Class 10 Science Metals and Non Metals Extra Questions

In this page we have Class 10 Science Metals and Non Metals Extra Questions & Questions answers . Hope you like them and do not forget to like , social share and comment at the end of the page.
a. True and False
b. Match the column
c. Fill in the blanks
d. Multiple Choice Questions
e. Very Short answer type
f. Short answer type
e. Long Answer type

True and false

  1. The composition of aqua-regia is Conc. HCl: Conc. HNO3 is 3: 1
  2. Metals are electronegative?
  3. Sodium chloride conducts electricity in solid state
  4. Chlorine is a half metal
  5. Cassiterite is not an ore of iron
  6. Electrical wires have a coating of an PVC insulting material
  7. Duralumin is a mixture of Copper and tin?
  8. Sodium Metal that can be easily cut with a knife
  9. The impurities (sand, silt, soil, gravel, etc.) present in the ore are called gangue


(4) False
(7) False
(8) True
(9) True

Match the column



Copper-Zinc : Brass
iron and carbon: Steel
lead and tin: Solder


Fill in the blanks

  1. The minerals from which metals can be conveniently and profitably extracted are called ______
  2. _______ is the process in which a carbonate ore is heated below melting point in absence of air
  3. ______ is the process in which metal oxides are reduced to molten metal by using carbon
  4. The process of purifying impure metal to obtain pure metal is called ________
  5. _____________ is the eating up of metal by action of air, moisture on their surface
  6. ________ is the homogenous mixture of two or more metals
  7. The elements that exhibit properties of both metals and non – metals are called ____________


(1) Ores
(2) Calcination
(4)Electrolytic Refining
(6) Alloy
(7) Metalloids

Multiple Choice Questions

(1) Which of the following non-metals is a liquid?
(a) Carbon
(b) Sulphur
(c) Phosphorus
(d) Bromine


Answer is D

(2) Which of the following methods is suitable for preventing an iron frying pan from rusting?
(a) Applying grease
(b) Applying paint
(c) Applying a coating of zinc
(d) All of the above.


Answer is C

Very Short Answer type(One Marks Questions)

Question 1
Which of the following metals will melt at body temperature?
Gallium, Magnesium, Caesium, Aluminium


Gallium & Caesium

Question 2
What are amphoteric oxides? Give two examples of amphoteric oxides.


Those oxides of metals which show both acidic as well as basic behaviour in aqueous solutions are called amphoteric oxides.

Question 3
Why do ionic compounds have high melting points?


In an ionic compound there is large electrostatic force of attraction between opposite charged ions. To overcome these forces a considerable amount of energy is needed therefore ionic compounds have high melting points.

Question 4
Why are ionic compounds usually hard?
Question 5
Write the chemical equation for the reaction of hot aluminium with steam.


The balanced chemical equation showing the reaction of aluminium with steam is -
2Al (s) + 3H2O (g) -> Al2O3 (s) + 3H2 (g)

Question 6
Name two highly malleable metals.


Gold and Silver

Question 7
Why do silver ornaments lose their shine when kept for some time?


silver react with the sulphur in air and becomes silver sulphide which is black in colour so the shine is lost

Question 8
Why do we use copper and aluminium wire for transmission of electric current?


They have low resistance and ductile

Short Answer type(2 Marks Question)

Question 1
Name two metals which react violently with cold water. Write any observation you would make when such a metal is dropped into water. How would you identify the gas evolved, if any, during the reactions?


etals at the top of the reactivity series (Sodium potassium) react readily (violently) with cold water forming hydroxides with the liberation of H2, the heat evolved is sufficient for the hydrogen to catch fire.
Na(s) + 2H2O(l) ? NaOH(aq) + H2(g) + large amount of heat energy catches fire
K(s) + 2H2O(l) ? KOH(aq) + H2(g) + large amount of heat energy
The gas evolved during these reactions burns with a popping sound which confirms that the gas is hydrogen (H2).

Question 2
Why do metals not evolve hydrogen gas with nitric acid?


Hydrogen gas is not evolved when a metal reacts with nitric acid because nitric acid is a strong oxidising oxidises with the hydrogen produced to forn water and the nitric acid itself gets reduced to any of nitrogen oxide(N2O,NO,NO2).

