Table of contents

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

1. A Review of General Chemistry

Lewis Structure

Organic Chemistry

1. A Review of General Chemistry

Lewis Structure

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Problem 55l

Textbook Question

How many valence electrons does each of the following contribute to a Lewis structure?
(l) ―1 charge

Verified step by step guidance

Understand the concept of valence electrons: Valence electrons are the outermost electrons of an atom that participate in chemical bonding. For a Lewis structure, we count the valence electrons of all atoms and adjust for any charges present.

Recognize the effect of a negative charge: A negative charge (−1) indicates that the molecule or ion has gained one extra electron. This extra electron must be added to the total count of valence electrons.

Determine the total valence electrons: First, calculate the sum of the valence electrons for all atoms in the molecule or ion. Then, add one additional electron to account for the −1 charge.

Write the Lewis structure: Use the total number of valence electrons (including the extra electron from the −1 charge) to distribute electrons around the atoms, ensuring that each atom satisfies the octet rule (or duet rule for hydrogen) where applicable.

Verify the structure: Ensure that the total number of electrons in the Lewis structure matches the calculated total valence electrons, and confirm that the formal charges on the atoms are consistent with the overall −1 charge.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial for determining how an atom will bond with others. They are involved in chemical bonding and reactions, and their number can vary depending on the element. For example, carbon has four valence electrons, while oxygen has six. Understanding the number of valence electrons helps in predicting the structure and reactivity of molecules.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds between atoms. This visual representation helps chemists understand the arrangement of electrons and the overall geometry of the molecule, which is essential for predicting its chemical behavior.

Charge Contribution

In the context of Lewis structures, the charge of an ion affects the total number of valence electrons considered. A negatively charged ion (anion) contributes additional electrons, while a positively charged ion (cation) has fewer. For example, a species with a -1 charge contributes one extra valence electron to the Lewis structure, which must be accounted for when drawing the structure and determining the overall electron count.

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