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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1:54 minutes

Problem 46a,b,c

Textbook Question

Which of the following molecules would you expect to have a dipole moment of zero?
a. CH₃CH₃
b. H₂C═O
c. CH₂Cl₂

Verified step by step guidance

Step 1: Understand the concept of dipole moment. A dipole moment arises when there is an uneven distribution of electron density in a molecule due to differences in electronegativity between bonded atoms. A molecule will have a dipole moment of zero if it is symmetrical and the bond dipoles cancel each other out.

Step 2: Analyze molecule (a) CH3CH3 (ethane). Ethane is a nonpolar molecule because it consists of two identical CH3 groups connected by a single bond. The molecule is symmetrical, and there is no net dipole moment as the bond dipoles cancel out.

Step 3: Analyze molecule (b) H2C═O (formaldehyde). Formaldehyde contains a polar C═O bond due to the significant electronegativity difference between carbon and oxygen. The molecule is not symmetrical, so the dipole moment does not cancel out, and the molecule has a net dipole moment.

Step 4: Analyze molecule (c) CH2Cl2 (dichloromethane). Dichloromethane has two polar C-Cl bonds and two C-H bonds. The molecule is not symmetrical because the chlorine atoms are more electronegative than hydrogen, leading to an uneven distribution of electron density. Therefore, CH2Cl2 has a net dipole moment.

Step 5: Conclude that the molecule with a dipole moment of zero is (a) CH3CH3, as it is the only molecule in the list that is symmetrical and nonpolar.

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Key Concepts

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

Molecular Polarity

Molecular polarity refers to the distribution of electrical charge across a molecule. A molecule is polar if it has a net dipole moment due to differences in electronegativity between atoms, leading to uneven charge distribution. Conversely, nonpolar molecules have symmetrical charge distributions, resulting in a dipole moment of zero.

Dipole Moment

The dipole moment is a vector quantity that measures the separation of positive and negative charges in a molecule. It is calculated as the product of the charge and the distance between the charges. A dipole moment of zero indicates that the molecule is nonpolar, meaning that the individual bond dipoles cancel each other out due to symmetry.

Symmetry in Molecules

Symmetry plays a crucial role in determining the polarity of a molecule. Molecules with symmetrical shapes, such as linear or tetrahedral arrangements, often have their dipole moments cancel out, resulting in nonpolar characteristics. In contrast, asymmetrical molecules typically exhibit a net dipole moment, indicating polarity.

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Related Practice

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:

g. I—Cl

h. H₂N—OH

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:

c. H₃C—NH₂

d. H₃C—Cl

Textbook Question

There are three isomers with molecular formula C₂H₂Cl₂. Draw their structures. Which one does not have a dipole moment?

Textbook Question

Explain why CH₃Cl has a greater dipole moment than CH₃F even though F is more electronegative than Cl.

Textbook Question

CH₃N₂⁺
HNO₃
N₃^-
CH₃CONH₂
O₃

b. Draw a structure for each of the species that shows approximate bond angles.

c. Which species have no dipole moment?

Textbook Question

Show the direction of the dipole moment in each of the following bonds (use the electronegativities given in [Table 1.3] ):

a. H3C—Br

b. H3C—Li

Textbook Question

Which of the following has a bond closest to the ionic end of the bond spectrum?

CH₃NH₂ CH₃CH₃ CH₃F CH₃OH

Textbook Question

Which of the following has a polar covalent bond?

CH₃NH₂ CH₃CH₃ CH₃F CH₃OH

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Which of the following molecules would you expect to have a dipole moment of zero? a. CH3CH3b. H2C═O c. CH2Cl2

Key Concepts

Molecular Polarity

Dipole Moment

Symmetry in Molecules

Watch next

Which of the following molecules would you expect to have a dipole moment of zero?
a. CH₃CH₃
b. H₂C═O
c. CH₂Cl₂