CBSE Class 10 · Chemistry
CBSE Class 10 Chemistry Metals and Non-metals Previous Year Questions
Help your child master CBSE Class 10 Chemistry Metals and Non-metals previous year questions with this expertly curated collection sourced from real board papers spanning 2021–2025. Every question — from 1-mark MCQs on reactivity series and alloys to 5-mark answers on electrolytic refining and metal extraction — comes with a detailed step-by-step solution so your child walks into the board exam fully prepared.
CBSE Class 10 Chemistry Metals and Non-metals — Questions with Solutions
The products formed when Aluminium and Magnesium are burnt in the presence of air respectively are?
Solution
Answer: Option (B) is correct.
When Aluminium (Al) is burnt in air, it reacts with oxygen to form Aluminium oxide (Al₂O₃): $$4Al + 3O_2 \rightarrow 2Al_2O_3$$ When Magnesium (Mg) is burnt in air, it reacts with oxygen to form Magnesium oxide (MgO): $$2Mg + O_2 \rightarrow 2MgO$$
When Aluminium (Al) is burnt in air, it reacts with oxygen to form Aluminium oxide (Al₂O₃): $$4Al + 3O_2 \rightarrow 2Al_2O_3$$ When Magnesium (Mg) is burnt in air, it reacts with oxygen to form Magnesium oxide (MgO): $$2Mg + O_2 \rightarrow 2MgO$$
The metals obtained from their molten chlorides by the process of electrolytic reduction are?
Solution
Answer: Option (B) is correct.
Highly reactive metals like calcium and magnesium cannot be obtained using common chemical reducing agents. They are extracted by electrolytic reduction of their molten chlorides:
• CaCl₂ → electrolysis → Calcium (Ca)
• MgCl₂ → electrolysis → Magnesium (Mg)
Highly reactive metals like calcium and magnesium cannot be obtained using common chemical reducing agents. They are extracted by electrolytic reduction of their molten chlorides:
• CaCl₂ → electrolysis → Calcium (Ca)
• MgCl₂ → electrolysis → Magnesium (Mg)
The formation of magnesium oxide is correctly shown in which option?
- ✓(A)
- ✗(B)
- ✗(C)
- ✗(D)
Solution
Answer: Option (A) is correct.
Magnesium (Mg) has 2 electrons in its outermost shell and loses 2 electrons to form Mg²⁺: $$\text{Mg} \rightarrow \text{Mg}^{2+} + 2e^-$$ Oxygen (O) has 6 electrons in its outermost shell and gains 2 electrons to form O²⁻: $$\text{O} + 2e^- \rightarrow \text{O}^{2-}$$ The oppositely charged ions attract each other to form the ionic bond in magnesium oxide (MgO): $$\text{Mg}^{2+} + \text{O}^{2-} \rightarrow \text{MgO}$$
Magnesium (Mg) has 2 electrons in its outermost shell and loses 2 electrons to form Mg²⁺: $$\text{Mg} \rightarrow \text{Mg}^{2+} + 2e^-$$ Oxygen (O) has 6 electrons in its outermost shell and gains 2 electrons to form O²⁻: $$\text{O} + 2e^- \rightarrow \text{O}^{2-}$$ The oppositely charged ions attract each other to form the ionic bond in magnesium oxide (MgO): $$\text{Mg}^{2+} + \text{O}^{2-} \rightarrow \text{MgO}$$
Aluminium powder is used in thermit welding because?
Solution
Answer: Option (B) is correct.
Aluminium powder reacts with iron (III) oxide in a highly exothermic reaction that produces molten iron, which is used to join railway tracks: $$Fe_2O_3 + 2Al \rightarrow 2Fe + Al_2O_3 + \text{Heat}$$
Aluminium powder reacts with iron (III) oxide in a highly exothermic reaction that produces molten iron, which is used to join railway tracks: $$Fe_2O_3 + 2Al \rightarrow 2Fe + Al_2O_3 + \text{Heat}$$
Two metals zinc and tin are dissolved separately in definite proportions in molten copper (the primary metal) to obtain two different alloys respectively known as?
Solution
Answer: Option (C) is correct.
$$\text{Copper (Cu)} + \text{Zinc (Zn)} \rightarrow \text{Brass}$$ $$\text{Copper (Cu)} + \text{Tin (Sn)} \rightarrow \text{Bronze}$$
$$\text{Copper (Cu)} + \text{Zinc (Zn)} \rightarrow \text{Brass}$$ $$\text{Copper (Cu)} + \text{Tin (Sn)} \rightarrow \text{Bronze}$$
Assertion (A): The metals high up in the reactivity series cannot be obtained from their compounds by heating with carbon.
Reason (R): Displacement reactions can also be used to obtain metal.
(A) Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of Assertion (A).
(B) Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A).
(C) Assertion (A) is true, but Reason (R) is false.
(D) Assertion (A) is false, but Reason (R) is true.
Reason (R): Displacement reactions can also be used to obtain metal.
(A) Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of Assertion (A).
(B) Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A).
(C) Assertion (A) is true, but Reason (R) is false.
(D) Assertion (A) is false, but Reason (R) is true.
Solution
Answer: Option (B) is correct.
Assertion (A) is true: Metals high in the reactivity series cannot be extracted by heating with carbon because these metals have a greater affinity for oxygen than carbon does.
Reason (R) is also true: Displacement reactions can be used to obtain metals. However, this is not the correct explanation for why highly reactive metals cannot be reduced by carbon — the two statements are independently true but unrelated in cause.
Assertion (A) is true: Metals high in the reactivity series cannot be extracted by heating with carbon because these metals have a greater affinity for oxygen than carbon does.
Reason (R) is also true: Displacement reactions can be used to obtain metals. However, this is not the correct explanation for why highly reactive metals cannot be reduced by carbon — the two statements are independently true but unrelated in cause.
Assertion (A): Ductility is that property of metals which enables copper to be used in making cooking utensils.
Reason (R): Copper is a metal which is ductile as well as malleable.
(A) Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of Assertion (A).
(B) Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A).
(C) Assertion (A) is true, but Reason (R) is false.
(D) Assertion (A) is false, but Reason (R) is true.
Reason (R): Copper is a metal which is ductile as well as malleable.
(A) Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of Assertion (A).
(B) Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A).
(C) Assertion (A) is true, but Reason (R) is false.
(D) Assertion (A) is false, but Reason (R) is true.
