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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3:19 minutes

Problem 9

Textbook Question

Which of the following has
a. the most polar bond?
b. the least polar bond?
NaI LiBr Cl₂ KCl

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 greater the electronegativity difference, the more polar the bond.

Step 2: Identify the electronegativity values of the elements involved. Use the periodic table to find the approximate electronegativity values: Na (0.93), I (2.66), Li (0.98), Br (2.96), Cl (3.16), and K (0.82).

Step 3: Calculate the electronegativity difference for each bond: NaI, LiBr, Cl2, and KCl. For example, for NaI, subtract the electronegativity of Na from I: |2.66 - 0.93|. Repeat this for the other bonds.

Step 4: Compare the electronegativity differences. The bond with the largest electronegativity difference will be the most polar, and the bond with the smallest electronegativity difference will be the least polar.

Step 5: Note that Cl2 is a bond between two identical atoms, so its electronegativity difference is zero, making it nonpolar. Use this information to determine which bond is the least polar and which is the most polar.

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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, in a bond between sodium (Na) and iodine (I), the significant difference in their electronegativities results in a highly polar bond.

Ionic vs. Covalent Bonds

Bonds can be classified as ionic or covalent based on the nature of the electron sharing. Ionic bonds occur between metals and nonmetals, where electrons are transferred, leading to charged ions. Covalent bonds involve the sharing of electrons between nonmetals. The type of bond influences the polarity, with ionic bonds generally being more polar than covalent bonds.

Bond Polarity

Bond polarity refers to the distribution of electrical charge across a bond. A polar bond has a significant difference in electronegativity between the two atoms, resulting in partial positive and negative charges. In contrast, nonpolar bonds, like Cl2, have equal sharing of electrons, leading to no charge separation. Understanding bond polarity is crucial for determining the most and least polar bonds among the given compounds.

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Related Practice

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

Textbook Question

Explain why HCl has a smaller dipole moment than HF, even though the H—Cl bond is longer than the H—F bond.

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.

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Textbook Question

Rank the bonds from most polar to least polar.

d. C—H, C—C, C—N

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Which of the following has a. the most polar bond? b. the least polar bond? NaI LiBr Cl2 KCl

Key Concepts

Electronegativity

Ionic vs. Covalent Bonds

Bond Polarity

Watch next

Which of the following has
a. the most polar bond?
b. the least polar bond?
NaI LiBr Cl₂ KCl