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 best describes the correct Lewis dot structure for the neutral compound CH2?

Carbon is bonded to two hydrogen atoms and has two lone pairs.

Carbon is bonded to two hydrogen atoms and has a complete octet with four bonds.

Carbon is bonded to two hydrogen atoms and has two unpaired electrons.

Carbon is bonded to two hydrogen atoms and has one lone pair.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the molecule CH2. Carbon has 4 valence electrons, and each hydrogen has 1 valence electron, so total valence electrons = 4 + 2(1) = 6 electrons.

Step 2: Recognize that carbon typically forms four bonds to complete its octet, while hydrogen forms only one bond to fill its duet (2 electrons).

Step 3: Since there are only 6 valence electrons total, it is impossible for carbon to form four bonds (which would require 8 electrons) or to have two lone pairs (which would require 4 electrons as lone pairs plus bonding electrons).

Step 4: Consider that carbon can form two single bonds with the two hydrogens, using 4 electrons, and the remaining 2 electrons will be unpaired on carbon, resulting in two unpaired electrons rather than lone pairs.

Step 5: Conclude that the correct Lewis structure for CH2 is carbon bonded to two hydrogen atoms with two unpaired electrons on carbon, reflecting the molecule's radical nature and incomplete octet.