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

4:55 minutes

Problem 25

Textbook Question

Using only your intuition, rank the following covalent bonds in terms of their polarity (1 = most polar; 6 = least polar). [You can use the periodic trend of electronegativity, but don't use actual numbers.]
(a) C―C
(b) C―O
(c) C―H
(d) C―F
(e) C―Cl
(f) C―S

Verified step by step guidance

Step 1: Recall the concept of bond polarity. Bond polarity arises due to the difference in electronegativity between two atoms in a covalent bond. The greater the difference in electronegativity, the more polar the bond.

Step 2: Use the periodic trend of electronegativity. Electronegativity increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table. For example, fluorine (F) is the most electronegative element, while sulfur (S) is less electronegative than oxygen (O) or chlorine (Cl).

Step 3: Compare the electronegativity of carbon (C) with each of the other atoms in the bonds provided: (a) C―C (same atoms, no electronegativity difference, nonpolar bond), (b) C―O (oxygen is more electronegative than carbon), (c) C―H (carbon and hydrogen have a small electronegativity difference), (d) C―F (fluorine is much more electronegative than carbon), (e) C―Cl (chlorine is more electronegative than carbon, but less so than fluorine), and (f) C―S (sulfur is slightly less electronegative than carbon).

Step 4: Rank the bonds in terms of polarity based on the electronegativity differences. The bond with the largest electronegativity difference will be the most polar, and the bond with the smallest or no electronegativity difference will be the least polar.

Step 5: Arrange the bonds in order of polarity: (1 = most polar, 6 = least polar). Based on the periodic trends, the ranking should be: (1) C―F, (2) C―O, (3) C―Cl, (4) C―H, (5) C―S, (6) C―C. Verify this ranking by consulting Figure 2.20 as instructed in the problem.

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.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a covalent bond. It varies across the periodic table, generally increasing from left to right and decreasing from top to bottom. This property is crucial for determining bond polarity, as a greater difference in electronegativity between two atoms leads to a more polar bond.

Covalent Bonding

Covalent bonding occurs when two atoms share electrons to achieve a full outer shell, resulting in a stable molecule. The nature of the bond can vary in polarity depending on the electronegativity of the atoms involved. Understanding the types of covalent bonds—nonpolar, polar, and ionic—is essential for ranking their polarity.

Polarity of Bonds

The polarity of a bond refers to the distribution of electrical charge across the bond. A polar bond has a significant difference in electronegativity between the two atoms, leading to partial positive and negative charges. In contrast, nonpolar bonds have equal sharing of electrons. Recognizing the polarity helps in predicting molecular behavior and interactions.

Watch next

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

Start learning

Using only your intuition, rank the following covalent bonds in terms of their polarity (1 = most polar; 6 = least polar). [You can use the periodic trend of electronegativity, but don't use actual numbers.] (a) C―C (b) C―O (c) C―H (d) C―F (e) C―Cl (f) C―S

Key Concepts

Electronegativity

Covalent Bonding

Polarity of Bonds

Watch next

Using only your intuition, rank the following covalent bonds in terms of their polarity (1 = most polar; 6 = least polar). [You can use the periodic trend of electronegativity, but don't use actual numbers.]
(a) C―C
(b) C―O
(c) C―H
(d) C―F
(e) C―Cl
(f) C―S