The following structure is an anion with three possible resonance contributors. One incomplete resonance form is shown below. Complete the given structure by adding nonbonding electrons and formal charges. Draw the two remaining resonance structures (in any order), including nonbonding electrons and formal charges.
Electronic Effects
The effect of electrons that are located in the chemical bonds within the atoms of the molecule is termed an electronic effect. The electronic effect is also explained as the effect through which the reactivity of the compound in one portion is controlled by the electron repulsion or attraction producing in another portion of the molecule.
Drawing Resonance Forms
In organic chemistry, resonance may be a mental exercise that illustrates the delocalization of electrons inside molecules within the valence bond theory of octet bonding. It entails creating several Lewis structures that, when combined, reflect the molecule's entire electronic structure. One Lewis diagram cannot explain the bonding (lone pair, double bond, octet) elaborately. A hybrid describes a combination of possible resonance structures that represents the entire delocalization of electrons within the molecule.
Using Molecular Structure To Predict Equilibrium
Equilibrium does not always imply an equal presence of reactants and products. This signifies that the reaction reaches a point when reactant and product quantities remain constant as the rate of forward and backward reaction is the same. Molecular structures of various compounds can help in predicting equilibrium.
The following structure is an anion with three possible resonance contributors. One incomplete resonance form is shown below. Complete the given structure by adding nonbonding electrons and formal charges. Draw the two remaining resonance structures (in any order), including nonbonding electrons and formal charges.
### Instructions
1. **Adding Nonbonding Electrons and Formal Charges:**
- Identify the lone pairs on each atom based on their typical valence electron count.
- Compute the formal charges for each atom and ensure the overall charge of the structure matches the given anion.
2. **Drawing Resonance Structures:**
- Use the net movement of electrons (lone pairs and pi bonds) to form the other resonance structures.
- Each contributed resonance structure should reflect the redistribution of electrons while keeping the net charge consistent.
## Resonance Structure Diagrams
Two more resonance structures need to be drawn, integrating nonbonding electrons and formal charges.
### Diagram: First Resonance Structure
*In the first empty grid*
### Diagram: Second Resonance Structure
*In the second empty grid*
Each resonance structure illustrates a possible distribution of pi electrons, ensuring the stabilization of the anion through delocalization.
## Conclusion
This exercise helps in understanding the concept of resonance, electron delocalization, and the significance of nonbonding electrons and formal charges. Mastery of these concepts is crucial for predicting the stability and reactivity of various organic and inorganic compounds.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F37e1710d-5d92-4416-9037-10beff7be39e%2Fac76861f-296e-4dcd-907b-643211895d7e%2Foakd3n.png&w=3840&q=75)
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