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 best describes the Lewis dot structure of a neutral H2S molecule?

Sulfur atom in the center with two double bonds to hydrogen atoms and no lone pairs on sulfur.

Sulfur atom in the center with two single bonds to hydrogen atoms and no lone pairs on sulfur.

Sulfur atom in the center with two single bonds to hydrogen atoms and two lone pairs on sulfur.

Sulfur atom in the center with one single bond and one double bond to hydrogen atoms and one lone pair on sulfur.

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Verified step by step guidance

Step 1: Identify the total number of valence electrons in the H2S molecule. Hydrogen has 1 valence electron each, and sulfur has 6 valence electrons, so total valence electrons = 2 × 1 + 6 = 8 electrons.

Step 2: Determine the central atom, which is sulfur because it is less electronegative than hydrogen and can form more bonds.

Step 3: Draw single bonds between the sulfur atom and each hydrogen atom. Each single bond represents 2 electrons, so 2 bonds use 4 electrons.

Step 4: Distribute the remaining valence electrons as lone pairs on the sulfur atom. Since 4 electrons are used in bonds, 4 electrons remain, which form two lone pairs on sulfur.

Step 5: Confirm that each hydrogen has a full valence shell (2 electrons) and sulfur has an octet (8 electrons total: 4 from bonds and 4 from lone pairs), ensuring the Lewis structure is complete and neutral.