Class 10 Science Chapter 3 Previous Year Questions - Metals and Non-metals

Ans: (c)
Mercury is a metal that is liquid at room temperature, while bromine is a non-metal that is also liquid at room temperature.

Ans: (c)
This means that the oxides of aluminum and zinc can react with both acids and bases. They can behave like acids in some reactions and like bases in others, making them versatile in chemical behavior.

Ans: (c)
The correct answer is (c) Copper and silver. These metals can be found in their pure, uncombined form (free state) in nature, as well as in compounds with other elements (combined state). This means they can exist both as standalone metals and as part of various minerals.

Ans: (b)
Metal ‘X’ is aluminum, which is used in the thermit process. When aluminum is heated with oxygen, it forms aluminum oxide (Y), which is amphoteric, meaning it can react with both acids and bases.

Ans: (i) Cathode – Pure copper Anode – Impure copper
(ii) Acidified Copper Sulphate; CuSO4
(iii) (A) Pure copper from the anode dissolves into electrolyte and an equivalent amount of pure metal from the electrolyte is deposited on cathode

The soluble impurities go into the solution whereas insoluble impurities settle down at the bottom of the anode.
OR
(iii) (B)  In Beaker A: The blue colour of the solution fades (or becomes colourless)
Reason – Zn is more reactive than copper
In Beaker B: No change in colour.
Reason – Silver is less reactive than Copper

Ans: (b)
Assertion (A) is correct because different metals react differently with water and acids. However, while Reason (R) is also true, it explains how we extract metals rather than directly explaining why their reactivities vary.

Ans: (a) Amphoteric oxide (zinc oxide) reacts with acids as well as bases to produce salt and water.  
(b) If kept in open, sodium metal reacts vigorously with air and catches fire / kerosene oil does not allow sodium to come in contact with air and catch fire.
(c) Nitric acid is a strong oxidising agent. It oxidises the hydrogen produced in the reaction to water.

Ans: (a) (i) Reduction Process- Roasting
Reason: Mercury has low reactivity.
(ii) Reduction Process- Roasting
Reason: Copper has low reactivity.
(iii) Reduction Process- Electrolytic Reduction.
Reason: Sodium has high reactivity.
OR
(b) (i) Change in appearance - White to black colour.
Reason: Silver sulphide is formed.
(ii) Change in appearance – Reddish brown to green colour.
Reason: Basic Copper Carbonate is formed.
(iii) Change in appearance- Grey to brown colour.
Reason: Rust (iron oxide) is formed.

Ans: Cinnabar  
Sulphide ore

Ans: Zn + H₂SO₄ → ZnSO₄ + H₂ (g)
Hydrogen burns with a pop sound when a burning matchstick is brought near it.

Ans: (c)
Assertion (A): A piece of zinc metal gets a reddish-brown coating when kept in copper sulfate solution for some time. This is true. When zinc is placed in a copper sulfate solution, a displacement reaction occurs where zinc displaces copper from copper sulfate. The copper then deposits on the zinc surface as a reddish-brown coating.
Reason (R): Copper is more reactive than zinc. This is false. In the reactivity series, zinc is more reactive than copper, which is why zinc can displace copper from copper sulfate.
Since Assertion (A) is true but Reason (R) is false, the correct answer is (c) (A) is true, but (R) is false

