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 SF_3^- ion?

SF_3^- has three single bonds between sulfur and fluorine, one lone pair on sulfur, and a negative formal charge on sulfur.

SF_3^- has three double bonds between sulfur and fluorine, no lone pairs on sulfur, and a negative formal charge on fluorine.

SF_3^- has two single bonds and one double bond between sulfur and fluorine, with two lone pairs on sulfur.

SF_3^- has three single bonds between sulfur and fluorine, no lone pairs on sulfur, and a negative formal charge on fluorine.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for the SF_3^- ion. Sulfur (S) has 6 valence electrons, each fluorine (F) has 7 valence electrons, and the negative charge adds 1 extra electron. So, total valence electrons = 6 + (3 × 7) + 1.

Step 2: Draw the skeletal structure with sulfur as the central atom bonded to three fluorine atoms. Connect each fluorine to sulfur with a single bond initially.

Step 3: Distribute the remaining valence electrons to complete the octets of the fluorine atoms first, since fluorine is highly electronegative and typically follows the octet rule strictly.

Step 4: Place any leftover electrons on the central sulfur atom as lone pairs. Check the total number of electrons used to ensure it matches the total valence electrons calculated in Step 1.

Step 5: Assign formal charges to each atom using the formula: $\text{Formal charge} = \text{Valence electrons} - \text{Nonbonding electrons} - \frac{1}{2} \times \text{Bonding electrons}$. Confirm that the negative charge is located on sulfur, consistent with the extra electron and the Lewis structure.