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 S2F2?

The two sulfur atoms are double-bonded to each other, and each sulfur is bonded to one fluorine atom, with no lone pairs on sulfur.

Each fluorine atom is bonded to both sulfur atoms, forming a four-membered ring.

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

Each sulfur atom is bonded to one fluorine atom and to the other sulfur atom, with each sulfur having one lone pair.

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Verified step by step guidance

Step 1: Identify the total number of valence electrons available for the molecule S2F2. Sulfur (S) has 6 valence electrons, and fluorine (F) has 7 valence electrons. Since there are 2 sulfur atoms and 2 fluorine atoms, calculate the total valence electrons as: $2 \times 6 + 2 \times 7$.

Step 2: Determine the skeletal structure of the molecule. Since the compound is S2F2, start by connecting the two sulfur atoms together, as sulfur atoms often bond to each other, and then attach one fluorine atom to each sulfur atom.

Step 3: Distribute the remaining valence electrons to satisfy the octet rule for each atom. Place lone pairs on the fluorine atoms first to complete their octets, then place any remaining electrons as lone pairs on the sulfur atoms.

Step 4: Check the bonding and lone pairs on sulfur atoms. Each sulfur should have one bond to the other sulfur atom, one bond to a fluorine atom, and one lone pair to complete its octet, consistent with the correct Lewis structure.

Step 5: Verify that the structure satisfies the octet rule for all atoms and that the total number of electrons used matches the total valence electrons calculated in Step 1.