Which of the following bonds are polar? (a) C—O, (b) Sl—F, (c) N—Cl, (d) C—Cl. Which is the more electronegative atom in each polar bond?

Verified step by step guidance

1. insert step 1> Determine the electronegativity values of the elements involved in each bond. You can refer to a periodic table with electronegativity values for this purpose.
2. insert step 2> Compare the electronegativity values of the two atoms in each bond. A bond is considered polar if there is a significant difference in electronegativity between the two atoms.
3. insert step 3> For each bond, if the difference in electronegativity is greater than approximately 0.5, the bond is polar.
4. insert step 4> Identify the more electronegative atom in each polar bond. The more electronegative atom will attract the shared electrons more strongly, resulting in a partial negative charge.
5. insert step 5> List the polar bonds and indicate the more electronegative atom for each.

Key Concepts

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. In a bond between two different atoms, the atom with higher electronegativity will attract the shared electrons more strongly, leading to a polar bond.

Polar Bonds

A polar bond occurs when there is a significant difference in electronegativity between the two atoms involved in the bond. This difference causes an uneven distribution of electron density, resulting in a dipole moment where one end of the bond is slightly negative and the other slightly positive. Bonds are considered polar if the electronegativity difference is typically greater than 0.4.

Dipole Moment

The dipole moment is a vector quantity that represents the separation of positive and negative charges in a polar bond. It is calculated as the product of the charge difference and the distance between the charges. A larger dipole moment indicates a stronger polarity, which can influence the physical properties of molecules, such as solubility and boiling points.