Which of the following bonds is the most polar?

• A. C–H
• B. O–F
• C. N–O
• D. H–F

Answer: (D)

Verified step by step guidance

1. Understand that bond polarity depends on the difference in electronegativity between the two atoms involved in the bond. The greater the difference, the more polar the bond.
2. Recall the approximate electronegativity values for the relevant atoms: Hydrogen (H) ~2.1, Carbon (C) ~2.5, Nitrogen (N) ~3.0, Oxygen (O) ~3.5, Fluorine (F) ~4.0.
3. Calculate the electronegativity difference for each bond: For C–H, difference = |2.5 - 2.1|; for O–F, difference = |3.5 - 4.0|; for N–O, difference = |3.0 - 3.5|; and for H–F, difference = |2.1 - 4.0|.
4. Compare these differences to determine which bond has the largest electronegativity difference, indicating the most polar bond.
5. Conclude that the bond with the greatest electronegativity difference (H–F) is the most polar among the options given.