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 59f

Textbook Question

Which atom in each pair would you expect to be the central atom in a Lewis structure?
(f) C vs. F

Verified step by step guidance

Identify the general rule for selecting a central atom in a Lewis structure: The central atom is typically the least electronegative element, as it is more likely to share its electrons and form bonds with surrounding atoms.

Compare the electronegativities of carbon (C) and fluorine (F). Carbon has an electronegativity of approximately 2.5, while fluorine has the highest electronegativity of all elements, approximately 4.0.

Since carbon is less electronegative than fluorine, it is more likely to serve as the central atom in a Lewis structure.

Consider the bonding capacity of each atom. Carbon typically forms four bonds due to its four valence electrons, making it well-suited to act as a central atom. Fluorine, on the other hand, usually forms only one bond because it has seven valence electrons and needs only one more to complete its octet.

Conclude that carbon (C) is the preferred central atom in this pair when constructing a Lewis structure, as it is less electronegative and has a higher bonding capacity than fluorine (F).

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Key Concepts

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

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 help visualize the arrangement of electrons and the connectivity of atoms, which is crucial for predicting molecular geometry and reactivity.

Central Atom

The central atom in a Lewis structure is typically the atom that can form the most bonds or has the highest valency. It is usually the least electronegative atom in a molecule, as it can effectively bond with surrounding atoms to create a stable structure.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. In the context of determining the central atom, the atom with lower electronegativity is often preferred, as it is more likely to share its electrons and form bonds with other atoms.

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Related Practice

Textbook Question

How many valence electrons does each of the following contribute to a Lewis structure?

(l) ―1 charge

Textbook Question

Show how the Lewis dot structure for each of the following atoms would overlap to form a single bond.

(b) C and O

Textbook Question

Which atom in each pair would you expect to be the central atom in a Lewis structure?

(b) C vs. O

Textbook Question

Which atom in each pair would you expect to be the central atom in a Lewis structure?

(d) C vs. N

Textbook Question

Given the atoms involved and the number of valence electrons remaining, complete the Lewis structure by placing bonds between atoms such that each has a full octet.

(d)

Textbook Question

Given the atoms involved and the number of valence electrons remaining, complete the Lewis structure by placing bonds between atoms such that each has a full octet.

(e)

Textbook Question

Draw the Lewis structure for the following molecular formulas.

(l) SO₄^2-

Textbook Question

Draw Lewis structures for the following free radicals.

a. The ethyl radical, CH₃—ĊH₂

b. The tert-butyl radical, (CH₃)₃C•

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