it gives it its shine
electrical conductivity
all the following luster, thermal and electrical conductivity (:
Most of the properties of a metal, including lustre, are due to the metallic bonding of the electrons.
Metallic bonds have the characteristics of a sea of mobile electrons.
Metallic crystal consists of an assemblage of positive ions immersed in a sea of mobile electrons. Thus, each electron belongs to a number of positive ions and each positive ion belong to a number of electrons. The force that binds a metal ion to a number of electrons within its sphere of influence is known as metallic bond. This force of attraction is strong and is thus responsible for a compact solid structure of metals
This depends on where you are taught- some call it a sea of electrons some a cloud some delocalised elctrons.
all the following luster, thermal and electrical conductivity (:
mobile electron is responsible for metallic bonding in metals
Most of the properties of a metal, including lustre, are due to the metallic bonding of the electrons.
Well metallic Bonds are positive metal ions surrounded by mobile electrons, in the bond the mobile electrons easily slide past one another when subjected to pressure. As for ionic crysal, pressure pushes ions of like charges into contact. They repel and crystal breaks apart.
Metallic bonds have the characteristics of a sea of mobile electrons.
They are just referred to as "delocalized" electrons
the attraction of metal ions to mobile electrons
Metallic substances have metallic bonds which create an electron cloud in which electrons are highly mobile. Ionic solids have ionic bonding in which electrons are not mobile. Note that by dissolving an ionic substance in water, you can obtain an electrically conductive solution. When dissolved, the ions become quite mobile.
Ability to conduct a current electric mabeability
because the atoms are larger and cannot be held together as strongly by the mobile electrons.
Metallic crystal consists of an assemblage of positive ions immersed in a sea of mobile electrons. Thus, each electron belongs to a number of positive ions and each positive ion belong to a number of electrons. The force that binds a metal ion to a number of electrons within its sphere of influence is known as metallic bond. This force of attraction is strong and is thus responsible for a compact solid structure of metals
Number of valence electrons-The greater the number of freely mobile valence electrons, the higher the charge of positive metal ion, the stronger the metallic bond. Size of metal atom or ion-The smaller the size of the metal ion, the closer the nuclei of metal cations are to the delocalized mobile electrons, the stronger the forces of attraction between the electrons and nuclei, the stronger the metallic bonds.