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 neutral sulfur hexabromide (SBr_6)?

Sulfur is surrounded by six bromine atoms, each forming a single bond, and sulfur has no lone pairs.

Sulfur is surrounded by six bromine atoms, each forming a single bond, and sulfur has one lone pair.

Sulfur is surrounded by six bromine atoms, each forming a double bond, and sulfur has two lone pairs.

Sulfur is surrounded by four bromine atoms, each forming a single bond, and sulfur has two lone pairs.

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Verified step by step guidance

Identify the central atom and the surrounding atoms in the molecule SBr_6. Sulfur (S) is the central atom, and it is bonded to six bromine (Br) atoms.

Determine the total number of valence electrons available. Sulfur has 6 valence electrons, and each bromine atom has 7 valence electrons. Calculate the total valence electrons for the molecule by adding sulfur's and all bromines' valence electrons.

Distribute the electrons to form bonds between sulfur and each bromine atom. Each single bond consists of 2 electrons. Since there are six bromine atoms, assign 2 electrons per bond, totaling 12 electrons used in bonding.

Assign the remaining electrons as lone pairs to the bromine atoms first to complete their octets. Each bromine needs 6 more electrons (3 lone pairs) after bonding to sulfur.

Check the sulfur atom's electron count after bonding. Since sulfur can expand its octet, it can accommodate 12 electrons (6 bonds × 2 electrons each) and does not need any lone pairs. Confirm that this matches the Lewis structure where sulfur is bonded to six bromines with single bonds and has no lone pairs.