Question

How is metal reactivity series useful?​

Answer 1

Explanation:

The reactivity series is a series of metals, in order of reactivity from highest to lowest. It is used to determine the products of single displacement reactions, whereby metal A will replace another metal B in a solution if A is higher in the series

Answer 2

Answer :

The metal reactivity series finds a great many number of uses, especially in the areas of Industrial Chemistry and extraction of metals from the environment as well as dictating the uses of specific metals. We use the series to determine the methods by which we will extract certain metals and what we will use them for.

Explanation :

Metals below Hydrogen in the reactivity series are typically found in the native state due to their extreme lack of reactivity. Such metals include Copper, Silver and Gold. Their lack of reactivity dictates their uses ; Gold is used in jewelry as it does not corrode. Silver is used for attractive finishes and  inside thermos flasks - it cannot react with any food or drink, but still reflect thermal energy effectively. Copper is used in electrical wiring as it is durable, can withstand being in the open and has good conductivity.

Metals above Hydrogen and below Carbon are extracted through the reduction of the metal ore by heating with Carbon. Iron and Zinc are extracted in this way, from Hematite ( $Fe_{2}O_{3}$ , with silica and phosphorus impurities ) and Zinc Blende ( $ZnS$ , also with similar impurities ), respectively.

The metals between Hydrogen and Carbon also have a range of applications. Zinc is used in the galvanisation of steel structures and Iron is used widely in infrastructure.

Metals above Carbon cannot be displaced by it. They form extremely stable compounds with other elements. Thus, we use electrolysis for the extraction of these metals. For example, Aluminium is extracted through electrolysis in a Hall - Heroult Cell, from the ore Bauxite ( $Al_{2}O_{3}$ , with similar impurities as to those present in Hematite ) which is dissolved in cryolite to improve conductivity.  

The high reactivity of these metals, while limiting their uses in the raw form, allow varied uses of the ionic compounds they form with Oxygen ( Oxides ), etc. Such compounds tend to have high melting points and excellent conductivity ( both thermal and electrical ) among other useful properties, allowing for applications in many different industrial processes. A good example would be how Magnesium Oxide ( $MgO$ ) blocks are used to line the walls of industrial furnaces due to their high heat resistance.