Metals & Non-metals Important Questions Class 10 2026

Metals and Non-Metals is one of the most important parts of Class 10 Chemistry. It introduces you to the chemical and physical properties of elements, helping you understand why some substances are shiny, ductile, and good conductors, while others are dull, brittle, and insulators.

This chapter helps you differentiate between metals and non-metals based on their physical properties like malleability, ductility, and conductivity, and chemical properties such as reactions with oxygen, water, acids, and bases. You also learn about corrosion, extraction of metals, and reactivity series, which are foundational concepts for higher classes and entrance exams.

These Class 10 Metals and Non-Metals Important Questions are designed to help you:

• Strengthen your conceptual understanding of metallic and non-metallic behavior.
• Revise reactions, properties, and applications effectively.
• Prepare thoroughly for both board exams and school tests through exam-focused practice.

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Chapter 3 Metals and Non-Metals Important Questions Answers

Q1. Three pieces of a rust free iron rod are completely coated with the following:

(i) plastic

(ii) oil paint

(iii) zinc

An identical scratch is made on each piece, thus exposing the iron. The pieces of iron are kept exposed to moist air for 10 days and then checked for rust formation.

(a) State if rusting will be observed at the point of the scratch on the three iron pieces.

(b) Give reasons for your answer in each case.

(c) Name the process of applying a protective zinc coating to steel or iron.

Answer: 

(a) Rusting will be observed on the scratched areas of some of the iron pieces.

(b) (i) Plastic Coating:

Observation: Rusting will occur.

Reason: The scratch exposes the iron underneath the plastic coating. Plastic is not reactive and does not offer any galvanic protection to the exposed iron, allowing moisture and oxygen to come in direct contact with it, leading to rusting.

(ii) Oil Paint Coating:

Observation: Rusting will occur.

Reason: Similar to the plastic coating, oil paint only acts as a physical barrier. Once scratched, it exposes the iron directly to moisture and oxygen, leading to rusting at the scratch.

Zinc Coating:

Observation: Rusting will not occur.

Reason: Zinc is more reactive than iron and undergoes oxidation in preference to iron (a process called sacrificial protection). Even if the iron is exposed at the scratch, the zinc coating prevents rusting by corroding itself instead of the iron.

(c) The process of applying a protective zinc coating to steel or iron is called galvanization.

Q2. Listed here is the reactivity of certain metals.

From the list above, identify the metal(s) that are likely to be found in a pure state in the Earth's crust.

Answer: 

From the given table, metals that are likely to be found in a pure (native) state in the Earth's crust are those that are least reactive and do not readily react with air, water, or dilute acids.

Based on the table:

Gold (Au):

• Does not oxidize or burn in air.
• Does not react with water or dilute acids.
• Gold is chemically inert and highly unreactive, so it is often found in its pure, metallic state in the Earth's crust.

Platinum (Pt):

• No reaction with air, water, or dilute acids.
• Platinum is also highly unreactive and often found in its pure, metallic state in nature.

Conclusion:

The metals Gold (Au) and Platinum (Pt) are the ones likely to be found in a pure state in the Earth's crust.

Q3. The blue-coloured solution of the sulphate salt of metal W is taken in a beaker. Metal powders X, Y and Z are added one after the other to the beaker. The colour changes occurring in the solution are shown below.

State what colour change, if any, will occur if metal X is again added to the green solution in the beaker. Explain why.

Answer: 

If metal X is added again to the green solution in the beaker, the solution will turn colorless.

Explanation:

The given series of reactions involves the displacement of metals from their sulphate solutions based on the reactivity series of metals.

In this sequence:

Metal X is more reactive than metal W, as it displaces metal W from its sulphate (W-SO₄), turning the solution colorless.

Metal Y is more reactive than metal X, displacing it from the solution to form a pink solution.

Metal Z is more reactive than metal Y, displacing it to form a green solution.

When metal X is added to the green solution (which is likely to be the sulphate of metal Z, Z-SO₄), the solution turns colorless because metal X is more reactive than metal Z and displaces it from its sulphate.