Solution
Answer: Option (D) is correct.
Assertion is false: Ductility (drawing into wires) is not the property that makes copper suitable for cooking utensils — malleability (hammering into sheets) is the relevant property.
Reason is true: Copper is indeed both ductile and malleable.
Assertion is false: Ductility (drawing into wires) is not the property that makes copper suitable for cooking utensils — malleability (hammering into sheets) is the relevant property.
Reason is true: Copper is indeed both ductile and malleable.
The most common method of extraction of metals from their oxide ores is:
Solution
Answer: Option (A) is correct.
The most common method is reduction with carbon (smelting). The metal oxide is heated with carbon, which acts as a reducing agent to remove oxygen and leave behind the pure metal. This is cost-effective and suitable for less reactive metals like iron, zinc, lead, and copper.
The most common method is reduction with carbon (smelting). The metal oxide is heated with carbon, which acts as a reducing agent to remove oxygen and leave behind the pure metal. This is cost-effective and suitable for less reactive metals like iron, zinc, lead, and copper.
Assertion (A): Hydrogen gas is not evolved when a metal reacts with nitric acid.
Reason (R): Nitric acid is a strong reducing agent and reduces the hydrogen produced in the reaction to water.
(A) Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of Assertion (A).
(B) Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A).
(C) Assertion (A) is true, but Reason (R) is false.
(D) Assertion (A) is false, but Reason (R) is true.
Reason (R): Nitric acid is a strong reducing agent and reduces the hydrogen produced in the reaction to water.
(A) Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of Assertion (A).
(B) Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A).
(C) Assertion (A) is true, but Reason (R) is false.
(D) Assertion (A) is false, but Reason (R) is true.
Solution
Answer: Option (C) is correct.
Assertion (A) is true: Hydrogen gas is not evolved when a metal reacts with nitric acid. The reaction instead forms metal nitrate, oxides of nitrogen, and water.
Reason (R) is false: Nitric acid is a strong oxidising agent, not a reducing agent. This is why no hydrogen is produced.
Assertion (A) is true: Hydrogen gas is not evolved when a metal reacts with nitric acid. The reaction instead forms metal nitrate, oxides of nitrogen, and water.
Reason (R) is false: Nitric acid is a strong oxidising agent, not a reducing agent. This is why no hydrogen is produced.
Assertion (A): Brass is prepared by first melting copper and then dissolving tin into it in a definite proportion.
Reason (R): The primary metal of brass is copper.
(A) Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of Assertion (A).
(B) Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A).
(C) Assertion (A) is true, but Reason (R) is false.
(D) Assertion (A) is false, but Reason (R) is true.
Reason (R): The primary metal of brass is copper.
(A) Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of Assertion (A).
(B) Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A).
(C) Assertion (A) is true, but Reason (R) is false.
(D) Assertion (A) is false, but Reason (R) is true.
Solution
Answer: Option (D) is correct.
Assertion (A) is false: Brass is made by mixing copper and zinc, not tin. Copper + Tin = Bronze.
Reason (R) is true: Copper is indeed the primary metal component of brass.
Assertion (A) is false: Brass is made by mixing copper and zinc, not tin. Copper + Tin = Bronze.
Reason (R) is true: Copper is indeed the primary metal component of brass.
Given below are reactions involving metals P, Q, R and S and their salt solutions in water.
Metal P salt solution + Q → Metal Q salt solution + P
Metal Q salt solution + R → Metal R salt solution + Q
Metal S salt solution + Q → Metal Q salt solution + S
Metal P salt solution + S → No reaction
Which metal is the MOST reactive?
Metal P salt solution + Q → Metal Q salt solution + P
Metal Q salt solution + R → Metal R salt solution + Q
Metal S salt solution + Q → Metal Q salt solution + S
Metal P salt solution + S → No reaction
Which metal is the MOST reactive?
Solution
Answer: Option (C) is correct.
A more reactive metal displaces a less reactive metal from its salt solution.
From Reaction 1: Q displaces P → $Q > P$
From Reaction 2: R displaces Q → $R > Q > P$
From Reaction 3: Q displaces S → $Q > S$
From Reaction 4: P does NOT displace S → $S > P$
Final order: $R > Q > S > P$
Metal R is the MOST reactive.
A more reactive metal displaces a less reactive metal from its salt solution.
From Reaction 1: Q displaces P → $Q > P$
From Reaction 2: R displaces Q → $R > Q > P$
From Reaction 3: Q displaces S → $Q > S$
From Reaction 4: P does NOT displace S → $S > P$
Final order: $R > Q > S > P$
Metal R is the MOST reactive.
(i) What is an alloy?
(ii) Write the composition of solder and the property which makes it suitable for welding electric wires?
(ii) Write the composition of solder and the property which makes it suitable for welding electric wires?
Answer
(i) Alloy:
An alloy is a mixture of two or more metals, or a metal and a non-metal, combined in definite proportions to achieve specific properties different from those of the individual elements — such as improved strength, hardness, or corrosion resistance.
Examples: Bronze = copper + tin. Steel = iron + carbon.
(ii) Composition of Solder:
Solder is an alloy of tin (Sn) and lead (Pb), most commonly 60% tin and 40% lead.
Suitable property: Solder has a low melting point (~183°C), allowing it to melt easily, flow into wire joints, and solidify quickly to form a strong, conductive bond without damaging surrounding components.
An alloy is a mixture of two or more metals, or a metal and a non-metal, combined in definite proportions to achieve specific properties different from those of the individual elements — such as improved strength, hardness, or corrosion resistance.
Examples: Bronze = copper + tin. Steel = iron + carbon.
(ii) Composition of Solder:
Solder is an alloy of tin (Sn) and lead (Pb), most commonly 60% tin and 40% lead.
Suitable property: Solder has a low melting point (~183°C), allowing it to melt easily, flow into wire joints, and solidify quickly to form a strong, conductive bond without damaging surrounding components.
During electrolytic refining of silver:
(i) What are the electrodes – cathode and anode made up of?
(ii) What is anode mud? Why is it called so?
(i) What are the electrodes – cathode and anode made up of?
(ii) What is anode mud? Why is it called so?
Answer
(i) Electrodes in electrolytic refining of silver:
• Anode: Made of impure silver (containing impurities like gold, copper, etc.).
• Cathode: Made of a thin sheet of pure silver, where refined silver is deposited.
