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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3:29 minutes

Problem 60d

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)

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Count the total number of valence electrons available for the molecule. In this case, you are given 12 valence electrons to work with.

Determine the central atom. Typically, the least electronegative atom (excluding hydrogen) is placed at the center of the structure.

Place single bonds (represented as lines) between the central atom and the surrounding atoms. Each single bond uses 2 electrons.

Distribute the remaining electrons as lone pairs around the outer atoms to satisfy their octet rule (8 electrons around each atom, except for hydrogen which only needs 2).

If there are still electrons left after satisfying the octet for the outer atoms, place the remaining electrons as lone pairs on the central atom. If the central atom does not have a full octet, consider forming double or triple bonds by sharing lone pairs from the outer atoms.

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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 use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules.

Octet Rule

The octet rule is a chemical rule of thumb that states atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. This rule is fundamental in determining how atoms will bond and interact in a molecule, particularly in covalent bonding.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom that are involved in forming bonds with other atoms. The number of valence electrons determines how an atom can bond and interact with others, influencing the structure and stability of molecules. In the context of the question, knowing the total number of valence electrons available is crucial for completing the Lewis structure correctly.

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Related Practice

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

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

(f) C vs. F

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•

Textbook Question

In addition to radicals, anions, and cations, a fourth class of reactive intermediates is carbenes. A neutral species, the simplest carbene has a molecular formula of CH₂.

(a) Draw the Lewis structure of CH₂.

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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)

Key Concepts

Lewis Structures

Octet Rule

Valence Electrons

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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)