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Case Based Questions: Metals and Non-Metals | Science Class 10 PDF Download

Q1: Read the source below and answer the questions that follow:

A teacher demonstrated an experiment in class where she took different samples of iron, copper, sulfur, and graphite. She performed the following tests:

  • Striking the samples with a hammer to test malleability.
  • Drawing them into wires to check ductility.
  • Testing their ability to conduct electricity by connecting them to a circuit.
  • Observing their appearance before and after rubbing with sandpaper to check for metallic lustre.

(a) Identify which of the given substances are metals and non-metals based on tests done and also give observation table. (1 mark)
(b) From above samples which non-metal is a good conductor of electricity? (2 marks)
(c) Name two metals that are poor conductors of heat. (1 mark, )

Ans:
(a) Iron and copper = Metals, Sulfur and graphite = Non-metals (based on malleability, ductility, and conductivity).Case Based Questions: Metals and Non-Metals | Science Class 10

(b) Graphite is a good conductor of electricity because it has free-moving electrons in its layered structure.
(c) Lead and mercury are poor conductors of heat.

Q2: Read the source below and answer the questions that follow:

Riya conducted an experiment where she burned magnesium ribbon and sulfur powder in separate test tubes and dissolved the products in water. She then tested both solutions with red and blue litmus papers.

  • Magnesium oxide turned red litmus blue.
  • Sulfur dioxide turned blue litmus red.

(a) Identify the nature of the products formed when magnesium and sulfur burn in oxygen. (1 mark)
(b) Write the balanced chemical equations for both reactions. (2 marks)
(c) Name a metal oxide that shows both acidic and basic properties. (1 mark)
OR
(c) What happens when sodium is exposed to air? (1 mark)

Ans:
(a) Magnesium oxide (MgO) is basic, and sulfur dioxide (SO₂) is acidic.
(b) Balanced equations:

  • Magnesium: 2Mg + O₂ → 2MgO
  • Sulfur: S + O₂ → SO₂

(c) Aluminium oxide (Al₂O₃) and zinc oxide (ZnO) are amphoteric oxides (show both acidic and basic properties).
OR
(c) Sodium reacts violently with oxygen, forming sodium oxide (Na₂O) and must be stored in kerosene to prevent accidental ignition.

Q3: Read the source below and answer the questions that follow:

Aryan added sodium, calcium, and iron to separate beakers containing cold water. He observed that:

  • Sodium reacted violently, producing heat and gas.
  • Calcium reacted moderately, forming bubbles and a cloudy solution.
  • Iron did not react with cold water.

(a) Identify the gases evolved in these reactions. (1 mark)
(b) Write the balanced equations for the reaction of sodium and calcium with water. (2 marks)
(c) Why does iron not react with cold water but react with steam? (1 mark)
OR
(c) Why is calcium stored in an air-tight container? (1 mark)

Ans:
(a) Hydrogen (H₂) gas is evolved in all reactions.
(b) Balanced equations:

  • 2Na + 2H₂O → 2NaOH + H₂
  • Ca + 2H₂O → Ca(OH)₂ + H₂

(c) Iron does not react with cold water but reacts with steam because of its low reactivity to form iron oxide and hydrogen gas.
Equation: 3Fe + 4H₂O → Fe₃O₄ + 4H₂
OR
(c) 
Calcium reacts with air and moisture to form calcium hydroxide, so it must be stored in airtight containers.

Q4: Read the source below and answer the questions that follow:

A student placed an iron nail in a beaker containing copper sulfate (CuSO₄) solution. After some time, he observed that the blue color faded, and a reddish-brown deposit appeared on the nail.

(a) Identify the reaction taking place. (1 mark)
(b) Write the balanced chemical equation for this reaction. (2 marks)
(c) What would happen if a copper wire was placed in iron sulfate (FeSO₄) solution? (1 mark)
OR
(c) Arrange the metals Fe, Cu, and Zn in order of reactivity. (1 mark)

Ans:
(a) This is a displacement reaction, where a more reactive metal (iron) displaces a less reactive metal (copper).
(b) Balanced equation: Fe + CuSO₄ → FeSO₄ + Cu
(c) No reaction occurs because copper is less reactive than iron.
OR
(c) Reactivity order: Zn > Fe > Cu.

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Q5: Read the source below and answer the questions that follow:

A teacher demonstrated an experiment where she placed iron nails in three test tubes:

  • Test Tube A: Contained only water.
  • Test Tube B: Contained boiled distilled water with oil.
  • Test Tube C: Contained anhydrous calcium chloride (dry air).

After a few days, the nails in Test Tube A rusted, but those in B and C did not.

(a) Identify the test tube in which iron nail will rust and state conditions required for rusting.  (1 mark)
(b) Write the balanced chemical equation for rusting of iron. (2 marks)
(c) Name one method to prevent rusting. (1 mark)
OR
(c) Why does oil prevent rusting? (1 mark)

Ans:
(a) In Test Tube A nail will start to rust and Rusting requires both oxygen and water.
(b) Balanced equation:
4Fe + 3O₂ + 6H₂O → 4Fe(OH)₃ → Fe₂O₃·xH₂O (rust)
(c) Galvanization (coating iron with zinc) prevents rusting.
OR
(c) 
Oil prevents rusting by forming a protective layer that blocks water and oxygen from reaching the iron surface.