This process aligns with the reactivity series of metals, where a more reactive metal always displaces a less reactive one from its compound.

Q4. A piece of iron rusts when it comes in contact with air and moisture. Prakash had two identical shiny iron pieces P and Q. To prevent the pieces from rusting, he coated piece P with oil paint and he galvanized piece Q with a coat of zinc metal. He noticed that the coatings were not complete and that a small part of the iron was exposed in both the pieces.

What is Prakash likely to observe about the exposed parts of the two iron pieces after some days? Explain why.

Answer: 

Prakash is likely to observe the following:

Piece P (coated with oil paint):

The exposed part of the iron piece will rust.

Reason: The oil paint acts as a barrier to air and moisture, but since the coating is incomplete, the exposed part remains in direct contact with air and moisture, leading to the formation of rust (Fe₂O₃⋅xH₂O).

Piece Q (galvanized with zinc):

The exposed part of the iron piece will not rust (or rust very slowly).

Reason: Galvanization involves coating the iron with zinc, which protects the iron even if the coating is incomplete. Zinc is more reactive than iron, so it preferentially reacts with air and moisture, undergoing oxidation to form a protective layer of zinc oxide and zinc hydroxide. This sacrificial protection prevents the iron from rusting.

Q5. A teacher asks her students to identify a metal, M. She gives them the following clues to help them.

(P) Its oxide reacts with both HCI and NaOH.

(Q) It does not react with hot or cold water but reacts with steam.

(R) It can be extracted by electrolysis of its ore.

(a) Identify the metal.

(b) Write the chemical equations for the reaction of the metal with HCI and NaOH respectively.

(c) What would happen if the metal is reacted with iron oxide?

Answer: 

(a) Identify the metal.

‍The metal M is aluminum (Al).
This identification is based on the following clues:

• (P): Its oxide (Al₂O₃​) is amphoteric, meaning it reacts with both acids (e.g., HCll) and bases (e.g., NaOH.
• (Q): Aluminum does not react with cold or hot water but reacts with steam, forming aluminum oxide and hydrogen gas.
• (R): Aluminum is extracted by electrolysis of its ore (bauxite) through the Hall-Héroult process.

(b) Write the chemical equations for the reaction of the metal with HCI and NaOH respectively.

‍Reaction with HCl (acid):

2Al+6HCl→2AlCl₃+3H₂↑

Aluminum reacts with hydrochloric acid to form aluminum chloride and release hydrogen gas.

Reaction with NaOH (base):
2Al+2NaOH+6H₂O→2NaAl(OH)₄+3H₂↑

Aluminum reacts with sodium hydroxide and water to form sodium aluminate and release hydrogen gas.

‍(c) What would happen if the metal is reacted with iron oxide?

‍When aluminum reacts with iron oxide (Fe₂O₃), a highly exothermic reaction known as the thermite reaction occurs. Aluminum reduces iron oxide to iron while forming aluminum oxide:2Al+Fe₂O₃→2Fe+Al₂O₃

_‍Outcome:

• Molten iron is produced.
• This reaction is used in the thermite welding process to join railway tracks or large metal components.

Q6. A metallic element, M, has the following properties:

- floats on water

- can be cut with a knife

- occurs naturally as its chloride, of formula MCI

- its oxide dissolves in water to form the hydroxide

(a) State the method of manufacture of the metal M. 

(b) Name the major byproduct obtained in the process.

Answer: 

(a) State the method of manufacture of the metal M. 

The metal M (sodium or potassium) is manufactured using the electrolysis of its molten chloride (e.g., sodium chloride for sodium, potassium chloride for potassium).

During the process:

• The molten chloride is electrolyzed in an electrolytic cell.
• The metal is produced at the cathode (reduction of metal ions to metal).
• Chlorine gas is released at the anode.

For sodium, the reaction is:
At cathode: Na⁺+e⁻→Na (l)
At anode: 2Cl⁻→Cl₂(g)+2e⁻

(b) Name the major byproduct obtained in the process.

