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

5:54 minutes

Problem 36b

Textbook Question

For the molecules shown, indicate the direction of the dipole moment.
(b)

Verified step by step guidance

Step 1: Analyze the molecular structure provided. The molecule shown is carbon tetrachloride (CCl₄), which consists of a central carbon atom bonded to four chlorine atoms in a tetrahedral geometry.

Step 2: Consider the electronegativity of the atoms involved. Chlorine is more electronegative than carbon, meaning the electron density will be pulled toward the chlorine atoms in each C-Cl bond.

Step 3: Evaluate the symmetry of the molecule. Carbon tetrachloride is a symmetrical molecule, with the chlorine atoms evenly distributed around the central carbon atom in a tetrahedral arrangement.

Step 4: Determine the net dipole moment. Due to the symmetrical arrangement of the chlorine atoms, the individual dipole moments of the C-Cl bonds cancel each other out, resulting in no net dipole moment for the molecule.

Step 5: Conclude that the molecule is nonpolar. Since the dipole moments cancel out, carbon tetrachloride does not have a net dipole moment, and the direction of the dipole moment is effectively zero.

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 vector quantity that represents the separation of positive and negative charges in a molecule. It is determined by the difference in electronegativity between atoms and the geometry of the molecule. A molecule with a dipole moment has a positive end and a negative end, indicating the direction of electron density.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons within a chemical bond. In the context of carbon tetrachloride (CCl4), chlorine is more electronegative than carbon, leading to polar covalent bonds. The difference in electronegativity between carbon and chlorine contributes to the overall dipole moment of the molecule.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. In CCl4, the tetrahedral geometry results from the four chlorine atoms symmetrically surrounding the central carbon atom. This symmetrical arrangement causes the individual bond dipoles to cancel out, resulting in a net dipole moment of zero, making the molecule nonpolar despite the polar bonds.

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

A single bond between two carbons with different hybridizations has a small dipole. What is the direction of the dipole in the indicated bonds?

Textbook Question

For each of the following compounds,

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.

a. CH₃CH=NCH₃

b. CH₃CH₂OH

c. CBr₄

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.

b. Use this information to evaluate the relative importance of the following two resonance contributors:

Textbook Question

The C≡N triple bond in acetonitrile has a dipole moment of about 3.6 D and a bond length of about 1.16 Å. Calculate the amount of charge separation in this bond. How important is the charge-separated resonance form in the structure of acetonitrile?

Textbook Question

For the molecules shown, indicate the direction of the dipole moment.

(a)

Textbook Question

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

(a)

Textbook Question

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

(b)

Textbook Question

Carbon dioxide (CO₂) has no dipole moment (μ = 0 D). The related molecule sulfur dioxide (SO₂) does have a dipole moment (μ = 1.6 D) Explain this observation.

Show more practices

Download the Mobile app

Privacy

Do not sell my personal information

Accessibility

Patent notice

Sitemap

For the molecules shown, indicate the direction of the dipole moment.(b)

Key Concepts

Dipole Moment

Electronegativity

Molecular Geometry

Watch next

For the molecules shown, indicate the direction of the dipole moment.
(b)