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 best Lewis dot structure for the neutral compound OCl_2?

O is the central atom with double bonds to each Cl atom; O has one lone pair, and each Cl has two lone pairs.

O is the central atom with single bonds to Cl atoms; O has three lone pairs, and each Cl has two lone pairs.

O is the central atom with two single bonds to Cl atoms; O has two lone pairs, and each Cl has three lone pairs.

Cl is the central atom with two single bonds to O atoms; Cl has two lone pairs, and each O has three lone pairs.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the molecule OCl_2. Oxygen (O) has 6 valence electrons, and each chlorine (Cl) atom has 7 valence electrons. Since there are two Cl atoms, calculate the total as: $6 + 2 \times 7$.

Step 2: Decide on the central atom. Generally, the least electronegative atom (except hydrogen) is the central atom. Between O and Cl, oxygen is less electronegative, so place O in the center and the two Cl atoms bonded to it.

Step 3: Draw single bonds between the central oxygen atom and each chlorine atom. Each single bond represents 2 electrons shared between atoms, so subtract these bonding electrons from the total valence electrons.

Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule for each atom. Start by completing the octets of the outer atoms (Cl), then place any leftover electrons on the central atom (O).

Step 5: Verify that all atoms have a complete octet (8 electrons around them) and that the total number of electrons used equals the total valence electrons calculated in Step 1. Adjust bonding (single or double bonds) if necessary to satisfy the octet rule and minimize formal charges.