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

4:33 minutes

Problem 46d,e,f

Textbook Question

Which of the following molecules would you expect to have a dipole moment of zero?
d. NH₃
e. H₂C═CH₂
f. H₂C═CHBr

Verified step by step guidance

Analyze the molecular geometry of each molecule. The dipole moment depends on the shape of the molecule and the distribution of electron density. For NH₃, the geometry is trigonal pyramidal due to the lone pair on nitrogen, which creates an asymmetrical distribution of charge.

For H₂C═CH₂ (ethylene), examine the molecular geometry. The molecule is planar, and the two carbon atoms are sp² hybridized. The symmetry of the molecule causes the dipole moments of the C-H bonds to cancel out.

For H₂C═CHBr, consider the geometry and the presence of the bromine atom. Bromine is more electronegative than hydrogen, creating a polar bond. The molecule is not symmetrical, so the dipole moments do not cancel out.

Compare the symmetry and electronegativity differences in each molecule. Molecules with symmetrical geometries and equal distribution of electronegativity (like H₂C═CH₂) will have a dipole moment of zero, while asymmetrical molecules (like NH₃ and H₂C═CHBr) will have a net dipole moment.

Conclude that H₂C═CH₂ is the molecule with a dipole moment of zero due to its symmetrical planar geometry and equal distribution of charge.

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.

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. Molecules with a dipole moment have a positive end and a negative end, while those with a dipole moment of zero are nonpolar, meaning their charge distribution is symmetrical.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. The shape of a molecule significantly influences its dipole moment. For example, molecules with symmetrical shapes, such as linear or tetrahedral arrangements, often have dipole moments of zero, as the individual bond dipoles cancel each other out.

Polarity of Bonds

The polarity of bonds is determined by the difference in electronegativity between the atoms involved. When two atoms with different electronegativities form a bond, the more electronegative atom attracts the shared electrons more strongly, creating a polar bond. In contrast, bonds between identical atoms or atoms with similar electronegativities are nonpolar, contributing to the overall polarity of the molecule.

Watch next

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

Start learning

Related Videos

Related Practice

Textbook Question

Account for the difference in the shape and color of the potential maps for ammonia and the ammonium ion in Section 1.11.

<IMAGE>

Textbook Question

Rank the bonds from most polar to least polar.

d. C—H, C—C, C—N

Textbook Question

Rank the bonds from most polar to least polar.

c. H—O, H—N, H—C

Textbook Question

Rank the bonds from most polar to least polar.

b. C—Cl, C—I, C—Br

Textbook Question

According to the potential map for the ammonium ion <IMAGE>, which atom has the greatest electron density?

Textbook Question

Two isomers of 1,2-dichloroethene are known. One has a dipole moment of 2.4 D; the other has zero dipole moment. Draw the two isomers, and explain why one has zero dipole moment.

CHCl=CHCl 1,2-dichloroethene

Textbook Question

1. Draw the Lewis structure.

2. Show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment.

3. Estimate whether the compound will have a large, small, or zero dipole moment.

g. HCN

h. CH₃CHO

i. H₂C=NH

Textbook Question

1. Draw the Lewis structure.

2. Show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment.

3. Estimate whether the compound will have a large, small, or zero dipole moment.

d. CH₃F

e. CF₄

f. CH₃OH

Show more practices

Download the Mobile app

Privacy

Do not sell my personal information

Accessibility

Patent notice

Sitemap

Which of the following molecules would you expect to have a dipole moment of zero? d. NH3 e. H2C═CH2 f. H2C═CHBr

Key Concepts

Dipole Moment

Molecular Geometry

Polarity of Bonds

Watch next

Which of the following molecules would you expect to have a dipole moment of zero?
d. NH₃
e. H₂C═CH₂
f. H₂C═CHBr