Q6: Read the source below and answer the questions that follow:

A chemistry teacher explained that metals lose electrons and non-metals gain electrons to form ionic bonds. She demonstrated this by showing the formation of sodium chloride (NaCl) where sodium donates an electron to chlorine.

(a) Identify which element is the electron donor and which is the electron acceptor in NaCl formation. (1 mark)
(b) Draw the electron dot structure for NaCl and explain why it is called an ionic bond. (2 marks)
(c) Why do ionic compounds have high melting and boiling points? (1 mark)
OR
(c) Why do ionic compounds conduct electricity in a molten or aqueous state? (1 mark)

Ans:
(a) Sodium (Na) is the electron donor, and Chlorine (Cl) is the electron acceptor.
(b) Electron dot structure:
Na • → Cl : → Na⁺ + Cl⁻
Ionic bonds are formed due to electrostatic attraction between oppositely charged ions.
(c) Ionic compounds have strong electrostatic forces between ions, requiring high energy to break these bonds.
OR
(c) Ionic compounds conduct electricity in a molten/aqueous state because ions are free to move and carry charge.

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Q7: Read the source below and answer the questions that follow:

A scientist demonstrated the electrolysis of molten aluminium oxide (Al₂O₃) in an industrial setup. Aluminium metal was collected at the cathode, while oxygen gas was released at the anode.

(a) Identify which electrode (cathode or anode) aluminium is deposited on. (1 mark)
(b) Write the reactions occurring at the cathode and anode. (2 marks)
(c) Name one more metal ores that can be refined using similar process? (1 mark)

Ans:
(a) Aluminium is deposited at the cathode (negative electrode).
(b) Reactions:

  • At cathode: Al³⁺ + 3e⁻ → Al
  • At anode: 2O²⁻ → O₂ + 4e⁻

(c) Sodium, magnesium and calcium are obtained by the electrolysis of their molten chlorides.

Q8: Read the source below and answer the questions that follow:

During a factory visit, students observed the manufacturing of brass, stainless steel, and bronze. The guide explained that alloys are stronger and more resistant to corrosion than pure metals.

(a) Identify the main metals present in brass and stainless steel. (1 mark)
(b) What are alloys? Why alloy of gold is widely used instead of pure gold? (2 marks)
(c) What is alloy in which one of the metal is mercury called? (1 mark)
OR
(c) Why is aluminium used for making aircraft parts? (1 mark)

Ans:
(a) Brass = Copper + Zinc, Stainless steel = Iron + Chromium + Nickel + Carbon.
(b) An alloy is a homogeneous mixture of two or more metals, or a metal and anon-metal.
Pure gold, known as 24 carat gold, is very soft. It is, therefore, not suitable for making jewellery. It is alloyed with either silver or copper to make it hard.
(c) Amalgum
OR
(c)
Aluminium is lightweight, corrosion-resistant, and strong, making it ideal for aircraft parts.

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Q9: Read the source below and answer the questions that follow:

A ship’s iron body was found to have rust patches, while the zinc-coated parts remained rust-free. The ship maintenance engineer explained that galvanization prevents rusting.

(a) Identify the chemical process causing rust formation. (1 mark)
(b) Write the balanced equation for the rusting of iron. (2 marks)
(c) What is the role of zinc in preventing rusting? (1 mark)
OR
(c) Name two other methods of rust prevention besides galvanization. (1 mark)

Ans:
(a) Rusting is an oxidation process where iron reacts with oxygen and moisture.
(b) Balanced equation:
4Fe + 3O₂ + 6H₂O → 4Fe(OH)₃ → Fe₂O₃·xH₂O (rust)
(c) Zinc forms a protective coating over iron and also acts as a sacrificial metal, preventing rusting.
OR
(c) 
Other methods of rust prevention include painting, oiling, and alloying (e.g., stainless steel).

Q10: Read the source below and answer the questions that follow:

Pratyush took sulfur powder on a spatula and heated it in a flame. He then collected the gas evolved by inverting a test tube over it. After the reaction, he took two strips of litmus paper (one dry and one moist) and exposed them to the collected gas. He observed that the dry litmus paper showed no change, while the moist litmus paper turned red.

(a) Identify the gas evolved and explain its effect on: (1 mark)
(i) Dry litmus paper
(ii) Moist litmus paper

(b) Write the balanced chemical equation for the reaction taking place. (2 marks)
(c) How does this experiment demonstrate the nature of the gas evolved? (1 mark)
OR
(c) Why does the gas turn moist litmus paper red but not affect dry litmus paper? (1 mark)

Ans:
(a) The gas evolved is sulfur dioxide (SO₂).
(i) Dry litmus paper: No change occurs because SO₂ does not ionize in the absence of water.
(ii) Moist litmus paper: Turns red, indicating the gas is acidic.
(b) Balanced Chemical Equation:
+ O→ SO+ O2
(c) This experiment demonstrates that SO₂ is an acidic oxide because it turns moist litmus paper red, confirming its acidic nature.
OR
(c) 
SO₂ dissolves in water to form sulfurous acid (H₂SO₃), which releases H⁺ ions, making the solution acidic and turning the litmus red.)

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