Use the example bond energies of ionic versus covalent bonds to complete the activity.

Question

Ionic Bonds:
• Li−Br=807kJ/mol
• NaCl=787kJ/molCovalent Bonds:
• H−H=432kJ/mol
• C−O=358kJ/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 general trend observed from the bond energies of ionic versus covalent bonds indicates that ionic bonds typically have higher bond energies compared to covalent bonds. For instance, the bond energies for Li−Br and NaCl are significantly higher (807 kJ/mol and 787 kJ/mol, respectively) than those of the covalent bonds H−H (432 kJ/mol) and C−O (358 kJ/mol). This pattern suggests that ionic bonds, which result from the electrostatic attraction between oppositely charged ions, are generally stronger than covalent bonds that involve the sharing of electrons. The special attribute that explains this difference is the nature of the forces at play; ionic bonds stem from strong electrostatic interactions, while covalent bonds rely on shared electron pairs, which usually result in weaker attraction compared to the robust forces in ionic bonding.