(ii) Anode mud:
Anode mud refers to the insoluble impurities that collect at the bottom of the electrolytic cell below the anode. As the impure silver anode dissolves, insoluble impurities (gold, sand, etc.) do not dissolve into the electrolyte — they fall and settle as a muddy deposit beneath the anode, hence the name “anode mud.”
• Anode: Made of impure silver (containing impurities like gold, copper, etc.).
• Cathode: Made of a thin sheet of pure silver, where refined silver is deposited.
(ii) Anode mud:
Anode mud refers to the insoluble impurities that collect at the bottom of the electrolytic cell below the anode. As the impure silver anode dissolves, insoluble impurities (gold, sand, etc.) do not dissolve into the electrolyte — they fall and settle as a muddy deposit beneath the anode, hence the name “anode mud.”
Consider the reactions of dil. hydrochloric acid with the following metals: Aluminium, Copper, Iron, Magnesium and Zinc. The correct observation is:
Solution
Answer: Option (C) is correct.
Reactivity order (descending): Magnesium > Aluminium > Zinc > Iron > Copper
• Magnesium reacts most vigorously with dilute HCl, rapidly producing hydrogen gas: $$Mg + 2HCl \rightarrow MgCl_2 + H_2$$ • Copper does not react with dilute HCl — it is less reactive than hydrogen and cannot displace it.
Reactivity order (descending): Magnesium > Aluminium > Zinc > Iron > Copper
• Magnesium reacts most vigorously with dilute HCl, rapidly producing hydrogen gas: $$Mg + 2HCl \rightarrow MgCl_2 + H_2$$ • Copper does not react with dilute HCl — it is less reactive than hydrogen and cannot displace it.
The most malleable metals are:
Solution
Answer: Option (D) is correct.
Malleability is the property by which a metal can be hammered or rolled into thin sheets without breaking.
• Gold is the most malleable metal known — it can be beaten into extremely thin sheets (gold leaf).
• Copper is also highly malleable and widely used in making sheets and wires.
Malleability is the property by which a metal can be hammered or rolled into thin sheets without breaking.
• Gold is the most malleable metal known — it can be beaten into extremely thin sheets (gold leaf).
• Copper is also highly malleable and widely used in making sheets and wires.
Oxides of aluminium and zinc are:
Solution
Answer: Option (B) is correct.
Aluminium oxide (Al₂O₃) and zinc oxide (ZnO) are amphoteric — they react with both acids and bases to form salts and water, exhibiting properties of both acidic and basic oxides.
Aluminium oxide (Al₂O₃) and zinc oxide (ZnO) are amphoteric — they react with both acids and bases to form salts and water, exhibiting properties of both acidic and basic oxides.
The metals produced by various reduction processes are not very pure. They contain impurities which must be removed to obtain pure metals. The most widely used process for refining impure metals is electrolytic refining. In this process, the chemical effect of electric current is used.
(a) Name the materials used to make anode and cathode in the refining of copper by this process?
(b) Name the salt of copper used as an electrolyte in this process and write its molecular formula?
(c)(i) What happens when a steady current is passed through the electrolyte? Name the part of the electrolytic cell where (1) pure copper is obtained and (2) impurities settle.
OR
(c)(ii) How is copper obtained from its sulphide? Write chemical equations involved in the process?
(a) Name the materials used to make anode and cathode in the refining of copper by this process?
(b) Name the salt of copper used as an electrolyte in this process and write its molecular formula?
(c)(i) What happens when a steady current is passed through the electrolyte? Name the part of the electrolytic cell where (1) pure copper is obtained and (2) impurities settle.
OR
(c)(ii) How is copper obtained from its sulphide? Write chemical equations involved in the process?
Answer
(a) Electrodes:
• Anode: Impure copper (Cu)
• Cathode: Pure copper (Cu)
(b) Electrolyte:
Copper(II) sulphate — CuSO₄
(c)(i) When steady current is passed:
The impure copper anode dissolves into the electrolyte as Cu²⁺ ions; simultaneously, Cu²⁺ ions from the electrolyte deposit as pure copper at the cathode.
1. Pure copper is obtained at the cathode.
2. Impurities settle below the anode as anode mud.
OR — (c)(ii) Extraction of Copper from its Sulphide Ore:
Step 1 — Roasting: $$2Cu_2S(s) + 3O_2(g) \xrightarrow{\text{Heat}} 4CuO(s) + 2SO_2(g)$$ Step 2 — Reduction: $$CuO(s) + C(s) \xrightarrow{\text{Heat}} Cu(s) + CO(g)$$
• Anode: Impure copper (Cu)
• Cathode: Pure copper (Cu)
(b) Electrolyte:
Copper(II) sulphate — CuSO₄
(c)(i) When steady current is passed:
The impure copper anode dissolves into the electrolyte as Cu²⁺ ions; simultaneously, Cu²⁺ ions from the electrolyte deposit as pure copper at the cathode.
1. Pure copper is obtained at the cathode.
2. Impurities settle below the anode as anode mud.
OR — (c)(ii) Extraction of Copper from its Sulphide Ore:
Step 1 — Roasting: $$2Cu_2S(s) + 3O_2(g) \xrightarrow{\text{Heat}} 4CuO(s) + 2SO_2(g)$$ Step 2 — Reduction: $$CuO(s) + C(s) \xrightarrow{\text{Heat}} Cu(s) + CO(g)$$
With the help of an activity, explain the conditions under which iron articles get rusted?
Answer
Rusting of iron occurs when iron reacts with both oxygen and moisture to form iron(III) oxide (rust). Both conditions are necessary.
Activity: Take three test tubes with clean iron nails labelled A, B, and C:
• Test Tube A: Pour water and cork — nails exposed to both air and water.
• Test Tube B: Pour boiled distilled water, float oil on top (blocks air), and cork — nails exposed to water only.
• Test Tube C: Place anhydrous calcium chloride inside and cork — nails exposed to dry air only.
Observations:
• Nails rust in Test Tube A — both air and water present.
• No rusting in Test Tube B — only water, no air.
• No rusting in Test Tube C — only dry air, no water.
Conclusion: Both moisture and oxygen are necessary conditions for iron to rust.
Activity: Take three test tubes with clean iron nails labelled A, B, and C:
• Test Tube A: Pour water and cork — nails exposed to both air and water.
• Test Tube B: Pour boiled distilled water, float oil on top (blocks air), and cork — nails exposed to water only.
