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 statements correctly describes the Lewis dot structure of neutral SO2Cl2 (thionyl chloride)?

Sulfur is the central atom, bonded to two oxygen atoms and two chlorine atoms, with two lone pairs on sulfur.

Sulfur is the central atom, bonded to two oxygen atoms and two chlorine atoms, with no lone pairs on sulfur.

Oxygen is the central atom, bonded to two sulfur atoms and two chlorine atoms.

Sulfur is the central atom, bonded to one oxygen atom and three chlorine atoms, with one lone pair on sulfur.

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Verified step by step guidance

Step 1: Identify the central atom in SO2Cl2. Generally, the least electronegative atom (excluding hydrogen) is the central atom. Here, sulfur (S) is less electronegative than oxygen (O) and chlorine (Cl), so sulfur is the central atom.

Step 2: Determine the total number of valence electrons. Sulfur has 6 valence electrons, each oxygen has 6, and each chlorine has 7. Calculate the total: $6 + 2 \times 6 + 2 \times 7 = 6 + 12 + 14 = 32$ valence electrons.

Step 3: Draw single bonds from sulfur to each of the two oxygen atoms and two chlorine atoms. Each bond uses 2 electrons, so 4 bonds use $4 \times 2 = 8$ electrons.

Step 4: Distribute the remaining electrons to satisfy the octet rule for the outer atoms first (oxygen and chlorine). Oxygen atoms often form double bonds with sulfur to complete their octet, which affects the bonding and lone pairs on sulfur.

Step 5: After placing bonds and lone pairs on outer atoms, check the sulfur atom's electrons. Sulfur can expand its octet, but in SO2Cl2, sulfur typically has no lone pairs, being bonded to two oxygens (with double bonds) and two chlorines (with single bonds). This matches the correct description.