Reactivity Series - Definition, Uses, Characteristics, FAQs

Edited By Team Careers360 | Updated on Jul 02, 2025 04:39 PM IST

What is reactivity series and which is the most reactive metal?

Reactivity series definition: The reactivity series is a collection of metals arranged in order of increasing reactivity. As a result, a reactivity series of metals can be defined as a group of metals arranged in decreasing order of reactivity. It's sometimes referred to as an activity series. Metals have reactivity due to their incomplete outer orbitals or their electrical structure. Because metals tend to lose electrons, they generate positively charged ions. Because their electrons are far from the positively charged nucleus, metals with high atomic numbers are more reactive. As a result, they can be simply removed. The table is the long tabular list of reactive metals:

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What is reactivity series and which is the most reactive metal?
The short trick to remembering reactivity series:
Important uses of Activity or reactive series:
1. Reaction of metals with water:
2. Reaction of metal with steam:
3. Reaction of metals with dilute acids:
4. In Displacement reaction:
5. In Extraction of metals:
Non-metals in the reactivity series:
Reactivity series characteristics include:

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Metal	Ion
Caesium (Cs)	Cs⁺
Rubidium (Rb)	Rb⁺
Potassium (K)	K⁺
Sodium (Na)	Na⁺
Lithium (Li)	Li⁺
Radium (Ra)	Ra²⁺
Barium (Ba)	Ba²⁺
Strontium (Sr)	Sr²⁺
Calcium (Ca)	Ca²⁺
Magnesium (Mg)	Mg²⁺
Beryllium (Be)	Be²⁺
Aluminum (Al)	Al²⁺
Titanium (Ti)	Ti⁴⁺
Manganese (Mn)	Mn²⁺
Zinc (Zn)	Zn²⁺
Chromium (Cr)	Cr³⁺
Iron (Fe)	Fe²⁺
Cadmium (Cd)	Cd²⁺
Cobalt (Co)	Co²⁺
Nickel (Ni)	Ni²⁺
Tin (Sn)	Sn²⁺
Lead (Pb)	Pb²⁺
Antimony (Sb)	Sb³⁺
Bismuth (Bi)	Bi³⁺
Copper (Cu)	Cu²⁺
Tungsten (W)	W³⁺
Mercury (Hg)	Hg²⁺
Silver (Ag)	Ag⁺
Gold (Au)	Au³⁺
Platinum (Pt)	Pt⁴⁺

In a reactive series of metals, the most reactive element is placed at the top thus, the most reactive metal is Caesium and the least reactive metal is placed at the bottom of the reactive series of metals thus, the least reactive metal is platinum.

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The short trick to remembering reactivity series:

Potassium (Please) Sodium (Stop) Calcium (Calling) Magnesium (Me) Aluminum (A) Carbon (Careless) Zinc (Zebra) Iron (Instead) Tin (Try) Lead (Learning) Hydrogen (How) Copper (Copper) Silver (Saves) Gold (Gold)

Please stop calling me a careless zebra instead try learning how copper saves gold.

This statement helps to learn the reactive series of metals.

Important uses of Activity or reactive series:

We already know that a metal activity series is a list of metals arranged in declining order of their reactivities. The reactive series tells you whether or not a metal may displace another in a single displacement reaction. It also contains information on metal reactivity in the presence of water and acid.

1. Reaction of metals with water:

A metal hydroxide and hydrogen are generated when it reacts with water . Sodium, for example, reacts quickly with cold water:

2Na(s)+2H₂O(l)2NaOH(aq)+H₂(g)

The more reactive the metal, the faster the reaction. Aluminum is unique in that it is a reactive metal that does not corrode when exposed to water. The surface of the iot naturally generates a thin coating of aluminium oxide, which keeps water away from the metal beneath.

