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 best describes the Lewis dot structure of the neutral compound SF_3?

Sulfur is the central atom, bonded to three fluorine atoms with single bonds, and has one lone pair of electrons.

Sulfur is the central atom, bonded to three fluorine atoms with single bonds, and has two lone pairs of electrons.

Sulfur is the central atom, bonded to three fluorine atoms with single bonds, and has no lone pairs.

Sulfur is the central atom, bonded to three fluorine atoms with double bonds, and has no lone pairs.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the molecule SF_3. 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 three fluorine atoms, calculate the total valence electrons as: $6 + 3 \times 7$.

Step 2: Identify the central atom, which is usually the least electronegative element. In this case, sulfur is the central atom, and the three fluorine atoms will be bonded to it.

Step 3: Form single bonds between the sulfur atom and each fluorine atom. Each single bond consists of 2 electrons, so subtract the electrons used in bonding from the total valence electrons.

Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule for the fluorine atoms first, since fluorine atoms typically complete their octet with three lone pairs.

Step 5: Assign any leftover electrons to the central sulfur atom as lone pairs. Then, determine the number of lone pairs on sulfur by considering the total electrons around it (bonding and nonbonding) to complete its octet or accommodate expanded octet if necessary.