* Metallic Bonding: Pure iron is a metal, and metals exhibit metallic bonding. This type of bonding involves a "sea" of delocalized electrons that are shared amongst all the metal atoms.

* Covalent Bonding: Covalent bonding involves the sharing of electrons between two specific atoms. These shared electrons form the bond between the atoms.

How Iron Works:

* In a bar of pure iron, the iron atoms are arranged in a crystal lattice.

* Each iron atom contributes its valence electrons to the "sea" of delocalized electrons.

* These delocalized electrons are not specifically bound to any particular atom. They are free to move throughout the metal structure.

* This free movement of electrons is what gives metals their characteristic properties like electrical conductivity and malleability.

Key Differences:

* Covalent bonds involve a fixed, shared pair of electrons between two specific atoms.

* Metallic bonds involve a shared "sea" of electrons that are not specifically bound to any one atom.

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