻**

**Objective:**
Learn how to draw the Lewis structure for the most stable azide ion, \(\text{N}_3^-\), including the representation of lone pairs.

**Instructions:**

1. **Understanding the Structure:**
- The azide ion \(\text{N}_3^-\) consists of three nitrogen atoms.
- It is important to distribute electrons to satisfy the octet rule for each nitrogen atom while considering formal charges.

2. **Drawing the Lewis Structure:**
- Start by connecting the three nitrogen atoms linearly.
- Place a negative charge on the structure to represent the extra electron in the azide ion.

3. **Including Lone Pairs:**
- Assign lone pairs on the outer nitrogen atoms to complete their octets.
- Ensure the formal charge distribution is as close to zero as possible, favoring a negative charge on the more electronegative atoms when needed.

4. **Tools and Tips:**
- Use the "Draw" tool to structure the bonds between nitrogen atoms.
- The "Rings" feature is not required in this linear structure.
- Check your work using the formal charge formula: Formal Charge = (Valence electrons) - (Non-bonding electrons) - 0.5*(Bonding electrons).

5. **Example Lewis Structure:**
- Represent the bonds as lines and lone pairs as dots around the nitrogen atoms. Common valid structures for \(\text{N}_3^-\) might show two N-N bonds with lone pairs completing the octets.

**Reference:**
- This exercise is adapted from McQuarrie, Rock, and Gallogly's "General Chemistry," 4th edition.

This activity helps you understand the basics of drawing Lewis structures for polyatomic ions, especially those with multiple resonance forms like the azide ion.

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