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 shows the complete Lewis dot structure for NF_3 (nitrogen trifluoride)?

N atom in the center with three double bonds to F atoms; N has no lone pairs; each F has two lone pairs.

N atom in the center with three single bonds to F atoms; N has three lone pairs; each F has two lone pairs.

N atom in the center with three single bonds to F atoms; N has no lone pairs; each F has three lone pairs.

N atom in the center with three single bonds to F atoms; N has one lone pair; each F has three lone pairs.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for NF_3. Nitrogen (N) has 5 valence electrons, and each fluorine (F) has 7 valence electrons. Since there are three fluorine atoms, calculate the total as $5 + 3 \times 7$.

Step 2: Arrange the atoms with nitrogen as the central atom because it is less electronegative than fluorine, and connect each fluorine atom to nitrogen with a single bond. Each single bond represents 2 shared electrons.

Step 3: Distribute the remaining valence electrons to complete the octets of the fluorine atoms first. Each fluorine needs 8 electrons total (including bonding electrons), so add lone pairs to each fluorine until their octet is complete.

Step 4: Place any leftover electrons on the central nitrogen atom as lone pairs. Check that nitrogen also has a complete octet (8 electrons total) by counting bonding and lone pair electrons.

Step 5: Confirm the Lewis structure by verifying that the total number of electrons used equals the total valence electrons calculated in Step 1, and that all atoms satisfy the octet rule where applicable.