# How do you explain metallic bonding in terms of the sparsely populated outermost orbitals of metal atoms?

By $\text{electronic delocalization}$ and consequent $\text{metallic bonding}$...........
A metal consists of a close-packed array of metal atoms that EACH contribute ONE or TWO or THREE (or more) electrons to the lattice. The result? Metallic bonding, which is aptly described as $\text{positive ions in a sea of electrons}$. Now the positively charged nuclear cores of the metal atoms can move with respect to each other without disrupting the electrostatic bond with the electronic cloud. And this gives rise to (i) $\text{malleability}$, the ability to be beaten out into a sheet; (ii) $\text{ductility}$, the ability to be drawn out into a wire; and (iii) generally good $\text{thermal}$ and $\text{electrical conductivities}$, which are common characteristics of metals.