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

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Which of the following is the correct number of valence electrons for the neutral compound BrF, and which Lewis dot structure represents it?

BrF has 10 valence electrons; the Lewis structure shows Br with one lone pair and a triple bond to F, which has one lone pair.

BrF has 12 valence electrons; the Lewis structure shows Br with two lone pairs and a double bond to F, which has two lone pairs.

BrF has 14 valence electrons; the Lewis structure shows Br with three lone pairs and a single bond to F, which has three lone pairs.

BrF has 16 valence electrons; the Lewis structure shows Br with four lone pairs and a single bond to F, which has four lone pairs.

Previous problemNext problem

Verified step by step guidance

Determine the total number of valence electrons by adding the valence electrons of each atom in the molecule. Bromine (Br) is in group 17, so it has 7 valence electrons, and fluorine (F) is also in group 17 with 7 valence electrons. Therefore, total valence electrons = 7 (Br) + 7 (F) = 14.

Draw a skeletal structure with Br and F connected by a single bond. Each single bond represents 2 shared electrons, so subtract these from the total valence electrons: 14 - 2 = 12 electrons remaining to be placed as lone pairs.

Distribute the remaining 12 electrons as lone pairs to satisfy the octet rule for each atom. Start by placing lone pairs on the more electronegative atom (F) to complete its octet, then place the remaining electrons on Br.

Count the electrons around each atom to ensure both have a full octet (8 electrons). Br should have three lone pairs (6 electrons) plus the bonding pair (2 electrons), and F should have three lone pairs (6 electrons) plus the bonding pair (2 electrons).

Confirm that the total number of electrons used in the Lewis structure equals the total valence electrons calculated initially (14 electrons), and that the structure matches the description: Br with three lone pairs and a single bond to F, which also has three lone pairs.