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: Neutral Compounds

General Chemistry

11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

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Multiple Choice

Which of the following is closest to the bond angle in ozone (O_3) as predicted by its Lewis structure?

90^ext{o}

117^ext{o}

120^ext{o}

104.5^ext{o}

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Verified step by step guidance

Step 1: Draw the Lewis structure of ozone (O_3). Ozone has a total of 18 valence electrons (6 from each oxygen atom). Arrange the atoms with one oxygen in the center and the other two on the sides, then distribute electrons to satisfy the octet rule as much as possible.

Step 2: Identify the electron domains around the central oxygen atom. In ozone, the central oxygen is bonded to two other oxygens and has one lone pair of electrons, giving a total of three regions of electron density (two bonding pairs and one lone pair).

Step 3: Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular geometry. Three electron domains around the central atom correspond to a trigonal planar electron geometry, but the presence of one lone pair changes the molecular shape to bent or angular.

Step 4: Understand that lone pairs repel more strongly than bonding pairs, which compresses the bond angle between the two oxygen atoms bonded to the central oxygen. The ideal trigonal planar angle is 120°, but the lone pair reduces this angle.

Step 5: Conclude that the bond angle in ozone is slightly less than 120°, typically around 117°, which matches the answer closest to the predicted bond angle based on the Lewis structure and VSEPR theory.