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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Problem 11e,f

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

Verified step by step guidance

Step 1: Understand the concept of bond polarity. Bond polarity arises due to the difference in electronegativity between two atoms in a bond. The atom with higher electronegativity attracts the shared electrons more strongly, acquiring a partial negative charge (δ−), while the less electronegative atom acquires a partial positive charge (δ+).

Step 2: Analyze the electronegativity of the atoms in the HO—Br bond. Oxygen (O) has a higher electronegativity compared to bromine (Br). Therefore, the shared electrons in the bond will be closer to the oxygen atom, making oxygen δ− and bromine δ+.

Step 3: Represent the polarity of the HO—Br bond using δ+ and δ− symbols. Place δ− on the oxygen atom and δ+ on the bromine atom to indicate the direction of electron density shift.

Step 4: Analyze the electronegativity of the atoms in the H3C—Li bond. Carbon (C) is more electronegative than lithium (Li). As a result, the shared electrons in the bond will be closer to the carbon atom, making carbon δ− and lithium δ+.

Step 5: Represent the polarity of the H3C—Li bond using δ+ and δ− symbols. Place δ− on the carbon atom and δ+ on the lithium atom to indicate the direction of electron density shift.

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Key Concepts

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

Polarity of Bonds

Polarity in chemical bonds arises from the difference in electronegativity between the atoms involved. When two atoms form a bond, the atom with higher electronegativity attracts the shared electrons more strongly, resulting in a partial negative charge (δ−) on that atom and a partial positive charge (δ+) on the other. This creates a dipole moment, indicating the direction of electron density and the bond's polarity.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It varies across the periodic table, with elements like fluorine being highly electronegative. Understanding the relative electronegativities of the atoms in a bond helps predict the bond's polarity, as greater differences lead to more polar bonds.

Dipole Moment

A dipole moment is a vector quantity that represents 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. In the context of polar bonds, the dipole moment points from the positive end (δ+) to the negative end (δ−), indicating the direction of the bond's polarity and influencing the molecule's overall behavior in electric fields.

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Related Practice

Textbook Question

(a) Rank the following bonds in terms of the strength of their bond dipole (1 = weakest, 6 = strongest).

(b) Which carbon has the largest δ⁺ ?

C―F, C―Br, C―I, C―H, C―C, C―Cl

Textbook Question

A mixture of seven amino acids (glycine, glutamate, leucine, lysine, alanine, isoleucine, and aspartate) is separated by chromatography. Explain why only six spots show up when the chromatographic plate is coated with ninhydrin and heated.

Textbook Question

Based on your answer to Assessment 2.22, would you expect a larger atom to be more or less electronegative than a smaller atom?

Textbook Question

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

(e)

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

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

Textbook Question

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

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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—Brf. H3C—Li

Key Concepts

Polarity of Bonds

Electronegativity

Dipole Moment

Watch next

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