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

Electronegativity

Organic Chemistry

1. A Review of General Chemistry

Electronegativity

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2:23 minutes

Problem 57d

Textbook Question

Rank the bonds from most polar to least polar.
d. C—H, C—C, C—N

Verified step by step guidance

Step 1: Understand the concept of bond polarity. Bond polarity arises due to the difference in electronegativity between the two atoms involved in the bond. The greater the difference in electronegativity, the more polar the bond.

Step 2: Recall the electronegativity values of the elements involved. Approximate electronegativity values are: Carbon (C) = 2.5, Hydrogen (H) = 2.1, and Nitrogen (N) = 3.0.

Step 3: Calculate the electronegativity difference for each bond: (1) For C—H, the difference is |2.5 - 2.1|. (2) For C—C, the difference is |2.5 - 2.5|. (3) For C—N, the difference is |2.5 - 3.0|.

Step 4: Compare the electronegativity differences. The bond with the largest difference is the most polar, and the bond with the smallest difference is the least polar.

Step 5: Rank the bonds from most polar to least polar based on the calculated electronegativity differences: C—N > C—H > C—C.

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Key Concepts

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

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. The difference in electronegativity between two bonded atoms determines the polarity of the bond; larger differences result in more polar bonds. For example, carbon (C) has a lower electronegativity than nitrogen (N), leading to a more polar C—N bond compared to C—C or C—H bonds.

Bond Polarity

Bond polarity refers to the distribution of electrical charge across a bond between two atoms. A polar bond occurs when there is an unequal sharing of electrons due to differences in electronegativity, resulting in partial positive and negative charges. In the context of the given bonds, the C—N bond is the most polar, followed by C—H, and C—C, which is nonpolar.

Dipole Moment

The dipole moment is a vector quantity that represents the polarity of a bond, calculated as the product of the charge difference and the distance between the charges. A higher dipole moment indicates a more polar bond. In the ranking of the bonds provided, the C—N bond has the highest dipole moment due to the significant electronegativity difference, while C—C has the lowest due to equal electronegativities.