• Test Tube C: Place anhydrous calcium chloride inside and cork — nails exposed to dry air only.
Observations:
• Nails rust in Test Tube A — both air and water present.
• No rusting in Test Tube B — only water, no air.
• No rusting in Test Tube C — only dry air, no water.
Conclusion: Both moisture and oxygen are necessary conditions for iron to rust.
(i) Name two metals which react violently with cold water?
(ii) Write a test to identify the gas evolved (if any) during the reaction of these metals with water?
(ii) Write a test to identify the gas evolved (if any) during the reaction of these metals with water?
Answer
(i) Two metals that react violently with cold water:
• Sodium (Na)
• Potassium (K)
(ii) Test for the gas evolved:
The gas evolved is hydrogen (H₂).
Test: Bring a burning splint near the mouth of the test tube. If hydrogen is present, it burns with a characteristic “pop” sound.
• Sodium (Na)
• Potassium (K)
(ii) Test for the gas evolved:
The gas evolved is hydrogen (H₂).
Test: Bring a burning splint near the mouth of the test tube. If hydrogen is present, it burns with a characteristic “pop” sound.
(a) “Displacement reactions also play a key role in extracting metals in the middle of the reactivity series.” Justify this statement with two examples.
(b) Why can metals high up in the reactivity series not be obtained by reduction of their oxides by carbon?
(b) Why can metals high up in the reactivity series not be obtained by reduction of their oxides by carbon?
Answer
(a) Two examples of displacement reactions in metal extraction:
Example 1 — Extraction of Zinc: $$ZnO + C \rightarrow Zn + CO_2$$ Carbon, being more reactive than zinc, displaces zinc from zinc oxide.
Example 2 — Extraction of Iron: $$Fe_2O_3 + 3C \rightarrow 2Fe + 3CO$$ Carbon displaces iron from iron ore (Fe₂O₃).
(b) Why highly reactive metals cannot be reduced by carbon:
Metals high in the reactivity series (Al, Ca, Na, etc.) are more reactive than carbon, so carbon cannot displace them from their oxides. Instead, these metals must be extracted by electrolysis.
Example 1 — Extraction of Zinc: $$ZnO + C \rightarrow Zn + CO_2$$ Carbon, being more reactive than zinc, displaces zinc from zinc oxide.
Example 2 — Extraction of Iron: $$Fe_2O_3 + 3C \rightarrow 2Fe + 3CO$$ Carbon displaces iron from iron ore (Fe₂O₃).
(b) Why highly reactive metals cannot be reduced by carbon:
Metals high in the reactivity series (Al, Ca, Na, etc.) are more reactive than carbon, so carbon cannot displace them from their oxides. Instead, these metals must be extracted by electrolysis.
A few pieces of granulated zinc are taken in a test tube and 2 mL of sodium hydroxide solution is added to it. When the contents are warmed, the product formed is:
Solution
Answer: Option (C) is correct.
The product formed is sodium zincate (Na₂ZnO₂) along with hydrogen gas: $$\text{Zn} + 2\text{NaOH} \xrightarrow{\text{warm}} \text{Na}_2\text{ZnO}_2 + \text{H}_2 \uparrow$$
The product formed is sodium zincate (Na₂ZnO₂) along with hydrogen gas: $$\text{Zn} + 2\text{NaOH} \xrightarrow{\text{warm}} \text{Na}_2\text{ZnO}_2 + \text{H}_2 \uparrow$$
(a) What is a reactivity series of elements? How is it developed? Arrange the following elements as they are arranged in the reactivity series: Aluminium, Calcium, Copper, Lead.
(b) Write the balanced chemical equation to show the reaction of iron (III) oxide ($\text{Fe}_2\text{O}_3$) with aluminium.
(b) Write the balanced chemical equation to show the reaction of iron (III) oxide ($\text{Fe}_2\text{O}_3$) with aluminium.
Answer
(a) Reactivity Series:
The reactivity series is a list of metals arranged in decreasing order of their reactivity. It is developed by comparing the reactions of metals with water, dilute acids, and through displacement reactions.
Order of given elements (most to least reactive):
Calcium > Aluminium > Lead > Copper
(b) Reaction of Fe₂O₃ with Aluminium (Thermite Reaction): $$\text{Fe}_2\text{O}_3 + 2\text{Al} \rightarrow 2\text{Fe} + \text{Al}_2\text{O}_3$$ Aluminium, being more reactive than iron, displaces iron from its oxide in this highly exothermic reaction.
The reactivity series is a list of metals arranged in decreasing order of their reactivity. It is developed by comparing the reactions of metals with water, dilute acids, and through displacement reactions.
Order of given elements (most to least reactive):
Calcium > Aluminium > Lead > Copper
(b) Reaction of Fe₂O₃ with Aluminium (Thermite Reaction): $$\text{Fe}_2\text{O}_3 + 2\text{Al} \rightarrow 2\text{Fe} + \text{Al}_2\text{O}_3$$ Aluminium, being more reactive than iron, displaces iron from its oxide in this highly exothermic reaction.
Show the formation of magnesium chloride by electron transfer. Write the name of the cation and anion present in the compound formed. (Atomic Number of Mg = 12, Cl = 17)
Answer
Electron Configuration:
• Mg (Z = 12): 2, 8, 2 — loses 2 electrons to achieve stability: $$\text{Mg} \rightarrow \text{Mg}^{2+} + 2e^-$$ • Cl (Z = 17): 2, 8, 7 — gains 1 electron to complete its octet: $$\text{Cl} + e^- \rightarrow \text{Cl}^-$$ Formation of MgCl₂: $$\text{Mg}^{2+} + 2\text{Cl}^- \rightarrow \text{MgCl}_2$$
Cation present: Magnesium ion (Mg²⁺)
Anion present: Chloride ion (Cl⁻)
• Mg (Z = 12): 2, 8, 2 — loses 2 electrons to achieve stability: $$\text{Mg} \rightarrow \text{Mg}^{2+} + 2e^-$$ • Cl (Z = 17): 2, 8, 7 — gains 1 electron to complete its octet: $$\text{Cl} + e^- \rightarrow \text{Cl}^-$$ Formation of MgCl₂: $$\text{Mg}^{2+} + 2\text{Cl}^- \rightarrow \text{MgCl}_2$$
Cation present: Magnesium ion (Mg²⁺)
Anion present: Chloride ion (Cl⁻)
How is zinc extracted from its ore? Name the processes involved in the extraction and write chemical equations for the reactions that occur during these processes.
