Rank the bonds from most polar to least polar.
c. H—O, H—N, H—C

Verified step by step guidance

1. 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.
2. Identify the electronegativity values of the atoms involved: Use the Pauling scale to find the electronegativity values. For reference: H = 2.1, O = 3.5, N = 3.0, C = 2.5.
3. Calculate the electronegativity differences for each bond: Subtract the electronegativity of hydrogen (H) from the electronegativity of the other atom in the bond. For example, for H—O, the difference is |3.5 - 2.1|.
4. Compare the electronegativity differences: Rank the bonds based on the magnitude of the electronegativity differences. A larger difference indicates a more polar bond.
5. List the bonds in order from most polar to least polar based on the calculated differences: This will provide the ranking of H—O, H—N, and H—C in terms of bond 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 becomes. For example, oxygen is more electronegative than hydrogen, leading to a polar bond in H—O.

Polarity of Bonds

The polarity of a bond is determined by the distribution of electrical charge across the bond. A polar bond occurs when there is a significant difference in electronegativity between the two atoms, resulting in a dipole moment. In the context of the question, H—O is the most polar due to the high electronegativity of oxygen compared to hydrogen.

Comparison of Bond Polarities

To rank bond polarities, one must compare the electronegativity values of the atoms involved. In the given bonds, H—O is the most polar, followed by H—N, and then H—C, as carbon has a lower electronegativity than nitrogen and oxygen. This ranking reflects the increasing ability of the atoms to attract shared electrons.