in the outer shells of the metal atoms are free to move. The metallic bond is the force of attraction between these free-moving (delocalised) electrons and positive metal ions close ionElectrically charged particle, formed when an atom or molecule gains or loses an electron
Metallic bonding is often described as an array of positive ions in a sea of electrons. The metal is held together by the strong forces of attraction between the delocalised electrons and the positive ions.
They have high melting and boiling points meaning they are solid at room temperature.
They are good conductors of heat and electricity.
They are shiny in their appearance.
They are malleable.
Metals conduct electricity because the electrons inside the metal are relatively free to move. So when electricity is pass through metals, electrons carry electricity and spread it all over the metal. The mobility of electrons is the reason why metals conduct electricity.
a metal made by combining two or more metallic elements, especially to give greater strength or resistance to corrosion.
Alloys are, for example, generally harder than pure metals. They are made up of atoms of different sizes, rather than being uniform. This means that the layers of atoms cannot slide over each other easily, making the whole alloy much stronger than any of the pure metals that the alloy contains in isolation