their valence electrons are free-roaming
they allow for the conductivity of electricity
APEX :) <3 JAmie
Metallic bonds have delocalized electrons.
they share all of their valence electrons
The formation of metallic bonds causes them to be flexible and strong. Metallic bonds become strong because positive and negative charged electrons have a strong force of attraction. Metallic bonds are flexible because of their malleability.
Most of the properties of a metal, including lustre, are due to the metallic bonding of the electrons.
Behavior of valence electrons. ?
Free- Roaming electrons, and conductivity
they share all of their valence electrons
The formation of metallic bonds causes them to be flexible and strong. Metallic bonds become strong because positive and negative charged electrons have a strong force of attraction. Metallic bonds are flexible because of their malleability.
An octet
Most of the properties of a metal, including lustre, are due to the metallic bonding of the electrons.
Behavior of valence electrons. ?
The electrons that form bonds are called valence electrons. These electrons are in the outer most shell of an atom.
Free- Roaming electrons, and conductivity
False
metals can conduct electricity, the valence electrons of nonmetals cannot roam freely
In metallic bonding, the valence electrons freely 'jump' from atom to atom, forming kind of an electron sea.
The number of valence electrons determines the strength of the metallic bond. The more the stronger the bond will be.
3+