Important Questions Class 10 Science Chapter 3 Metals and Non-metals
CBSE Important Questions Class 10 Science – Metals and Non-metals
Metals and Non-metals is the third chapter of Class 10 Science. It explains the physical and chemical properties of metals and non-metals, how metals react with oxygen, water and acids, the activity series of metals, the formation of ionic compounds, and how metals are protected from corrosion.
Important Questions Class 10 Science Chapter 3 Metals and Non-metals
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These CBSE important questions cover the activity series, displacement reactions such as zinc in copper sulphate and copper sulphate in an iron pot, the formation of magnesium oxide by transfer of electrons, why ionic compounds conduct electricity in solution, and why aluminium does not corrode easily. Every question has a clear answer in simple English.
CBSE Important Questions Class 10 Science – Metals and Non-metals
Q1. Why can the reaction of metals with water, hydrogen and acid not be used to compare the reactivity of metals? (1 mark)
Answer:
Not all metals react with these reagents. Hence, the reactions of metals with water, hydrogen and acids cannot be used to compare the reactivity of all metals.
Q2. Define the activity series of metals. (1 mark)
Answer:
The activity (reactivity) series is a list of common metals arranged in order of their decreasing reactivity.
Q3. Explain why zinc metal can displace copper from copper sulphate solution but copper cannot displace zinc from zinc sulphate solution. (2 marks)
Answer:
Zinc is more reactive than copper, so it displaces copper from copper sulphate solution.
Zn (s) + CuSO₄ (aq) → ZnSO₄ (aq) + Cu (s)
Copper is less reactive than zinc, so it cannot displace zinc from zinc sulphate solution.
Q4. What happens when metals react with acids? (1 mark)
Answer:
Metals react with dilute acids to form a salt and liberate hydrogen gas.
Zn (s) + 2HCl (aq) → ZnCl₂ (aq) + H₂ (g)
Q5. Show the formation of MgO by the transfer of electrons between the combining atoms. Why are aqueous solutions of ionic compounds able to conduct electricity? (2 marks)
Answer:
Magnesium (2, 8, 2) loses its two outer electrons to form Mg²⁺, and oxygen (2, 6) gains these two electrons to form O²⁻. The oppositely charged ions are held together to form magnesium oxide.
Aqueous solutions of ionic compounds conduct electricity because, in solution, the forces of attraction between the oppositely charged ions become weak and the ions become free to move. These moving ions carry the current.
Q6. Give reasons for the following: (i) Metals are regarded as electro-positive elements. (ii) When a piece of copper metal is added to a solution of zinc sulphate, no change takes place, but the blue colour of copper sulphate fades away when a piece of zinc is placed in its solution. (iii) Articles made of aluminium do not corrode even though aluminium is an active metal. (3 marks)
Answer:
(i) Metals lose electrons and form positive ions when they form bonds, so they are called electro-positive elements.
(ii) A more reactive metal can displace a less reactive metal from its salt solution. Copper is less reactive than zinc, so it cannot displace zinc and no change takes place. Zinc is more reactive than copper, so it displaces copper from copper sulphate, and the blue colour fades.
(iii) Aluminium reacts with oxygen in the air to form a thin, protective layer of aluminium oxide, which prevents further corrosion of the metal.
Q7. What is the activity series of metals? Rearrange the following metals in an increasing order of reactivity: Aluminium, Zinc and Mercury. (2 marks)
Answer:
The activity series of metals is the list of metals arranged in order of their decreasing reactivity.
Increasing order of reactivity: Mercury < Zinc < Aluminium
Q8. (a) Arrange the metals Zn, Mg, Al, Cu and Fe in a decreasing order of reactivity. (b) What would you observe when you put (i) some zinc pieces into blue copper sulphate solution? (ii) some copper pieces into green ferrous sulphate solution? (4 marks)
Answer:
(a) Decreasing order of reactivity: Mg > Al > Zn > Fe > Cu
(b) (i) The blue colour of the copper sulphate solution fades and a reddish-brown layer of copper forms, because zinc displaces copper from the solution.
