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 H2S2?

Each sulfur atom is bonded to one hydrogen atom and the two sulfur atoms are connected by a single bond.

Both hydrogen atoms are bonded to the same sulfur atom, and the two sulfur atoms are connected by a single bond.

The two sulfur atoms are connected by a double bond, and each sulfur atom is bonded to one hydrogen atom.

Each sulfur atom is bonded to two hydrogen atoms and the two sulfur atoms are not bonded to each other.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the molecule H2S2. Hydrogen has 1 valence electron each, and sulfur has 6 valence electrons each. Calculate the total by adding these together: $2 \times 1 + 2 \times 6$.

Step 2: Consider the typical bonding patterns for hydrogen and sulfur. Hydrogen usually forms 1 bond (to complete its duet), and sulfur typically forms 2 bonds to satisfy the octet rule, but can vary due to its position in the periodic table.

Step 3: Draw a skeletal structure where the two sulfur atoms are connected. Since sulfur atoms can bond to each other, connect the two sulfur atoms with a single bond initially, then attach each hydrogen atom to a sulfur atom.

Step 4: Assign electrons to complete the octet for sulfur atoms and duet for hydrogen atoms. Place lone pairs on sulfur atoms as needed to complete their octets after bonding.

Step 5: Evaluate the possible structures given in the problem by comparing them to the bonding and electron count rules. The correct Lewis structure will have each sulfur bonded to one hydrogen and the two sulfurs connected by a single bond, matching the total valence electrons and typical bonding patterns.