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 51m
7. Gases3h 49m
8. Thermochemistry2h 35m
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 34m
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

Determine the Lewis Dot Structure for the disulfur dichloride molecule, S₂Cl₂.

Lewis Dot Structure of disulfur dichloride (S2Cl2) showing sulfur and chlorine atoms.

Alternative Lewis Dot Structure of disulfur dichloride (S2Cl2) with different bonding representation.

Another representation of Lewis Dot Structure for disulfur dichloride (S2Cl2) highlighting sulfur and chlorine bonds.

Final Lewis Dot Structure of disulfur dichloride (S2Cl2) illustrating sulfur and chlorine atoms.

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Verified step by step guidance

Identify the total number of valence electrons in the S2Cl2 molecule. Sulfur (S) has 6 valence electrons and chlorine (Cl) has 7 valence electrons. Therefore, the total number of valence electrons is 2(6) + 2(7) = 26 electrons.

Determine the central atoms in the molecule. In S2Cl2, the sulfur atoms are central, with each sulfur atom bonded to one chlorine atom and to each other.

Draw a skeletal structure with the sulfur atoms in the center and chlorine atoms on the ends: Cl-S-S-Cl.

Distribute the remaining valence electrons to satisfy the octet rule. Start by placing lone pairs on the outer chlorine atoms to complete their octets, then place any remaining electrons on the sulfur atoms.

Ensure that each atom has a complete octet (8 electrons) and adjust the structure if necessary to minimize formal charges, ensuring the most stable configuration.

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