Reactivity Series
Master the Reactivity Series in Minutes
Explore how the metals differ in their reactivity, how they lose electrons, and how they interact with water, acids, and other metal salts. Learn the full order using a simple mnemonic, and master key applications to solve exam questions confidently.
1.0Learning Outcomes
After completing this lesson, you will be able to:
- Define the reactivity series and explain the basis of its arrangement.
- Memorize the reactivity series of metals using a simple mnemonic.
- Predict whether a displacement reaction will occur between given elements.
- Explain the chemical behavior of metals with water and dilute acids based on their position.
- Solve NCERT and board-level questions accurately.
The reactivity series is a ranking chart that informs us how active some metals are compared to others. The reactivity series assists scientists and students in predicting the results of chemical reactions, knowing which metals are able to displace others from salt solutions, and selecting appropriate methods for retrieving metals from ores. Let’s learn about it in detail.
2.0What is the Reactivity Series?
The Reactivity Series is an ordered list of elements, primarily metals, in order of their chemical reactivity. This indicates that the most reactive metal comes first at the top, followed by the least reactive one at the bottom. A metal's reactivity is determined by the ease with which it can lose electrons to become positive ions (cations). Potassium and sodium are highly reactive metals which lose electrons readily and vigorously react with water and acids. Copper, silver, and gold are less reactive metals that are stable and do not react or do so very weakly.
3.0Reactivity Series of Metals – The Full List
Here's the entire Reactivity Series of metals, ranking from most reactive to least reactive:
Note: Hydrogen is not a metal but is listed to compare how metals respond to acids.
* Metals higher than hydrogen on the list react with acids to form hydrogen gas.
* Metals lower than hydrogen do not push out hydrogen from acids.
Example:
Zinc (Zn) is higher than hydrogen. Therefore, it reacts with hydrochloric acid:
Zn + 2HCl → ZnCl₂ + H₂↑
But Copper (Cu) doesn't react with hydrochloric acid, as it comes below hydrogen in the series.
4.0Reactivity Series of Non-Metals
Whereas metals lose electrons, non-metals gain electrons in reactions. Although there is no specific reactivity series for non-metals, we can still make some sort of arrangement for common non-metals according to their reactivity.
Here's a rough order of the reactivity series of non-metals:
- Fluorine (F)
- Oxygen (O)
- Chlorine (Cl)
- Bromine (Br)
- Iodine (I)
- Sulfur (S)
- Phosphorus (P)
- Carbon (C)
- Hydrogen (H)
Fluorine is the most reactive of the non-metals. It reacts violently with nearly all elements. On the contrary, carbon and hydrogen are less reactive.
This order enables us to comprehend:
* Displacement reactions among halogens.
* Combustion and oxidation reactions.
* Which non-metal will predominate in a redox reaction?
Example:
Chlorine will displace bromine from its compound:
Cl₂ + 2KBr → 2KCl + Br₂
Because chlorine is higher in the reactivity series of non-metals.
5.0Mnemonic to Remember the Reactivity Series
To remember the reactivity series of metals for class 10 in a snap, students can adopt this playful mnemonic:
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Each word stands for a metal:
- P – Potassium
- S – Sodium
- C – Calcium
- M – Magnesium
- A – Aluminium
- Z – Zinc
- I – Iron
- L – Lead
- H – Hydrogen
- C – Copper
- S – Silver
- G – Gold
- P – Platinum
This easy sentence assists students in memorising the order without tension.
6.0Significance and Applications of the Reactivity Series
The reactivity series tricks are more than just a chemistry subject. It has practical applications in science and other aspects of life. Let's discuss how this information assists us in daily life and science.
a) Predicting Reactions
The reactivity series informs us which metal will react and to what extent. Sodium and potassium, for instance, react with cold water, whereas iron only reacts with steam.
Example:
Sodium reacts with water:
2Na + 2H₂O → 2NaOH + H₂↑
But copper won't react with water at all.
b) Displacement Reactions
A more reactive metal can displace a less reactive metal from its salt solution.
Example:
Zinc is more reactive and thus displaces copper from copper sulfate:
Zn + CuSO₄ → ZnSO₄ + Cu
This principle is applied in most chemical industries.
c) Metal Extraction
The reactivity series assists in selecting the appropriate process to extract metals from their ores.
* Very reactive metals (such as aluminium) are obtained by electrolysis.
* Less reactive metals (such as iron) can be obtained by carbon reduction.
d) Preventing Corrosion
Metals low in the series, such as gold and platinum, do not react and are corrosion resistant. That is why they are used to make jewellery.
For other metals, their reactivity informs us how to coat them or paint them in order to protect them.
e) Storage of Reactive Metals
Metals such as sodium and potassium react rapidly with air and water. So they are stored under oil to avoid unsafe reactions.
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8.0Supporting Study Materials
This study material CBSE Notes and NCERT Solutions for the Chapter "Chemical Reactions and Equations" on Oxidation and Reduction Topics is designed according to the latest CBSE Class 10 Science syllabus and NCERT guidelines. It provides clear explanations of key concepts, definitions, examples, and important questions to help students understand redox reactions, corrosion, and rancidity, and prepare effectively for examinations.
9.0Previous Year Questions (PYQs)
Q1. A metal 'X' is dipped in an aqueous solution of Aluminium Sulphate [Al₂(SO₄)₃]. No reaction is observed. When the same metal 'X' is dipped in Copper Sulphate (CuSO₄) solution, a blue-to-green colour change occurs. Identify metal 'X' from the choices: Iron, Zinc, or Magnesium. Explain your choice. (CBSE Board)
Answer
- Identified Metal 'X': Iron (Fe).
- Explanation: 1. According to the reactivity series, Aluminium is highly reactive. Since metal 'X' gives no reaction with Al₂(SO₄)₃, 'X' must be below Aluminium. This rules out Magnesium (which is higher than Aluminium).
2. Metal 'X' successfully displaces Copper from CuSO₄ (fading the blue solution to green). Both Iron and Zinc can do this.
3. However, a green solution (FeSO₄) is formed when Iron replaces Copper, whereas Zinc forms a colourless solution (ZnSO₄). Thus, metal 'X' is Iron. - Chemical Equation: Fe (s) + CuSO₄ (aq) → FeSO₄ (aq) [Green] + Cu (s)
10.030-Second Revision
- Most reactive metal: Potassium (K)
- Least reactive metal: Gold (Au)
- Metals higher in the series are more reactive
- More reactive metals displace less reactive metals
- Potassium reacts most vigorously with water
- Copper, Silver, Gold are least reactive
- Hydrogen is placed in the middle of the series
- Metals above hydrogen can liberate hydrogen from acids
- Metals below hydrogen cannot displace hydrogen from acids
- Remember: Higher in Series = More Reactive
11.0Recommended Next Topics
- Extraction of Metals (Metallurgy)
- Corrosion and its Prevention
- Chemical Properties of Acids and Bases
- Double Displacement Reactions