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 Lewis dot structure of the neutral compound hydrogen peroxide (H2O2)?

Each oxygen atom is bonded to one hydrogen atom and to each other by a single bond; each oxygen has two lone pairs.

The two oxygen atoms are connected by a triple bond, and each oxygen is bonded to one hydrogen atom; each oxygen has one lone pair.

Each oxygen atom is bonded to one hydrogen atom and to each other by a double bond; each oxygen has two lone pairs.

Each oxygen atom is bonded to two hydrogen atoms and to each other by a double bond; each oxygen has one lone pair.

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Verified step by step guidance

Step 1: Identify the molecular formula and connectivity of hydrogen peroxide (H2O2). It consists of two oxygen atoms and two hydrogen atoms. Each hydrogen is bonded to an oxygen atom, and the two oxygen atoms are bonded to each other.

Step 2: Determine the type of bond between the two oxygen atoms. Consider the typical bonding patterns of oxygen, which usually forms two bonds to satisfy the octet rule. A single bond between the oxygens is common in H2O2.

Step 3: Assign lone pairs to each oxygen atom. Oxygen has six valence electrons, and after forming bonds, the remaining electrons are placed as lone pairs to complete the octet. Each oxygen typically has two lone pairs in H2O2.

Step 4: Confirm the bonding and lone pairs satisfy the octet rule for each oxygen atom and the duet rule for each hydrogen atom (which only needs two electrons).

Step 5: Conclude that the Lewis structure of H2O2 shows each oxygen bonded to one hydrogen and to each other by a single bond, with each oxygen having two lone pairs.