Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

4. Molecular Compounds

Dipole Moment (Simplified)

GOB Chemistry

4. Molecular Compounds

Dipole Moment (Simplified)

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2:42 minutes

Problem 131c

Textbook Question

Select the more polar bond in each of the following pairs:
c. Br―Cl or S―Cl

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.

Look up the electronegativity values of the elements involved: Bromine (Br), Chlorine (Cl), and Sulfur (S). For reference, the electronegativity values are approximately: Br = 2.8, Cl = 3.0, and S = 2.5.

Calculate the electronegativity difference for each bond: For Br―Cl, subtract the electronegativity of Br from Cl (|3.0 - 2.8|). For S―Cl, subtract the electronegativity of S from Cl (|3.0 - 2.5|).

Compare the electronegativity differences: The bond with the larger electronegativity difference will be more polar.

Conclude which bond is more polar based on the comparison of the electronegativity differences.

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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. In the context of the given pairs, understanding the electronegativity values of bromine, chlorine, and sulfur is essential to determine which bond is more polar.

Bond Polarity

Bond polarity refers to the distribution of electrical charge across a bond between two atoms. A polar bond occurs when there is a significant difference in electronegativity, leading to an unequal sharing of electrons. This results in a dipole moment, where one end of the bond is slightly negative and the other slightly positive, influencing the bond's overall polarity.

Dipole Moment

The dipole moment is a vector quantity that represents the separation of positive and negative charges in a bond. It is calculated as the product of the charge difference and the distance between the charges. A higher dipole moment indicates a more polar bond, making it a crucial factor in comparing the polarity of the bonds in the given pairs.