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Science [5 marks Questions]

Metals and Non-Metals · CBSE STD 10 (CBSE - English Medium). 23 questions.

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Question 15 Marks
A black metal oxide XO is used as a catalyst in the preparation of oxygen gas from potassium chlorate. The oxide XO is also used in ordinary dry cells. The metal oxide XO cannot be reduced satisfactorily with carbon to form metal X.
  1. Name the metal X.
  2. Name the metal oxide XO.
  3. Which reducing agent can be used to reduce XO to obtain metal X?
  4. Name another metal which can also be extracted by the reduction of its oxide with the above reducing agent.
Answer
  1. Manganese.
  2. Manganese dioxide.
  3. Aluminium.
  4. Chromium.
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Question 25 Marks
Metal A burns in air, on heating, to form an oxide $A _2 O _3$ whereas another metal B burns in air only on strong heating to form an oxide BO. The two oxides $A _2 O _3$ and BO can react with hydrochloric acid as well as sodium hydroxide solution to form the corresponding salts and water.
a. What is the nature of oxide $A _2 O _3$ ?
b. What is the nature of oxide BO?
c. Name one metal like A.
d. Name one metal like B.
Answer
a. The oxide $A _2 O _3$ is amphoteric, which can react with both acids and bases to form salt and water.
b. The oxide BO is amphoteric, which can react with both acids and bases to form salt and water.
c. Aluminium is a metal like A , which forms $Al _2 O _3$ on reacting with oxygen.
d. Zinc is a metal like B which forms ZnO on strongly heating in air (oxygen).
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Question 35 Marks
A metal X which is resistant to corrosion is produced by the electrolysis of its molten oxide whereas another metal Y which is also resistant to corrosion is produced by the reduction of its oxide with carbon. Metal X can be used in powder form in thermite welding whereas metal Y is used in making cathodes of ordinary dry cells.
  1. Name the metals X and Y.
  2. Which of the two metals is more reactive : X or Y?
  3. Name one ore or metal X. Also write its chemical formula.
  4. Name one ore of metal Y. Also write its chemical formula.
  5. Name one alloy of metal X and one alloy of metal Y.
Answer
a. $X$ is aluminium and $Y$ is zinc.
b. X is more reactiv e than Y .
c. Bauxite; $Al _2 O _3 .2 HO$.
d. Calamine, $ZnCO _3$
e. Alloy of metal X : Duralumin ; Allo y of metal Y : Brass.
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Question 45 Marks
State and explain the reaction, if any, of the following metals with a solution of copper sulphate:
  1. Gold.
  2. Copper.
  3. Zinc.
  4. Mercury.
Answer
  1. Gold, being less reactive than copper, cannot displace copper from copper sulphate solution and hence, no reaction occurs.
  2. Copper reacts with copper sulphate to form copper and copper sulphate solution. So, practically no reaction occurs between them.
  3. Zinc is more reactive than copper and hence, displaces copper from its solution to form zinc sulphate solution and copper metal.
  4. $Zn ( s )+ CuSO _4( aq ) \rightarrow ZnSO _4( aq )+ Cu ( s )$
  5. Mercury, being less reactive than copper, cannot displace copper from copper sulphate solution and hence, no reaction occurs.
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Question 55 Marks
You are given samples of three metals — sodium, magnesium and copper. Suggest any two activities to arrange them in order of their decreasing reactivities.
Answer
  1. When sodium, magnesium and copper are left in air, sodium reacts vigorously with oxygen to form sodium oxide, magnesium reacts with oxygen to form magnesium oxide only on heating , whereas copper does not burn in air even on strong heating. It reacts only on prolonged heating. This shows that sodium is most reactive, then magnesium and copper is the least reactive among the three.
  2. Sodium reacts vigorously with cold water to form sodium hydroxide and hydrogen, magnesium does not react with cold water but reacts with hot water to form magnesium hydroxide and hydrogen but copper does not react even with steam. This shows that sodium is highly reactive; magnesium is less reactive than sodium and copper is the least reactive among the three.
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Question 65 Marks
An element X forms two oxides XO and $XO _2$. The oxide XO has no action on litmus solution but oxide $XO _2$ turns litmus solution red.
a. What is the nature of oxide XO ?
b. What is the nature of oxide $XO _2$ ?
c. Would you call element $X$ a metal or a non-metal? Give reason for your choice.
d. Can you give an example of element like $X$ ?
