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

Determine the Lewis Dot Structure for the following ion:O₂^2–.

Lewis Dot Structure for the O2 2- ion with a single bond.

Lewis Dot Structure for the O2 2- ion with a double bond.

Lewis Dot Structure for the O2 2- ion with a double bond and lone pairs.

Lewis Dot Structure for the O2 2- ion with a double bond and lone pairs on the sides.

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Verified step by step guidance

Identify the total number of valence electrons for the O2^2- ion. Each oxygen atom has 6 valence electrons, and the 2- charge indicates an additional 2 electrons, giving a total of 14 valence electrons.

Arrange the two oxygen atoms side by side and connect them with a single bond. This single bond accounts for 2 of the 14 valence electrons.

Distribute the remaining 12 valence electrons around the oxygen atoms to satisfy the octet rule. Start by placing 6 electrons (3 pairs) around each oxygen atom.

Check if each oxygen atom has a complete octet. If not, consider forming a double bond by sharing a pair of electrons between the oxygen atoms.

Verify the formal charges on each oxygen atom to ensure the most stable structure. The formal charge should be minimized and ideally be zero for each atom in the ion.