Ans: (i) Transfer of electrons during the creation of magnesium chloride:
(ii) The two properties of ions Compounds are:
(a) Solubility: Electrovalent compounds are generally soluble in water and insoluble in solvents such as kerosene, petrol, etc.
(b) Conduction of Electricity: The conduction of electricity through a solution involves the movement of charged particles. A solution of an ionic compound in water contains ions, which move to the opposite electrodes when electricity is passed through the solution. Ionic compounds in the solid state do not conduct electricity because movement of ions in the solid is not possible due to their rigid structure. But ionic compounds conduct electricity in the molten state. This is possible in the molten state since the elecrostatic forces of attraction between the oppositely charged ions are overcome due to the heat. Thus, the ions move freely and conduct electricity.
(iii) (A) Sodium atom has one electron in its outermost shell. If it loses the electron from its M shell then its L shell now becomes the outermost shell and that has a stable octet. The nucleus of this atom still has 11 protons but the number of electrons has become 10, so there is a net positive charge giving us a sodium cation Na⁺. On the other hand chlorine has seven electrons in its outermost shell and it requires one more electron to complete its octet. If sodium and chlorine were to react, the electron lost by sodium could be taken up by chlorine. After gaining an electron, the chlorine atom gets a unit negative charge, because its nucleus has 17 protons and there are 18 electrons in its K, L and M shells. This gives us a chloride anion Cl^–.

(B) (i) The conduction of electricity through a solution involves the movement of charged particles. A solution of an ionic compound in water contains ions, which move to the opposite electrodes when electricity is passed through the solution. Ionic compounds in the solid state do not conduct electricity because the movement of ions in the solid is not possible due to their rigid structure. But ionic compounds conduct electricity in the molten state. This is possible in the molten state since the electrostatic forces of attraction between the oppositely charged ions are overcome due to the heat. Thus, the ions move freely and conduct electricity.
(ii) When electricity is passed through a solution of sodium chloride in water, hydrogen gas is released twice as much as oxygen gas is released at the anode.

Ans: (a) An ore of mercury is cinnabar, and mercury is present in it in the form of mercury sulfide (HgS).
(b) When zinc carbonate (ZnCO₃) is heated strongly in a limited supply of air, it undergoes thermal decomposition to produce zinc oxide (ZnO), carbon dioxide (CO₂), and water (H₂O):
ZnCO₃(s) → ZnO(s) + CO₂(g)
(c) (I) The metal A in this case is iron (Fe), and the reaction taking place is called a thermite reaction or the thermite process.
(II) The chemical equation for the reaction of iron (A) with iron(III) oxide (Fe₂O₃) is:
2Al(s) + Fe₂O₃(s) → 2Fe(s) + Al₂O₃(s)
This reaction is highly exothermic and is used in various industrial applications, including joining railway tracks due to its high heat generation and the ability to melt and fuse metals.

Ans: (b)
In the thermite process, aluminum (Al) is used because of its high reactivity and ability to reduce metal oxides, such as iron oxide, to produce molten iron.
When aluminum is burnt in air, it forms aluminum oxide (Al₂O₃), which is an amphoteric oxide (meaning it can react with both acids and bases).
Therefore, X is aluminum (Al) and Y is aluminum oxide (Al₂O₃), making the correct answer (b) Al and Al₂O₃.

Ans: (A) Copper is a reactive element. When it is heated in the air, it forms black copper oxide (CuO).
(B) Metal oxides are categorised as amphoteric oxides that react with both acids as well as bases to create salts and water. Amphoteric oxides, among many others, include lead oxide and zinc oxide. These oxides are oxygen compounds that show both acidic and basic characteristics. These undergo a neutralisation reaction to form water and salt.
Example: 
(C) 

OR

(C) (i)

(ii) The gas formed is sulphur dioxide which is colourless and poisonous. 
(iii) The nature of the gas is acidic. 
(iv) SO₂ gas has no effect on dry litmus paper because it shows acidic behavior only in the presence of water

Ans: Calcium hydroxide reacts with carbon dioxide present in the atmosphere to form calcium carbonate which results in milkiness/white ppt. / formation of calcium carbonate

• Copper: Yes, gas evolved. The reaction of copper with dilute hydrochloric acid is as follows: ��(�)+2���(��)→����2(��)+�2(�)

Cu(s)+2HCl(aq)→CuCl2(aq)+H2(g)

• Iron: Yes, gas evolved. The reaction of iron with dilute hydrochloric acid is as follows: ��(�)+2���(��)→����2(��)+�2(�)

Fe(s)+2HCl(aq)→FeCl2(aq)+H2(g)

• Magnesium: No, no gas evolved. Magnesium does not react with dilute hydrochloric acid.
• Zinc: Yes, gas evolved. The reaction of zinc with dilute hydrochloric acid is as follows: ��(�)+2���(��)→����2(��)+�2(�)

Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g)

So, the correct observations are for copper, iron, and zinc.

