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 NF₃?

Nitrogen is bonded to two fluorine atoms and has two lone pairs of electrons.

Nitrogen is bonded to three fluorine atoms and has no lone pairs of electrons.

Nitrogen is bonded to three fluorine atoms and has one lone pair of electrons.

Nitrogen is bonded to four fluorine atoms and has no lone pairs of electrons.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for NF₃. 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: Draw the skeletal structure with nitrogen as the central atom bonded to three fluorine atoms. This is because nitrogen is less electronegative than fluorine and typically forms the central atom in such molecules.

Step 3: Assign bonding electrons by placing a single bond (2 electrons) between nitrogen and each fluorine atom. This accounts for $3 \times 2 = 6$ electrons used in bonding.

Step 4: Distribute the remaining valence electrons as lone pairs to complete the octets of the fluorine atoms first, since fluorine atoms require 8 electrons around them to be stable.

Step 5: Place any leftover electrons on the nitrogen atom as lone pairs. Then, check that nitrogen has a complete octet by counting bonding and lone pair electrons around it. This will confirm the number of lone pairs on nitrogen.