Answer
Zinc occurs as sulphide (ZnS) or carbonate (ZnCO₃) ores. These are first converted to ZnO, then reduced.
Process 1 — Roasting (for sulphide ores): $$2\text{ZnS}(s) + 3\text{O}_2(g) \xrightarrow{\text{Heat}} 2\text{ZnO}(s) + 2\text{SO}_2(g)$$ Process 2 — Calcination (for carbonate ores): $$\text{ZnCO}_3(s) \xrightarrow{\text{Heat}} \text{ZnO}(s) + \text{CO}_2(g)$$ Process 3 — Reduction of Zinc Oxide with Carbon: $$\text{ZnO}(s) + \text{C}(s) \xrightarrow{\text{Heat}} \text{Zn}(s) + \text{CO}(g)$$
Process 1 — Roasting (for sulphide ores): $$2\text{ZnS}(s) + 3\text{O}_2(g) \xrightarrow{\text{Heat}} 2\text{ZnO}(s) + 2\text{SO}_2(g)$$ Process 2 — Calcination (for carbonate ores): $$\text{ZnCO}_3(s) \xrightarrow{\text{Heat}} \text{ZnO}(s) + \text{CO}_2(g)$$ Process 3 — Reduction of Zinc Oxide with Carbon: $$\text{ZnO}(s) + \text{C}(s) \xrightarrow{\text{Heat}} \text{Zn}(s) + \text{CO}(g)$$
Name a metal found in the earth’s crust:
(i) In free state
(ii) In the form of its compound
State where each of these metals are placed in the reactivity series of metals?
(i) In free state
(ii) In the form of its compound
State where each of these metals are placed in the reactivity series of metals?
Answer
(i) Metal found in free state: Gold (Au)
Gold is found in its native (uncombined) state in nature because it is one of the least reactive metals.
(ii) Metal found in the form of its compound: Iron (Fe)
Iron is found as compounds such as Fe₂O₃ and Fe₃O₄ in nature, requiring reduction to extract the pure metal.
Position in the reactivity series:
• Gold (Au) — placed at the bottom (least reactive).
• Iron (Fe) — placed in the middle (moderately reactive).
Gold is found in its native (uncombined) state in nature because it is one of the least reactive metals.
(ii) Metal found in the form of its compound: Iron (Fe)
Iron is found as compounds such as Fe₂O₃ and Fe₃O₄ in nature, requiring reduction to extract the pure metal.
Position in the reactivity series:
• Gold (Au) — placed at the bottom (least reactive).
• Iron (Fe) — placed in the middle (moderately reactive).
(a) Sodium metal is stored under kerosene oil. Why?
(b) Some metal oxides are soluble in water. What are the aqueous solutions of these oxides called? Write one example of such a solution.
(c) At ordinary temperature, the surface of metals such as magnesium, aluminium, zinc etc. is covered with a thin layer. What is the composition of this layer? State its importance.
(b) Some metal oxides are soluble in water. What are the aqueous solutions of these oxides called? Write one example of such a solution.
(c) At ordinary temperature, the surface of metals such as magnesium, aluminium, zinc etc. is covered with a thin layer. What is the composition of this layer? State its importance.
Answer
(a) Sodium stored under kerosene oil:
Sodium is highly reactive and reacts vigorously with both water and oxygen in air. Kerosene oil creates a protective barrier, preventing sodium from coming in contact with moisture and oxygen — making storage safe.
(b) Aqueous solutions of metal oxides:
These are called alkaline (basic) solutions. When metal oxides dissolve in water, they form hydroxides.
Example: $$\text{MgO} + \text{H}_2\text{O} \rightarrow \text{Mg(OH)}_2$$
(c) Composition and importance of the thin layer:
The thin layer is composed of metal oxides (MgO on magnesium, Al₂O₃ on aluminium, ZnO on zinc).
Importance: This oxide layer acts as a protective barrier preventing further oxidation and corrosion of the metal underneath, thereby extending its lifespan.
Sodium is highly reactive and reacts vigorously with both water and oxygen in air. Kerosene oil creates a protective barrier, preventing sodium from coming in contact with moisture and oxygen — making storage safe.
(b) Aqueous solutions of metal oxides:
These are called alkaline (basic) solutions. When metal oxides dissolve in water, they form hydroxides.
Example: $$\text{MgO} + \text{H}_2\text{O} \rightarrow \text{Mg(OH)}_2$$
(c) Composition and importance of the thin layer:
The thin layer is composed of metal oxides (MgO on magnesium, Al₂O₃ on aluminium, ZnO on zinc).
Importance: This oxide layer acts as a protective barrier preventing further oxidation and corrosion of the metal underneath, thereby extending its lifespan.
Cinnabar is an ore of a metal ‘X’. When this ore is heated in air, it is first converted into oxide of ‘X’ (XO) and then reduced to metal ‘X’ on further heating. Identify metal ‘X’ and write chemical equations for the reactions that occur in the above processes.
Answer
The metal ‘X’ is Mercury (Hg). Cinnabar is mercury sulphide (HgS).
Reaction 1 — Heating HgS in air forms mercury oxide: $$\text{HgS}(s) + \text{O}_2(g) \xrightarrow{\text{Heat}} \text{HgO}(s) + \text{SO}_2(g)$$ Reaction 2 — Further heating reduces HgO to mercury: $$\text{HgO}(s) \xrightarrow{\text{Heat}} \text{Hg}(l) + \text{O}_2(g)$$
Reaction 1 — Heating HgS in air forms mercury oxide: $$\text{HgS}(s) + \text{O}_2(g) \xrightarrow{\text{Heat}} \text{HgO}(s) + \text{SO}_2(g)$$ Reaction 2 — Further heating reduces HgO to mercury: $$\text{HgO}(s) \xrightarrow{\text{Heat}} \text{Hg}(l) + \text{O}_2(g)$$
Observe the following diagram showing an experiment to determine the conditions under which a metal ‘M’ corrodes.
List your observations in each of the three cases A, B, and C with reason if the metal ‘M’ is generally protected against corrosion by the method of galvanization.
List your observations in each of the three cases A, B, and C with reason if the metal ‘M’ is generally protected against corrosion by the method of galvanization.Answer
Observations:
• Test Tube A: Metal corrodes — both air (oxygen) and water are present, which are the two conditions necessary for corrosion.