Ans: Potassium is kept immersed in kerosene because it reacts vigorously with air and water. The reaction with air forms a layer of potassium oxide on the surface, while the reaction with water produces potassium hydroxide. Both of these reactions release hydrogen gas, which is highly flammable. By keeping potassium immersed in kerosene, it is protected from air and water, preventing any unwanted reactions.

Ans: (a) Gold and silver are highly malleable metals so, they are used for making jewellery.
(b) Certain metals, such as stainless steel, copper, and aluminium, are used for making cooking utensils due to their specific properties. Stainless steel is chosen for its durability, corrosion resistance, and ease of cleaning. Copper is an excellent conductor of heat, allowing for even distribution of heat during cooking. Aluminium is lightweight and has good thermal conductivity, making it suitable for cookware. These metals provide the necessary characteristics required for efficient and safe cooking.

Ans:

Ans: 

(b) The formation of calcium oxide (CaO) involves the transfer of electrons. Calcium (Ca) donates two electrons to oxygen (O) to form Ca²⁺ cation and O^2- anion. The ionic bond is formed between these ions to create calcium oxide.
(c) In calcium oxide (CaO), the ions present are Ca²⁺ (calcium cation) and O^2- (oxygen anion).
(d) Four important characteristics of calcium oxide (CaO) are:

• It is a white, crystalline solid.
• It has a high melting and boiling point.
• It is an ionic compound.
• It is commonly used as a desiccant and in cement production.

Ans: Three differentiating features between the processes of galvanisation and alloying are as follows:

• Definition: Galvanisation is the process of applying a protective zinc coating to iron or steel to prevent corrosion, while alloying is the process of combining two or more metals or metals with a non-metal to create a new material with enhanced properties.
• Purpose: Galvanisation is primarily used to protect the base metal from corrosion by providing a sacrificial layer of zinc, whereas alloying is done to improve specific properties of the metal, such as strength, hardness, or resistance to corrosion.
• Procedure: In galvanisation, the metal is coated with zinc through processes like hot-dip galvanisation or electroplating. On the other hand, alloying involves melting and mixing different metals or adding non-metallic elements to create an alloy with the desired properties.

Ans: (a) Complete and balance the following chemical equations:
(i) AI₂O₃ + 6HCl → 2AlCl₃ + 3H₂O
(ii) K₂O + H₂O → 2KOH
(iii) Fe + 2H₂O → Fe(OH)₂ + H₂
(b) Observations:

• When element 'X' is treated with copper sulphate solution, no reaction occurs.
• When element 'X' is treated with zinc sulphate solution, 'X' displaces zinc from the solution, resulting in the formation of 'X' sulphate and zinc metal.
• When element 'X' is treated with silver nitrate solution, 'X' displaces silver from the solution, resulting in the formation of 'X' nitrate and silver metal.

Based on the observations, the increasing order of reactivities is:
Cu < Ag < X < Zn

Ans: 

(ii) Ionic compounds are solids because the particles that make up ionic compounds are held together by strong electrostatic bonds.

Ans: (a) (i) The malleability and ductility properties of gold make it suitable for ornaments. (ii) Silver and gold. 
(iii) Gallium and caesium have so low melting points that they melt even on keeping them in the palm.

(b) Formation of the ionic compound CaO (calcium oxide) with an electron-dot structure:

Calcium oxide (CaO) is formed through the transfer of electrons between calcium (Ca) and oxygen (O) atoms. Calcium, with an atomic number of 20, loses two electrons to achieve a stable electron configuration similar to that of a noble gas (argon), while oxygen, with an atomic number of 8, gains two electrons to complete its valence shell.

