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 boron trichloride (BCl_3)?

B atom in the center with three double bonds to Cl atoms; each Cl atom has two lone pairs; B has no lone pairs.

B atom in the center with three single bonds to Cl atoms; each Cl atom has three lone pairs; B has no lone pairs.

B atom in the center with three single bonds to Cl atoms; each Cl atom has two lone pairs; B has one lone pair.

B atom in the center with three single bonds to Cl atoms; each Cl atom has one lone pair; B has two lone pairs.

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Verified step by step guidance

Step 1: Identify the total number of valence electrons available for bonding. Boron (B) has 3 valence electrons, and each chlorine (Cl) atom has 7 valence electrons. Since there are three Cl atoms, total valence electrons = 3 (from B) + 3 × 7 (from Cl) = 24 electrons.

Step 2: Determine the bonding framework. Boron is the central atom because it is less electronegative than chlorine. Connect the boron atom to each chlorine atom with a single bond initially. Each single bond represents 2 electrons.

Step 3: Distribute the remaining electrons as lone pairs on the chlorine atoms to complete their octets. Each Cl atom needs 8 electrons total (including bonding electrons). Since each Cl is bonded with one single bond (2 electrons), add 6 electrons (3 lone pairs) to each Cl atom.

Step 4: Check the boron atom's electron count. Boron is an exception to the octet rule and is stable with 6 electrons around it (3 single bonds × 2 electrons each). Therefore, boron has no lone pairs and does not form double bonds in BCl₃.

Step 5: Confirm the Lewis structure: Boron in the center with three single bonds to chlorine atoms; each chlorine atom has three lone pairs; boron has no lone pairs. This matches the correct Lewis dot structure for BCl₃.