Which of the following is NOT a characteristic of metallic bonding?

The characteristic that is NOT associated with metallic bonding is the transferring of electrons between different elements. In metallic bonding, metal atoms share their valence electrons rather than transferring them. This results in the formation of a "sea of delocalized electrons," where electrons are free to move throughout the metal lattice, contributing to properties like electrical conductivity and malleability.

Metallic bonding primarily involves the attraction between closely packed metal atoms and the collective, delocalized electrons around them. This attribute allows metals to conduct electricity well, as the free-moving electrons can carry an electrical charge efficiently.

In contrast, transferring of electrons is a key feature of ionic bonding, where one atom donates an electron to another, leading to the formation of charged ions that attract each other. Thus, while characteristics like attraction between metal atoms, the formation of a delocalized electron sea, and high electrical conductivity are hallmarks of metallic bonding, the concept of electron transfer pertains to a different type of bonding altogether.