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2. Reaction of metal with steam:

When magnesium is first added to water, it reacts slowly, but a coating of insoluble magnesium hydroxide forms. This shields the metal and prevents it from reacting. When steam is run over hot magnesium, however, a strong reaction occurs:

Mg(s)+H₂O(g)MgO(s)+H₂(g)

Magnesium is oxidised, gaining oxygen to form magnesium oxide, while water is reduced in this reaction. It loses oxygen in order to produce hydrogen. The relative resistance to oxidation of a metal is proportional to its position in the reactivity series; in general, the lower a metal's position in the reactivity series, the stronger its resistance to oxidation.

3. Reaction of metals with dilute acids:

A salt and hydrogen are generated when a metal combines with a dilute acid. Magnesium, for example, reacts quickly with dilute hydrochloric acids;

Mg(s)+2HCl(aq)MgCl₂(aq)+H₂(g)

The more reactive the metal, the quicker the reaction. A metal in the reactivity series below hydrogen will not react with dilute acids.

4. In Displacement reaction:

Only a metal that fits above it in the reactivity sequence can displace another metal from a complex. When a more reactive metal (one that forms positive ions more easily) displaces a less reactive reactive metal from a compound, a displacement reaction occurs.

Example- Magnesium is more reactive than copper, hence the reaction will be:

Mg(s)+CuSO₄(aq)MgSO₄(aq)+Cu(s)

platinum, however, is less reactive than copper and thus can't displace copper from the solution for copper sulphate. Silver is less reactive than copper and is therefore not removing the solution for copper sulphate.

5. In Extraction of metals:

Most metals are only present in compounds because they have already reacted with other elements. As a result, the metal must be removed from the ore containing the metal complex.

The below table shows the reactivity of common and most used metals which can react with water or acids:

Metal	Reactivity
Potassium	Reacts with water.
Sodium
Lithium
Barium
Strontium
Calcium
Magnesium	Reacts with acid
Aluminum
Manganese
Zinc
Chromium
Iron
Cadmium
Cobalt
Nickel
Tin
Lead
Hydrogen	Include for comparison.
Antimony	Highly unreactive
Bismuth
Copper
Mercury
Silver
Gold
Platinum

Metals ranging from potassium to calcium are extremely reactive, reacting even with water. Acids can react with metals ranging from magnesium to lead. In normal settings, metals ranging from copper to platinum are highly unreactive and do not react with any other substance. This is why platinum and gold are resistant to corrosion and do not create oxides. Metals like zinc, aluminium, magnesium, and calcium, on the other hand, readily form oxide.

Non-metals in the reactivity series:

Although hydrogen is a nonmetal, it is included in the reactivity series because it aids in the comparison of metal reactivity and also used in extraction of metals. Carbon is also placed in the reactive series and metals like zinc and iron can be displaced by the oxides of carbon and metal like copper can be extracted using carbon and hydrogen.

NCERT Chemistry Notes:

Reactivity series characteristics include:

As we progress through the reactivity series, the electropositive character decreases. In the presence of oxygen, potassium and sodium make superoxide, but in the absence of oxygen, they produce their own oxides.

K+O₂→KO₂

Because we progress down the reactivity series, metals' reducing power increases. As a result, potassium is the most powerful reducing agent.
As we progress through the activity series, the tendency for metals to become oxidised is reduced.
Also, as we progress down the reactivity scale, metals' capacity to convert water to hydrogen decreases. Because potassium and sodium are very reactive, they combine with cold water to produce hydrogen gas, which is ignited by the heat generated during the reaction.

2K+2H₂O→2KOH+H₂

All metals in the activity series above hydrogen have the ability to liberate hydrogen gas by reducing hydrogen ions from dilute hydrochloric or sulphuric acid.
A metal higher in the reactivity series can replace a metal lower in the series to form the latter metal's salt solutions. The faster the displacement reaction, the greater the gap between the locations of two metals.
Common reducing agents are incapable of reducing metal oxides such as potassium, sodium, calcium, magnesium, and aluminum.

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Frequently Asked Questions (FAQs)

1. 1. Question: What is metal reactivity?

