Which of the following bonds has the largest electronegativity difference?

• A. O–Cl
• B. Na–F
• C. N–O
• D. C–H

Answer: (B)

Verified step by step guidance

1. Identify the electronegativity values of each element involved in the bonds. Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. Commonly used values are from the Pauling scale.
2. List the electronegativity values for each element: for example, Oxygen (O), Chlorine (Cl), Sodium (Na), Fluorine (F), Nitrogen (N), Carbon (C), and Hydrogen (H).
3. Calculate the electronegativity difference for each bond by subtracting the smaller electronegativity value from the larger one: \(\Delta EN = |EN_1 - EN_2|\).
4. Compare the calculated electronegativity differences for all the bonds: O–Cl, Na–F, N–O, and C–H.
5. The bond with the largest electronegativity difference is the one where the two atoms have the greatest difference in their ability to attract electrons, which often corresponds to a more ionic character.