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

Resonance Structures

General Chemistry

11. Bonding & Molecular Structure

Resonance Structures

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Multiple Choice

Determine which of the following drawings would be the best structure for the N₂O molecule.

All are equally stable

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Verified step by step guidance

Step 1: Begin by counting the total number of valence electrons available for the N2O molecule. Nitrogen (N) has 5 valence electrons and oxygen (O) has 6 valence electrons. Therefore, the total number of valence electrons for N2O is 5 + 5 + 6 = 16 electrons.

Step 2: Evaluate each structure (a, b, c) to ensure that the total number of valence electrons used in the structure matches the calculated total of 16 electrons. Check that each atom satisfies the octet rule, where possible.

Step 3: Consider the formal charges for each atom in the structures. The formal charge is calculated using the formula: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (Bonding Electrons/2). Calculate the formal charges for each atom in structures a, b, and c.

Step 4: Compare the formal charges calculated in Step 3. The most stable structure will have formal charges closest to zero, and any negative formal charge should ideally reside on the more electronegative atom, which is oxygen in this case.

Step 5: Analyze the resonance and bond order in each structure. The best structure will have a reasonable bond order and resonance stability, contributing to the overall stability of the molecule.