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 statements correctly describes the Lewis dot structure of neutral SBr2?

Sulfur is the central atom, bonded to two bromine atoms, with two lone pairs on sulfur.

Sulfur is the central atom, bonded to two bromine atoms, with no lone pairs on sulfur.

Bromine is the central atom, bonded to two sulfur atoms, with two lone pairs on bromine.

Sulfur is the central atom, bonded to two bromine atoms, with one lone pair on sulfur.

Previous problemNext problem

Verified step by step guidance

Step 1: Determine the total number of valence electrons for the molecule SBr2. Sulfur (S) is in group 16 and has 6 valence electrons, and each bromine (Br) atom is in group 17 with 7 valence electrons. Calculate the total by adding these together: $6 + 2 \times 7$.

Step 2: Identify the central atom. Generally, the least electronegative atom (excluding hydrogen) is the central atom. Between sulfur and bromine, sulfur is less electronegative, so sulfur will be the central atom bonded to two bromine atoms.

Step 3: Draw single bonds between the central sulfur atom and each bromine atom. Each single bond represents 2 electrons shared between atoms, so subtract these bonding electrons from the total valence electrons.

Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule for each atom. Start by completing the octets of the outer atoms (bromine), then place any leftover electrons on the central atom (sulfur).

Step 5: Count the lone pairs on the central sulfur atom after distributing electrons. This will help determine which statement correctly describes the Lewis structure, focusing on the number of lone pairs on sulfur.