Metallic bonds are responsible for many properties of metals, such as conductivity. Why is this possible?(1 point)ResponsesThe bonds can shift because valence electrons are held loosely and move freely.The bonds can shift because valence electrons are held loosely and move freely.Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.An attraction between a positive charge and a negative charge is created.An attraction between a positive charge and a negative charge is created.Metals have low electronegativity, so they are conductive because they pass charges easily.Metals have low electronegativity, so they are conductive because they pass charges easily.

Answer 1

The correct response is: The bonds can shift because valence electrons are held loosely and move freely.

In metallic bonds, the valence electrons are not bound to individual atoms but are instead delocalized, forming a "sea of electrons" that can move freely throughout the metal lattice. This ability to move enables metals to conduct electricity and heat efficiently, as the free electrons can easily carry charge and energy.