Use the example bond energies of ionic versus covalent bonds to complete the activity. Ionic: Li–Br = 807 kJ/mol, NaCl = 787 kJ/mol Covalent: H–H = 432 kJ/mol, C–O = 358 kJ/mol What is the general trend you notice about the bond energies for ionic versus covalent bonds? What can be inferred from this pattern? What special attribute can explain why this difference occurs? Construct your argument in three to five sentences.

Answer 1

The bond energies for ionic compounds, such as Li–Br (807 kJ/mol) and NaCl (787 kJ/mol), are generally higher than those for covalent compounds like H–H (432 kJ/mol) and C–O (358 kJ/mol). This trend suggests that ionic bonds, which involve the electrostatic attraction between oppositely charged ions, are stronger than the covalent bonds formed by the sharing of electron pairs between atoms. The special attribute that explains this difference is the nature of the interactions: ionic bonds are formed through strong electrostatic forces, while covalent bonds are reliant on partial electron sharing, which creates less overall attraction. Consequently, the higher bond energies in ionic compounds indicate a greater stability and strength compared to those of covalent compounds.