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 Lewis dot structures is the most likely structure for the neutral compound CO$_2$?

O--C=O, with one oxygen atom single-bonded and the other double-bonded to carbon, and the carbon atom having one lone pair

O--C--O, with each oxygen atom having three lone pairs and the carbon atom having two lone pairs

O=C=O, with each oxygen atom having two lone pairs

O=C--O, with one oxygen atom double-bonded and the other single-bonded to carbon, and the single-bonded oxygen having three lone pairs

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the CO$_2$ molecule. Carbon has 4 valence electrons, and each oxygen has 6 valence electrons, so total valence electrons = 4 + 2 \times 6 = 16.

Step 2: Draw a skeletal structure with carbon as the central atom bonded to two oxygen atoms. Connect each oxygen to carbon with a single bond initially, using 4 electrons (2 bonds \times 2 electrons each).

Step 3: Distribute the remaining electrons to satisfy the octet rule for the outer atoms (oxygen atoms first). Add lone pairs to oxygen atoms until each has 8 electrons total (including bonding electrons).

Step 4: Check the central atom (carbon) for an octet. If carbon does not have 8 electrons, form double bonds by converting lone pairs from oxygen atoms into bonding pairs between carbon and oxygen until carbon has a full octet.

Step 5: Verify the formal charges on each atom to ensure the most stable Lewis structure. The structure with the smallest formal charges (ideally zero) on all atoms and full octets is the most likely Lewis structure for CO$_2$.