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 SF_2?

Sulfur is the central atom with two double bonds to fluorine atoms and no lone pairs on sulfur.

Sulfur is the central atom with one single bond and one double bond to fluorine atoms and one lone pair on sulfur.

Sulfur is the central atom with two single bonds to fluorine atoms and two lone pairs on sulfur.

Fluorine is the central atom with single bonds to two sulfur atoms.

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Verified step by step guidance

Step 1: Identify the total number of valence electrons in the molecule SF_2. Sulfur (S) is in group 16 and has 6 valence electrons, and each fluorine (F) atom is in group 17 with 7 valence electrons. Calculate the total by adding these together: $6 + 2 \times 7$.

Step 2: Determine the central atom. Generally, the less electronegative atom is the central atom. Between sulfur and fluorine, sulfur is less electronegative, so sulfur will be the central atom.

Step 3: Draw single bonds between the central sulfur atom and each fluorine atom. Each single bond represents 2 electrons shared between atoms.

Step 4: Distribute the remaining valence electrons to satisfy the octet rule. Start by completing the octets of the fluorine atoms (each fluorine needs 8 electrons total, including bonding electrons). Then place any leftover electrons as lone pairs on the sulfur atom.

Step 5: Check the formal charges and the octet rule for all atoms. Ensure that sulfur has a complete octet and that the structure has no unnecessary charges. This will confirm that sulfur has two single bonds to fluorine atoms and two lone pairs on sulfur.