The questions of chapter metals and non metals all in one place to access. This question bank make the students useful to prepare for the 10th board exams.
2. 1. Why is sodium kept immersed in kerosene oil?
Ans. Sodium reacts so vigorously with oxygen that it catches fire when kept in the opens. Hence, to protect accidental fires, it is kept
immersed in kerosene oil because it neither reacts nor dissolves in kerosene.
2. Write equations for the reactions of
(i) iron with steam
(ii) calcium and potassium with water
Solution: (i) Iron reacts with steam to form a magnetic oxide of Fe with the liberation of H2.
3Fe(s) + 4H2O(g) → Fe3O4(s) + 4H2(g)
(ii) Calcium reacts with water to form calcium hydroxide and hydrogen.
Ca(s) + 2H2O(I) → Ca(OH)2(aq) + H2(g)
Potassium reacts with cold water violently immediately with evolution of H2 which catches fire.
2K(s) + 2H2O(I) → 2KOH(aq) + 2H2(g)
3. 3. Samples of four metals A, B, C and D were taken and added to the following solution one by one. The results obtained have been tabulated as
follows
Use the Table above to answer the following questions about metals A, B, C and D.
1. Which is the most reactive metal?
2. What would you observe if B is added to a solution of Copper (II) sulphate?
3. Arrange the metals A, B, C and D in the order of decreasing reactivity.
Solution:
(i) Metal B is the most reactive as it gives displacement reaction with iron (II) sulphate.
Metal Iron(II) sulphate Copper(II) sulphate Zinc sulphate Silver Nitrate
A No reaction Displacement – –
B Displacement – – –
C No reaction No reaction No reaction Displacement
D No reaction No reaction No reaction No reaction
4. (ii) When metal B is added to copper (II) sulphate solution, a displacement reaction will take place because of which the blue colour of copper (II)
sulphate solution will fade and a red-brown deposit of copper will be formed on metal B.
(iii)Metal B is the most reactive because it displaces iron from its salt solution. Metal A is less reactive because it displaces copper from its salt
solution. Metal C is still less reactive because it can displace only silver from its salt solution and metal D is the least reactive because it cannot
displace any metal from its salt solution. Hence, the decreasing order of reactivity of the metals is B > A > C > D.
4. Which gas is produced when dilute hydrochloric acid is added to a reactive metal? Write the chemical reaction when iron reacts with dilute H2SO4.
Solution: Hydrogen gas is liberated when dilute HCl is added to a reactive metal.
Fe(s) + H2SO4(aq) → FeSO4(aq) + H2(g)
5. What would you observe when zinc is added to a solution of iron (II) sulphate? Write the chemical reaction that takes place.
Solution: Zinc is more reactive (more electropositive) than iron. Therefore Zinc displaces Iron from its salt solution. The colour of ferrous sulphate is
pale green, which turns colourless.
FeSO4 + Zn → ZnSO4 + Fe(s)
Light green Zinc
sulphate(Colourless)
6. (i) Write the electron-dot structures for sodium, oxygen and magnesium.
(ii) Show the formation of Na2O and MgO by the transfer of electrons.
(iii)What are the ions present in these compounds?
Solution:
5. ( ii)
(iii) Ions present in Na2O are Na+ and O2-
Ions present in MgO are Mg2+ and O2-
7.Why do ionic compounds have high melting points?
Ans. There are strong forces of attraction between oppositely charged ions in ionic compounds. Considerable amount of energy is
required to break strong inter-ionic force of attraction. Therefore, they have high melting points.
8. What chemical process is used for obtaining a metal from its oxide?
Reduction method is used to obtain metal from its oxide. Ex: Zinc oxide is reduced to metallic zinc by Heating with carbon.
ZnO + C → Zn + CO
Ex: Lead oxide is reduced to lead by heating with carbon
PbO +C → Pb + CO
6. 9. Metallic oxides of zinc, magnesium and copper were heated with the following metals.
Solution:
A more reactive metal can displace a less reactive metal from its oxide. Among Zinc, Magnesium, and Copper metals, magnesium is the most reactive,
copper is the least reactive metal and zinc is less reactive .The displacement reaction will take place in the following cases
7. 10. You are given a hammer, a battery, a bulb, wires and a switch.
(a) How could you use them to distinguish between samples of metals and non-metals?
