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Updated on 24th August, 2023 , 7 min read
Metals are a group of elements that are widely used in various industries and in daily life. They are characterized by their high conductivity, ductility, and malleability. However, not all metals have the same reactivity. Some metals react with acids and water, while others do not. The reactivity series of metals is a list of metals arranged in the order of their decreasing reactivity. In this article, we will explain the reactivity series of metals and its importance in chemistry.
The reactivity series of metals is a list of metals arranged in the order of their decreasing reactivity. The most reactive metal is placed at the top of the list, and the least reactive metal is placed at the bottom. The reactivity series of metals is based on the ability of metals to displace other metals from their compounds. The more reactive a metal is, the more likely it is to displace another metal from its compound. The table below shows the metals along with their ions-
Reactivity Series of Metals | Ions Formed |
Cesium | Cs+ |
Francium | Fr+ |
Rubidium | Rb+ |
Potassium | K+ |
Sodium | Na+ |
Lithium | Li+ |
Barium | Ba2+ |
Radium | Ra2+ |
Strontium | Sr2+ |
Calcium | Ca2+ |
Magnesium | Mg2+ |
Beryllium | Be2+ |
Aluminium | Al3+ |
Titanium | Ti4+ |
Manganese | Mn2+ |
Zinc | Zn2+ |
Chromium | Cr3+ |
Iron | Fe3+ |
Cadmium | Cd2+ |
Cobalt | Co2+ |
Nickel | Ni2+ |
Tin | Sn2+ |
Lead | Pb2+ |
Hydrogen | H+ (Non-Metal, Reference for Comparison) |
Antimony | Sb3+ |
Bismuth | Bi3+ |
Copper | Cu2+ |
Tungsten | W3+ |
Mercury | Hg2+ |
Silver | Ag+ |
Platinum | Pt4+ |
Gold | Au3+ |
The reactivity series of metals is important in chemistry because it helps predict the outcome of a reaction between a metal and a compound. For example, if a metal is more reactive than another metal in a compound, it will displace the less reactive metal from the compound. This knowledge is used in various industrial applications, such as the extraction of metals from their ores and in the production of alloys.
The following is the reactivity series of metals, arranged in order of their decreasing reactivity:
The reactivity series of metals can be divided into two groups: highly reactive metals and less reactive metals. The highly reactive metals are at the top of the list, and the less reactive metals are at the bottom.
The highly reactive metals are the metals that are most likely to react with water and acids. These metals include potassium, sodium, calcium, and magnesium.
The less reactive metals are the metals that do not react with water or acids. These metals include zinc, iron, tin, lead, copper, silver, gold, and platinum.
The reactivity of metals is affected by several factors, including:
The table below shows the various metal reactions with oxygen, water, and common acids:
Metal | Reaction with Water | Reaction with Oxygen | Reaction with Acids |
Potassium | Reacts violently, producing hydrogen gas and a strong alkaline solution. | Reacts vigorously, forming a white oxide powder | Reacts vigorously, producing hydrogen gas and a salt |
Sodium | Reacts vigorously, producing hydrogen gas and a strong alkaline solution | Reacts vigorously, forming a white oxide powder | Reacts vigorously, producing hydrogen gas and a salt |
Calcium | Reacts slowly with cold water, rapidly with hot water, producing hydrogen gas and a weak alkaline solution | Reacts with oxygen at high temperatures, forming calcium oxide | Reacts with dilute acids, producing hydrogen gas and a salt |
Magnesium | Reacts slowly with cold water, rapidly with hot water, producing hydrogen gas and a weak alkaline solution | Burns brightly in air, forming a white oxide powder | Reacts with dilute acids, producing hydrogen gas and a salt |
Aluminium | Does not react with water | Forms a thin layer of oxide on its surface, which prevents further reaction | Reacts with dilute acids, producing hydrogen gas and a salt |
Zinc | Does not react with water | Reacts with oxygen, forming a white oxide powder | Reacts with dilute acids, producing hydrogen gas and a salt |
Iron | Does not react with water | Reacts with oxygen, forming a reddish-brown oxide | Reacts with dilute acids, producing hydrogen gas and a salt |
Tin | Does not react with cold water, reacts slowly with hot water | Reacts with oxygen at high temperatures, forming tin dioxide | Reacts with concentrated acids, producing hydrogen gas and a salt |
Lead | Does not react with water | Reacts slowly with oxygen, forming a thin oxide layer | Reacts with concentrated acids, producing hydrogen gas and a salt |
Copper | Does not react with water | Does not react with oxygen at room temperature, but can form copper oxide at high temperatures | Reacts with concentrated acids, producing hydrogen gas and a salt |
Silver | Does not react with water | Does not react with oxygen | Does not react with dilute acids, but can react with concentrated acids |
Gold | Does not react withand water | Does not react with oxygen | Does not react with acids |
Note: The table is not exhaustive and may not include all reactions of each metal with water, oxygen, and acids. It is intended as a general guide to the reactivity of metals with these substances.
In addition to shedding light on the properties and reactivity of metals, the reactivity series holds significant practical value. One of its key applications is in predicting the outcome of various reactions involving metals, such as those with water, acids, and single displacement reactions. By referring to the activity series, these reactions can be anticipated, and their products predicted.
Metals that are more reactive than calcium, including calcium itself, can undergo a reaction with cold water to generate the corresponding hydroxide and release hydrogen gas. For instance, when potassium reacts with water, it produces potassium hydroxide and H2 gas, as indicated by the chemical equation below:
2K + 2H2O → 2KOH + H2
Thus, by consulting the reactivity series of metals, it becomes possible to anticipate and forecast the reactions that will occur between metals and water.
Metals that rank higher than lead on the activity series can form salts when they react with hydrochloric acid or sulfuric acid, accompanied by the release of hydrogen gas. One instance of such a reaction is the one that occurs between zinc and sulfuric acid, which generates zinc sulfate and H2 gas as products, as shown by the following chemical equation:
Zn + H2SO4 → ZnSO4 + H2
Therefore, by utilizing the reactivity series, it is possible to anticipate and forecast the reactions that will take place between certain metals and acids.
High-ranking metals on the reactivity series can readily reduce the ions of low-ranking metals. Consequently, low-ranking metals can be easily displaced by high-ranking metals in single displacement reactions between them. A notable example of such a reaction is the displacement of copper from copper sulfate by zinc, which can be represented by the chemical equation below:
Zn (s) + CuSO4 (aq) → ZnSO4 (aq) + Cu (s)
This principle has practical applications in the extraction of metals. For instance, titanium is obtained from titanium tetrachloride through a single displacement reaction with magnesium. Hence, the reactivity series of metals can be utilized to anticipate and forecast the outcome of single displacement reactions.
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