# How does metallic bonding account for the common properties of metals?

Well, the common properties of metals are $\text{malleability}$, $\text{ductility}$, and $\text{thermal, and electrical conductivity.}$
And the prevailing view of metals does tend to account for the these properties. Metals are often described as $\text{positive ions in a sea of electrons}$.
Each metal ATOM contributes 1 or 2 (or more) valence electrons to the metallic lattice, with the result that the resultant metals are held in position by delocalized bonds between the cations and the electron sea, and can move with respect to each other WITHOUT disrupting the strength of the metal-metal bonds; and hence metals are $\text{malleable}$, able to beaten out into a sheet; $\text{ductile}$, able to be drawn out into a wire; and thermally and electrically conductive, by reason of the delocalized electrons, which can carry thermal and electrical energy across the lattice.