Question 3
When calcium metal is added to water the gas evolved does not catch fire but the same gas evolved on adding sodium metal to water catches fire. Why is it so?
Question 4
A metal that exists as a liquid at room temperature is obtained by heating sulphide in the presence of air. Identify the metal and its ore and give the reaction involved.


Hg is the metal and the ore is HgS. It is called Cinnabar.
HgS + O2 ------> Hg + SO2

Question 5
Why do ionic compounds conduct electricity in molten state?
Question 6
A metal A, which is used in thermite process, when heated with oxygen gives an oxide B, which is amphoteric in nature. Identify A and B. Write down the reactions of oxide B with HCI and NaOH.
Question 7
What the constituents are of solder alloy? Which property of solder makes it suitable for welding electrical wires?
Question 8
Name a metal which is poor conductor of electricity and a non metal which is good conductor of electricity.


Tungsten and Bismuth are metals which is poor conductor of electricity
Graphite are non-metal which is good conductor of electricity

Question 9
Name two metals which are found in nature in the Free State.
Justify the statement – ‘All ores are minerals but all minerals are not ores’. Give one example which can be called both ore and mineral.
Question 10
Describe briefly the method to obtain mercury from cinnabar. Write the chemical equation for the reactions involved in the process.


Cinnabar is the main ore of mercury. Mercury is obtained from its ore by Roasting. when cinnabar is heated in air, it is first converted into mercuric oxide. Mercuric oxide is then reduced to mercury on further heating.
2HgS(s) +3 O2 (g) + Heat ? 2HgO(s) + 2SO2 (g)
2HgO(s)+Heat-> 2Hg(l)+O2(g)

The reaction of metal ‘X’ with Fe2O3 is highly exothermic and is used to join railway tracks. Identify the metal ‘X’. Write the chemical equation of the reaction.
Question 11
Name the constituents of bronze and write its two uses.


Copper with 12% time .Sometimes alluminium /nickel/zinc are also mixed
Coins & medals, Churchbell

Question 12
Name a metal/non-metal:
(a) Which makes iron hard and strong?
(b) Which is alloyed with any other metal to make an amalgam?
(c) Which is used to galvanise iron articles?
(d) Whose articles when exposed to air form a black coating?
Question 13)
An alloy has low melting point and is therefore used for electrical fuse. Name the alloy and write its constituents.


Solder ( Tin + Lead)

Question 14
Give reasons for the following:
(i) Gold and silver are used to make jewellery.
(ii) Carbonate and sulphide ores are generally converted into oxide ores prior to reduction during the process of extraction.
Question 15
Differentiate between roasting and calcinations processes giving one example of each.


Roasting is a process of converting sulphide ores into oxides by heating strongly in the presence of excess air.
Roasting : 2ZnS(s) + 3O2 (g) -> 2ZnO(s) + 2SO2 (g)
Calcination is a process of converting carbonate ores into oxides by heating strongly in limited air.
Calcination : ZnCO3 (s) -> ZnO(s) + CO2 (g).

Question 16
A substance X which is an oxide of a metal is used intensively in the cement industry. This element is present in bones also. On treatment with water it forms a solution which turns red litmus blue. Identify X and also write the chemical reactions involved.
Question 17
Why sodium is kept immersed in kerosene oil?


Sodium is high reactive element. If it is kept in open it can explosively react with oxygen to catch fire. Hence to prevent accidental damage sodium is immersed in kerosene oil

Long Answer type

Question (1)
Give reasons:
(i) Reactivity of A1 decreases if it is dipped in HNO3
(ii) Carbon cannot reduce the oxides of Na or Mg.
(iii) NaCI is not a conductor of electricity in solid state whereas it does conduct electricity in aqueous solution as well as in molten state.
(iv) Metals like Na, K, Ca and Mg are never found in their free state in nature.
Question 2
Metals replace hydrogen from dilute acids, whereas non-metals do not. Why?


Non-metals do not displace hydrogen from dilute acids is because unlike metals, non-metals do not have a tendency to lose electrons but to gain electrons. Metals have a tendency to lose electrons. These electrons, which are readily lost by reactive metals like sodium, potassium etc are accepted by hydrogen ions of the acids, reducing them to hydrogen gas (H2).

Question 3
What is meant by refining of metals? Describe the electrolytic refining of copper with a neat labeled diagram.
Question 4
An ore on heating in air produces sulphur dioxide. Which process would you suggest for its concentration? Describe briefly any two steps involved in the conversion of this concentrated ore into related metal.
Question 5
Why aluminum oxide is considered an amphoteric oxide?