Answer
a. The oxide XO is neutral in nature as it has no action on litmus solution.
b. The oxide $XO _2$ is acidic in nature as it turns litmus solution red.
c. The element $X$ is a non-metal because it forms an acidic and neutral oxide, which is the property of a non-metal.
d. Carbon is a non-metal like the element X .
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Question 75 Marks
When an object made of metal A is kept in air for a considerable time, it loses its shine and becomes almost black due to the formation of a layer of substance B. When an object made of another metal C is kept in damp air for a considerable time, it gets covered with a green layer of substance D. Metal A is the best conductor of electricity whereas metal C is the next best conductor of electricity.
  1. What is metal A?
  2. What is metal C?
  3. Name the substance B.
  4. Name the substance D.
  5. What type of chemical can be used to remove the green layer from metal C and clean it? Why?
Answer
  1. Silver.
  2. Copper.
  3. Silver sulphide.
  4. Basic copper carbonate.
  5. Dilute acid solution; The acid sol ution dissolves green coloured basic copper carbonate present on the corroded copper object makes it look shiny, red brown again.
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Question 85 Marks
Write the equations for the reactions of:
  1. Magnesium with dilute hydrochloric acid.
  2. Aluminium with dilute hydrochloric acid.
  3. Zinc with dilute hydrochloric acid.
  4. Iron with dilute hydrochloric acid.
Name the products formed in each case. Also indicate the physical states of all the substances involved.
Answer
  1. $\text{Mg(s)}+2\text{HCl(aq)}\rightarrow\text{MgCl}_2\text{(aq)}+\text{H}_2\text{(g)}$
The products formed are maginisium chloride and hydrogen.
  1. $2\text{Al(s)}+6\text{HCl(aq)}\rightarrow2\text{AlCl}_3\text{(aq)}+3\text{H}_2\text{(g)}$
The products formed are aluminium chloride and hydrogen.
  1. $\text{Zn(s)}+2\text{HCl(aq)}\rightarrow\text{ZnCl}_2\text{(aq)}+\text{H}_2\text{(g)}$
The products formed are zinc chloride and hydrogen.
  1. $\text{Fe(s)}+2\text{HCl(aq)}\rightarrow\text{FeCl}_2\text{(aq)}+\text{H}_2\text{(g)}$
The products formed are iron chloride and hydrogen.
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Question 95 Marks
Explain why, a salt which does not conduct electricity in the solid state becomes a good conductor in molten state.
Answer
Although solid ionic compounds are made up of ions but they do not conduct electricity in solid state. This is because in the solid ionic compound, the ions are held together in fixed positions by strong electrostatic forces and cannot move freely. However, when we dissolve the ionic solid in water or melt it, the crystal structure is broken down and ions become free to move and conduct electricity.
Thus, an aqueous solution of an ionic compound conducts electricity because there are plenty of free ions in the solution which are able to conduct electric current.
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Question 105 Marks
Four metals P, Q, R and S are all obtained by the reduction of their oxides with carbon. Metal P is used to form a thin layer over the sheets of metal S to prevent its corrosion. Metal Q is used for electroplating tiffin boxes made of metal S whereas metal R is used in making car batteries. Metals Q and R form an alloy called solder. What are metals P, Q, R and S? How have you arrived at this conclusion?
Answer
  • Metal P is zinc; Metal Q is tin; Metal R is lead; Metal S is iron.
  • Metal P (zinc) is used to form a thin layer on metal S (iron) by the process of galvanisation to prevent its corrosion.
  • Metal Q (tin) i s used for electroplating tiffin boxes made of metal S (iron).
  • Metal R (lead) is used in making car batteries.
  • Metals Q (tin) and R (lead) form an alloy called solder .
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Question 115 Marks
Compare the properties of ionic compounds and covalent compounds.
Answer
Ionic compounds
  1. Ionic compounds are usually crystalline solids.
  2. Ionic compounds have high melting and boiling points.
  3. Ionic compounds are usually soluble in water.
Covalent compounds
  1. Covalent compounds are usually liquids or gases.
  2. Covalent compounds have low melting and boiling points.
  3. Covalent compounds are usually insoluble in water.
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Question 125 Marks
State any five physical properties of metals and five physical properties of non-metals.
