Metals and non-metals are elements classified by their physical and chemical properties.
Metals usually lose electrons, while non-metals usually gain electrons during chemical reactions.
Metals and non-metals shape many daily objects, from electric wires to cooking vessels and medicines. Important Questions Class 10 Science Chapter 3 help students practise properties, reactions, ionic compounds, extraction of metals, corrosion, and alloys. CBSE 2026 questions often test reactivity order, balanced equations, displacement reactions, and reasoning-based applications. Students should focus on exact observations, correct chemical equations, and the reason behind each property.
Key Takeaways
- Metals: Metals are generally lustrous, malleable, ductile, sonorous, and good conductors.
- Non-metals: Non-metals usually form acidic or neutral oxides and gain electrons during reactions.
- Reactivity Series: A more reactive metal displaces a less reactive metal from its salt solution.
- Corrosion: Iron rusts only when both air and moisture are present.
Important Questions Class 10 Science Chapter 3 Structure 2026
| Area |
Key Concept |
Exam Focus |
| Properties |
Metals, non-metals, ionic compounds |
Definitions, exceptions, comparisons |
| Reactions |
Oxygen, water, acids, salt solutions |
Balanced equations, observations |
| Metallurgy |
Ores, extraction, refining, corrosion |
Process-based answers |
Important Questions Class 10 Science Chapter 3 Overview
Important Questions Class 10 Science Chapter 3 begin with basic differences between metals and non-metals. These answers build the base for reactions, extraction, and corrosion.
Q1. What Are Metals And Non-metals?
Metals are elements that usually lose electrons and form positive ions. Non-metals usually gain electrons and form negative ions.
Metals are generally shiny, malleable, ductile, and good conductors. Non-metals are usually dull, brittle, and poor conductors.
Final Answer: Metals form cations, and non-metals form anions.
Q2. What Does Class 10 Science Chapter 3 Mainly Test?
Class 10 Science Chapter 3 mainly tests properties, reactions, reactivity series, ionic compounds, extraction, and corrosion.
Students must connect observations with chemical behaviour. For example, sodium reacts violently with water because it is highly reactive.
Final Answer: The chapter tests both theory and chemical equations.
Q3. Why Are Metals Used In Daily Life?
Metals are used because they conduct heat, conduct electricity, and can be shaped easily. Their malleability and ductility make them useful.
Copper is used in wires because it conducts electricity. Aluminium is used in utensils because it conducts heat.
Final Answer: Metals are useful because of conductivity, strength, and shape flexibility.
Metals And Non-metals Class 10 Important Questions On Physical Properties
Metals and Non-metals Class 10 Important Questions often start with physical properties. Students must also remember exceptions because NCERT asks reasoning questions.
Q4. What Are The Main Physical Properties Of Metals?
Metals are lustrous, hard, malleable, ductile, sonorous, and good conductors of heat and electricity.
Gold and silver are highly malleable. Copper and silver are excellent conductors of heat.
Final Answer: Metals show metallic lustre, malleability, ductility, sonority, and conductivity.
Q5. What Is Malleability?
Malleability is the property of metals to be beaten into thin sheets. Gold and silver are among the most malleable metals.
This property helps metals form sheets, foils, and plates. Aluminium foil is a common example.
Final Answer: Malleability helps metals form thin sheets.
Q6. What Is Ductility?
Ductility is the property of metals to be drawn into thin wires. Gold is one of the most ductile metals.
Copper and aluminium are used in wires because they are ductile and conductive.
Final Answer: Ductility helps metals form wires.
Q7. Why Are School Bells Made Of Metals?
School bells are made of metals because metals are sonorous. Sonorous materials produce sound when struck.
A metal bell vibrates and gives a clear ringing sound.
Final Answer: Metals are sonorous, so they are used in bells.
Q8. What Are The Main Physical Properties Of Non-metals?
Non-metals are generally dull, brittle, non-malleable, non-ductile, and poor conductors. They may be solids or gases.
Bromine is the only liquid non-metal. Graphite is a non-metal that conducts electricity.
