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 best describes the Lewis dot structure of neutral NBr (nitrogen monobromide)?

Nitrogen and bromine are connected by a single bond, with two lone pairs on bromine and two lone pairs on nitrogen.

Nitrogen and bromine are connected by a triple bond, with one lone pair on bromine and no lone pairs on nitrogen.

Nitrogen and bromine are connected by a single bond, with three lone pairs on bromine and one lone pair on nitrogen.

Nitrogen and bromine are connected by a double bond, with two lone pairs on bromine and two lone pairs on nitrogen.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for bonding in NBr. Nitrogen has 5 valence electrons, and bromine has 7 valence electrons, so the total is $5 + 7 = 12$ valence electrons.

Step 2: Connect nitrogen and bromine with a single bond first, which uses 2 electrons. Subtract these from the total valence electrons to find how many remain for lone pairs.

Step 3: Distribute the remaining electrons as lone pairs to satisfy the octet rule for both atoms. Remember that nitrogen typically forms three bonds and has one lone pair, while bromine usually has three lone pairs when bonded with a single bond.

Step 4: Check the formal charges on both atoms to ensure the most stable Lewis structure. The best structure will have formal charges closest to zero.

Step 5: Confirm that the nitrogen has one lone pair and bromine has three lone pairs with a single bond between them, which matches the correct Lewis structure description.