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 is the correct number of valence electrons for the neutral compound SiF4, and which Lewis structure best represents it?

28 valence electrons; Si at the center with double bonds to each F atom, each F with two lone pairs

24 valence electrons; Si at the center with single bonds to F atoms, each F with two lone pairs

36 valence electrons; Si at the center with single bonds to F atoms, each F with four lone pairs

32 valence electrons; Si at the center with four single bonds to F atoms, each F with three lone pairs

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Verified step by step guidance

Determine the total number of valence electrons by adding the valence electrons of each atom in the molecule. Silicon (Si) is in group 14 and has 4 valence electrons, and each fluorine (F) atom is in group 17 with 7 valence electrons. Since there are 4 fluorine atoms, calculate the total as: $4 + 4 \times 7$.

Sum the valence electrons to find the total number available for bonding and lone pairs in the molecule.

Draw the Lewis structure by placing the silicon atom at the center because it is less electronegative and can form multiple bonds, then connect each fluorine atom to silicon with a single bond initially.

Distribute the remaining valence electrons as lone pairs around the fluorine atoms to complete their octets. Each fluorine should have three lone pairs (6 electrons) after forming a single bond with silicon.

Check that the silicon atom has a complete octet by counting the electrons shared in bonds (each single bond counts as 2 electrons). Confirm that the total number of electrons used in bonds and lone pairs equals the total valence electrons calculated.