Aluminium oxide is called Amphoteric oxide because it has both acidic and basic properties.
Basic property :
Al2O3 + H+ ----> Al3+ + H2O

Acidic properties:
Al2O3 + OH- + H2O----> [Al(OH)4]-

Question 6
State the property utilize in the following:
(a) Graphite in making electrodes.
(b) Electrical wires are coated with polyvinyl chloride (PVC) or a rubber like material.
(c) Metal alloys are used for making bells and strings of musical instruments.
Question 7
Explain with the help of an activity that metals conduct electricity. Draw a diagram for the same.


We need Bulb,Battery, Metal Nail and wires

(1) Connect one of bulb with nail by wire
(2) connect second end of a bulb with the wire to the battery
(3) connect battery with the metal nail by wire

We will observed Bulb will glow.
And this proves Metals conduct electricity.

Question 8
Name a metal which has very low melting point and a non-metal which has very high melting point.


Caesium and gallium metals have low melting point. Diamond a allotrope of carbon has very high melting point which is a non metal

Question 9
Write one example of each of the following:
(a) Most malleable metal and most ductile metal.
(b) The best conductor of heat and the poorest conductor of heat.
(c) A metal with highest melting point and a metal with lowest melting point.
Question 10
(a) Which metal from the following can displace zinc from zinc sulphate solution?
Lead, copper, magnesium, silver
Write the equation of the chemical reaction involved.
(b) Arrange metals Ca, Al, Cu and Au in decreasing order of reactivity.


agnesium will displace zinc from its sulphate
g(s) + ZnSO4(aq) ---> MgSO4(aq) +Zn(s)

Decreasing order of reactivity of metals:
Ca > Al > Zn > Cu > Ag > Au

Question 11
(a) A substance X, an oxide of a metal, is used extensively in the cement industry. This element is found in our bones also. On treatment with water it forms a solution which turns red litmus blue. Identify X and also write the chemical reaction involved.
(b) Choose a metal from the following metals which reacts only with hot water:
Sodium, magnesium, iron
Mention the products formed during the reaction.
Question 12
Food cans are coated with tin rather than zinc.
Give suitable reason for the following
(a)Shining surface of metals is tarnished after some time.
(b) Sodium and potassium are kept under kerosene oil.
(c) Generally no hydrogen gas is involved when metals react with dilute nitric acid
(d) Some alkali metals can be cut with a knife.
Question 13
How metals can be differentiated from non – metals on the basis of any three chemical properties?
Question 14
(a) Support your answer with chemical equations in each case. What happen when magnesium ribbon is burnt in air? What is the state of the metal oxide in the product formed?
(b) An element A forms two oxides AO and AO2.The oxide AO is neutral whereas the oxide AO2 is acidic in nature. Would you call element A a metal or non – metal?
Question 15
(a) What are the bases which are soluble in water called?
(b) Write any four uses of bases.
Question 16
When a copper wire is left in silver nitrate solution, it is observed that the solution turns bluish green.
(a) Explain the observation.
(b) Write the balanced chemical equation to represent the change taking place.
Question 17
What happens when a piece of:
(a) Aluminium metal is added to dilute hydrochloric acid.
(b) Zinc metal is added to copper sulphate solution.
(c) Silver metal is added to copper sulphate solution.
Also write balanced chemical equation, if the reaction occurs.


(a) Aluminium is more reactive than hydrogen and is placed above hydrogen in the reactivity series. Thus, when aluminium metal is added to dilute HCl, it displaces hydrogen from the acid and forms aluminium chloride and hydrogen gas. Following is the chemical equation for the reaction

2Al (s) + 6HCl (aq) -> 2AlCl3 (s) + 3H2 (g)

(b) Zn + CuSO4 -> ZnO4 + Cu

(c) Ag+ CuSO4 ->No reaction

Question 18
Write balanced chemical equation for the reaction of:
(a) aluminium when heated in air. Write the name of product.
(b) iron with steam and name the products obtained.
(c) calcium with cold water. Why does calcium start floating in water?