The metal reactivity sequence, also known as the set of operations, is the order in which metals' reactivities are organized. Metals have a proclivity for losing electrons and forming cations. Some lead to the formation of metal oxides with the ambient oxygen.

2. 2. Question: Nonmetals are reactive or non-reactive?

The boiling point of non-metal characteristics is low, and other non-metals are gases. Similarly, non-metals do not conduct heat well, and solid nonmetals are dull and brittle. Many nonmetals are very reactive, whereas others are completely inert. The number of electrons in the outer quantity of energy determines this.

3. 3. Question: Why is gold a nonreactive metal?

Ans: Among all the elements in the periodic table, gold is one of the least reactive. Gold does not react with oxygen found in the air, water, or alkalis. That is why it does not corrode. It does not, however, react with halogens.

4. 4. Question: What does a reactivity series show?

The reactivity series shows metal in order of reactivity. The reactivity of a metal can be determined by observing its responses in both competition and displacement processes. It shows the reactivity of metal towards water and acid and also it helps in the displacement reactions and for the extraction of metals.

5. 5. Question: What metal has the least amount of reactivity?

Transition metals are the elements in the periodic table that are far less reactive, with metals like gold and platinum near the bottom of the list, demonstrating little in the way of chemical reactivity with common reagents.

6. How does the reactivity series influence the choice of fire extinguishing methods?

The reactivity series is crucial in choosing appropriate fire extinguishing methods, especially for metal fires. Water, which is effective for many fires, can react violently with highly reactive metals like sodium or potassium. For such metals, special dry powder extinguishers are used. Understanding the reactivity series helps in selecting safe and effective firefighting techniques.

7. Can the reactivity series be used to predict the solubility of metal compounds?

While the reactivity series doesn't directly predict solubility, it can provide some insights. Generally, compounds of metals high in the series (more reactive) tend to be more soluble in water than those of less reactive metals. However, other factors like lattice energy and hydration energy also play crucial roles in determining solubility.

8. Why are some reactive metals used in fireworks?

Reactive metals are often used in fireworks because of their ability to produce bright colors and spectacular effects when they burn. Metals like sodium, potassium, and magnesium, which are high in the reactivity series, readily react with oxygen in the air when heated, producing intense light and color. Their high reactivity contributes to the vibrant displays in fireworks.

9. How does the reactivity series help in understanding the concept of passivation?

The reactivity series helps explain passivation, where some reactive metals become less reactive due to a protective layer. For example, aluminum is high in the reactivity series but resists corrosion due to a thin, protective oxide layer. Understanding an element's position in the series and its tendency to form protective layers helps predict and utilize passivation in various applications.

10. Can the reactivity series be used to predict the stability of coordination compounds?

While the reactivity series primarily deals with simple ionic and covalent compounds, it can provide some insights into coordination compound stability. Generally, metals lower in the series (less reactive) tend to form more stable coordination compounds. However, other factors like ligand field stabilization energy and the nature of the ligands also play crucial roles in determining stability.

11. How does the reactivity series help in predicting displacement reactions?

The reactivity series helps predict displacement reactions by showing which metals can displace others from their compounds. A more reactive metal will displace a less reactive metal from its salt solution. For example, zinc can displace copper from copper sulfate solution because zinc is higher in the reactivity series than copper.

12. What is the significance of hydrogen's position in the reactivity series?

Hydrogen's position in the reactivity series is significant because it serves as a reference point. Metals above hydrogen in the series can displace hydrogen from acids, while those below cannot. This helps in predicting which metals will react with acids and the products of these reactions.

13. Can the reactivity series be used to predict the strength of acids?

While the reactivity series primarily deals with metals, it can indirectly relate to acid strength. Metals high in the series can displace hydrogen from acids more easily, which can give an indication of acid strength. However, for a comprehensive understanding of acid strength, other factors like bond dissociation energy and electronegativity must be considered.