Zn (s) + CuSO₄ (aq) → ZnSO₄ (aq) + Cu (s)
(ii) No change is observed, because copper is less reactive than iron and cannot displace it from ferrous sulphate solution.
Q9. State the reason for the following behaviour of zinc metal: on placing a piece of zinc metal in a solution of mercuric chloride, it acquires a shining silvery surface, but when it is placed in a solution of magnesium sulphate, no change is observed. (2 marks)
Answer:
Zinc is more reactive than mercury, so it displaces mercury from mercuric chloride and a shiny layer of mercury forms on its surface.
Zn (s) + HgCl₂ (aq) → ZnCl₂ (aq) + Hg (l)
Zinc is less reactive than magnesium, so it cannot displace magnesium from magnesium sulphate and no change is observed.
Q10. A solution of copper sulphate was kept in an iron pot. After a few days, the iron pot was found to have a number of holes in it. Explain with the help of an equation what reaction took place. (3 marks)
Answer:
A more reactive metal displaces a less reactive metal from its salt solution. Iron is more reactive than copper, so the iron of the pot displaces copper from copper sulphate solution. As the iron gets used up in the reaction, holes appear in the pot.
Fe (s) + CuSO₄ (aq) → FeSO₄ (aq) + Cu (s)
Q11. A metal 'X' displaces metal 'Y' from its salt solution. Which will be nearer to the top of the reactivity series? (2 marks)
Answer:
Metal 'X' will be nearer to the top of the reactivity series. A metal can displace another metal from its salt solution only if it is more reactive, so X is more reactive than Y.
Related Study Material on Extramarks
- Important Questions Class 10 Science Chapter 1 – Chemical Reactions and Equations
- Important Questions Class 10 Science Chapter 2 – Acids, Bases and Salts
- Important Questions Class 10 Science Chapter 3 – Metals and Non-metals
- Important Questions Class 10 Science Chapter 4 – Carbon and Its Compounds
- Important Questions Class 10 Science – Life Processes
Q.1 Give reasons:
(a) Platinum, gold and silver are used to make jewellery.
(b) Sodium, potassium and lithium are stored under oil.
(c) Aluminium is a highly reactive metal, yet it is used to make utensils for cooking.
(d) Carbonate and sulphide ores are usually converted into oxides during the process of extraction.
Marks:3
Ans
1. Platinum, gold, and silver are used to make jewellery because they are very less reactive metals. Also they are lustrous and do not corrode easily.
2. Sodium, potassium, and lithium are very reactive metals. They react vigorously with air as well as water; therefore, they are kept immersed in kerosene oil in order to prevent their contact with air and moisture.
3. Aluminium is a highly reactive metal and is resistant to corrosion. This is because aluminium reacts with oxygen present in air to form a thin layer of aluminium oxide. This oxide layer is very stable and prevents further reaction of aluminium with oxygen. Also, it is light in weight and a good conductor of heat. Hence, it is used to make cooking utensils.
4. Carbonate and sulphide ores are usually converted into oxides during the process of extraction because it is easier to obtain metals from their oxides as compared to their carbonates and sulphides.
CBSE Class 10 Science Important Questions
FAQs (Frequently Asked Questions)
Reactivity series, ionic compounds, amphoteric oxides, extraction of metals, corrosion, and displacement reactions are most important. These topics appear in reasoning and equation-based questions.
This article includes 40 solved questions from Important Questions Class 10 Science Chapter 3. The questions cover properties, reactions, metallurgy, corrosion, and NCERT exercise patterns.
Yes, Metals and Non-metals is important for CBSE 2026. It includes direct definitions, activity-based observations, balanced equations, and application-based reasoning.
Practise by grouping questions into properties, reactions, ionic compounds, metallurgy, and corrosion. This pattern matches the NCERT chapter flow.
Important equations include reactions of metals with oxygen, water, dilute acids, and salt solutions. Roasting, calcination, thermit reaction, and ionic compound formation are also important.