Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

11. Bonding & Molecular Structure

Lewis Dot Structures: Ions

General Chemistry

11. Bonding & Molecular Structure

Lewis Dot Structures: Ions

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Multiple Choice

Which of the following is the correct Lewis dot structure for the azide ion (N₃⁻)?

N-N≡N with a lone pair on the central nitrogen

N=N=N with no lone pairs

N⁻-N=N⁺ with a lone pair on the central nitrogen

N≡N⁺-N⁻ with a lone pair on the terminal nitrogen

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Verified step by step guidance

Understand that the azide ion (N₃⁻) consists of three nitrogen atoms and carries a negative charge. The goal is to distribute electrons to satisfy the octet rule for each nitrogen atom while accounting for the overall charge.

Calculate the total number of valence electrons available. Each nitrogen atom has 5 valence electrons, and the ion has an additional electron due to the negative charge, giving a total of 16 valence electrons.

Arrange the nitrogen atoms linearly and begin by placing a single bond between each pair of nitrogen atoms. This initial setup uses 4 electrons, leaving 12 electrons to distribute.

Distribute the remaining electrons to satisfy the octet rule for each nitrogen atom. Consider placing triple bonds and lone pairs where necessary. The structure N≡N⁺-N⁻ with a lone pair on the terminal nitrogen satisfies the octet rule and accounts for the charge distribution.

Verify the formal charges for each nitrogen atom in the structure. The terminal nitrogen with a lone pair should have a formal charge of -1, the central nitrogen should have a formal charge of +1, and the other terminal nitrogen should have a formal charge of 0, ensuring the overall charge of the ion is -1.