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 SF_4 (sulfur tetrafluoride)?

Sulfur is surrounded by four fluorine atoms and no lone pairs of electrons.

Sulfur is surrounded by four fluorine atoms and two lone pairs of electrons.

Sulfur is surrounded by five fluorine atoms and no lone pairs of electrons.

Sulfur is surrounded by four fluorine atoms and one lone pair of electrons.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons in SF_4. Sulfur (S) is in group 16 and has 6 valence electrons, and each fluorine (F) atom is in group 17 with 7 valence electrons. Since there are 4 fluorine atoms, calculate the total valence electrons as: $6 + 4 \times 7$.

Step 2: Draw the skeletal structure with sulfur as the central atom bonded to four fluorine atoms. Each S-F bond represents 2 electrons shared between sulfur and fluorine.

Step 3: Subtract the electrons used in bonding from the total valence electrons to find the remaining electrons. These remaining electrons will be placed as lone pairs on the atoms, starting with fluorine atoms to complete their octets.

Step 4: After placing lone pairs on fluorine atoms, check how many electrons remain. Assign any leftover electrons as lone pairs on the central sulfur atom.

Step 5: Confirm the Lewis structure by verifying that sulfur has an expanded octet (which is possible for elements in period 3 and beyond) and that the total number of electrons used matches the total valence electrons calculated initially. This will show that sulfur is surrounded by four fluorine atoms and one lone pair of electrons.