• Test Tube B: Metal does NOT corrode — only water is present; no air/oxygen.
• Test Tube C: Metal does NOT corrode — only dry air is present; no moisture.
Conclusion: Both water and air (oxygen) are necessary for corrosion.
Galvanization: Yes, galvanization protects metal ‘M’ from corrosion. It involves coating the metal with a thin layer of zinc, which acts as a barrier preventing contact with moisture and oxygen, thereby preventing corrosion.
• Test Tube A: Metal corrodes — both air (oxygen) and water are present, which are the two conditions necessary for corrosion.
• Test Tube B: Metal does NOT corrode — only water is present; no air/oxygen.
• Test Tube C: Metal does NOT corrode — only dry air is present; no moisture.
Conclusion: Both water and air (oxygen) are necessary for corrosion.
Galvanization: Yes, galvanization protects metal ‘M’ from corrosion. It involves coating the metal with a thin layer of zinc, which acts as a barrier preventing contact with moisture and oxygen, thereby preventing corrosion.
Aluminium oxide is an amphoteric oxide. Justify this statement giving chemical equations for the reactions involved?
Answer
Aluminium oxide (Al₂O₃) is an amphoteric oxide because it reacts with both acids and bases.
Reaction with Acid (acts as a base): $$\text{Al}_2\text{O}_3(s) + 6\text{HCl}(aq) \rightarrow 2\text{AlCl}_3(aq) + 3\text{H}_2\text{O}(l)$$
Reaction with Base (acts as an acid): $$2\text{NaOH}(aq) + 2\text{Al}(s) \rightarrow 2\text{NaAlO}_2(aq) + \text{H}_2\uparrow$$ Since Al₂O₃ reacts with both acids and bases forming salts, it is classified as amphoteric.
Reaction with Acid (acts as a base): $$\text{Al}_2\text{O}_3(s) + 6\text{HCl}(aq) \rightarrow 2\text{AlCl}_3(aq) + 3\text{H}_2\text{O}(l)$$
Reaction with Base (acts as an acid): $$2\text{NaOH}(aq) + 2\text{Al}(s) \rightarrow 2\text{NaAlO}_2(aq) + \text{H}_2\uparrow$$ Since Al₂O₃ reacts with both acids and bases forming salts, it is classified as amphoteric.
Design an activity to show that metals are good conductors of heat and have high melting points?
Answer
Activity: Testing Heat Conductivity and High Melting Point of Metals
Materials: Aluminium or copper wire, clamp stand, wax, pin, spirit lamp or candle.
Procedure:
1. Clamp an aluminium or copper wire horizontally on a stand.
2. Fix a pin to the free end of the wire using wax.
3. Heat the wire near the clamped end using a spirit lamp.
4. Observe whether the pin falls and whether the wire itself melts.
Observations:
• Heat travels along the wire and the wax melts — the pin falls at the far end.
• The metal wire does NOT melt even when strongly heated.
Conclusions:
• Metals are good conductors of heat — heat is rapidly transmitted along the wire.
• Metals have high melting points — the wire remains solid under direct heating.
Materials: Aluminium or copper wire, clamp stand, wax, pin, spirit lamp or candle.
Procedure:
1. Clamp an aluminium or copper wire horizontally on a stand.
2. Fix a pin to the free end of the wire using wax.
3. Heat the wire near the clamped end using a spirit lamp.
4. Observe whether the pin falls and whether the wire itself melts.
Observations:
• Heat travels along the wire and the wax melts — the pin falls at the far end.
• The metal wire does NOT melt even when strongly heated.
Conclusions:
• Metals are good conductors of heat — heat is rapidly transmitted along the wire.
• Metals have high melting points — the wire remains solid under direct heating.
Study the experimental set-up given in the figure and answer the following questions:
(a) Identify which metals from the following can be used as “metal sample” in the given set-up: Aluminium, Copper, Iron, Lead, Silver?
(b) Write balanced chemical equations for the reaction in each case?
(a) Identify which metals from the following can be used as “metal sample” in the given set-up: Aluminium, Copper, Iron, Lead, Silver?
(b) Write balanced chemical equations for the reaction in each case?
Answer
(a) Metals that can be used as “metal sample”:
Aluminium and Iron — these react with water/steam to produce hydrogen gas.
Copper, Silver, and Lead do not react with water to release hydrogen under standard conditions.
(b) Balanced Chemical Equations:
For Aluminium (reacts with water): $$2\text{Al}(s) + 6\text{H}_2\text{O}(l) \rightarrow 2\text{Al(OH)}_3(aq) + 3\text{H}_2(g)$$ For Iron (reacts with steam): $$3\text{Fe}(s) + 4\text{H}_2\text{O}(g) \rightarrow \text{Fe}_3\text{O}_4(s) + 4\text{H}_2(g)$$ Copper, Lead, and Silver — no reaction with water.
Aluminium and Iron — these react with water/steam to produce hydrogen gas.
Copper, Silver, and Lead do not react with water to release hydrogen under standard conditions.
(b) Balanced Chemical Equations:
For Aluminium (reacts with water): $$2\text{Al}(s) + 6\text{H}_2\text{O}(l) \rightarrow 2\text{Al(OH)}_3(aq) + 3\text{H}_2(g)$$ For Iron (reacts with steam): $$3\text{Fe}(s) + 4\text{H}_2\text{O}(g) \rightarrow \text{Fe}_3\text{O}_4(s) + 4\text{H}_2(g)$$ Copper, Lead, and Silver — no reaction with water.
During electrolytic refining of copper, the anode, the cathode and the electrolyte used respectively are:
Solution
Answer: Option (A) is correct.
In the electrolytic refining of copper:
• Anode (+): Impure copper — dissolves as Cu²⁺ ions into the electrolyte.
• Cathode (−): Pure copper — Cu²⁺ ions are reduced and deposited as pure copper.
• Electrolyte: Acidified copper sulphate solution — provides Cu²⁺ ions for the process.
In the electrolytic refining of copper:
• Anode (+): Impure copper — dissolves as Cu²⁺ ions into the electrolyte.
• Cathode (−): Pure copper — Cu²⁺ ions are reduced and deposited as pure copper.
• Electrolyte: Acidified copper sulphate solution — provides Cu²⁺ ions for the process.