The electron-dot structure of CaO can be represented as follows:

In this structure, the calcium atom loses its two valence electrons to oxygen, resulting in a Ca²⁺cation and an O^2- anion. The electrostatic attraction between these oppositely charged ions forms the ionic bond in calcium oxide (CaO).

Ans: Sodium, magnesium and aluminium have a higher affinity towards oxygen than carbon because these are highly reactive metals. Hence, carbon cannot reduce the oxides of sodium, magnesium and aluminium to their respective metals. These metals are placed at the top of the reactivity series. Highly reactive metals like Na, Mg, Al, etc. are extracted by electrolytic reduction of their molten chlorides or oxides. Electrolytic reduction is brought about by passing electric current through the molten state. Metal gets deposited at the cathode.
NaCl ⇌ Na⁺ + Cl–
At cathode : Na⁺ + e^– → Na
At anode : 2Cl^– → Cl₂ + 2e^–

Ans: (i) On heating, mercuric oxide decomposes to give mercury and oxygen.

(ii) On heating a mixture of cuprous oxide and cuprous sulphide, copper and sulphur dioxide are produced.

(iii) When aluminium is heated with manganese dioxide, manganese and aluminium oxide are formed.

(iv) Ferric oxide reacts with aluminium to produce aluminium oxide and iron.

(v) On calcination, zinc carbonate produces zinc oxide and carbon dioxide.

Ans: (a) (i) Sodium
(ii) Iodine
(iii) Mercury
(iv) Gold
(v) Silver
(vi) Carbon
(b) Alloys are stronger than the metals from which they are made, more resistant to corrosion, have lower melting points, and have lower electrical conductivity. Solder is an alloy of lead and tin. An amalgam is an alloy of mercury with another metal.

Ans: After approximately 30 minutes, the student would observe that the strip of iron would start to show signs of corrosion or rusting. This is because iron is more reactive than copper, aluminium, and zinc and will displace the iron from the iron sulphate solution, forming iron oxide (rust) on its surface.

Ans: (a) The colour of the ferrous sulphate solution in test tube (I) will match the colour of the solution in test tube II when a piece of copper is dropped in it. This is because copper is less reactive than iron and will not displace iron from ferrous sulphate solution, resulting in no change in the colour of the solution.
(b) The colour of the ferrous sulphate solution will fade and a black mass will be deposited on the surface of the metal when a piece of aluminium or zinc is dropped in test tube III or IV. This is because aluminium and zinc are more reactive than iron and will displace iron from the ferrous sulphate solution, forming iron oxide (black mass) on their surfaces.

Ans: The ore that produces brisk effervescence when treated with dilute hydrochloric acid is a carbonate ore. One example of a carbonate ore is limestone (CaCO₃).
Steps to obtain metal from the enriched ore:

• Calcination: The ore is heated strongly in the absence of air to convert it into metal oxide.
  CaCO₃(s) → CaO(s) + CO₂(g)
• Reduction: The metal oxide is then reduced using a suitable reducing agent, such as carbon or hydrogen, to obtain the metal.
  CaO(s) + C(s) → Ca(s) + CO(g)

Ans: The substances present in the air with which silver reacts are hydrogen sulphide (H₂S) and sulphur compounds. Silver reacts with these substances to form a black layer of silver sulphide (Ag₂S) on its surface. The substances present in the air with which copper reacts are moisture, carbon dioxide (CO₂), and oxygen (O₂). Copper reacts with these substances to form a green layer of copper carbonate (CuCO₃) or copper hydroxide (Cu(OH)₂) on its surface.

Ans: (a)

(b) (i) Metals conduct electricity due to the flow of free electrons present in them.
(ii) The reaction of iron (III) oxide, Fe₂O₃ with aluminium is highly exothermic and the iron produced melts. This molten iron is used to join cracked iron parts of machines and railway tracks.

