How to Remember the Reactivity Series Easily (With Mnemonics & Examples)
The reactivity series is essential in chemistry and helps students understand various practical and theoretical applications related to this topic. Whether you are preparing for school exams or want to know why certain metals rust or extract differently, learning the reactivity series provides great clarity for chemical reactions and real-world examples.
This concept also appears across many chapters and is a foundation for various types of chemistry questions.
What is Reactivity Series in Chemistry?
A reactivity series refers to the arrangement of metals in the order of their reactivity, from the highest to the lowest. This concept appears in chapters related to displacement reactions, metallic and non-metallic minerals, and metals and non-metals, making it a foundational part of your chemistry syllabus.
The reactivity series helps us predict the behavior of metals in reactions with water, acids, and salts and is particularly helpful for understanding concepts like rusting, corrosion, and extraction of metals.
Standard Reactivity Series Table
The reactivity series of metals lists metals from most to least reactive. It is a quick reference for predicting chemical changes, especially in reactions involving metals, water, and acids.
| Reactivity Order | Element (Symbol) | Notable Feature |
|---|---|---|
| 1 (Most Reactive) | Potassium (K) | Reacts violently with water |
| 2 | Sodium (Na) | Reacts quickly with water |
| 3 | Calcium (Ca) | Reacts with cold water |
| 4 | Magnesium (Mg) | Reacts with hot water/steam |
| 5 | Aluminium (Al) | Forms protective oxide layer |
| 6 | Zinc (Zn) | Corrodes easily |
| 7 | Iron (Fe) | Prone to rusting |
| 8 | Lead (Pb) | Reacts slowly with acids |
| 9 | Hydrogen (H) | Reference (non-metal) |
| 10 | Copper (Cu) | Rarely reacts, forms green patina |
| 11 | Mercury (Hg) | Very weak reactivity |
| 12 | Silver (Ag) | Does not react with acids easily |
| 13 | Gold (Au) | Does not corrode |
| 14 (Least Reactive) | Platinum (Pt) | Most resistant |
How to Remember: Reactivity Series Mnemonics & Tricks
Many students use memory tricks to learn the reactivity series easily. Here are some popular sentences:
- Please Stop Calling Me A Zebra In Lovely Happy Cities - Smart Girls Please!
(Potassium, Sodium, Calcium, Magnesium, Aluminium, Zinc, Iron, Lead, Hydrogen, Copper, Silver, Gold, Platinum) - Another simple one: "Peter Sells Cars Made And Zinc In Large Heavy Cages, Securely Guarded by Plato."
- Make your own fun rhyme for quick revision before your exams!
Understanding the Reactivity Pattern
Metals at the top of the series lose electrons the easiest, which makes them highly reactive. This is why potassium and sodium react quickly with water or air. As you go down, the attraction between the metal’s outermost electrons and nucleus increases, so losing electrons becomes harder and the reactivity drops. This is also why gold and platinum barely react and are used for jewelry and electrical contacts.
Applications & Examples
The reactivity series is used in many practical and exam-based scenarios:
- Predicting displacement reactions (e.g., zinc can displace copper from copper sulphate: Zn + CuSO₄ → ZnSO₄ + Cu)
- Selecting methods for extraction of metals from ores
- Understanding corrosion and rusting of iron
- Explaining which metals produce hydrogen with acids (those above hydrogen in the series do)
- Lab experiments involving single displacement reactions
Reactivity Series of Non-Metals
While the main reactivity series is for metals, non-metals like halogens (fluorine, chlorine, bromine, iodine) also have their own reactivity pattern. For halogens, reactivity decreases down the group: Fluorine > Chlorine > Bromine > Iodine. This is often discussed when learning about properties of non-metals and their chemical behavior.
Try This Yourself
- Use the reactivity series to predict: Will magnesium displace iron from iron sulphate solution?
- Name two metals that won’t react with dilute hydrochloric acid.
- Write the balanced equation when zinc is put in copper sulphate solution.
- Remember a mnemonic and recite the order without looking!
Lab or Experimental Tips
Remember, always add small pieces of highly reactive metals (like sodium or potassium) to water gently and use tongs in experiments. In Vedantu live classes, teachers use colored charts or model kits to help you quickly identify metal order and predict outcomes of reactions like displacement or corrosion.
Frequent Related Errors
- Confusing metals that are close together in the series (e.g., confusing copper and silver positions).
- Forgetting that hydrogen is included just for reference, even though it is not a metal.
- Assuming all metals react with acids – in reality, those below hydrogen in the series do not.
- Using wrong mnemonics and mixing up the order during quick revision or in MCQs.
- Believing that a metal’s hardness determines reactivity – it actually depends on electron loss tendency.
