Which one of the following bonds has the most ionic character?

• A. Na–Cl
• B. N–O
• C. H–Cl
• D. C–O

Answer: (A)

Verified step by step guidance

1. Understand that ionic character in a bond depends on the difference in electronegativity between the two atoms involved. The greater the difference, the more ionic the bond tends to be.
2. Look up or recall the electronegativity values of the atoms involved: Sodium (Na), Chlorine (Cl), Nitrogen (N), Oxygen (O), Hydrogen (H), and Carbon (C).
3. Calculate the electronegativity difference for each bond by subtracting the smaller electronegativity value from the larger one. For example, for Na–Cl, calculate \(\left| \chi_{\text{Na}} - \chi_{\text{Cl}} \right|\).
4. Compare the electronegativity differences for all the given bonds: Na–Cl, N–O, H–Cl, and C–O. The bond with the largest difference will have the most ionic character.
5. Conclude that the bond with the highest electronegativity difference is the most ionic, which in this case is expected to be Na–Cl due to the large difference between a metal and a nonmetal.