Ans: (a) The series of metals in decreasing order of reactivity is called the reactivity series of metals. The metals at the top are most reactive and metals at the bottom are least reactive.(b) The metals in the middle of the reactivity series are obtained from their ores by chemical reduction with a suitable reducing agent, e.g.
ZnO + C → Zn + CO
The metals at the top of the series are obtained by electrolytic reduction of their molten orc.
Al₂O₃  → 2Al³⁺ + 3O^2-
At cathode: 2Al³⁺ + 6e^- → 2Al
At anode: O^2- - 2e^- → O
O + O → O₂

Ans: (a) Extraction of metals of medium reactivity: The metals in the middle of the reactivity series are zinc, iron, lead, etc. The carbonate ores first need to get converted to oxides as it is easier to get metal from their oxides.
(b) Copper glance (Cu₂S) when heated in air gets partially oxidised to copper oxide which further reacts with the remaining copper glance to give copper metal.

Ans: To find out the conditions under which iron rusts, you can perform the following activity:

• Take three test tubes and label them as A, B, and C.
• Fill test tube A with water, test tube B with water and oil, and test tube C with water and salt.
• Place a small piece of iron nail in each test tube and allow them to stand undisturbed for a few days.
• Observe the test tubes regularly and note any changes in the appearance of the iron nails.
• After a few days, check for the presence of rust on the iron nails in each test tube.
• Analyze the results and determine the conditions under which iron rusts.

Ans: (i) The type of bond in compound Z is an ionic bond.
(ii) Ionic compounds generally have high melting and boiling points due to the strong electrostatic forces of attraction between the positive and negative ions.
(iii) Ionic compounds like compound Z do not dissolve in non-polar solvents like kerosene or petrol. They are only soluble in polar solvents.
(iv) No, compound Z will not be a good conductor of electricity in a solid state because the ions are held in a fixed position and cannot move. However, it may conduct electricity when dissolved in water or molten state as the ions become free to move and carry electric charge.

Ans: When metal surfaces are exposed to moist air, they can undergo oxidation. This oxidation leads to the formation of metal oxides on the surface of the metal. In the case of copper, the surface acquires a greenish coating called copper(II) oxide (CuO). Copper(II) oxide gives the surface a dull appearance. In the case of silver, the surface acquires a blackish coating called silver sulfide (Ag₂S). Silver sulfide also gives the surface a dull appearance.

Ans:(a) The process of slowly eating up metals due to their conversion into oxides, carbonates, sulphides, etc., by the action of atmospheric gases and moisture is called corrosion.
(b) The corrosion of iron is called rusting.
(c) Silver articles become black after some time when exposed to air. This is due to the formation of a coating of black silver sulphide (Ag₂S) on its surface by the action of H₂S gas present in the air.
(d) Corrosion of iron is a serious problem. Every year large amount of money is spent to replace damaged iron articles. Corrosion causes damage to car bodies, bridges iron railings, ships and to all objects made of metals especially those of iron.
(e) Corrosion of iron is prevented by coating it with a layer of oil. The reason is that the layer of oil does not allow air and water to reach the surface of iron. Corrosion of iron can also be prevented by painting, greasing, galvanising, anodising, electroplating or making alloys. 

Ans: (i) Most metals do not evolve hydrogen gas when they react with nitric acid because nitric acid is a strong oxidizing agent. It oxidizes hydrogen gas produced during the reaction to water and itself gets reduced to nitrogen oxides. Therefore, instead of hydrogen gas, the products obtained are nitrogen oxides.
(ii) Zinc oxide is considered an amphoteric oxide because it shows both acidic and basic properties. It reacts with acids to form zinc salts and water, exhibiting basic characteristics. Additionally, it reacts with bases to form zincates and water, showing acidic properties. This ability to react with both acids and bases classifies it as an amphoteric oxide.