Uses of Reactivity Series in Real Life
The reactivity series is widely used to explain why iron rusts, why gold and platinum do not corrode, and why zinc is used for stabilizing or protecting iron from rusting (galvanization). It is also critical in how metals are extracted and separated during industrial and laboratory processes.
Relation with Other Chemistry Concepts
The reactivity series is closely related to electrochemical series and redox reactions, helping students bridge the gap to learn about electron transfer, oxidation-reduction, and applications in batteries and extraction industry. Understanding the position of a metal will also help with periodic table trends and properties.
Step-by-Step Reaction Example
1. Write the reaction: When zinc is placed into a copper sulphate solution.2. Balanced equation: Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s)
3. Zinc is higher in the reactivity series, so it replaces copper.
4. The blue color of copper sulphate fades as copper metal forms and settles.
5. This demonstrates single displacement, predicted using the reactivity series.
Final Wrap-Up
We explored reactivity series—its order, patterns, practical usage, and importance in chemical reactions and metal extraction. Understanding this topic not only helps predict chemical outcomes but also builds a strong foundation in chemistry. For more in-depth lessons, practical tricks, and exam-winning strategies, keep exploring notes and live sessions on Vedantu.
FAQs on Reactivity Series: Definition, Order & Applications
1. What is the reactivity series of metals?
The reactivity series is a ranked list of metals based on their decreasing chemical reactivity.
This order helps predict how metals react with water, acids, and other substances.
Common order:
Potassium (K) > Sodium (Na) > Calcium (Ca) > Magnesium (Mg) > Aluminium (Al) > Zinc (Zn) > Iron (Fe) > Lead (Pb) > Copper (Cu) > Silver (Ag) > Gold (Au).
2. Which metal is most reactive?
Potassium (K) is the most reactive common metal in the reactivity series.
Key points:
- Potassium reacts explosively with water.
- Sodium (Na) is second in reactivity.
- These metals are kept under oil to prevent dangerous reactions with air or moisture.
3. How can I remember the reactivity series easily?
You can use a mnemonic to recall the reactivity series order.
Example mnemonic sentence:
Please Stand Carefully My Aunt Zara Is Late Having Cooked Smart Gravy.
This stands for:
Potassium, Sodium, Calcium, Magnesium, Aluminium, Zinc, Iron, Lead, Hydrogen, Copper, Silver, Gold.
4. What is the use of the reactivity series in daily life?
The reactivity series explains many real-life chemistry phenomena.
- Helps understand rusting and corrosion of metals.
- Guides extraction methods for different metals.
- Predicts the outcome of displacement reactions in laboratories.
- Explains why some metals can displace others from solutions or acids.
5. Why does hydrogen appear in the reactivity series if it’s a non-metal?
Hydrogen is included for reference when comparing metals' reactivity with acids.
- Metals above hydrogen can displace hydrogen from acids.
- It helps predict whether a metal will react with acids to produce hydrogen gas.
6. What is a displacement reaction in context of the reactivity series?
A displacement reaction is a chemical reaction where a more reactive metal replaces a less reactive metal from its compound.
For example:
- Zinc + Copper Sulphate → Zinc Sulphate + Copper
- Zinc is above copper in the series, so it can displace copper from the solution.
7. Is there a reactivity series for non-metals?
Yes, there is a reactivity series for non-metals, mainly for halogens.
- The order is based on their ability to accept electrons (oxidizing power).
- Most reactive to least: Fluorine > Chlorine > Bromine > Iodine.
8. Can the order of metals in the reactivity series change?
The standard reactivity series is generally fixed for common conditions.
However,
- Temperature changes, surface area, or catalysts can affect observed reactivity in special cases.
- Lab experiments or unusual conditions may cause slight shifts, but standard order remains for most school-level purposes.
9. How is the reactivity series related to metal extraction?
The position of a metal in the reactivity series decides the extraction method used.
- Highly reactive metals (like K, Na, Ca) are extracted by electrolysis.
- Moderate metals (like Zn, Fe, Pb) use reduction with carbon.
- Least reactive metals (like Ag, Au) are found naturally and need minimal extraction.
10. What types of exam questions are asked about the reactivity series?
Common exam questions on the reactivity series include:
- Arrange metals in order of reactivity
- Explain displacement reactions using series
- Choose correct extraction method for a metal
- State a mnemonic to recall the order
- Predict whether a reaction will take place using the series
11. Why are gold and silver placed at the bottom of the reactivity series?
Gold (Au) and Silver (Ag) are among the least reactive metals.
- They do not react easily with air, water, or acids.
- This explains why they are found in pure form in nature and are valued for making jewellery and coins.
12. Can two metals have similar reactivity in the series?
Some metals have similar reactivity and may appear close together in the series.
- Their positions may be based on specific reaction criteria.
- Standard lab conditions maintain the accepted order.
