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

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Problem 49d

Textbook Question

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

Verified step by step guidance

Step 1: Identify the atoms in the molecule that typically have lone pairs. In this structure, chlorine (Cl) is the atom that will have lone pairs because it is a halogen and typically has three lone pairs when bonded to one other atom.

Step 2: Recall that chlorine has seven valence electrons. When it forms a single bond, one electron is shared with the bonded atom, leaving six electrons to be arranged as three lone pairs.

Step 3: Draw the three lone pairs around the chlorine atom. These lone pairs should be evenly spaced to minimize electron repulsion, forming a tetrahedral-like arrangement with the bond.

Step 4: Examine the rest of the molecule. The positively charged carbon (indicated by the '+' sign) does not have lone pairs because it has lost an electron, resulting in a formal positive charge.

Step 5: Verify the structure to ensure that all atoms follow the octet rule where applicable, and that the formal charges are consistent with the given structure.

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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 how to identify and represent lone pairs is essential for accurately drawing molecular structures.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons. They provide a visual way to understand the arrangement of electrons and the connectivity of atoms. Mastery of drawing Lewis structures is fundamental in organic chemistry for predicting molecular behavior and reactivity.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are involved in forming bonds with other atoms. The number of valence electrons determines how an atom can bond and interact with others. Knowing how to count and distribute valence electrons is key to constructing accurate molecular representations.

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