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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2:25 minutes

Problem 57c

Textbook Question

Rank the bonds from most polar to least polar.
c. H—O, H—N, H—C

Verified step by step guidance

Determine the concept of bond polarity: Bond polarity arises due to the difference in electronegativity between the two atoms in a bond. The greater the difference in electronegativity, the more polar the bond.

Identify the electronegativity values of the atoms involved: Use the Pauling scale to find the electronegativity values. For reference: H = 2.1, O = 3.5, N = 3.0, C = 2.5.

Calculate the electronegativity differences for each bond: Subtract the electronegativity of hydrogen (H) from the electronegativity of the other atom in the bond. For example, for H—O, the difference is |3.5 - 2.1|.

Compare the electronegativity differences: Rank the bonds based on the magnitude of the electronegativity differences. A larger difference indicates a more polar bond.

List the bonds in order from most polar to least polar based on the calculated differences: This will provide the ranking of H—O, H—N, and H—C in terms of bond polarity.

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Key Concepts

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

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. The greater the difference in electronegativity between two bonded atoms, the more polar the bond becomes. For example, oxygen is more electronegative than hydrogen, leading to a polar bond in H—O.

Polarity of Bonds

The polarity of a bond is determined by the distribution of electrical charge across the bond. A polar bond occurs when there is a significant difference in electronegativity between the two atoms, resulting in a dipole moment. In the context of the question, H—O is the most polar due to the high electronegativity of oxygen compared to hydrogen.

Comparison of Bond Polarities

To rank bond polarities, one must compare the electronegativity values of the atoms involved. In the given bonds, H—O is the most polar, followed by H—N, and then H—C, as carbon has a lower electronegativity than nitrogen and oxygen. This ranking reflects the increasing ability of the atoms to attract shared electrons.

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Related Practice

Textbook Question

Which of the following molecules would you expect to have a dipole moment of zero?

g. BeCl₂

h. BF₃

Textbook Question

If the dipole moment of CH₃F is 1.847 D and the dipole moment of CD₃F is 1.858 D, which is more electronegative: hydrogen or deuterium?

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.

b. C—Cl, C—I, C—Br

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

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

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Rank the bonds from most polar to least polar. c. H—O, H—N, H—C

Key Concepts

Electronegativity

Polarity of Bonds

Comparison of Bond Polarities

Watch next

Rank the bonds from most polar to least polar.
c. H—O, H—N, H—C