Question
Metallic bonds are responsible for many properties of metals, such as conductivity. Why is this possible?
(1 point)
An attraction between a positive charge and a negative charge is created.
The bonds can shift because
• valence electrons are held loosely and move freely.
Metals have low electronegativity, so they are conductive because they pass charges easily.
Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.
(1 point)
An attraction between a positive charge and a negative charge is created.
The bonds can shift because
• valence electrons are held loosely and move freely.
Metals have low electronegativity, so they are conductive because they pass charges easily.
Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.
Answers
GPT-4o mini
The correct reason why metallic bonds allow for conductivity in metals is:
**The bonds can shift because valence electrons are held loosely and move freely.**
In metallic bonding, the valence electrons are not bound to any specific atom and can move freely throughout the metal lattice. This "sea of electrons" allows metals to conduct electricity effectively, as the free-moving electrons can carry an electric charge throughout the material.
**The bonds can shift because valence electrons are held loosely and move freely.**
In metallic bonding, the valence electrons are not bound to any specific atom and can move freely throughout the metal lattice. This "sea of electrons" allows metals to conduct electricity effectively, as the free-moving electrons can carry an electric charge throughout the material.