Name and explain the most widely used method for refining impure metals?
Answer
The most widely used method is Electrolytic Refining.
Process:
1. Anode (+) — Impure metal: When current is passed, the impure metal dissolves into the electrolyte as metal ions.
2. Cathode (−) — Pure metal: Metal ions from the electrolyte gain electrons and deposit as pure metal.
3. Electrolyte: A solution of the metal salt maintains the flow of ions.
Advantages:
• Produces metals of very high purity.
• Insoluble impurities settle as anode mud (e.g., gold, silver can be recovered).
Example — Refining of Copper:
Anode (+): Impure copper | Cathode (−): Pure copper | Electrolyte: Acidified CuSO₄
At Cathode (−) — pure copper deposited: $$Cu^{2+} + 2e^- \rightarrow Cu$$ At Anode (+) — impure copper dissolves: $$Cu \rightarrow Cu^{2+} + 2e^-$$
• Soluble impurities remain dissolved in the electrolyte.
• Insoluble impurities settle as anode mud below the anode.
Process:
1. Anode (+) — Impure metal: When current is passed, the impure metal dissolves into the electrolyte as metal ions.
2. Cathode (−) — Pure metal: Metal ions from the electrolyte gain electrons and deposit as pure metal.
3. Electrolyte: A solution of the metal salt maintains the flow of ions.
Advantages:
• Produces metals of very high purity.
• Insoluble impurities settle as anode mud (e.g., gold, silver can be recovered).
Example — Refining of Copper:
Anode (+): Impure copper | Cathode (−): Pure copper | Electrolyte: Acidified CuSO₄
At Cathode (−) — pure copper deposited: $$Cu^{2+} + 2e^- \rightarrow Cu$$ At Anode (+) — impure copper dissolves: $$Cu \rightarrow Cu^{2+} + 2e^-$$
• Soluble impurities remain dissolved in the electrolyte.
• Insoluble impurities settle as anode mud below the anode.
With the help of chemical equations differentiate between roasting and calcination? How is metal reduced from the product obtained after roasting/calcination of the ore? Write the chemical equation for the reaction involved?
Answer
Roasting:
Heating a sulphide ore in the presence of excess air (oxygen) to convert it into its oxide form.
Example: $$2\text{ZnS}(s) + 3\text{O}_2(g) \xrightarrow{\text{Heat}} 2\text{ZnO}(s) + 2\text{SO}_2(g)$$
Calcination:
Heating a carbonate ore in the absence of air to convert it into its oxide form by removing CO₂.
Example: $$\text{ZnCO}_3(s) \xrightarrow{\text{Heat}} \text{ZnO}(s) + \text{CO}_2(g)$$
Reduction of Metal from the Oxide Obtained:
After roasting or calcination produces the metal oxide, it is reduced using carbon as a reducing agent.
Example: $$\text{ZnO}(s) + \text{C}(s) \xrightarrow{\text{Heat}} \text{Zn}(s) + \text{CO}(g)$$
Carbon displaces oxygen from zinc oxide, producing pure zinc metal and carbon monoxide gas.
Heating a sulphide ore in the presence of excess air (oxygen) to convert it into its oxide form.
Example: $$2\text{ZnS}(s) + 3\text{O}_2(g) \xrightarrow{\text{Heat}} 2\text{ZnO}(s) + 2\text{SO}_2(g)$$
Calcination:
Heating a carbonate ore in the absence of air to convert it into its oxide form by removing CO₂.
Example: $$\text{ZnCO}_3(s) \xrightarrow{\text{Heat}} \text{ZnO}(s) + \text{CO}_2(g)$$
Reduction of Metal from the Oxide Obtained:
After roasting or calcination produces the metal oxide, it is reduced using carbon as a reducing agent.
Example: $$\text{ZnO}(s) + \text{C}(s) \xrightarrow{\text{Heat}} \text{Zn}(s) + \text{CO}(g)$$
Carbon displaces oxygen from zinc oxide, producing pure zinc metal and carbon monoxide gas.
With the help of balanced chemical equations state the process of extracting:
(i) mercury from its ore called cinnabar, and
(ii) copper from its sulphide ore.
(i) mercury from its ore called cinnabar, and
(ii) copper from its sulphide ore.
Answer
(i) Extraction of Mercury from Cinnabar (HgS):
Step 1 — Roasting: $$\text{HgS}(s) + \text{O}_2(g) \xrightarrow{\text{Heat}} \text{HgO}(s) + \text{SO}_2(g)$$ Step 2 — Reduction on further heating: $$\text{HgO}(s) \xrightarrow{\text{Heat}} \text{Hg}(l) + \text{O}_2(g)$$
(ii) Extraction of Copper from Copper(I) Sulphide (Cu₂S):
Step 1 — Roasting: $$2\text{Cu}_2\text{S}(s) + 3\text{O}_2(g) \xrightarrow{\text{Heat}} 4\text{CuO}(s) + 2\text{SO}_2(g)$$ Step 2 — Reduction by carbon: $$\text{CuO}(s) + \text{C}(s) \xrightarrow{\text{Heat}} \text{Cu}(s) + \text{CO}(g)$$
Step 1 — Roasting: $$\text{HgS}(s) + \text{O}_2(g) \xrightarrow{\text{Heat}} \text{HgO}(s) + \text{SO}_2(g)$$ Step 2 — Reduction on further heating: $$\text{HgO}(s) \xrightarrow{\text{Heat}} \text{Hg}(l) + \text{O}_2(g)$$
(ii) Extraction of Copper from Copper(I) Sulphide (Cu₂S):
Step 1 — Roasting: $$2\text{Cu}_2\text{S}(s) + 3\text{O}_2(g) \xrightarrow{\text{Heat}} 4\text{CuO}(s) + 2\text{SO}_2(g)$$ Step 2 — Reduction by carbon: $$\text{CuO}(s) + \text{C}(s) \xrightarrow{\text{Heat}} \text{Cu}(s) + \text{CO}(g)$$
(a) What is thermite process? Where is this process used? Write a balanced chemical equation for the reaction involved?
(b) Where does the metal aluminium used in the process occur in the reactivity series of metals?
(c) Name the substances that get oxidised and reduced in the process?
(b) Where does the metal aluminium used in the process occur in the reactivity series of metals?
(c) Name the substances that get oxidised and reduced in the process?
