Bonds: Including Carbon Compounds Quick Check
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Question
Metallic bonds are responsible for many properties of metals, such as conductivity. Why is this possible?(1 point)

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.

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.

Metals have low electronegativity, so they are conductive because they pass charges easily.

Metallic bonds are responsible for many properties of metals, such as conductivity. This is because the bonds can shift because valence electrons are held loosely and move freely. That is option C.

What are metallic bonds?

Metallic bonds are defined as those bonds that causes the electrostatic attraction between metal cations and delocalized electrons of another metallic substance.

The characteristics of a metallic compound with metallic bonds include the following:

strength,

malleability,

ductility,

thermal and electrical conductivity,

opacity and

luster.

The metallic bonds of these metallic atoms gives them conductivity features because the electrons from the outer shells of the metal atoms are delocalised , and are free to move through the whole structure.

Learn more about metals here:

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