QQuestionChemistry
QuestionChemistry
Draw the Lewis structure for the azide $\left(\mathrm{N}_{3}^{-}\right)$ion.
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:I'll solve this Lewis structure problem step by step:
Step 2:: Determine the total number of valence electrons
- Total valence electrons: $$(3 \times 5) + 1 = 16$$ electrons
- Nitrogen (N) has 5 valence electrons - We have 3 nitrogen atoms - The ion has a - 1 charge, which adds 1 more electron
Step 3:: Arrange the atoms
- Place the three nitrogen atoms in a linear arrangement - The central nitrogen will connect to the two outer nitrogens
Step 4:: Create initial single bonds
- Remaining electrons: $$16 - 6 = 10$$ electrons
- Draw single bonds between the central nitrogen and the two outer nitrogens
Step 5:: Add remaining electrons as lone pairs
- Distribute the remaining $$10$$ electrons as lone pairs
- Prioritize outer atoms first - Each outer nitrogen will have 3 lone pairs - The central nitrogen will have 1 lone pair
Step 6:: Check formal charges
\mathrm{N} \equiv \mathrm{N}^{-} \equiv \mathrm{N}
- Verify that the structure minimizes formal charges - The structure will have a resonance form with electrons delocalized Final Lewis Structure: (Triple bond between outer nitrogens, with a negative charge)
Final Answer
The Lewis structure for the azide ion \left(\mathrm{N}_{3}^{-}\right) is a linear structure with triple bonds and a negative charge.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students