ZnO + 2HCl →  ZnCl₂   + H₂ O

ZnO + 2NaOH + H₂ O →  Na₂   (Zn (OH)₄ )

(iii) Metals conduct electricity because they have a large number of free or delocalized electrons. These electrons are not bound to any particular atom and can move freely throughout the metal lattice. When a potential difference is applied across a metal, these free electrons can easily move and carry an electric current.

Ans: The reverse of the given chemical reaction is not possible because it violates the principle of conservation of mass. In the forward reaction, zinc (Zn) displaces copper (Cu) from copper sulfate (CuSO₄) to form zinc sulfate (ZnSO₄) and copper. However, in the reverse reaction, copper cannot displace zinc from zinc sulfate, as copper is less reactive than zinc. Hence, the reverse of this reaction is not feasible.

Ans: (a) It is a process in which a metal reacts with substances present in the air to form surface compounds.
(b) Rusting.
(c) Black layer on its surface due to formation of Ag₂S.
(d) It makes the metal weak and brittle, which is a serious problem.
(e) Oiling, painting, greasing, galvanisation, and alloying can prevent iron from corrosion.

Ans: (a) When a metal is attacked by substances around it, such as moisture, acids, etc., it is said to corrode and this process is called corrosion. Corrosion of iron is called rusting.
(b) Coating formed on silver is black and that formed on copper is green.
(c) Damages caused by corrosion:

• It causes damage to car bodies and bridges.
• It damages iron railings and ships.

Prevention of corrosion:

• Corrosion can be prevented by oiling, painting, greasing and galvanising.
• Corrosion can be prevented by galvanising and alloying.

Ans: (i) It is easier to convert metal oxides to metals as compared to carbonates and sulphides. Therefore carbonates are calcinated and sulphides are roasted to oxides.
(ii) There are electrostatic forces of attraction between the cations and anions in ionic compounds which are difficult to break. Therefore ionic compounds have high melting points.
(iii) Metals above hydrogen evolve hydrogen gas and metals below hydrogen do not evolve hydrogen when treated with an acid. That is when hydrogen has been assigned a place in the reactivity series of metals.
(iv) Even if the zinc layer is broken, it will preferentially be oxidised because it is more reactive than iron.
(v) The wires carrying current in homes have a coating of PVC. This is because PVC is an insulating substance and protects from electric shock.

Ans: Carbonic acid is formed.
CO₂ + H₂O → H₂CO₃

Ans: 2Al(s) + 3H₂O (g) → Al₂O₃(s) + 3H₂(g)

Ans:

(b) It is an ionic compound.
Physical properties:
(i) It is hard and solid.
(ii) It has a high melting and boiling point.
(iii) It is soluble in water.

Ans: (A) Sodium and magnesium have a tendency to react with oxygen rather than carbon because these are highly reactive metals. They have a greater affinity for oxygen than for carbon. Hence, their oxides are stable. The reduction of these metallic oxides with carbon requires very high temperature and at that temperature, metals react with carbon to form their corresponding carbides. Hence, carbon cannot reduce the oxides of Na or Mg. 
(B) Galvanisation is a process of formation of thin layer over metal surface. It prevents further contact of metal surface with atmosphere and reduces the corrosion level. So, iron articles are galvanised with a thin layer of zinc over them. Since zinc is more reactive than iron, it undergoes oxidation more readily than iron. As a result, iron articles remain protected. 
(C) Metals such as Na, K, Ca and Mg are highly reactive metals and hence they are not found in their free state in nature. Na, K, Ca and Mg  are alkali and alkaline Earth metals. They are the most reactive metals and readily react with atmospheric oxygen and other gases. Therefore, they are found in nature in the form of their compounds.

Ans: Silver and gold are least reactive metals and are often found in their native or free state. Aluminium is a very reactive metal and is never found in free state, but in combined state.