Final answer:
Both metallic and ionic bonds involve electrostatic attractions between positive and negative charges. However, they differ in that electrons in metallic bonds are delocalized, while in ionic bonds they are localized around individual atoms.
Step-by-step explanation:
When comparing metallic and ionic bonds, one should consider various aspects of their nature and behavior. Metallic bonds involve a lattice-like structure of positively charged metal ions surrounded by a sea of delocalized valence electrons that are free to move, which allows for properties such as electrical conductivity. On the other hand, ionic bonds occur between atoms with a large difference in electronegativity, typically between metals and non-metals, and involve the transfer of electrons with atoms being held together by electrostatic forces. The electrons in iconic bonds are not freely movable like in metallic bonds but rather localized around individual atoms.
The characteristic that is shared by both metallic and ionic bonds is E. The bonds come from electric interactions between positive and negative charges. This is due to the electrostatic attraction between cations and anions in ionic bonds, and between cations and the sea of electrons in metallic bonds.