Question

Use the examples:

Ionic bonds: Li-Br = 807kj/mol NaCl = 787 kj/mol
Covalent bonds: H-H = 432 kj/mol, C-O = 358 kj/mol

What is the general trend you see 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 3 or more sentences

Answer 1

The general trend observed is that ionic bonds tend to have higher bond energies compared to covalent bonds. For instance, the bond energy of Li-Br is 807 kJ/mol and NaCl is 787 kJ/mol, while the highest among the covalent bonds given, H-H, is only 432 kJ/mol and C-O is 358 kJ/mol. This pattern can be attributed to the nature of ionic bonds, which result from the strong electrostatic attraction between oppositely charged ions, leading to a more stable and stronger interaction. In contrast, covalent bonds involve the sharing of electron pairs between atoms, which, while strong, do not achieve the same level of attractive force as ionic interactions because they rely on the overlapping of electron clouds rather than the strong electrostatic forces that characterize ionic bonds.