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 PSF3 (phosphorus sulfur trifluoride)?

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

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

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

Fluorine is the central atom, bonded to one phosphorus atom and one sulfur atom, with two lone pairs on fluorine.

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Verified step by step guidance

Identify the central atom in PSF3 by considering electronegativity and bonding capacity. Typically, the least electronegative atom that can form multiple bonds is the central atom. Between phosphorus (P), sulfur (S), and fluorine (F), phosphorus is less electronegative and can form more bonds, so it is usually the central atom.

Determine the number of valence electrons for each atom: phosphorus has 5, sulfur has 6, and fluorine has 7 valence electrons. Calculate the total valence electrons available for bonding in PSF3 by adding these values considering the number of each atom.

Arrange the atoms with phosphorus in the center, bonded to one sulfur atom and three fluorine atoms. Draw single bonds between phosphorus and each of these atoms initially.

Distribute the remaining valence electrons to satisfy the octet rule for the surrounding atoms first (fluorine and sulfur), placing lone pairs as needed. Then check the central atom phosphorus to see if it has a complete octet or if any lone pairs remain.

Verify the Lewis structure by counting all electrons around each atom to ensure the octet rule is satisfied (or expanded octet for phosphorus if applicable) and confirm that the structure matches the description: phosphorus bonded to one sulfur and three fluorines, with no lone pairs on phosphorus.