Final Answer: Non-metals usually lack metallic properties.
Q9. Give Four Important Exceptions In Metals And Non-metals.
Four important exceptions are mercury, iodine, graphite, and alkali metals. These exceptions prevent classification by physical properties alone.
- Mercury is a liquid metal.
- Iodine is a lustrous non-metal.
- Graphite conducts electricity.
- Sodium and potassium are soft metals.
Final Answer: Chemical properties classify elements more clearly.
Class 10 Science Chapter 3 Questions And Answers On Chemical Properties
Class 10 Science Chapter 3 questions and answers often test reactions with oxygen, water, acids, and salt solutions. Balanced equations are important in this section.
Q10. How Do Metals React With Oxygen?
Metals react with oxygen to form metal oxides. Most metal oxides are basic in nature.
General reaction:
Metal + Oxygen → Metal oxide
Example:
2Cu + O₂ → 2CuO
Copper forms black copper(II) oxide on heating.
Final Answer: Metals generally form basic oxides with oxygen.
Q11. What Are Amphoteric Oxides?
Amphoteric oxides react with both acids and bases to form salt and water. Aluminium oxide and zinc oxide are common examples.
Example:
Al₂O₃ + 6HCl → 2AlCl₃ + 3H₂O
Al₂O₃ + 2NaOH → 2NaAlO₂ + H₂O
Final Answer: Al₂O₃ and ZnO are amphoteric oxides.
Q12. How Do Non-metals React With Oxygen?
Non-metals react with oxygen to form acidic or neutral oxides. Sulphur forms sulphur dioxide on burning.
Reaction:
S + O₂ → SO₂
SO₂ dissolves in water to form sulphurous acid.
Final Answer: Non-metals usually form acidic or neutral oxides.
Q13. Compare Chemical Properties Of Metals And Non-metals.
Metals and non-metals differ mainly in oxide formation, ion formation, and acid reactions. These differences help identify them in experiments.
| Basis |
Metals |
Non-metals |
| Ions formed |
Positive ions |
Negative ions |
| Oxides |
Mostly basic |
Acidic or neutral |
| Reaction with dilute acids |
Many release hydrogen |
Usually do not release hydrogen |
Final Answer: Metals lose electrons, while non-metals gain electrons.
Q14. How Do Metals React With Water?
Metals react with water to form metal oxides or metal hydroxides and hydrogen gas. Reactivity differs from metal to metal.
Potassium and sodium react violently with cold water:
2Na + 2H₂O → 2NaOH + H₂ + heat
Iron reacts only with steam:
3Fe + 4H₂O → Fe₃O₄ + 4H₂
Final Answer: Reactive metals form hydroxides and hydrogen with water.
Q15. Why Is Sodium Kept Immersed In Kerosene Oil?
Sodium is kept in kerosene because it reacts violently with air and water. Kerosene prevents contact with moisture and oxygen.
If sodium contacts water, hydrogen gas evolves and may catch fire.
Final Answer: Kerosene prevents accidental sodium reactions.
Q16. How Do Metals React With Dilute Acids?
Reactive metals react with dilute acids to form salt and hydrogen gas. The reaction rate depends on metal reactivity.
General reaction:
Metal + Dilute acid → Salt + Hydrogen
Example:
Fe + H₂SO₄ → FeSO₄ + H₂
Final Answer: Metals above hydrogen displace hydrogen from dilute acids.
Q17. Why Does Copper Not React With Dilute HCl?
Copper does not react with dilute HCl because it is below hydrogen in the reactivity series. It cannot displace hydrogen from acid.
No bubbles appear when copper is added to dilute hydrochloric acid.
Final Answer: Copper is less reactive than hydrogen.
Reactivity Series Class 10 Important Questions
Reactivity series class 10 questions decide displacement reactions and extraction methods. Students should remember the order from potassium to gold.
Q18. What Is Reactivity Series?
Reactivity series is the arrangement of metals in decreasing order of reactivity. Potassium is near the top, and gold is near the bottom.
