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 carbon disulfide (CS_2)?

The central carbon atom forms a triple bond with one sulfur atom and a single bond with the other sulfur atom.

The central carbon atom forms two single bonds with two sulfur atoms, and carbon has two lone pairs.

The central carbon atom forms two single bonds with two sulfur atoms, and each sulfur atom has two lone pairs.

The central carbon atom forms two double bonds with two sulfur atoms, and all atoms have a complete octet.

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Verified step by step guidance

Identify the central atom in the molecule CS_2, which is carbon because it is less electronegative than sulfur and can form multiple bonds.

Determine the total number of valence electrons available: Carbon has 4 valence electrons, and each sulfur has 6 valence electrons, so total valence electrons = 4 + 2 × 6 = 16.

Distribute electrons to form bonds between carbon and sulfur atoms. Start by placing single bonds between carbon and each sulfur, using 4 electrons (2 per bond).

Complete the octets of the sulfur atoms by adding lone pairs, then check if carbon has a complete octet. If carbon does not have 8 electrons, form double bonds by sharing lone pairs from sulfur with carbon.

Confirm that the final Lewis structure has carbon forming two double bonds with the two sulfur atoms, and that all atoms have a complete octet, which satisfies the octet rule for this molecule.