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 SF3N?

Sulfur is the central atom, bonded to three fluorine atoms and one nitrogen atom, with one lone pair on sulfur.

Nitrogen is the central atom, bonded to three sulfur atoms and one fluorine atom, with no lone pairs on nitrogen.

Fluorine is the central atom, bonded to three sulfur atoms and one nitrogen atom, with one lone pair on fluorine.

Sulfur is the central atom, bonded to three nitrogen atoms and one fluorine atom, with two lone pairs on sulfur.

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Verified step by step guidance

Step 1: Determine the central atom by considering electronegativity and bonding capacity. Typically, the least electronegative atom (excluding hydrogen) is the central atom. Here, sulfur (S), nitrogen (N), and fluorine (F) are present. Fluorine is the most electronegative and usually terminal, so it is unlikely to be central. Between sulfur and nitrogen, sulfur is less electronegative and can expand its octet, making it a good candidate for the central atom.

Step 2: Count the total number of valence electrons for the molecule SF3N. Sulfur has 6 valence electrons, each fluorine has 7, and nitrogen has 5. Calculate the sum: $6 + (3 \times 7) + 5$.

Step 3: Arrange the atoms with sulfur in the center bonded to three fluorine atoms and one nitrogen atom. Draw single bonds connecting sulfur to each fluorine and to nitrogen. Each bond represents 2 electrons.

Step 4: Distribute the remaining valence electrons to satisfy the octet rule for the terminal atoms first (fluorine and nitrogen). Fluorine atoms typically have three lone pairs, and nitrogen usually has one lone pair if bonded to sulfur.

Step 5: Assign any leftover electrons to the central sulfur atom as lone pairs. Since sulfur can have an expanded octet, it may have one lone pair after bonding to the four atoms. Confirm that the total number of electrons used matches the total valence electrons calculated in Step 2.