Bonding among metals is possible due to the presence of a "sea" of mobile valence electrons that are not strongly bound to any particular atom. These electrons are free to move throughout the entire metal lattice and are attracted to positively charged metal ions. This attraction between the positively charged metal ions and the mobile valence electrons results in a strong metallic bond that holds the metal atoms together.

The metallic bond is a non-directional bond, which means that it does not have a specific direction. This allows metal atoms to pack together efficiently in a regular arrangement, forming a crystalline structure. The strong metallic bond also allows metals to be malleable and ductile, meaning they can be easily deformed without breaking.

In summary, the presence of mobile valence electrons that are not strongly bound to any particular atom is what makes bonding among metals possible, resulting in the formation of a strong, non-directional metallic bond.