Order:
K > Na > Ca > Mg > Al > Zn > Fe > Pb > H > Cu > Hg > Ag > Au
Final Answer: Reactivity decreases from potassium to gold.
Q19. What Is Displacement Reaction Class 10?
A displacement reaction occurs when a more reactive metal displaces a less reactive metal from its salt solution.
General reaction:
Metal A + Salt of Metal B → Salt of Metal A + Metal B
Example:
Fe + CuSO₄ → FeSO₄ + Cu
Final Answer: Iron displaces copper from copper sulphate solution.
Q20. What Happens When Zinc Is Added To Iron(II) Sulphate Solution?
Zinc displaces iron from iron(II) sulphate solution because zinc is more reactive than iron. Zinc forms zinc sulphate.
Reaction:
Zn + FeSO₄ → ZnSO₄ + Fe
The solution changes because iron metal forms.
Final Answer: Zinc displaces iron from FeSO₄ solution.
Q21. Why Can Copper Displace Silver From Silver Nitrate Solution?
Copper displaces silver because copper is more reactive than silver. Copper atoms lose electrons and form copper ions.
Reaction:
Cu + 2AgNO₃ → Cu(NO₃)₂ + 2Ag
Silver deposits as a grey solid.
Final Answer: Copper is above silver in the reactivity series.
Ionic Compounds Class 10 Questions With Answers
Ionic compounds class 10 questions connect electron transfer with properties. Metals form cations, and non-metals form anions.
Q22. How Is Sodium Chloride Formed?
Sodium chloride forms by transfer of one electron from sodium to chlorine. Sodium becomes Na⁺, and chlorine becomes Cl⁻.
Electron transfer:
Na → Na⁺ + e⁻
Cl + e⁻ → Cl⁻
Oppositely charged ions attract strongly.
Final Answer: NaCl is an ionic compound.
Q23. How Is Magnesium Chloride Formed?
Magnesium chloride forms when magnesium transfers two electrons to two chlorine atoms. Magnesium becomes Mg²⁺.
Electron transfer:
Mg → Mg²⁺ + 2e⁻
2Cl + 2e⁻ → 2Cl⁻
Formula formed: MgCl₂
Final Answer: MgCl₂ contains Mg²⁺ and Cl⁻ ions.
Q24. Why Do Ionic Compounds Have High Melting Points?
Ionic compounds have high melting points because strong electrostatic forces hold their ions together. A large amount of energy breaks these forces.
NaCl, CaO, and MgCl₂ are examples of high-melting ionic compounds.
Final Answer: Strong inter-ionic attraction causes high melting points.
Q25. Why Do Ionic Compounds Conduct Electricity In Molten State?
Ionic compounds conduct electricity in molten state because ions become free to move. Solid ionic compounds do not conduct due to fixed ions.
In aqueous solution, ions also move towards opposite electrodes.
Final Answer: Mobile ions conduct electricity.
Extraction Of Metals Class 10 Important Questions
Extraction of metals class 10 questions depend on the metal’s position in the reactivity series. Highly reactive metals need electrolysis.
Q26. What Are Minerals, Ores And Gangue?
Minerals are naturally occurring compounds or elements in the earth’s crust. Ores are minerals from which metals can be profitably extracted.
Gangue means impurities such as soil and sand present in ore.
Final Answer: Ore contains enough metal for profitable extraction.
Q27. How Are Metals Extracted Based On Reactivity?
Metals are extracted by different methods based on their reactivity. Highly reactive metals need electrolytic reduction.
| Metal Position |
Examples |
Extraction Method |
| High reactivity |
K, Na, Ca, Mg, Al |
Electrolysis |
| Medium reactivity |
Zn, Fe, Pb |
Reduction using carbon |
| Low reactivity |
Cu, Ag, Au |
Heating or native state |
Final Answer: Extraction method depends on reactivity.
Q28. What Is Roasting?
Roasting is heating sulphide ore strongly in excess air to form metal oxide. It prepares the ore for reduction.
