Which of the following compounds displays the greatest ionic character in its bonds?

• A. CO
• B. NaCl
• C. HCl
• D. CH4

Answer: (B)

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 (less covalent) the bond is.
2. Recall the electronegativity values of the elements involved: Sodium (Na) has a low electronegativity, Chlorine (Cl) has a high electronegativity, Carbon (C), Oxygen (O), and Hydrogen (H) have intermediate values.
3. Calculate or estimate the electronegativity difference for each compound: For example, for NaCl, subtract the electronegativity of Na from that of Cl; for HCl, subtract H from Cl; for CO, subtract C from O; and for CH4, subtract C from H.
4. Compare these differences: The compound with the largest electronegativity difference will have the greatest ionic character in its bonds.
5. Conclude that NaCl has the greatest ionic character because it involves a metal (Na) and a nonmetal (Cl) with a large electronegativity difference, leading to a highly ionic bond.