CBSE Class 10 Science • Chapter 3 • Revision 2026
Metals and Non-metals Class 10 Worksheet
Practise CBSE Science Chapter 3 with this Metals and Non-metals Class 10 worksheet. Revise physical and chemical properties, the reactivity series, ionic compounds, metal extraction and corrosion. Use the explanations, MCQs, worked equations and case-based questions below to prepare for chapter tests and strengthen your understanding.
Why is copper used for electrical wires? Why is sodium stored under kerosene? Why does solid sodium chloride fail to conduct electricity, while molten sodium chloride conducts it? These questions connect the properties of materials with their structure and reactivity.
A worksheet on Metals and Non-metals Class 10 helps you apply these ideas to unfamiliar situations. Instead of memorising isolated facts, practise explaining a property, predicting a reaction and supporting your answer with a balanced equation. The questions and answers on this page provide practice alongside your chapter worksheet.
Begin with Your Chapter Notes
Review our Metals and Non-metals Class 10 notes and mind map before attempting the questions. Use the notes for explanations and the mind map to recall the connections between properties, reactions, extraction and uses.
What to Revise for Metals and Non-metals Class 10
- Physical properties of metals and non-metals, including important exceptions.
- Reactions of metals with oxygen, water, dilute acids and salt solutions.
- The reactivity series and displacement reactions.
- Electron transfer and the formation of ionic compounds.
- Properties of ionic compounds.
- Minerals, ores, roasting, calcination and reduction.
- Electrolytic refining, corrosion prevention and alloys.
Metals and Non-metals: Properties and Exceptions
| Property | Metals: General Behaviour | Non-metals: General Behaviour |
|---|---|---|
| Lustre | Usually shiny when freshly cleaned. | Usually dull; iodine is a lustrous exception. |
| Malleability | Usually can be hammered into sheets. | Solid non-metals are usually brittle. |
| Ductility | Usually can be drawn into wires. | Generally cannot be drawn into wires. |
| Electrical conductivity | Generally good conductors. | Generally poor conductors; graphite conducts electricity. |
| Physical state | Usually solid at room temperature; mercury is liquid. | May be solid or gaseous; bromine is liquid at room temperature. |
| Nature of oxides | Often basic; aluminium oxide and zinc oxide are amphoteric. | Often acidic; some, such as carbon monoxide, are neutral. |
Avoid Statements with “All”
Write “metals are generally hard” rather than “all metals are hard”. Sodium and potassium are soft enough to be cut with a knife. Similarly, graphite shows that a non-metal can conduct electricity. Exceptions are important in Metals and Non-metals Class 10 MCQs.
Important Chemical Reactions with Balanced Equations
Metals with Oxygen
Many metals react with oxygen to form metal oxides. Magnesium burns to form magnesium oxide:
2Mg(s) + O2(g) → 2MgO(s)
Metals with Water
Reaction conditions depend on the metal. Sodium reacts vigorously with cold water, while iron reacts with steam under suitable heating conditions.
2Na + 2H2O → 2NaOH + H2
3Fe + 4H2O → Fe3O4 + 4H2
, with steam.
Metals with Dilute Acids
Many metals above hydrogen in the reactivity series release hydrogen from dilute hydrochloric acid. Copper does not release hydrogen from dilute hydrochloric acid under ordinary conditions.
Zn + 2HCl → ZnCl2 + H2
Metals with Salt Solutions
A more reactive metal can displace a less reactive metal from its salt solution. For example:
Zn + CuSO4 → ZnSO4 + Cu
Reactivity Series Class 10: How to Use It
K > Na > Ca > Mg > Al > Zn > Fe > Pb > H > Cu > Hg > Ag > Au
This school-level sequence runs from higher to lower reactivity. Hydrogen is included as a reference for comparing the ability of metals to release hydrogen from suitable dilute acids.
Worked Example: Predict a Displacement Reaction
Will copper react with zinc sulphate solution?
Zinc is above copper in the reactivity series.
Copper is less reactive than zinc.
Copper cannot displace zinc from zinc sulphate solution.
No displacement reaction occurs under the usual conditions.
Ionic Compounds and Electron Transfer
Metals commonly lose electrons to form positive ions, while non-metals gain electrons to form negative ions. Electrostatic attraction between oppositely charged ions forms an ionic bond. The resulting compound is electrically neutral overall.
Formation of Magnesium Chloride
Magnesium loses two electrons:
Mg → Mg2+ + 2e−
Two chlorine atoms gain one electron each:
2Cl + 2e− → 2Cl−
One Mg2+ ion combines with two Cl− ions.
The formula is MgCl2.
These steps describe electron transfer. The overall reaction between the elements is Mg + Cl2 → MgCl2.
Ionic compounds generally have high melting points because strong attractions hold their ions together. In a solid, the ions are fixed in position. When molten, or dissolved in water where soluble, their mobile ions can carry electric current.
Extraction of Metals: Roasting and Calcination
A mineral is a naturally occurring material containing a metal or its compounds. An ore is a mineral deposit from which a metal can be extracted economically. The extraction method depends on the metal’s reactivity and the nature of its ore.
| Feature | Roasting | Calcination |
|---|---|---|
| Common application | Conversion of sulphide ores into oxides. | Conversion of carbonate ores into oxides. |
| Heating conditions | Strong heating in excess air. | Strong heating in limited or no air. |
| Zinc example | 2ZnS + 3O2 → 2ZnO + 2SO2 | ZnCO3 → ZnO + CO2 |
Converting an ore to its oxide is often followed by reduction. For zinc, a textbook example is: ZnO + C → Zn + CO, on heating. Highly reactive metals such as sodium and aluminium require electrolytic extraction rather than reduction of their oxides using carbon.
