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 correct Lewis dot structure for hydrogen peroxide (H2O2)?

H–O=O–H, with each O atom having one lone pair

H–O–O–H, with each O atom having three lone pairs

H–O–O–H, with each O atom having two lone pairs

H–O–O–H, with no lone pairs on the O atoms

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Verified step by step guidance

Step 1: Determine the total number of valence electrons in hydrogen peroxide (H2O2). Hydrogen has 1 valence electron each, and oxygen has 6 valence electrons each. Calculate the sum: $2 \times 1 + 2 \times 6$.

Step 2: Draw the skeletal structure connecting the atoms. Since H atoms can only form one bond, and O atoms can form two bonds, connect the atoms as H–O–O–H.

Step 3: Assign bonding electrons to the bonds between atoms. Each single bond represents 2 electrons. Count these electrons and subtract from the total valence electrons to find the remaining electrons to be placed as lone pairs.

Step 4: Distribute the remaining electrons as lone pairs on the oxygen atoms to satisfy the octet rule. Each oxygen atom should have enough lone pairs so that it has 8 electrons total (counting bonding and lone pairs).

Step 5: Verify the structure by checking that each atom has a complete octet (or duet for hydrogen) and that the total number of electrons used equals the total valence electrons calculated in Step 1.