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

Previous problemNext problem

6:09 minutes

Problem 5a,b

Textbook Question

For each pair of compounds, predict which one has the higher molecular dipole moment, and explain your reasoning.
a. ethyl chloride or ethyl iodide
b. 1-bromopropane or cyclopropane

Verified step by step guidance

Step 1: Understand the concept of molecular dipole moment. The dipole moment is a measure of the separation of positive and negative charges in a molecule. It depends on the electronegativity of atoms and the geometry of the molecule.

Step 2: Analyze the electronegativity of the halogens involved. Chlorine is more electronegative than iodine, which means it will create a larger dipole moment when bonded to carbon. Compare ethyl chloride (C2H5Cl) and ethyl iodide (C2H5I) based on this property.

Step 3: Consider the molecular geometry and bond polarity for ethyl chloride and ethyl iodide. The C-Cl bond is more polar than the C-I bond due to the higher electronegativity of chlorine, leading to a higher dipole moment for ethyl chloride.

Step 4: For 1-bromopropane (C3H7Br) and cyclopropane (C3H6), evaluate the presence of polar bonds. 1-bromopropane has a polar C-Br bond, while cyclopropane is a non-polar molecule due to its symmetrical ring structure.

Step 5: Conclude that 1-bromopropane will have a higher dipole moment than cyclopropane because it contains a polar bond, whereas cyclopropane's symmetrical structure results in no net dipole moment.

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.

Molecular Dipole Moment

The molecular dipole moment is a measure of the overall polarity of a molecule, determined by the vector sum of all individual bond dipoles. It depends on both the difference in electronegativity between bonded atoms and the geometry of the molecule. A higher dipole moment indicates a more polar molecule, which affects properties like solubility and boiling point.

Electronegativity

Electronegativity is the tendency of an atom to attract electrons in a chemical bond. In a molecule, the atom with higher electronegativity will attract shared electrons more strongly, creating a dipole. The difference in electronegativity between atoms in a bond contributes to the bond's polarity, influencing the overall dipole moment of the molecule.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. It plays a crucial role in determining the dipole moment, as the spatial orientation of polar bonds can either enhance or cancel out the overall dipole. For example, linear or symmetrical geometries may result in a net dipole moment of zero, even if individual bonds are polar.

Watch next

Master Differences between ionic, polar and covalent bonds with a bite sized video explanation from Johnny

Start learning

For each pair of compounds, predict which one has the higher molecular dipole moment, and explain your reasoning. a. ethyl chloride or ethyl iodide b. 1-bromopropane or cyclopropane

Key Concepts

Molecular Dipole Moment

Electronegativity

Molecular Geometry

Watch next

For each pair of compounds, predict which one has the higher molecular dipole moment, and explain your reasoning.
a. ethyl chloride or ethyl iodide
b. 1-bromopropane or cyclopropane