Example:
2ZnS + 3O₂ → 2ZnO + 2SO₂
Final Answer: Roasting converts sulphide ore into oxide.
Q29. What Is Calcination?
Calcination is heating carbonate ore strongly in limited air to form metal oxide. It removes carbon dioxide from the ore.
Example:
ZnCO₃ → ZnO + CO₂
Final Answer: Calcination converts carbonate ore into oxide.
Q30. What Is Electrolytic Refining Of Copper?
Electrolytic refining purifies impure copper using electricity. Impure copper acts as anode, and pure copper acts as cathode.
Acidified copper sulphate solution acts as electrolyte. Pure copper deposits on the cathode.
Final Answer: Insoluble impurities settle as anode mud.
Corrosion Class 10 Important Questions
Corrosion class 10 questions focus on rusting, prevention, and daily-life examples. Iron rusts only when both air and moisture are present.
Q31. What Is Corrosion?
Corrosion is the slow damage of a metal surface by air, moisture, or chemicals. Rusting of iron is a common example.
Iron forms a brown flaky coating called rust when exposed to moist air.
Final Answer: Corrosion damages metals through chemical reactions.
Q32. What Conditions Are Necessary For Rusting Of Iron?
Both air and water are necessary for rusting of iron. Iron does not rust in dry air or air-free water.
In NCERT activity, iron nails rust only when exposed to both air and water.
Final Answer: Rusting needs oxygen and moisture.
Q33. How Can Rusting Of Iron Be Prevented?
Rusting can be prevented by painting, oiling, greasing, galvanising, chrome plating, anodising, or making alloys.
Galvanisation protects iron by coating it with zinc.
Final Answer: Zinc coating prevents contact with air and moisture.
Q34. What Is An Alloy?
An alloy is a homogeneous mixture of two or more metals or a metal and a non-metal. Alloying improves metal properties.
Examples include brass, bronze, solder, and stainless steel.
Final Answer: Stainless steel is an alloy of iron with chromium and nickel.
Q35. Why Is Aluminium Used For Cooking Utensils Despite Being Reactive?
Aluminium is used because it forms a protective oxide layer. This layer prevents further reaction and corrosion.
Aluminium also conducts heat well, which makes it suitable for utensils.
Final Answer: Aluminium oxide protects the metal surface.
Metals And Non-metals Important Questions From NCERT Exercises
Metals and non-metals important questions often come from NCERT exercise patterns. These answers need exact reasoning and balanced equations.
Q36. Why Are Platinum, Gold And Silver Used To Make Jewellery?
Platinum, gold, and silver are used in jewellery because they are lustrous and less reactive. They do not corrode easily.
Gold and silver are also highly malleable, so they can be shaped into ornaments.
Final Answer: They are shiny, less reactive, and malleable.
Q37. Why Are Food Cans Coated With Tin And Not Zinc?
Food cans are coated with tin because tin is less reactive than zinc. Zinc may react with food acids and contaminate food.
Tin protects iron from corrosion without reacting easily with food.
Final Answer: Zinc is more reactive than tin.
Q38. Why Are Carbonate And Sulphide Ores Converted Into Oxides?
Carbonate and sulphide ores are converted into oxides because metal oxides are easier to reduce. Reduction gives the pure metal.
Sulphide ores undergo roasting. Carbonate ores undergo calcination.
Final Answer: Oxide ores are easier to reduce.
Q39. Why Is Lemon Juice Used To Clean Tarnished Copper Vessels?
Lemon juice cleans copper vessels because it contains acid. The acid reacts with the green basic copper carbonate layer.
The layer dissolves, and the copper surface becomes shiny again.
Final Answer: Acid removes basic copper carbonate.
Q40. Which Solution Did The Fake Goldsmith Use To Dissolve Gold?
The fake goldsmith used aqua regia. Aqua regia dissolves gold, though hydrochloric acid and nitric acid alone cannot.
Aqua regia is a 3:1 mixture of concentrated HCl and concentrated HNO₃.
Final Answer: The solution was aqua regia.
CBSE Class 10 Science All Chapters at a Glance