(b) Assess the usefulness of these tests in distinguishing between metals and nonmetals.
Solution:
1. Metals are malleable and can be easily drawn into sheets by hitting with hammer. On the other hand if we beat non-metals they break down and
they cannot be drawn into sheets as they are non-malleable. Metals of good conductors of electricity hence they make bulb when you connect
metals with a battery, wire and bulb. Similarly If non-metals are bad conductors of electricity chance they fail to lit up the bulb on connecting
with wire and battery.
2. These experiments can be helpful to demonstrate the malleability and electric conductivity of the metals and non-metals
11. What are amphoteric oxides? Give two examples of amphoteric oxides
Solution: Oxides that react with both acids and bases to form salt and water are known as amphoteric oxides. Examples: ZnO and Al2O3.
Amphoteric oxides are the one which reacts with both acids and bases to form salt and water. Examples: Lead oxide – ZnO and Aluminium oxide –
Al2O3.
12.. Name two metals which will displace hydrogen from dilute acids, and two metals which will not.
Solution: Zinc (Zn) and Magnesium (Mg) are the two metals which will displace Hydrogen from dilute acids as they are very reactive metals. Gold (Au)
and Silver (Ag) are the metals which will not replace Hydrogen from dilute acids as these metals are less reactive.
13. In the electrolytic refining of a metal M, what would you take as the anode, the cathode and the electrolyte?
Solution: In the process of electrolytic refining of metal called ‘M’, An impure and thick block of metal M. is considered as anode, Thin strip or wire of
pure metal M is taken as anode A suitable salt solution of metal M is considered as the electrolyte.
8. 9. Pratyush took sulphur powder on a spatula and heated it. He collected the gas evolved by inverting a test tube over it, as shown in figure below.
(a) What will be the action of gas on
(i) dry litmus paper?
(ii) moist litmus paper?
(b) Write a balanced chemical equation for the reaction taking place.
Solution: a) When sulphur powder is burnt in the air sulphur-dioxide is formed.
(i) Sulphur-dioxide does not have any effect on dry litmus paper.
(ii) Sulphur-dioxide turn the moist litmus paper from blue to red as contact of SO2 with water turns to sulfurous acid.
(b) S(s) + O2(g) → SO2(g)
SO2(g) + H2O →H2SO3
10. State two ways to prevent the rusting of iron.
Solution:The two ways to prevent the rusting of iron are as follows:-
1. Oiling, Painting or greasing: - By applying a layer of paint or grease on iron object,
2. the surface of iron object won’t come in contact with air and moisture.
3. Galvanization: - Galvanisation is a method of protecting steel and iron from rusting by coating them with a thin layer of zinc.
4. The galvanised article is protected against rusting even if the zinc coating is broken.
11. What type of oxides are formed when nonmetals combine with oxygen?
Solution: When non-metals combine with oxygen it forms either acidic or neutral oxides. Ex: SO2, NO2is an acidic oxide; CO is a neutral oxide.
9. 12. Give reasons
(a) Platinum, gold and silver are used to make jewellery.
(b) Sodium, potassium and lithium are stored under oil.
(c) Aluminium is a highly reactive metal, yet it is used to make utensils for cooking.
(d) Carbonate and sulphide ores are usually converted into oxides during the process of extraction
1. Platinum, gold and silver are used to make jewellery for these metals are very less reactive hence they are not affected by air, water or most
chemicals. These metals have a lot of lustre and they are malleable and ductile in nature.
2. Sodium, potassium and lithium readily reacts with water to produce a lot of heat. As a result Hydrogen evolved in the reaction results in fire. On
exposure to water they react with moisture (water droplets) present in the atmosphere, In order to prevent contact with water hence these
metals are stored under oil.
3. Though aluminium is a highly reactive metal, it is resistant to corrosion. This is because aluminium reacts with oxygen present in air to
form a thin layer of aluminium oxide. This oxide layer is very stable and prevents further reaction of aluminium with oxygen. Also, it is light
in weight and a good conductor of heat. Hence, it is used to make cooking utensils.
4. Carbonate and sulphide ores are usually converted into oxides during the process of extraction because metals can be easily extracted
from their oxides rather than from their carbonates and sulphides.
13. You must have seen tarnished copper vessels being cleaned with lemon or tamarind juice. Explain why these sour substances are effective
in cleaning the vessels.
