Metals - Properties of metals

Metallic Bonding: Defined as the electrostatic attraction between a lattice of positive metal ions ($M^{n+}$) and a 'sea' of delocalized electrons.

Electrical Conductivity: Metals conduct electricity because the delocalized electrons are free to move throughout the giant metallic lattice when a voltage is applied.

Malleability and Ductility: Metals can be hammered into shapes or drawn into wires because the layers of positive ions can slide over each other without breaking the metallic bond, as the sea of electrons acts as a 'glue'.

Thermal Conductivity: Heat energy is transferred through metals by the vibration of closely packed ions and the kinetic energy carried by rapidly moving delocalized electrons.

Alloys: An alloy is a mixture of a metal with other elements. Alloys are harder than pure metals because atoms of different sizes disrupt the regular arrangement of the lattice, making it difficult for layers to slide over one another.

Reactivity Series: Metals are arranged in order of their ability to lose electrons and form positive ions. Metals higher in the series, such as $K$ and $Na$, react more vigorously with water and acids than those lower down, like $Cu$ or $Ag$.

Chemical Properties: Metals generally react with oxygen to form basic oxides (e.g., $MgO$), and with dilute acids to produce a salt and hydrogen gas ($H_2$).