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 represents the correct Lewis dot structure for the neutral compound sulfur dibromide (SBr2)?

A central S atom with two single bonds to Br atoms, and two lone pairs on S; each Br has three lone pairs.

A central S atom with single bonds to Br atoms, and no lone pairs on S; each Br has three lone pairs.

A central S atom with one single bond and one double bond to Br atoms, and one lone pair on S; each Br has two lone pairs.

A central S atom with double bonds to each Br atom, and no lone pairs on S; each Br has two lone pairs.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the molecule. Sulfur (S) is in group 16 and has 6 valence electrons, and each bromine (Br) atom is in group 17 with 7 valence electrons. Since there are two Br atoms, total valence electrons = 6 (S) + 2 × 7 (Br) = 20 electrons.

Step 2: Draw the skeletal structure with sulfur as the central atom bonded to two bromine atoms. Connect each Br to S with a single bond initially. Each single bond represents 2 electrons.

Step 3: Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for each atom. Start by completing the octets of the outer atoms (Br), then place any leftover electrons on the central atom (S).

Step 4: Check the formal charges on each atom to ensure the most stable structure. The formal charge is calculated by: $\text{Formal charge} = \text{Valence electrons} - \text{Nonbonding electrons} - \frac{1}{2} \times \text{Bonding electrons}$. The best Lewis structure has formal charges closest to zero.

Step 5: Confirm that the central sulfur atom has two single bonds to bromine atoms, two lone pairs on sulfur, and each bromine atom has three lone pairs, which satisfies the octet rule and results in minimal formal charges.