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

Which of the following resonance structures for OCN⁻ will contribute most to the correct structure of OCN⁻?

Structure with a triple bond between C and N, and a single bond between O and C

Structure with a double bond between O and C, and a double bond between C and N

Structure with a single bond between O and C, and a double bond between C and N

Structure with a single bond between O and C, and a triple bond between C and N

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Verified step by step guidance

Identify the total number of valence electrons for the OCN⁻ ion. Oxygen (O) has 6 valence electrons, carbon (C) has 4, nitrogen (N) has 5, and the negative charge adds 1 more electron, totaling 16 valence electrons.

Draw the possible resonance structures for OCN⁻. Consider different arrangements of single, double, and triple bonds between the atoms while ensuring the total number of valence electrons remains 16.

Evaluate each resonance structure based on formal charges. The formal charge is calculated using the formula: \( \text{Formal Charge} = \text{Valence Electrons} - \text{Non-bonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons} \).

Determine the most stable resonance structure by minimizing formal charges. The structure with the smallest formal charges on each atom, and ideally with negative charges on the more electronegative atoms, will be the most stable.

Conclude that the structure with a triple bond between C and N, and a single bond between O and C, is the most stable due to optimal formal charge distribution, with the negative charge residing on the more electronegative oxygen atom.