Metals and Non-metals Class 10 MCQ Questions with Answers
1. Which non-metal conducts electricity?
A. Sulphur
B. Graphite
C. Phosphorus
D. Oxygen
Answer: B. Graphite has mobile electrons that allow electrical conduction.
2. Which oxide reacts with both acids and bases?
A. Na2O
B. CaO
C. Al2O3
D. CO2
Answer: C. Aluminium oxide is amphoteric.
3. Why does molten sodium chloride conduct electricity?
A. Its ions can move
B. It becomes a metal
C. It contains only neutral molecules
D. Its ions disappear
Answer: A. Mobile ions carry charge through the molten compound.
Metals and Non-metals Class 10 Case Study Questions
Case Study: Testing Iron in Salt Solutions
A student places clean iron nails in separate solutions of copper sulphate and zinc sulphate. A reddish-brown deposit forms in the copper sulphate experiment, while no displacement is observed in the zinc sulphate experiment.
- Name the reddish-brown deposit.
- Write the balanced equation for the reaction.
- Arrange zinc, iron and copper in decreasing reactivity.
- Explain the absence of displacement in zinc sulphate.
Answers:
The deposit is copper.
Fe + CuSO4 → FeSO4 + Cu.
Reactivity order: Zn > Fe > Cu.
Iron is less reactive than zinc and cannot displace it.
Important Questions and Extra Practice
Use these Metals and Non-metals Class 10 important questions to check your understanding. Explain the reason behind each answer and include an equation where relevant.
- Explain why sodium is stored under kerosene.
- Distinguish malleability from ductility.
- Explain why aluminium resists further corrosion despite being reactive.
- Describe the formation and properties of an ionic compound.
- Compare roasting and calcination using zinc ores.
- Explain the electrode arrangement in electrolytic refining of copper.
- Describe how galvanisation protects iron.
- Explain why alloys are used instead of pure metals for some purposes.
For your 2026 revision, attempt these questions and your worksheet before consulting the notes. Follow this with NCERT exercise questions and verified previous year questions. Pay particular attention to exceptions, reaction conditions and the reasons behind extraction methods.
Related CBSE Class 10 Science Resources
Clear your doubts using the Metals and Non-metals Class 10 notes and mind map . Revise equation balancing with the Chemical Reactions and Equations worksheet with answers .
Explore our CBSE Class 10 Science worksheet collection for more chapter practice.
Frequently Asked Questions
How should I use the Metals and Non-metals Class 10 worksheet?
Revise your notes, attempt the worksheet independently and review each answer carefully. Check whether errors involve an exception, reactivity order, equation or scientific explanation. Reattempt difficult questions after revising the relevant concept.
Why is sodium stored under kerosene?
Sodium reacts vigorously with oxygen and moisture. Storing it under kerosene limits contact with air and water and prevents unwanted reactions.
Why does aluminium resist corrosion even though it is reactive?
Aluminium develops a thin, protective oxide layer that limits further contact between the metal and its surroundings. Anodising increases the thickness of this protective layer.
Why do ionic compounds conduct electricity when molten but not when solid?
Their ions exist in both states. In a solid, the ions are fixed in a lattice and cannot move freely. In the molten state, the ions become mobile and carry electric current.
Why do ionic compounds generally have high melting points?
Strong electrostatic attractions hold oppositely charged ions together. Considerable energy is needed to overcome these attractions during melting.
What is the difference between malleability and ductility?
Malleability is the ability to be hammered or rolled into thin sheets. Ductility is the ability to be drawn into wires. Aluminium foil illustrates malleability, while copper wire illustrates ductility.
Why is hydrogen included in the reactivity series?
Hydrogen acts as a reference for comparing metals. Many metals above hydrogen can displace it from suitable dilute acids, while metals below it generally cannot under ordinary conditions.
Do all metals release hydrogen with nitric acid?
No. Nitric acid is an oxidising acid, so hydrogen is generally not evolved in the usual way. NCERT notes that magnesium and manganese can evolve hydrogen with very dilute nitric acid.
Does roasting always produce the final metal?
No. In common examples such as zinc sulphide, roasting produces an oxide, which is then reduced to obtain the metal. The complete sequence depends on the ore and the metal’s reactivity.
Why are highly reactive metals extracted by electrolysis?
Their compounds are difficult to reduce using common reducing agents such as carbon. Electrolysis supplies the energy needed to obtain the metal from a suitable molten electrolyte.
What happens during electrolytic refining of copper?
Impure copper is the anode, a thin sheet of pure copper is the cathode and acidified copper sulphate solution is the electrolyte. Copper dissolves from the anode and deposits on the cathode; some insoluble impurities collect as anode mud.
Why do silver articles turn black?
Silver reacts with sulphur-containing substances in the air to form a surface layer of silver sulphide, which appears black.
Why does copper develop a green coating?
In moist air containing carbon dioxide, copper gradually develops a green coating of basic copper carbonate.
What is galvanisation?
Galvanisation coats iron or steel with zinc. The coating limits contact with air and moisture, and zinc also provides protection because it is more reactive than iron.
What are alloys, and why are they useful?
Alloys are mixtures of a metal with other elements. They are made to obtain useful properties such as greater hardness or corrosion resistance. Brass contains copper and zinc, while stainless steel contains iron with chromium and other elements.
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