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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5:04 minutes

Problem 37a,b,c

Textbook Question

Draw complete Lewis structures, including lone pairs, for the following compounds.
(a)
(b)
(c)

Verified step by step guidance

Identify the total number of valence electrons for each compound. For pyridine (C5H5N), count the valence electrons from carbon (4 each), hydrogen (1 each), and nitrogen (5).

Draw the skeletal structure for pyridine, ensuring that the nitrogen atom is part of the six-membered ring and alternating double bonds are present. Add lone pairs to the nitrogen atom to complete its octet.

For pyrrolidine (C4H9N), count the valence electrons from carbon, hydrogen, and nitrogen. Draw a five-membered ring with nitrogen, ensuring that nitrogen has a lone pair and a hydrogen atom attached to it.

For furan (C4H4O), count the valence electrons from carbon, hydrogen, and oxygen. Draw a five-membered ring with oxygen, ensuring that oxygen has two lone pairs and alternating double bonds are present in the ring.

Check each structure to ensure that all atoms have complete octets (except hydrogen, which should have a duet) and that the total number of valence electrons used matches the number calculated initially.

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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 of a molecule and the lone pairs of electrons that may exist. They are essential for visualizing the arrangement of electrons in molecules, showing how atoms are bonded and the presence of any lone pairs. This helps in predicting the geometry, reactivity, and properties of the molecule.

Heterocyclic Compounds

Heterocyclic compounds are cyclic compounds that have atoms of at least two different elements as members of their ring(s). In the given question, pyridine, pyrrolidine, and furan are examples of heterocycles containing nitrogen and oxygen atoms. Understanding the role of these heteroatoms is crucial as they influence the electronic structure and reactivity of the compounds.

Lone Pairs and Formal Charge

Lone pairs are pairs of valence electrons that are not shared with another atom and are sometimes represented in Lewis structures. They can affect the shape and reactivity of molecules. Formal charge is a concept used to determine the charge distribution within a molecule, calculated by assuming equal sharing of electrons in bonds. Correctly assigning lone pairs and formal charges is vital for accurate Lewis structures.