Answer
Properties of metals:
  1. Metals are malleable i.e. they can be beaten into thin sheets with a hammer.
  2. Metals are ductile i.e. they can be drawn into thin wires.
  3. Metals are good conductors of heat and electricity.
  4. Metals are lustrous.
  5. Metals are generally hard.
Properties of non-metals:
  1. Non-metals are non-malleable i.e. they cannot be beaten into thin sheets with a hammer.
  2. Non-metals are non-ductile i.e. they cannot be drawn into thin wires
  3. Non-m etals are bad conductors of heat and electricity.
  4. Non-m etals are non- lustrous.
  5. Non-m etals are generally soft.
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Question 135 Marks
Draw the electron-dot structures of the following compounds and state the type of bonding in each case:
i. KCl
ii. $NH _3$
iii. CaO
iv. $N _2$
v. $CaCl _2$​​​​​​​
Answer
  1. KCl - lonic bond
  1. $NH _3$ - Covalent bond
  1. CaO - lonic bond
  1. $N _2$ - Covalent bond
  1. $CaCl _2$ - lonic bond
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Question 145 Marks
State one use each of the following metals:
Copper, Aluminium, Iron, Silver, Gold, Mercury
Answer
  1. Copper – Copper is used to make wires to carry electric current.
  2. Aluminium – Aluminium foils are used in packaging of food materials.
  3. Iron – Iron is used to make utensils.
  4. Silver – Silver is used to make jewellery.
  5. Gold – Gold is used to make jewellery.
  6. Mercury – Mercury is used in thermometers.
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Question 155 Marks
An element A which is a part of common salt and kept under kerosene reacts with another element B of atomic number 17 to give a product C. When an aqueous solution of product C is electrolysed then a compound D is formed and two gases are liberated.
  1. What are A and B?
  2. Identify C and D.
  3. What will be the action of C on litmus solution? Why?
  4. State whether element B is a solid, liquid or gas at room temperature.
  5. Write formula of the compound formed when element B reacts with an element E having atomic number 5.
Answer
  1. A is sodium and B is chlo rine.
  2. C is sodium chloride and D is sodium hydroxide.
  3. C will have no effect on litmus solution since it is neutral in nature.
  4. B is a gas at room temperature.
  5. EB3.
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Question 165 Marks
What is meant by ‘rusting of iron’? With the help of labelled diagrams, describe an activity to find out the conditions under which iron rusts.
Answer
When an iron object is left in damp air (or water) for a considerable time, it gets covered with a red-brown flaky substance called rust. This is called rusting of iron. Experiment to show that rusting of Iron requires both, air and water: We take three test-tubes and put one clean iron nail in each of the three test-tubes:
  1. In the first test-tube containing iron nail, we put some anhydrous calcium chloride and close its mouth with a tight cork . Anhydrous calcium chloride absorbs water moisture from the damp air present in the test-tube and make it dry. In this way, the iron nail in the first test-tube is kept in dry air (having no water vapour in it).
  2. In the second test-tube containing iron nail , we put boiled distilled water. Boiled water does not contain any dissolved air (or oxygen) in it (this is because the process of boiling removes all the dissolved air from it). A layer of oil is put over boiled water in the test-tub e to prevent the outside air from mixing with boiled water. In this way, the iron nail in the second test-tube is kept in air free boiled water.
  3. In the third test-tube containing an iron nail, we put unboiled wa ter so that about two-thirds of nail is immersed in water and the rest is a bove the water, exposed to damp air. In this way , the iron nail in the third test-tube has been placed in air and water together.
The mouth of all three test tube s is cl osed with a cork and it is kept aside for about one week.
After one week, we observe the iron nails kept in all the three test-tubes, one by one. We find that,
  1. No rust is seen on the surface of iron nai l kept in dry air (water-f ree air) in the first test-tube. This tells us that rusting of iron does not take place in air alone.
  2. No rust is seen on the surface of iron nail kept in air-free, boiled water in the second testtube. This tells us that rusting of iron does not take place in water alone.
  3. Red-brown rust is seen on the surface of iron nail kept in the presence of both air and water together the third test-tube. This tells us that rusting of iron takes pla ce in the presence of both air and water together.
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Question 175 Marks
Draw the electron-dot structures of the following compounds and state the type of bonding in each case:
i. $CO _2$
ii. MgO
iii. H,O
iv. HCl
v. $MgCl _2$
Answer
  1. $CO _2$ - Covalent bond
  1. MgO - lonic bond
  1. $H_2O$ - Covalent bond
  1. HCl - Covalent bond
  1. $MgCl _2$ - lonic bond
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Question 185 Marks
What is meant by refining of a metal? Name the most widely used method for the refining of impure metals obtained by various reduction processes. Describe this method with the help of a labelled diagram by taking the example of any metal.
