Arrange the bonds in each of the following sets in order of increasing polarity: (c) C—S, B— F, N — O.

Verified step by step guidance

1. Identify the concept of bond polarity: Bond polarity is determined by the difference in electronegativity between the two atoms involved in the bond. The greater the difference, the more polar the bond.
2. List the electronegativities of the elements involved: Carbon (C) = 2.55, Sulfur (S) = 2.58, Boron (B) = 2.04, Fluorine (F) = 3.98, Nitrogen (N) = 3.04, Oxygen (O) = 3.44.
3. Calculate the electronegativity differences for each bond: C—S, B—F, and N—O.
4. Compare the electronegativity differences: The bond with the smallest difference is the least polar, and the bond with the largest difference is the most polar.
5. Arrange the bonds in order of increasing polarity based on the calculated electronegativity differences.

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, fluorine is the most electronegative element, which significantly influences the polarity of bonds involving fluorine.

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 between the two atoms, leading to a dipole moment. Nonpolar bonds, on the other hand, occur when the electronegativities are similar, resulting in an even distribution of charge.

Comparative Bond Analysis

Comparative bond analysis involves evaluating the bonds in a set based on their polarity by comparing the electronegativities of the atoms involved. By determining the electronegativity values for each atom in the bonds C—S, B—F, and N—O, one can rank the bonds from least to most polar, providing insight into their chemical behavior.