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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2:56 minutes

Problem 6

Textbook Question

Which of the following compounds have a dipole moment of zero?

Verified step by step guidance

Step 1: Understand the concept of dipole moment. Dipole moment arises due to the difference in electronegativity between atoms in a molecule and the asymmetry in the molecular geometry. A molecule will have a dipole moment of zero if the individual bond dipoles cancel each other out due to symmetry.

Step 2: Analyze compound A. The molecule has two chlorine atoms and two hydrogen atoms symmetrically arranged around the double bond. The molecule is symmetrical, and the bond dipoles cancel each other out, resulting in a dipole moment of zero.

Step 3: Analyze compound B. The molecule has one chlorine atom and one hydrogen atom on each carbon of the double bond. The arrangement is not symmetrical, and the bond dipoles do not cancel each other out, resulting in a nonzero dipole moment.

Step 4: Analyze compound C. The molecule has two chlorine atoms on one carbon and two hydrogen atoms on the other carbon of the double bond. This arrangement is asymmetrical, and the bond dipoles do not cancel each other out, resulting in a nonzero dipole moment.

Step 5: Analyze compound D. The molecule has one chlorine atom and one hydrogen atom on each carbon of the double bond, but the arrangement is symmetrical. The bond dipoles cancel each other out, resulting in a dipole moment of zero.

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Key Concepts

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

Dipole Moment

A dipole moment is a measure of the separation of positive and negative charges in a molecule. It occurs when there is an uneven distribution of electron density, leading to a polar bond. The dipole moment is a vector quantity, having both magnitude and direction, and is crucial for understanding molecular polarity and interactions.

Molecular Symmetry

Molecular symmetry refers to the balanced arrangement of atoms in a molecule. Symmetrical molecules, such as those with a uniform distribution of charge, often have a dipole moment of zero. Understanding symmetry helps predict the physical properties of molecules, including their polarity and reactivity.

Polar vs. Nonpolar Molecules

Polar molecules have a significant dipole moment due to the presence of polar bonds and an asymmetrical shape, while nonpolar molecules have no net dipole moment. Nonpolar molecules can arise from symmetrical arrangements of identical atoms or from the cancellation of dipole moments in larger molecules, making it essential to analyze molecular structure to determine polarity.

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Related Practice

Textbook Question

Given the Lewis structures, indicate the direction of the dipole moment, if there is one.

(e)

Textbook Question

Use the symbols δ⁺ and δ⁻ to show the direction of the polarity of the indicated bond in each of the following compounds:

e. HO—Br

f. H₃C—Li

Textbook Question

After examining the potential maps for LiH, HF, and H₂, answer the following questions:

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a. Which compounds are polar?

b. Why does LiH have the largest hydrogen?

c. Which compound has the hydrogen that would be most apt to attract a negatively charged molecule?

Textbook Question

Rank the following compounds from highest dipole moment to lowest dipole moment:

Textbook Question

In what direction is the dipole moment in calicene? Explain.

Textbook Question

The C=O double bond has a dipole moment of about 2.4 D and a bond length of about 1.23 Å.

a. Calculate the amount of charge separation in this bond.

Textbook Question

1. From what you remember of electronegativities, show the direction of the dipole moments of the following bonds.

2. In each case, predict whether the dipole moment is relatively large (electronegativity difference >0.5) or small.

a. C—Cl

b. C—H

c. C—Li

d. C—N

e. C—O

Textbook Question

For each alkene, indicate the direction of the dipole moment. For each pair, determine which compound has the larger dipole moment

b. cis-1,2-dibromoethene or trans-2,3-dibromobut-2-ene

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