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 the correct Lewis dot structure for sulfur trioxide (SO_3), a neutral compound?

Sulfur atom in the center with three single bonds to three oxygen atoms; each oxygen has three lone pairs.

Sulfur atom in the center with one double bond and two single bonds to oxygen atoms; each oxygen has two lone pairs.

Sulfur atom in the center with three triple bonds to three oxygen atoms; each oxygen has one lone pair.

Sulfur atom in the center with three double bonds to three oxygen atoms; each oxygen has two lone pairs.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the molecule. Sulfur (S) has 6 valence electrons, and each oxygen (O) atom has 6 valence electrons. Since there are three oxygen atoms, total valence electrons = 6 (S) + 3 × 6 (O) = 24 electrons.

Step 2: Arrange the atoms with sulfur in the center and three oxygen atoms surrounding it. Connect each oxygen atom to sulfur with a single bond initially. Each single bond represents 2 electrons, so 3 single bonds use 6 electrons.

Step 3: Distribute the remaining electrons to satisfy the octet rule for the oxygen atoms first. Each oxygen needs 8 electrons total (including bonding electrons). After placing lone pairs on oxygens, check if sulfur has a complete octet. If sulfur lacks an octet, consider forming double bonds by sharing lone pairs from oxygen atoms with sulfur.

Step 4: Evaluate resonance structures and formal charges. The most stable Lewis structure minimizes formal charges and satisfies the octet rule for all atoms. For SO_3, the best structure has sulfur forming three double bonds with oxygen atoms, each oxygen having two lone pairs, and sulfur having an expanded octet.

Step 5: Confirm that the final Lewis structure is neutral overall, with no formal charges or minimized formal charges, and that it matches the description: sulfur in the center with three double bonds to oxygen atoms, each oxygen having two lone pairs.