The major byproduct of this process is chlorine gas (Cl₂​).

This process is highly efficient and widely used for producing sodium and other reactive metals.

Q7. A metal oxide on being heated with carbon does NOT produce carbon dioxide.

Give a possible explanation for this behaviour of the metal oxide.

Answer: 

If a metal oxide does not produce carbon dioxide when heated with carbon, the most likely explanation is that the metal in the metal oxide is more reactive than carbon.

• The reduction of a metal oxide by carbon depends on the reactivity of the metal relative to carbon.
• If the metal is more reactive than carbon (e.g., metals like aluminum or magnesium), carbon cannot reduce the metal oxide effectively.
• This is because the bond between the metal and oxygen in the metal oxide is stronger than the bond carbon can form with oxygen to produce carbon dioxide.
• Metals high in the reactivity series (e.g., aluminum, magnesium, calcium) have oxides that are not reduced by carbon.
• Instead, these oxides require more energy-intensive methods like electrolysis for reduction.

This behavior can be summarized using the reactivity series, where metals above carbon in the series are resistant to reduction by carbon.

Q8. Krunal now replaces the iron plate with a silver plate. He sees that there is no deposition of copper on the silver plate before starting the current.

Which of the following could be the reason?

a. Silver is more reactive than iron.

b. Silver is less reactive than copper.

c. Silver is a poorer conductor of electricity than iron. 

d. Silver is a better conductor of electricity than copper.

Answer: (b) Silver is less reactive than copper

Explanation: 

In an electrochemical reaction, a metal that is more reactive will displace a less reactive metal from its solution.

Iron is more reactive than copper, so copper deposits on the iron plate when used. However, silver is less reactive than copper. Therefore, silver cannot displace copper ions from the solution to form a copper deposit.

The reactivity series of metals confirms this:

Potassium > Sodium > Calcium > Magnesium > Aluminum > Zinc > Iron > Tin > Lead > Hydrogen > Copper > Silver > Gold

This aligns with the observation that no deposition occurs on the silver plate before the current is applied.

Q9. After a few minutes, even before he turned the switch on, he noticed that copper was deposited on the iron plate.

This could have been due to

a. electrolysis

b. a combination reaction

c. electroplating

d. a displacement reaction

Answer: 

(d) a displacement reaction

Explanation:

Even before the switch was turned on, the deposition of copper on the iron plate occurred because iron is more reactive than copper in the reactivity series. When the iron plate was placed in the solution containing Cu²⁺ ions (like copper sulfate solution), a displacement reaction occurred:

Fe (s)+Cu2+(aq)→Fe²⁺(aq)+Cu 

In this reaction:

• Iron (Fe) displaced copper (Cu) from its compound because iron has a higher tendency to lose electrons and form ions compared to copper.

Q10. Which of the following is likely to happen when the current is started?

a. Iron will be deposited on the copper plate.

b. Copper will continue to be deposited on the iron plate.

c. No reaction will occur at the iron plate or at the copper plate.

d. The copper already deposited on the iron plate will go back into the solution.

Answer

(d) The copper already deposited on the iron plate will go back into the solution.

Explanation: 

When a current flows in an electrolytic setup involving iron and copper:

• Copper ions (Cu²⁺) in solution are reduced at the cathode to form copper metal.
• Iron atoms at the anode are oxidized to Fe²⁺, dissolving into the solution.

Iron will be deposited on the copper plate.

• Unlikely, as Fe²⁺ ions are not being introduced into the solution, and copper ions are more likely to be reduced.

Copper will continue to be deposited on the iron plate.

• This is possible only if the iron plate is acting as the cathode in the circuit, as Cu²⁺ ions are reduced to metallic copper.

No reaction will occur at the iron plate or at the copper plate.

• Unlikely, since current is flowing and redox reactions will occur at the electrodes.

The copper already deposited on the iron plate will go back into the solution.

• This will happen if the iron plate is made the anode. The deposited copper will oxidize back into Cu²⁺, entering the solution.

Some More Important Question Answers of Class 10 Science chapter 3

Q1. Why does calcium float when it reacts with water?

