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 is the correct Lewis dot structure for phosphorus tribromide, PBr_3?

Phosphorus atom in the center with three single bonds to bromine atoms, and one lone pair on phosphorus; each bromine has three lone pairs.

Phosphorus atom in the center with three double bonds to bromine atoms, and no lone pairs on phosphorus; each bromine has two lone pairs.

Phosphorus atom in the center with three single bonds to bromine atoms, and no lone pairs on phosphorus; each bromine has three lone pairs.

Phosphorus atom in the center with three single bonds to bromine atoms, and two lone pairs on phosphorus; each bromine has two lone pairs.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available. Phosphorus (P) has 5 valence electrons, and each bromine (Br) atom has 7 valence electrons. Since there are three bromine atoms, calculate the total as: $5 + 3 \times 7 = 26$ valence electrons.

Step 2: Place the phosphorus atom in the center because it is less electronegative than bromine, and arrange the three bromine atoms around it.

Step 3: Form single bonds between the phosphorus atom and each bromine atom. Each single bond consists of 2 electrons, so 3 bonds use $3 \times 2 = 6$ electrons.

Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule. Start by placing lone pairs on the bromine atoms to complete their octets. Each bromine needs 8 electrons total (including bonding electrons), so add three lone pairs (6 electrons) to each bromine.

Step 5: Assign any leftover electrons to the phosphorus atom as lone pairs. Since phosphorus can have an expanded octet but typically in PBr$_3$ it has one lone pair, place one lone pair (2 electrons) on phosphorus to complete its octet.