Metallic bonds are responsible for many properties of metals, such as conductivity. Why is this possible?

Question

An attraction between a positive charge and a negative charge is created.
Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.
Metals have low electronegativity, so they are conductive because they pass charges easily.
The bonds can shift because valence electrons are held loosely and move freely.

Answer 1

The correct explanation for why metallic bonds contribute to the conductivity of metals is:

The bonds can shift because valence electrons are held loosely and move freely.

In metallic bonding, atoms release some of their electrons, which become delocalized and form a "sea of electrons" that can move freely throughout the metal lattice. This mobility of valence electrons allows metals to conduct electricity efficiently, as electrical charges can flow easily when a potential difference is applied.