Ans. When calcium metal is added to water, it reacts slowly compared to sodium and potassium. It forms calcium hydroxide which is only sparingly soluble, and hydrogen gas is released:

Ca+2H2​O→Ca(OH)2​+H2​↑

The hydrogen bubbles formed stick to the surface of calcium, making the piece lighter and causing it to float on water. This is why calcium appears to rise during the reaction. The reaction also makes the water slightly milky due to insoluble calcium hydroxide. 

Q2. Define amphoteric oxides with two examples.

Ans.  Amphoteric oxides are those which react with both acids and bases to form salt and water. Aluminium oxide and zinc oxide are common examples.
For example:

Al2​O3​+6HCl→2AlCl3​+3H2​O

Al2​O3​+2NaOH→2NaAlO2​+H2​O

Thus, these oxides behave like acidic oxides with bases and basic oxides with acids. This property of dual behaviour is very important in metallurgy where amphoteric oxides dissolve in both acids and alkalies.

Q3. Write chemical equations to show the reaction of aluminium with:

(a) Dilute HCl (b) NaOH

Ans. Aluminium is reactive and shows amphoteric nature.

(a) With dilute HCl:  2Al+6HCl→2AlCl3​+3H2​↑

Here aluminium reacts like a typical metal with acid to release hydrogen gas.

(b) With NaOH: Al+2NaOH+6H2​O→2NaAl(OH)4​+3H2​↑

This shows aluminium also reacts with bases. Thus aluminium is amphoteric in nature and reacts both ways.

Q4. Why does a shiny copper vessel turn green after some time?

Ans.  When copper is kept exposed to moist air for a long period, it loses its shine and develops a green layer. This layer is formed due to the reaction of copper with carbon dioxide, oxygen, and water vapour in the air. The product is basic copper carbonate:

Cu+H2​O+CO2​+O2​→CuCO3​⋅Cu(OH)2

This green coating is also called patina, which protects the copper beneath from further corrosion. That is why old copper structures often appear greenish in colour.

Q5. Name two metals which can melt on the palm and explain why.

Ans. Gallium and caesium are two metals that can melt on the palm. Their melting points are very low around 30°C for gallium and 28.5°C for caesium. The normal temperature of the human body (≈37°C) is enough to melt them. This shows that not all metals have very high melting points. Such metals are used in making temperature-sensitive devices and fuses.

Q6. Describe an activity to show that both air and water are necessary for rusting of iron.

Ans.  Take three test tubes with clean iron nails. In tube A, put water and leave open to air. In tube B, add boiled water (air removed) and a thin layer of oil on top to prevent oxygen entry. In tube C, keep anhydrous calcium chloride (absorbs moisture) and close the tube tightly. After a few days, the nail in tube A rusts, but in B and C it does not. This proves that both oxygen and water are required for rusting. 

Q7. Write an activity to show that iron displaces copper from copper sulphate solution.

Ans. Take blue copper sulphate solution in a beaker and suspend a clean iron nail in it. After a few hours, the blue colour fades and a reddish-brown layer of copper is deposited on the iron. This happens because iron is more reactive than copper and displaces it from its salt solution:

Fe+CuSO4​→FeSO4​+Cu

Thus we can understand that this activity demonstrates the reactivity series of metals. 

Q8. Why does magnesium not react with cold water but reacts with steam?

Ans. Magnesium is covered with a thin protective oxide film that prevents it from reacting with cold water. But when steam is passed over hot magnesium, the reaction occurs to form magnesium oxide and hydrogen gas:

Mg+H2​O(g)→MgO+H2​↑

This shows magnesium is less reactive than sodium and calcium but more reactive than many transition metals.

Q9. Explain electrolytic refining of copper with reactions.

Ans. In electrolytic refining, the anode is impure copper, the cathode is a thin sheet of pure copper, and the electrolyte is acidified copper sulphate solution. When current is passed:
At anode: Cu→Cu2++2e−

At cathode: Cu2++2e−→Cu

Thus, pure copper is deposited on the cathode. Impurities like gold and silver fall as anode mud while more reactive metals dissolve in solution. This gives copper of 99.9% purity. 

