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 SiF_2?

Si is the central atom with two single bonds to F atoms, and no lone pairs on Si.

Si is the central atom with two double bonds to F atoms, and no lone pairs on Si.

F is the central atom with single bonds to two Si atoms, and each F has three lone pairs.

Si is the central atom with two single bonds to F atoms, and Si has one lone pair.

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Verified step by step guidance

Identify the total number of valence electrons for the molecule SiF_2. Silicon (Si) has 4 valence electrons, and each fluorine (F) atom has 7 valence electrons. Since there are two fluorine atoms, calculate the total as: $4 + 2 \times 7 = 18$ valence electrons.

Determine the central atom. Silicon is less electronegative than fluorine, so Si will be the central atom with the two fluorine atoms bonded to it.

Draw single bonds between the central Si atom and each F atom. Each single bond represents 2 electrons, so 2 bonds use $2 \times 2 = 4$ electrons.

Distribute the remaining electrons to satisfy the octet rule. Place lone pairs on the fluorine atoms first to complete their octets (each F needs 6 more electrons as lone pairs), then place any leftover electrons as lone pairs on the silicon atom.

Check the formal charges and the octet rule for each atom. The correct Lewis structure will have Si as the central atom bonded to two F atoms with single bonds, and Si will have one lone pair to complete its octet, matching the given correct answer.