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

Bonding Preferences

Organic Chemistry

1. A Review of General Chemistry

Bonding Preferences

Previous problemNext problem

4:58 minutes

Problem 49b

Textbook Question

Draw in all missing lone pairs for the following molecules.
(b)

Verified step by step guidance

Step 1: Identify atoms in the molecule that typically have lone pairs. Oxygen atoms are the most common atoms to have lone pairs in organic molecules.

Step 2: Analyze the structure. The molecule contains three oxygen atoms: one in a hydroxyl group (-OH), one in a carbonyl group (C=O), and one as part of a carboxylate group (-COO⁻).

Step 3: Assign lone pairs to the hydroxyl group (-OH). The oxygen in the hydroxyl group has two lone pairs because it is bonded to one hydrogen atom and follows the octet rule.

Step 4: Assign lone pairs to the carbonyl group (C=O). The oxygen in the carbonyl group has two lone pairs because it is double-bonded to carbon and follows the octet rule.

Step 5: Assign lone pairs to the carboxylate group (-COO⁻). The negatively charged oxygen in the carboxylate group has three lone pairs because the negative charge indicates an extra electron, and the other oxygen in the carboxylate group has two lone pairs as it is double-bonded to carbon.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above

Video duration:

Play a video:

Was this helpful?

Key Concepts

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

Lone Pairs

Lone pairs 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 where to place lone pairs is essential for accurately representing molecular structures and predicting molecular behavior.

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 are fundamental for understanding molecular geometry, resonance, and reactivity. Drawing complete Lewis structures, including all lone pairs, is vital for analyzing chemical properties.

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 bonds, and the number of lone pairs. It helps in assessing the stability of a molecule and determining the most favorable Lewis structure. Minimizing formal charges across a molecule often leads to more stable configurations.

Watch next

Master What is a valence electron? with a bite sized video explanation from Johnny

Start learning