Answer
The process of purifying impure metals is called refining of metals. Electrolytic refining is the most widely used method for the refining of impure metals obtained
by various reduction processes. In an electrolytic tank, acidified copper sulphate $\left( CuSO _4^{+}\right.$dil ute $\left.H _2 O _4\right)$ solution forms the electrolyte. A block of impure copper is made into an anode by connecting the positive terminal of a power supply (battery). A thin strip of highly pure copper metal is the cathode of the cell. The negative terminal of the power supply is connected to it.

A small electric curr ent is passed through the cell. Atoms from the anode enter the electrolyte. The copper from the anode gets converted into copper sulphide. An equal number of copper atoms from the solution get deposited on the cathode. This is to keep the concentration of the solution constant. Impurities from the anode block either remain in solution or collect below the anode, as they are unable to displace copper from the sulphate solution. The insoluble impurities remain in the electrolyte and are called anode mud. Copper sulphate solution contains ions of $Cu ^{2+}$ and $SO _4{ }^{2-}$. The following reactions take place at the anode and cathode when an electric current is passed. $\text{At cathode:}\ \ \ \ \ \ \ \ \ \ \ \ \ \text{Cu}^{2+}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \xrightarrow[\text{(Reduction)}]{+2\text{electrons}}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Cu}\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Copper ion}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Copper atom}\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{(From electrolyte)}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{(Deposits on cathode)}$ $\text{At anode:}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Cu}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \xrightarrow[\text{(oxidation)}]{-2\text{electrons}}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Cu}^{2+}\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Copper atom}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Copper ion}\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{(From impure anode)}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{(Goes into electrolyte)}$ Pure copper is scraped or removed from the cathode. Anode becomes thinner as the electrolysis process proceeds. Some important metals like gold and silver are present in the anode mud. These can be recovered separately.
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Question 195 Marks
State five uses of metals and five of non-metals.
Answer
Uses of metals:
  1. Lead metal is used in making car batteries.
  2. Zinc is used for galvanizing iron to protect it from rusting.
  3. Iron, copper and aluminium are used to make utensils.
  4. Copper and aluminium metals are used to make electrical wires.
  5. Aluminium is used to make aluminium foil for packaging materials.
Uses of non-metals:
  1. Hydrogen is used in the hydrogenation of vegetable oils.
  2. Carbon is used to make electrodes of electrolytic cells and dry cells.
  3. Nitrogen is used in the manufacture of ammonia, nitric acid and fertilizers.
  4. Sulphur is used for producing sulphuric acid.
  5. Liquid hydrogen is used as rocket fuel.
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Question 205 Marks
A metal which exists as a liquid at room temperature is obtained by heating its sulphide ore in the presence of air.
  1. Name the metal and write its chemical symbol.
  2. Write the name and formula of the sulphide ore.
  3. Give the equations of chemical reactions involved in the production of metal from its sulphide ore.
  4. Name a common device in which this metal is used.
  5. Can this metal displace copper from copper sulphate solution? Why?
Answer
  1. Mercury, Hg.
  2. Cinnabar, HgS.
  3. $\ \ \ \ \ \ \ \ \ 2\text{HgS}\text{(s)}\ \ \ \ \ \ \ \ \ \ \ \ \ \ +\ \ \ \ \ \ \ \ \ \ \ 3\text{O}_2\xrightarrow{\ \ \ \ \text{Rcesting}\ \ \ }\ \ \ \ \ \ \ 2\text{Hg(s)}\ \ \ \ \ \ \ \ \ \ +\ \ \ \ \ \ \ \ \ \ \ \text{2SO}_2\text{(g)}\\\text{Mercury (II) Sulphide}\ \ \ \ \ \ \ \ \ \ \ \text{Oxygen}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Mercury (II) Oxide}\ \ \ \ \ \ \ \ \text{Sulphur dioxide}$
$\ \ \ \ \ \ \ \ \ \ \ \ 2\text{HgO}\text{(s)}\ \ \ \ \ \ \ \ \ \ \xrightarrow[\text{Rcesting}]{\ \ \ \ \text{Heat}\ \ \ }\ \ \ \ \ \ \ \ \ 2\text{Hg(l)}\ \ \ \ \ +\ \ \ \ \ \text{O}_2\text{(g)}\\\text{Mercury (III) Oxide}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Mercury metal}\ \ \ \ \ \ \ \text{Oxygen}$
  1. Thermometer.
  2. No; Because it is less reactive than copper.
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Question 215 Marks
State one use each of the following non-metals:
Hydrogen, Carbon (as Graphite), Nitrogen, Sulphur
Answer
  1. Hydrogen – Hydrogen is used in the hydrogenation of vegetable oils.
  2. Carbon is used to make electrodes of electrolytic cells and dry cells.
  3. Nitrogen is used in the manufacture of ammonia, nitric acid and fertilizers.
  4. Sulphur is used in making sulphuric acid.
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Question 225 Marks
How are metals refined by the electrolytic process? Describe the electrolytic refining of copper with the help of a neat labelled diagram.
