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 NF_3 (nitrogen trifluoride)?

Nitrogen is the central atom, bonded to three fluorine atoms, with one lone pair on nitrogen.

Fluorine is the central atom, bonded to three nitrogen atoms, with one lone pair on fluorine.

Nitrogen is the central atom, bonded to three fluorine atoms, with two lone pairs on nitrogen.

Nitrogen is the central atom, bonded to three fluorine atoms, with no lone pairs on nitrogen.

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Verified step by step guidance

Step 1: Identify the total number of valence electrons in 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 valence electrons as: $5 + 3 \times 7$.

Step 2: Determine the central atom. Generally, the least electronegative atom (excluding hydrogen) is the central atom. Between nitrogen and fluorine, nitrogen is less electronegative, so nitrogen will be the central atom bonded to three fluorine atoms.

Step 3: Draw single bonds between the central nitrogen atom and each fluorine atom. Each bond represents 2 electrons, so subtract $3 \times 2$ electrons from the total valence electrons to account for bonding.

Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule. First, complete the octet for each fluorine atom by adding lone pairs until each fluorine has 8 electrons total (including bonding electrons). Then, place any leftover electrons on the nitrogen atom as lone pairs.

Step 5: Count the lone pairs on nitrogen after distributing electrons. Since nitrogen started with 5 valence electrons and shares three bonds (6 electrons), the remaining electrons form one lone pair on nitrogen. This confirms the Lewis structure: nitrogen central atom bonded to three fluorines with one lone pair on nitrogen.