Arrange the bonds in each of the following sets in order of increasing polarity: (b) O—Cl,S—Br, C—P

Verified step by step guidance

1. Identify the electronegativity values for each element involved in the bonds: O, Cl, S, Br, C, and P.
2. Calculate the electronegativity difference for each bond: O—Cl, S—Br, and C—P.
3. Recall that the greater the difference in electronegativity between two atoms, the more polar the bond.
4. Compare the calculated electronegativity differences to determine the order of increasing polarity.
5. Arrange the bonds from the smallest to the largest electronegativity difference, indicating increasing polarity.

Key Concepts

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 will be. For example, oxygen is more electronegative than chlorine, leading to a polar bond in O—Cl.

Bond Polarity

Bond polarity refers to the distribution of electrical charge across a bond between two atoms. A bond is considered polar if there is a significant difference in electronegativity between the two atoms, resulting in a dipole moment. Nonpolar bonds occur when atoms have similar electronegativities, leading to an even distribution of charge.

Comparative Bond Analysis

Comparative bond analysis involves evaluating the bonds based on their electronegativity differences to determine their relative polarities. By comparing the electronegativities of the atoms involved in each bond, one can rank the bonds from least to most polar. This analysis is essential for understanding the behavior of molecules in various chemical contexts.