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 statements correctly describes the Lewis dot structure of the neutral compound Cl2O?

The oxygen atom is bonded to two chlorine atoms, with one lone pair on oxygen and four lone pairs on each chlorine.

The oxygen atom forms a double bond with one chlorine and a single bond with the other, with one lone pair on oxygen.

The oxygen atom is bonded to two chlorine atoms, with two lone pairs on oxygen and three lone pairs on each chlorine.

The oxygen atom is bonded to one chlorine atom and has three lone pairs, while the other chlorine is not bonded.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the molecule Cl2O. Chlorine (Cl) has 7 valence electrons each, and oxygen (O) has 6 valence electrons. Calculate the sum: $2 \times 7 + 6$.

Step 2: Draw a skeletal structure for Cl2O. Since oxygen is less electronegative than chlorine, oxygen is typically the central atom bonded to two chlorine atoms.

Step 3: Connect the atoms with single bonds initially. Each single bond represents 2 electrons shared between atoms. 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. Oxygen typically has 2 lone pairs (4 electrons), and each chlorine atom typically has 3 lone pairs (6 electrons) to complete their octets.

Step 5: Verify the structure by checking that each atom has a complete octet and that the total number of electrons used (bonding + lone pairs) equals the total valence electrons calculated in Step 1.