(a) 4Al(s)+3O2(g)-->2Al2O3(s)
product Name is - aluminium oxide

(b) Fe + H2O ---- > Fe(OH)2
Iron hydroxide

(c) Actually, when calcium reacts with water, the reaction is less vigorous and it forms calcium hydroxide with release of hydrogen gas, but the heat evolved is not sufficient for hydrogen gas to catch fire and so it sticks over the surface of calcium hydroxide and the wall of container which do not let the calcium hydroxide to sink and it continues to float on the water surface .

The reaction involved is :
Ca + 2H2O --> Ca(OH)2 + H2

Question 19
Iron displaces copper from copper sulphate solution, zinc displaces iron from iron sulphate solution and copper displaces silver from silver nitrate solution. On the basis of these reactions arrange the four metals involved in order of their reactivity. Give balanced chemical equations in each case.


The reactivity order is as follows:

The reactions are:
Fe(s) + CuSO4(aq) -> Cu(s) +FeSO4(aq)
Zn(s) +FeSO4(aq) -> Fe(s) + ZnSO4(aq)
Cu(s)+ 2AgNO3(aq) -> 2Ag(s)+Cu (NO3)2(aq)

Question 20
The atomic number of magnesium is 12 and of chlorine is 17. Show the formation of magnesium chloride by the transfer of electrons.
Question 21v
(a) Write the electron – dot structure for calcium and sulphur.
(b) Show the formation of CaS by the transfer of electrons.
(c) Name the ions present in this compound CaS.
(Atomic number of Ca = 20, S = 16)
Question 22
Write balanced chemical equations for the following reactions:
(a) Calcium carbonate on reaction with hydrochloric acid gives calcium chloride, water and carbon dioxide.
(b) Nitrogen reacts with hydrogen under pressure to form ammonia.
(c) Carbon disulphide burns in air to give carbon dioxide and sulphur dioxide.


(a) CaCO3 + 2HCl -> CaCl2 + CO2 + H2O

(b) N+ 3H2  -> 2NH3

(c) CS2 + 3O2 -> 2SO2 + CO2

Question 23
Write chemical equations for the following reactions:
(a) A piece of calcium metal is dropped in water.
(b) Steam is passed over red hot iron.
(c) Zinc sulphide is heated in air.


Ca(s) + 2H2O(l) -> Ca(OH)2 (aq) +  H2 (g)

3Fe(s) + 4H 2 O (g) -> Fe 3 O 4(s) + 4H 2 (g)

2ZnS(s) + 3O2  ->   2ZnO(s) + 2SO (g)

Question 24
Define the terms:
(i) Mineral (ii) Ore (iii) Gangue.
Question 25
What is meant by concentration of an ore? Why is it necessary to concentrate an ore before processing? Name an ore of mercury and copper.
Question 26
Differentiate between the following:
(a) Reaction of magnesium and calcium with water.
(b) Roasting and calcinations processes giving an example of each.
(c) Nature of metal and non – metal oxides with an example.
Question 27
How can sodium be obtained from sodium chloride?
Question 28
(i) Define the term ‘anode mud’. Name the electrode made of pure metal.
(ii) Give the reactions taking place at cathode and at anode during the electrolytic refining of copper.
Question 29
(a) Ores of both zinc and mercury are sulphide ores. Explain the methods used to extract these metals from their ores.
(b) Can we store concentrated solution of sodium hydroxide in a zinc container? Explain.
Question 30
If a strip of aluminium with clean surface is dipped into an aqueous solution of copper sulphate for some time, the surface of the strip becomes brown. State the reason for this. Write balanced chemical equation for the reaction.
Question 31
Which metal is more reactive between copper and iron? How can you prove it?
Question 32
Distinguish between the following:
(a) Electrolytic reduction and electrolytic refining.
(b) Mineral and ore.
(c) Alloys and amalgams.





Question 33
Name two metals which do not corrode easily. Give an example in each of the following case to support that:
(a) Corrosion of some metals is an advantage.
(b) Corrosion of a metal is a serious problem.


This Metals and Non Metals Class 10 Extra questions with answers is prepared keeping in mind the latest syllabus of CBSE . This has been designed in a way to improve the academic performance of the students. If you find mistakes , please do provide the feedback on the mail.

Also Read

Class 10 Maths Class 10 Science

Latest Updates
Synthetic Fibres and Plastics Class 8 Practice questions

Class 8 science chapter 5 extra questions and Answers

Mass Calculator

3 Fraction calculator

Garbage in Garbage out Extra Questions7