Q10. Explain the extraction of zinc from zinc carbonate ore (calamine).

Ans.
Zinc is extracted from its carbonate ore ZnCO₃. First, the ore is heated strongly in the absence of air (calcination) to give zinc oxide:

ZnCO3​→ZnO+CO2​↑

Then zinc oxide is reduced with carbon at high temperature:

ZnO+C→Zn+CO↑

The zinc vapours are collected and condensed to get pure metal. This method works because zinc is moderately reactive and can be reduced by carbon. 

Q11. Show the formation of magnesium chloride with electron transfer.

Ans. Magnesium has two valence electrons which it loses to form Mg²⁺. Each chlorine atom gains one electron to form Cl⁻. The transfer of electrons gives MgCl₂:

Mg→Mg2++2e−

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Cl+e−→Cl−

Thus, two chloride ions combine with one Mg²⁺ ion to form MgCl₂. Ionic compounds like MgCl₂ are hard solids with high melting points due to strong electrostatic attraction. 

Q12. Why can carbon not reduce the oxides of sodium, magnesium, or aluminium?

Ans. Sodium, magnesium and aluminium are highly reactive metals and lie above carbon in the reactivity series. Their oxides are very stable and the bond with oxygen is stronger than carbon’s affinity for oxygen. Hence carbon cannot reduce them. They are obtained by electrolytic reduction of their molten salts or oxides (e.g., electrolysis of molten NaCl for sodium, Hall-Héroult process for aluminium).

Q13. Why does silver tarnish and copper turn green on exposure to air? How can we clean them?

Ans. Silver reacts with traces of hydrogen sulphide in air to form black silver sulphide (Ag₂S). Copper reacts with carbon dioxide and moisture to form green basic copper carbonate (CuCO₃·Cu(OH)₂). These are forms of corrosion. Copper vessels can be cleaned with lemon juice or tamarind as acids dissolve the basic carbonate. Silver is cleaned by polishing or using mild chemical dips.

Q14. What is an alloy? Give composition and uses of brass, bronze, and solder.

Ans.  An alloy is a homogeneous mixture of two or more metals (or metals and non-metals).

• Brass: Cu + Zn (used in musical instruments, door handles).
• Bronze: Cu + Sn (used for statues, medals).
• Solder: Pb + Sn (low melting alloy used for joining wires).

Alloys have improved properties such as strength, hardness, resistance to corrosion, or lower melting point.

Q15. Why is hydrogen gas generally not evolved when metals react with nitric acid?

Ans. Nitric acid is a strong oxidising agent. It oxidises any nascent hydrogen produced into water, so instead of H₂ gas we get nitrogen oxides (NO, NO₂, N₂O) along with the metal nitrate. Example: Cu+4HNO3​→Cu(NO3​)2​+2NO2​+2H2​O

Thus, metals generally do not release hydrogen with HNO₃, except very unreactive ones like Mg and Mn with dilute nitric acid.

Q16. How can we use displacement reactions to arrange metals in decreasing order of reactivity?

Ans. If a metal can displace another from its salt solution, it is more reactive. For example, Fe displaces Cu from CuSO₄ but not Zn from ZnSO₄. This means Fe is more reactive than Cu but less than Zn. By performing such pairwise displacement experiments with solutions of different salts, we can arrange metals into a reactivity series.

Q17. Design an activity to show metals conduct electricity. Why do they conduct?

Ans. Make a circuit using a battery, a bulb and wires. Replace a portion of the wire with a metal strip (like copper or aluminium). The bulb glows, showing metals conduct electricity. Metals conduct because they have free moving electrons in their structure which can flow under an electric field. This property makes metals useful in making wires and cables. \

Q18. Differentiate between calcination and roasting with examples.

Ans. 

