Question
Metallic bonds are responsible for many properties of metals, such as conductivity. Why is this possible?(1 point)
Responses
The 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.
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.
Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.
Responses
The 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.
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.
Two metals bonded together are going to be more conductive than a metal bonded with a nonmetal.
Answers
GPT-4o mini
The correct response is:
**The bonds can shift because valence electrons are held loosely and move freely.**
Metallic bonds allow for the delocalization of valence electrons, which can move freely throughout the metal lattice. This free movement of electrons contributes to the electrical conductivity, malleability, and ductility of metals.
**The bonds can shift because valence electrons are held loosely and move freely.**
Metallic bonds allow for the delocalization of valence electrons, which can move freely throughout the metal lattice. This free movement of electrons contributes to the electrical conductivity, malleability, and ductility of metals.