Answer
For the refining of an impure metal by the process of electrolysis, a thick block of impure metal is made anode (connected to +ve terminal of the battery) and a thin strip of the pure metal is made cathode (connected to -ve terminal of battery). A water soluble salt (of the metal to be refined) is taken as electrolyte. On passing current, impure metal dissolves from the anode and goes into the electrolyte solution. And pure metal from the electrolyte deposits on the cathode. Electrolytic refining of copper: In an electrolytic tank, acidified copper sulphate $\left( CuSO _4^{+}\right.$dil ute $\left.H _2 O _4\right)$ solution forms the electrolyte. A block of impure copper is made into an anode by connectig the positive terminal of a power supply (battery). A thin strip of highly pure copper metal is the cathode of the cell. The negative terminal of the power supply is connected to it.
A small electric curr ent is passed through the cell. Atoms from the anode enter the electrolyte. The copper from the anode gets converted into copper sulphide. An equal number of copper atoms from the solution get deposited on the cathode. This is to keep the concentration of the solution constant. Impurities from the anode block either remain in solution or collect below the anode, as they are unable to displace copper form the sulphate solution. The insoluble impurities remain in the electrolyte and are called anode mud. Copper sulphate solution contains ions of $Cu ^{2+}$ and $SO _4{ }^{2-}$. . The following reactions take
place at the anode and cathode when an electric current is passed. $\text{At cathode:}\ \ \ \ \ \ \ \ \ \ \ \ \ \text{Cu}^{2+}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \xrightarrow[\text{(Reduction)}]{+2\text{electrons}}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Cu}\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Copper ion}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Copper atom}\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{(From electrolyte)}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{(Deposits on cathode)}$ $\text{At anode:}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Cu}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \xrightarrow[\text{(oxidation)}]{-2\text{electrons}}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Cu}^{2+}\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Copper atom}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{Copper ion}\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{(From impure anode)}\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{(Goes into electrolyte)}$ Pure copper is scraped or removed from the cathode. Anode becomes thinner as the electrolysis process proceeds. Some important metals like gold and silver are present in the anode mud. These can be recovered separately.
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Question 235 Marks
No chemical reaction takes place when granules of a rusty-brown solid A are mixed with the powder of another solid B. However, when the mixture is heated, a reaction takes place between its components. One of the products C is a metal and settles down in the molten state while the other product D floats over it. It was observed that the reaction is highly exothermic.
  1. What could the solids A and B be?
  2. What are the products C and D most likely to be?
  3. Write the chemical equation for the reaction between A and B leading to the formation of C.and D. Mention the physical sates of all the reactants and products in this equation and indicate the heat change which takes place.
  4. What is the special name of such a reaction? State one use of such a reaction.
  5. Name any two types of chemical reactions under which the above reaction can beclassified.
Answer
  1. A is iron ( III ) oxide and B is aluminium powder.
  2. C is molten iron metal and D is aluminium oxide.
  3. $\ \ \ \ \ \ \ \text{Fe}_2\text{O}_3\text{(s)}\ \ \ \ \ +\ \ \ \ \ 2\text{Al(s)}\ \ \ \ \ \ \ \ \ \xrightarrow{\ \ }\ \ \ \ \ \ \ \ 2\text{Fe(l)}\ \ \ \ \ \ \ +\ \ \ \ \ \ \ \ \text{Al}_2\text{O}_3\text{(s)}\ \ \ \ \ \ \ +\ \ \ \ \text{Heat}\\\text{Iron(III)}\text{Oxide}\ \ \ \text{Aluminium powder}\ \ \ \ \ \ \ \text{Iron metal}\ \ \ \ \ \ \ \ \text{Aluminium oxide}$
  4. This reaction is called thermite reaction. It is used for welding of broken pieces of heavy iron objects like railway tracks, etc.
  5. Displacement reactions and oxidation-reduction reactions.
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[5 marks Questions] - Science STD 10 Questions - Vidyadip