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 Lewis dot structures provides a reasonable representation of SO_2?

O≡S–O with three lone pairs on each oxygen and no lone pairs on sulfur

O–S=O with two lone pairs on each oxygen and one lone pair on sulfur

O–S–O with three lone pairs on each oxygen and two lone pairs on sulfur

O=S=O with one lone pair on each oxygen and one lone pair on sulfur

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Verified step by step guidance

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

Step 2: Draw a skeletal structure connecting sulfur to the two oxygen atoms. Typically, sulfur is the central atom because it is less electronegative than oxygen.

Step 3: Distribute the valence electrons to satisfy the octet rule for each atom, starting by placing lone pairs on the outer atoms (oxygen) and then on sulfur. Remember that each bond (single, double, or triple) counts as 2 electrons shared between atoms.

Step 4: Consider resonance structures and formal charges to find the most stable Lewis structure. Calculate formal charges using the formula: $\text{Formal charge} = \text{Valence electrons} - (\text{Nonbonding electrons} + \frac{1}{2} \times \text{Bonding electrons})$ for each atom.

Step 5: Identify the structure with the lowest formal charges and complete octets on all atoms. The reasonable Lewis structure for SO_2 has one sulfur-oxygen single bond and one sulfur-oxygen double bond, with lone pairs arranged to minimize formal charges, matching the structure: O–S=O with two lone pairs on each oxygen and one lone pair on sulfur.