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)

Previous problemNext problem

2:59 minutes

Problem 133a

Textbook Question

Show the dipole arrow for each of the following bonds:
a. Si―Cl

Verified step by step guidance

Determine the electronegativity of each atom in the bond. Silicon (Si) has an electronegativity of approximately 1.90, and chlorine (Cl) has an electronegativity of approximately 3.16.

Calculate the difference in electronegativity between the two atoms: ΔEN = |EN(Cl) - EN(Si)|. This difference will help determine the polarity of the bond.

Since chlorine (Cl) has a higher electronegativity than silicon (Si), the shared electrons in the bond will be pulled closer to the chlorine atom, creating a partial negative charge (δ⁻) on Cl and a partial positive charge (δ⁺) on Si.

Draw the dipole arrow pointing from the less electronegative atom (Si) to the more electronegative atom (Cl). The arrow should have a cross at the tail (near Si) to indicate the positive end, and the arrowhead should point toward Cl to indicate the negative end.

Label the bond with the partial charges: δ⁺ near Si and δ⁻ near Cl, to clearly show the direction of the dipole moment.

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.

Dipole Moment

A dipole moment is a measure of the separation of positive and negative charges in a molecule, indicating the polarity of a bond. It arises when there is a difference in electronegativity between the two atoms involved in the bond, leading to an uneven distribution of electron density. The dipole is represented by an arrow pointing from the positive end to the negative end, with the length of the arrow indicating the strength of the dipole.

Electronegativity

Electronegativity is the tendency of an atom to attract electrons in a chemical bond. It is a key factor in determining the polarity of a bond; the greater the difference in electronegativity between two bonded atoms, the more polar the bond will be. In the case of the Si-Cl bond, silicon has a lower electronegativity compared to chlorine, resulting in a polar bond with a dipole moment.

Bond Polarity

Bond polarity refers to the distribution of electrical charge over the atoms joined by the bond. A bond can be classified as nonpolar if the electron density is evenly distributed, or polar if there is an unequal sharing of electrons. In the Si-Cl bond, the significant difference in electronegativity leads to a polar bond, which can be represented by a dipole arrow pointing towards the more electronegative chlorine atom.