* Metallic Bonding: Metals form metallic bonds, where valence electrons are delocalized and shared throughout the entire structure. This creates a "sea of electrons" that allows for high electrical conductivity and malleability.
* Electron Configuration: Metals tend to have a relatively small number of valence electrons in their outer shell. This is because their electron configurations often have one, two, or three electrons in their outermost shell. These electrons are relatively easily removed, contributing to the metallic bond.
* Nonmetal Bonding: Nonmetals, in contrast, tend to have more valence electrons. They usually have four or more electrons in their outermost shell. Nonmetals often form covalent bonds, sharing electrons with other atoms to achieve a full outer shell (octet rule).
Example:
* Sodium (Na) has one valence electron.
* Chlorine (Cl) has seven valence electrons.
Key Takeaway: The tendency for metals to have fewer valence electrons is directly related to their characteristic metallic bonding. This allows for the formation of a mobile "sea of electrons" that is responsible for many of the unique properties of metals.
