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 a valid Lewis dot structure for the neutral compound ozone (O_3)?

O–O–O with three lone pairs on each O atom

O≡O–O with no lone pairs on the central O and four lone pairs on each terminal O

O–O=O with two lone pairs on the central O and two lone pairs on each terminal O

O=O–O with one lone pair on the central O and three lone pairs on each terminal O

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the ozone (O_3) molecule. Each oxygen atom has 6 valence electrons, so for three oxygen atoms, total valence electrons = 3 × 6 = 18 electrons.

Step 2: Draw a skeletal structure connecting the three oxygen atoms. Since ozone is a triatomic molecule, the atoms are connected linearly: O–O–O. Assign single bonds initially between the oxygen atoms, which use 2 electrons per bond.

Step 3: Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for each oxygen atom. Remember that each oxygen atom should ideally have 8 electrons around it (including bonding and lone pairs).

Step 4: Consider resonance structures and formal charges to find the most stable Lewis structure. Calculate the formal charge on each oxygen atom using the formula: $\text{Formal Charge} = \text{Valence Electrons} - \text{Nonbonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons}$. The best Lewis structure minimizes formal charges and places negative charges on the more electronegative atoms.

Step 5: Identify the correct Lewis structure that matches the description: O–O=O with two lone pairs on the central oxygen and two lone pairs on each terminal oxygen, which satisfies the octet rule and has the lowest formal charges.