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

Formal Charges

Organic Chemistry

1. A Review of General Chemistry

Formal Charges

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5:08 minutes

Problem 63a,b

Textbook Question

Draw the missing lone-pair electrons and assign the missing formal charges for the following:
a.
b.

Verified step by step guidance

Step 1: Analyze the given structure. The molecule consists of a carbon atom bonded to three hydrogen atoms and an oxygen atom. The oxygen atom is also bonded to a hydrogen atom.

Step 2: Recall that oxygen typically has two lone pairs of electrons in its neutral state. Add two lone pairs to the oxygen atom to complete its octet.

Step 3: Calculate the formal charge for each atom. Use the formula: Formal charge = (Valence electrons) - (Non-bonding electrons) - (Bonding electrons / 2). For oxygen, valence electrons = 6, non-bonding electrons = 4 (two lone pairs), and bonding electrons = 4 (two bonds).

Step 4: Verify the formal charge for carbon. Carbon typically has a formal charge of 0 when it forms four bonds. In this structure, carbon is bonded to three hydrogens and one oxygen, satisfying its octet.

Step 5: Confirm the formal charge for hydrogen atoms. Hydrogen typically has a formal charge of 0 when it forms one bond. Each hydrogen atom in the structure is bonded to either carbon or oxygen, which is consistent with this rule.

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Key Concepts

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

Lone Pair Electrons

Lone pair electrons are pairs of valence electrons that are not involved in bonding and are localized on a single atom. They play a crucial role in determining the geometry and reactivity of molecules. Understanding how to identify and represent lone pairs is essential for accurately drawing Lewis structures and predicting molecular shapes.

Formal Charge

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and half the number of bonding electrons. It helps in assessing the stability of a molecule and determining the most favorable Lewis structure. Assigning formal charges correctly is vital for understanding the distribution of electrons in a molecule.

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 provide a visual representation of the arrangement of electrons and help predict molecular geometry and reactivity. Mastery of drawing Lewis structures is fundamental in organic chemistry for analyzing molecular interactions and properties.