14. How does the reactivity series relate to the concept of redox reactions?

The reactivity series is closely tied to redox (reduction-oxidation) reactions. Elements higher in the series are more likely to be oxidized (lose electrons) and act as reducing agents. Conversely, elements lower in the series are more likely to be reduced (gain electrons) and act as oxidizing agents. This relationship is fundamental in understanding and predicting redox reactions.

15. Why are some reactive metals used as sacrificial anodes?

Reactive metals are used as sacrificial anodes to protect less reactive metals from corrosion. For example, zinc (more reactive) is often used to protect iron (less reactive) in galvanization. The zinc corrodes preferentially, "sacrificing" itself to protect the iron. This application directly utilizes the principles of the reactivity series.

16. How does the reactivity series influence the extraction methods of metals?

The reactivity series greatly influences metal extraction methods. Metals low in the series (less reactive) can be extracted by heating their ores with carbon. More reactive metals require electrolysis or more complex reduction processes. This is why copper and iron were used earlier in human history than aluminum, despite aluminum being more abundant.

17. How does the reactivity series help in understanding corrosion?

The reactivity series helps explain why some metals corrode more easily than others. Metals higher in the series are more prone to corrosion because they react more readily with oxygen and water in the environment. This is why iron rusts easily, while gold does not corrode under normal conditions.

18. Can the reactivity of an element change under different conditions?

While an element's position in the reactivity series is generally fixed, its apparent reactivity can change under different conditions. Factors like temperature, pressure, concentration, and the presence of catalysts can affect the rate and extent of reactions, making an element appear more or less reactive.

19. Why are some reactive metals found in their native state in nature?

While it seems counterintuitive, some highly reactive metals like gold and platinum are found in their native state because they are so unreactive that they don't easily combine with other elements. Their low position in the reactivity series means they resist oxidation and other chemical changes, allowing them to exist in pure form in nature.

20. How does the reactivity series influence the recycling of metals?

The reactivity series is important in metal recycling processes. Less reactive metals like copper and gold can be recycled more easily through melting and reforming. More reactive metals might require chemical processes to separate them from compounds. Understanding these differences helps in designing efficient and cost-effective recycling methods.

21. Why is the reactivity series important in chemistry?

The reactivity series is crucial because it allows chemists to predict the outcomes of chemical reactions, determine which metals can displace others from their compounds, and understand the relative stability of different elements. It's a fundamental tool in understanding chemical behavior and designing experiments or industrial processes.

22. Why are some highly reactive metals stored in oil?

Highly reactive metals like sodium and potassium are often stored in oil to prevent them from reacting with air or moisture. The oil acts as a barrier, preventing contact with oxygen and water, which would otherwise cause rapid oxidation or even explosive reactions. This storage method is a direct application of understanding the reactivity series.

23. How does the reactivity series influence the choice of materials in construction and engineering?

The reactivity series is crucial in selecting materials for construction and engineering. Less reactive metals are often preferred for exposed structures or in corrosive environments. For example, copper or stainless steel might be chosen over iron for outdoor use due to their lower reactivity and resistance to corrosion.

24. How does the reactivity series help in understanding battery technology?

The reactivity series is fundamental in battery design. Batteries work on the principle of electron transfer between elements of different reactivities. A more reactive metal (anode) loses electrons to a less reactive metal or non-metal (cathode). Understanding these relationships helps in selecting appropriate materials for efficient and long-lasting batteries.

25. Can the reactivity series be used to predict the formation of alloys?

While the reactivity series doesn't directly predict alloy formation, it can provide insights. Metals with similar reactivities are more likely to form solid solutions (alloys). However, metals far apart in the series might not mix well or could form intermetallic compounds. The series can also help predict which metal in an alloy might be more susceptible to corrosion.

26. Can non-metals be included in the reactivity series?

While the reactivity series primarily focuses on metals, some non-metals can be included for comparison. Hydrogen, for example, is often included in the series. Other non-metals like oxygen and chlorine can be considered in terms of their ability to react with metals, but they're not typically part of the standard reactivity series.

