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 the neutral compound SO_2?

SO_2 has a central sulfur atom bonded to two oxygen atoms, both with single bonds, and no lone pairs on sulfur.

SO_2 has a central sulfur atom bonded to two oxygen atoms, with one double bond and one single bond, and a lone pair on sulfur.

SO_2 has a central sulfur atom bonded to two oxygen atoms, both with double bonds, and no lone pairs on sulfur.

SO_2 has a central oxygen atom bonded to two sulfur atoms, each with a single bond.

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Verified step by step guidance

Identify the central atom in SO_2, which is sulfur (S), because it is less electronegative than oxygen (O) and can form more bonds.

Determine the total number of valence electrons available: sulfur has 6 valence electrons, and each oxygen has 6 valence electrons, so total valence electrons = 6 + 2 \times 6 = 18.

Draw a skeleton structure with sulfur in the center bonded to two oxygen atoms. Initially, connect sulfur to each oxygen with a single bond, using 4 electrons (2 bonds \times 2 electrons each).

Distribute the remaining electrons to satisfy the octet rule for the oxygen atoms first, then place any leftover electrons on sulfur. Adjust bonding by forming double bonds if necessary to minimize formal charges and satisfy the octet rule.

Check formal charges on each atom to find the most stable Lewis structure. The correct structure typically has one double bond and one single bond between sulfur and oxygen atoms, with a lone pair on sulfur to complete its octet.