• Calcination: heating carbonate ore in the absence of air. Example: ZnCO3​→​ZnO+CO2

• Roasting: heating sulphide ore in the presence of excess air. Example: 2ZnS+3O2​→​​2ZnO+2SO2

Thus, calcination is for carbonates while roasting is for sulphides. Both processes convert ores into oxides for easier reduction.

Q19. What precautions and observations are seen while burning magnesium ribbon?

Ans.  Here are the precautions and observations are seen while burning magnesium ribbon:

• Precautions: (1) The ribbon should be cleaned with sandpaper to remove oxide coating. (2) Do not look at the flame directly as it is dazzling.
• Observations: Magnesium burns with a bright white flame and forms a white powder of magnesium oxide (MgO). (2Mg+O2​→2MgO)

Q20. Name two metals that occur in native state and explain why.

Ans. Gold and platinum are found in the native state. This is because they are very unreactive metals and lie at the bottom of the reactivity series. They do not combine with oxygen, carbon dioxide or moisture under normal conditions. Due to their lustre and inertness, they are used for making jewellery, coins and ornaments.

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Video Lecture: Must-watch for Quick Revision

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Here are some extra Questions for Practice, to ace your board exams!

Q1. Differentiate between corrosion and rusting with examples.

Q2. Which property of metals makes them suitable for making bells and wires? Explain.

Q3. Why are alloys preferred over pure metals? Give two reasons.

Q4. Explain with equations the extraction of zinc from zinc blende (ZnS).

Q5. A student dipped iron nails in copper sulphate solution. What changes will be observed after 20 minutes? Write the reaction.

Q6. What is the difference between electrolytic refining and galvanization?

Q7. Why does aluminium foil not corrode easily even though aluminium is a highly reactive metal?

Q8. State two safety precautions while burning magnesium ribbon in the laboratory.

Q9. What is calcination? Give one example with a chemical equation.

Q10. Name one metal that is: (i) stored in kerosene, (ii) highly ductile, (iii) liquid at room temperature.

Benefits of Class 10: Metals and Non-Metals - Important Questions

Using Class 10 metals and non-metals for important questions offers several advantages:

• These questions cover all the key topics in the chapter, making sure that you don’t miss any important concepts.
• Regular practice will help you review important topics.
• As you become familiar with various types of questions, your confidence will increase, reducing exam anxiety.
• Practicing under timed conditions helps improve your speed, which is essential in finishing the exam on time.
• With the help of metal and non-metal important questions in Class 10, students will become confident in solving each question of this chapter. 

How to use Class 10 metals and non-metals for important questions? 

Just practicing from the class 10 metals and nonmetals and using it correctly includes a little bit of difference. Here are some tips to help students use the metals and nonmetals important questions correctly:

• Before any questions, make sure you've fully understood the concepts of metals and nonmetals.
• Break down your practice into specific topics like reactivity with acids, the properties of metals and non-metals, and the extraction of metals. This will help you master each section.
• Consistent practice is essential. Aim to solve a few questions every day—at least 15 questions each day—so you don’t feel anxious about the exam.
• Solving previous year's question papers will give you an idea of the question pattern and difficulty level.
• Don’t hesitate to ask your teacher or peers if you find certain questions difficult. Group discussions often provide new ideas. 

FAQs

Q1. How many marks are usually allotted to this chapter in Class 10 board exams?

Ans.  Typically, this chapter carries around 3 to 5 marks in the final exam, often divided between reaction-based and reasoning questions.

Q2. Which topics from Metals and Non-Metals are most important for exams?

Ans.  Reactivity series, corrosion, properties of metals and non-metals, and extraction of metals are the most frequently tested topics.

Q3. Are diagrams necessary in this chapter?

Ans. Yes, simple diagrams like the setup for electrolysis or extraction processes help you present answers better and can earn extra marks.

Q4. How can I easily remember the reactivity series?

Ans. Use mnemonics such as “Please Stop Calling Me A Zebra Instead Try Learning How Copper Saves Gold” to recall the order.

Q5. How should I revise this chapter before the exam?

Ans. Go through your summary notes, practice reaction equations, and revise the reactivity series and corrosion prevention methods one day before the exam.