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 correctly describes the bonding in the Lewis dot structure of neutral SO_2?

SO_2 has two single bonds between sulfur and each oxygen atom.

SO_2 has two double bonds between sulfur and each oxygen atom.

SO_2 has a triple bond between sulfur and one oxygen atom, and a single bond to the other.

SO_2 has one single bond and one double bond between sulfur and the two oxygen atoms.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for SO_2. Sulfur (S) has 6 valence electrons, and each oxygen (O) has 6 valence electrons, so total valence electrons = 6 + 2 \times 6 = 18.

Step 2: Draw a skeletal structure with sulfur as the central atom bonded to two oxygen atoms. Connect sulfur to each oxygen with a single bond initially, which uses 2 electrons per bond.

Step 3: Distribute the remaining electrons to satisfy the octet rule for the oxygen atoms first, placing lone pairs around each oxygen to complete their octets.

Step 4: Check the octet of the sulfur atom. If sulfur does not have a complete octet, form double bonds by converting lone pairs from oxygen atoms into bonding pairs between sulfur and oxygen.

Step 5: Confirm the formal charges on each atom to ensure the most stable Lewis structure. The best structure minimizes formal charges, which leads to one double bond and one single bond between sulfur and the two oxygen atoms.