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

2. Molecular Representations

Intermolecular Forces

Organic Chemistry

2. Molecular Representations

Intermolecular Forces

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Multiple Choice

Which of these phenomena result from hydrogen bonding?

Nonpolar nature of methane

High boiling point of water

Weak van der Waals forces in noble gases

Low melting point of iodine

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Verified step by step guidance

Identify the nature of hydrogen bonding: Hydrogen bonding is a type of dipole-dipole interaction that occurs between molecules where hydrogen is covalently bonded to a highly electronegative atom, such as oxygen, nitrogen, or fluorine.

Consider the properties of water: Water (H₂O) is a polar molecule with hydrogen atoms bonded to oxygen, which is highly electronegative. This allows for hydrogen bonds to form between water molecules.

Analyze the effect of hydrogen bonding on boiling points: Hydrogen bonds are relatively strong intermolecular forces, which require more energy to break. This results in a higher boiling point for substances like water, where hydrogen bonding is prevalent.

Evaluate the other options: Methane (CH₄) is nonpolar and does not exhibit hydrogen bonding. Noble gases have weak van der Waals forces due to their full electron shells and lack of polarity. Iodine (I₂) is a nonpolar molecule with low melting points due to weak intermolecular forces.

Conclude which phenomenon is due to hydrogen bonding: The high boiling point of water is a direct result of hydrogen bonding, as it requires significant energy to overcome these strong intermolecular forces.