Which of the following bonds is the most polar due to the greatest difference in electronegativity between the two atoms?

• A. N–O
• B. S–Cl
• C. C–H
• 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 or look up the electronegativity values of the atoms involved: Hydrogen (H), Fluorine (F), Nitrogen (N), Oxygen (O), Sulfur (S), Chlorine (Cl), and Carbon (C).
3. Calculate the electronegativity difference for each bond by subtracting the smaller electronegativity value from the larger one. For example, for H–F, calculate \(\left| \chi_{F} - \chi_{H} \right|\) where \(\chi\) represents electronegativity.
4. Compare the calculated differences for all bonds: N–O, S–Cl, C–H, and H–F. The bond with the largest difference is the most polar.
5. Conclude that since H–F has the greatest electronegativity difference among the options, it is the most polar bond.