27. How does the reactivity series relate to the concept of electronegativity?

The reactivity series is inversely related to electronegativity. Elements high in the reactivity series (like alkali metals) have low electronegativity, meaning they readily give up electrons. Elements low in the series (like halogens) have high electronegativity, meaning they tend to attract electrons. This relationship helps in predicting the nature of chemical bonds and compound formation.

28. Can the reactivity series be used to predict the strength of chemical bonds?

Yes, the reactivity series can give insights into bond strength. Generally, metals higher in the series form stronger ionic bonds with non-metals because they lose electrons more easily. However, when it comes to metallic bonds, metals higher in the series often form weaker bonds because their electrons are less tightly held.

29. Why are some metals more reactive than others?

The reactivity of metals is primarily determined by how easily they lose electrons to form positive ions. Metals higher in the reactivity series lose electrons more readily, making them more reactive. This is influenced by factors such as atomic size, nuclear charge, and electron configuration.

30. How does the reactivity series relate to the periodic table?

The reactivity series generally correlates with an element's position in the periodic table. Elements on the left side of the periodic table (like alkali and alkaline earth metals) are typically more reactive, while those on the right side (like noble gases) are less reactive. This trend is due to electron configuration and atomic structure.

31. What role does electron configuration play in the reactivity series?

Electron configuration is crucial in determining an element's position in the reactivity series. Elements with fewer electrons in their outer shell (valence electrons) are generally more reactive because they can more easily lose these electrons to form positive ions. This is why alkali metals, with one valence electron, are at the top of the series.

32. How is the reactivity series determined?

The reactivity series is determined through experimental observations of how different elements react with water, acids, and oxygen. Scientists compare the ease and speed of these reactions, as well as the products formed, to rank elements in order of their reactivity.

33. How does the reactivity of metals change as you move down the reactivity series?

As you move down the reactivity series, the reactivity of metals decreases. This means that metals at the top of the series (like potassium and sodium) react more vigorously with water and acids, while metals at the bottom (like copper and gold) are less reactive and may not react at all under normal conditions.

34. What is the correct order of the reactivity series from most to least reactive?

The general order of the reactivity series from most to least reactive is: Potassium, Sodium, Lithium, Calcium, Magnesium, Aluminum, Zinc, Iron, Lead, Hydrogen, Copper, Mercury, Silver, Gold, Platinum. However, it's important to understand the concept rather than memorizing the exact order.

35. Can the position of an element in the reactivity series change over time?

The relative positions of elements in the reactivity series are based on fundamental properties and don't change over time. However, our understanding and measurement of reactivity can improve, leading to minor adjustments in the series. Additionally, the discovery of new elements or isotopes might lead to additions to the series.

36. Why doesn't the reactivity series perfectly align with the order of elements in the periodic table?

While there's a general correlation between the reactivity series and the periodic table, they don't align perfectly. This is because reactivity is influenced by multiple factors, including atomic size, electron configuration, and ionization energy. The periodic table is organized primarily by atomic number, which doesn't always directly correspond to reactivity.

37. How does the reactivity series relate to the concept of standard reduction potentials?

The reactivity series is closely related to standard reduction potentials. Generally, the more negative the standard reduction potential of a metal, the higher it is in the reactivity series. This is because a more negative potential indicates a greater tendency to be reduced (gain electrons), which correlates with lower reactivity in the series.

38. How does the reactivity series help in understanding the formation of ores?

The reactivity series helps explain ore formation. Highly reactive metals are usually found in nature as compounds (ores) because they readily react with other elements. Less reactive metals may be found in their native state. For instance, iron is typically found as iron oxide ores, while gold is often found in its pure form.

39. What is the reactivity series in chemistry?

The reactivity series is a list of elements arranged in order of their chemical reactivity, from most reactive to least reactive. It primarily focuses on metals but also includes hydrogen. This series helps predict how readily an element will undergo chemical reactions, particularly with water, acids, and oxygen.

