How do metals bond with each other

Metallic bonding  

Metals have low ionization energies. Therefore, their valence electrons are easily delocalized (attracted to the neighbouring metal atoms). These delocalized electrons are then not associated with a specific metal atom.  Since the electrons are “free”, the metal atoms have become cations, and the electrons are free to move throughout the whole crystalline structure.

We say that a metal consists of an array of cations immersed in a sea of electrons. The electrons act as a “glue” holding the cations together.

Metallic bonds are the attractive forces between the metal cations and the sea of electrons.

(Hope this helps) Sky

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Explanation:

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fe 55.85 g/mol and h2o 18.02 g/mol.