Answer
(a) Thermite Process:
The thermite process is a displacement reaction in which aluminium powder reacts with metal oxides to produce free metals in a highly exothermic reaction. It is used for welding and joining broken metal parts, particularly railway tracks.
Balanced Chemical Equation: $$\text{Fe}_2\text{O}_3 + 2\text{Al} \xrightarrow{\text{heat}} 2\text{Fe} + \text{Al}_2\text{O}_3$$
(b) Position of Aluminium in the Reactivity Series:
Aluminium is placed high in the reactivity series, above iron. This greater reactivity enables aluminium to displace iron from its oxide.
(c) Substances oxidised and reduced:
• Substance oxidised: Aluminium (Al) — oxidised to Al₂O₃.
• Substance reduced: Iron(III) oxide ($\text{Fe}_2\text{O}_3$) — reduced to Fe.
The thermite process is a displacement reaction in which aluminium powder reacts with metal oxides to produce free metals in a highly exothermic reaction. It is used for welding and joining broken metal parts, particularly railway tracks.
Balanced Chemical Equation: $$\text{Fe}_2\text{O}_3 + 2\text{Al} \xrightarrow{\text{heat}} 2\text{Fe} + \text{Al}_2\text{O}_3$$
(b) Position of Aluminium in the Reactivity Series:
Aluminium is placed high in the reactivity series, above iron. This greater reactivity enables aluminium to displace iron from its oxide.
(c) Substances oxidised and reduced:
• Substance oxidised: Aluminium (Al) — oxidised to Al₂O₃.
• Substance reduced: Iron(III) oxide ($\text{Fe}_2\text{O}_3$) — reduced to Fe.
Write balanced chemical equations to explain what happens when:
(a) Mercuric oxide is heated.
(b) Mixture of cuprous oxide and cuprous sulphide is heated.
(c) Aluminium is reacted with manganese dioxide.
(d) Ferric oxide is reduced with aluminium.
(e) Zinc carbonate undergoes calcination.
(a) Mercuric oxide is heated.
(b) Mixture of cuprous oxide and cuprous sulphide is heated.
(c) Aluminium is reacted with manganese dioxide.
(d) Ferric oxide is reduced with aluminium.
(e) Zinc carbonate undergoes calcination.
Answer
(a) Mercuric oxide is heated: $$2\text{HgO} \xrightarrow{\text{heat}} 2\text{Hg} + \text{O}_2$$
(b) Cuprous oxide and cuprous sulphide heated: $$2\text{Cu}_2\text{O} + \text{Cu}_2\text{S} \xrightarrow{\text{heat}} 6\text{Cu} + \text{SO}_2$$
(c) Aluminium reacted with manganese dioxide: $$3\text{MnO}_2 + 4\text{Al} \xrightarrow{\text{heat}} 3\text{Mn} + 2\text{Al}_2\text{O}_3$$
(d) Ferric oxide reduced with aluminium: $$\text{Fe}_2\text{O}_3 + 2\text{Al} \xrightarrow{\text{heat}} 2\text{Fe} + \text{Al}_2\text{O}_3$$
(e) Zinc carbonate undergoes calcination: $$\text{ZnCO}_3 \xrightarrow{\text{heat}} \text{ZnO} + \text{CO}_2$$
(b) Cuprous oxide and cuprous sulphide heated: $$2\text{Cu}_2\text{O} + \text{Cu}_2\text{S} \xrightarrow{\text{heat}} 6\text{Cu} + \text{SO}_2$$
(c) Aluminium reacted with manganese dioxide: $$3\text{MnO}_2 + 4\text{Al} \xrightarrow{\text{heat}} 3\text{Mn} + 2\text{Al}_2\text{O}_3$$
(d) Ferric oxide reduced with aluminium: $$\text{Fe}_2\text{O}_3 + 2\text{Al} \xrightarrow{\text{heat}} 2\text{Fe} + \text{Al}_2\text{O}_3$$
(e) Zinc carbonate undergoes calcination: $$\text{ZnCO}_3 \xrightarrow{\text{heat}} \text{ZnO} + \text{CO}_2$$
Explore More CBSE Class 10 Chemistry Chapters
Frequently Asked Questions
What does the Metals and Non-metals chapter cover in CBSE Class 10 Chemistry? ⌄
The Metals and Non-metals chapter in CBSE Class 10 covers the physical and chemical properties of metals, the reactivity series, methods of extraction (roasting, calcination, reduction, and electrolysis), alloys, corrosion, and the nature of ionic bonds. Students learn to write balanced equations for metal reactions with water, acids, and oxygen, and compare metal reactivity using displacement reactions.
How many marks does Metals and Non-metals carry in the CBSE Class 10 board exam? ⌄
Metals and Non-metals is part of the Chemical Substances unit in CBSE Class 10 Science, which carries the highest weightage in the board paper. Questions from this chapter appear across all formats — 1-mark MCQs, Assertion-Reason, 2-mark short answers, 3-mark application questions, and 5-mark long answers — making it one of the most marks-rich chapters your child can prepare thoroughly.
What are the most important topics in Class 10 Metals and Non-metals? ⌄
The highest-yield topics are: the reactivity series and displacement reactions, extraction of metals (roasting, calcination, reduction with carbon, and electrolytic reduction for highly reactive metals), electrolytic refining of copper, the thermite reaction, alloy compositions (brass, bronze, solder), corrosion and prevention (galvanisation), and amphoteric oxides of aluminium and zinc. Writing and balancing chemical equations for all these processes is tested every year.
What are common mistakes students make in Metals and Non-metals? ⌄
A very common error is confusing brass (copper + zinc) with bronze (copper + tin). Students also incorrectly state that nitric acid is a reducing agent — it is a strong oxidising agent. Writing unbalanced chemical equations for roasting and reduction, and mixing up the anode and cathode in electrolytic refining, are also frequently seen mistakes. Practising previous year questions with solutions helps your child avoid all of these in the actual exam.
How does Angle Belearn help students score well in Metals and Non-metals? ⌄
Angle Belearn’s CBSE specialists curate chapter-wise question banks directly from real board papers, paired with clear step-by-step solutions for every question type — MCQs, Assertion-Reason, short answers, and 5-mark long answers. Students who practise regularly on Angle Belearn develop the habit of writing structured, complete answers that earn full marks in board evaluations, and they enter the exam with the confidence that comes from having already solved the exact questions examiners have set.