40. Why is gold at the bottom of the reactivity series?

Gold is at the bottom of the reactivity series because it is one of the least reactive metals. It has a stable electron configuration and does not readily lose electrons to form ions. This stability is why gold doesn't tarnish or corrode easily, making it valuable for jewelry and certain industrial applications.

41. What is the relationship between the reactivity series and standard electrode potentials?

The reactivity series is closely related to standard electrode potentials. In general, the more negative the standard electrode potential of a metal, the higher it is in the reactivity series. This is because a more negative potential indicates a greater tendency to lose electrons, which correlates with higher reactivity.

42. How does the reactivity series relate to the concept of oxidation?

The reactivity series is closely related to oxidation. Elements higher in the series are more easily oxidized (lose electrons) than those lower down. This is why metals at the top of the series, like potassium and sodium, readily oxidize in air, while gold at the bottom remains stable.

43. How does the concept of ionization energy relate to the reactivity series?

Ionization energy, the energy required to remove an electron from an atom, is inversely related to an element's position in the reactivity series. Elements with lower ionization energies are generally higher in the reactivity series because they more easily lose electrons to form positive ions, making them more reactive.

44. How does the reactivity series influence the choice of catalysts in chemical reactions?

While the reactivity series doesn't directly determine catalyst choice, it can provide insights. Metals in the middle of the series, like nickel and platinum, often make good catalysts because they can form temporary bonds with reactants without being too reactive themselves. Understanding an element's position in the series can help in selecting potential catalysts for specific reactions.

45. How does the reactivity series help in understanding the Earth's crust composition?

The reactivity series helps explain why certain elements are more abundant in the Earth's crust than others. Less reactive metals like gold and platinum are rare in the crust because they don't readily form compounds. More reactive elements like aluminum and calcium are abundant because they easily form stable compounds with oxygen and other elements.

46. How does the reactivity series help in understanding the formation of complex ions?

The reactivity series can provide insights into complex ion formation. Metals lower in the series (less reactive) often form more stable complex ions because they have a higher tendency to accept electron pairs from ligands. This is why transition metals, which are generally in the middle to lower part of the series, commonly form complex ions.

47. Why are some reactive metals used in chemical synthesis as reducing agents?

Reactive metals high in the series are often used as reducing agents in chemical synthesis because they readily lose electrons. For example, sodium borohydride, containing the reactive metal sodium, is a powerful reducing agent used in organic synthesis. The position of a metal in the reactivity series can indicate its effectiveness as a reducing agent.

48. How does the reactivity series relate to the concept of electrochemical cells?

The reactivity series is fundamental to understanding electrochemical cells. In a galvanic cell, the more reactive metal (higher in the series) serves as the anode and undergoes oxidation, while the less reactive metal (lower in the series) serves as the cathode and undergoes reduction. This difference in reactivity drives the flow of electrons, generating electricity.

49. Can the reactivity series help in predicting the products of electrolysis?

Yes, the reactivity series can help predict electrolysis products. During the electrolysis of molten compounds or aqueous solutions, the cathode reaction often involves the reduction of the metal ion. The ease of this reduction is related to the metal's position in the reactivity series. Metals lower in the series are more easily reduced and thus more likely to be produced at the cathode.

50. Why are some reactive metals used in metallurgy for metal extraction?

Highly reactive metals are sometimes used in metallurgy to extract less reactive metals from their ores. This process, called aluminothermic or thermite reactions, uses the high reactivity of metals like aluminum to reduce metal oxides of less reactive metals. For example, aluminum can be used to extract iron from iron oxide in a highly exothermic reaction.

51. How does the reactivity series relate to the concept of electroplating?

The reactivity series is crucial in electroplating processes. Typically, a less reactive metal (lower in the series) is plated onto a more reactive metal (higher in the series). This arrangement ensures that the plating adheres well and doesn't spontaneously reduce back to its ionic form. Understanding the relative positions of metals in the series helps in designing effective electroplating processes.