Answer:
Copper reacts with moist carbon dioxide in air to form a layer of basic copper carbonate on its surface.The sour substances such as lemon or
tamarind juice contain acids. These acids dissolve the coating of copper oxide or basic copper carbonate present on the surface of tarnished
copper vessels and makes them shining red-brown again
.
10. 14. A man went door to door posing as a goldsmith. He promised to bring back the glitter of old and dull gold ornaments. An unsuspecting lady gave a
set of gold bangles to him which he dipped in a particular solution. The bangles sparkled like new but their weight was reduced drastically. The lady
was upset but after a futile argument the man beat a hasty retreat. Can you play the detective to find out the nature of the solution he had used?
Solution: Goldsmith used the solution called Aqua regia which is called as royal water in Latin. . It is the mixture of concentrated Hydrochloric acid and
concentrated nitric acid in the ratio of 3:1. Aqua regia is capable of dissolving noble metals like gold and platinum. When upper-layer of dull gold
ornament is dissolved they lose their weight.
15.Give reasons why copper is used to make hot water tanks and not steel (an alloy of iron).
Answer:
(i) Copper is a better conductor of heat than steel.
(ii) Copper does not corrode easily. But steel corrodes easily.
(iii) Copper does not react with water at any temperature, whereas iron reacts with water on heating.
11. One Marks Questions
● Give name for a molten metal that catches fire in chlorine gas and gives off white fumes?
● Which metals do not corrode easily?
● What are alloys?
● Give name for a metal that forms two types of oxides and rusts in moisture; write their formulae also
● Name two metals which can displace hydrogen from dilute HCL.
● Give name for a metal used in hot water systems
● Metals replace hydrogen from acid, whereas non-metals do not. Why?
● Are metals electronegative or electropositive?
● Give name for a metal used in long distance cables wires
● Give name for a metal added to gold to harden it
● Name the metal which occurs below copper in the reactivity series. Also name the metal that lies just above hydrogen in the
reactivity series
● Name a metal used in structural engineering
● Name a metal used as fuse wire
● Name a brittle metal, which is used to galvanize iron
● Name a non-metal which is hard and has high melting point.
● Name a metal whose chloride and sulphate salts are both insoluble
● Name a metallic chloride that is soluble in hot water but insoluble in cold water.
● Arrange the following metals in the decreasing order of chemical reactivity; placing the most active first. Cu, Mg, Fe, Na, Ca,
Zn.
● Name the anode, the cathode and the electrolyte used in the electrolytic refining of impure copper.
● Mention one physical property each of a metal and a non metal which is exceptional to their general properties.
12. Answers
1. Sodium
2. Noble metals such as gold and platinum do not corrode easily
. 3. Alloys are homogenous mixture of elements where one elements is metal and another element can be metal or nonmetal.
4. The metal that forms two types of its oxide and rust in moisture is iron. The formulas of its oxides are : FeO;Fe2O3
5. Iron and Aluminium
6. Copper
7. Metals have the tendency to loose electron i.e they are electron donor.Now Hydrogen is also electron donor,So That is why metals displace hydrogen
from dilute Non-Metals have the tendency to gain electron i.e electron acceptor ,so they don't replace hydrogen
8. Metals are electropositive elements because they can form positive ions by losing electrons
9. Copper
10. Copper
11. Mercury is just below copper and lead is just above hydrogen
12. Iron
13. Copper, Silver , Tin-lead alloy are used in making fuse
14. Zinc
15. Lead
16. Lead chloride
17. Na > Ca > Mg > Zn > Fe > Cu (least active).
18. Anode: The anode used for this process is made up impure.
Cathode: The cathode used for the electrolysis is pure copper sheets.
Electrolyte: Copper sulphate solution is used as an electrolyte in this process
19.Mercury is a metal which is liquid at room temperature. Iodine is a non-metal which is lustrous
13. Two Marks Questions
● Q 1.A copper plate was dipped in AgNO3 solution. After certain time silver from the solution was deposited on the copper
plate. State the reason why it happened. Give the chemical equation of the reaction involved.
Ans. When copper is dipped in silver nitrate , copper being more reactive than silver, displaces silver from it's solution to form copper nitrate.
The black layer is silver.
The solution is copper nitrate ( blue).
Cu + AgNO3 -------> Cu(NO3)2 + Ag.
● Q 2.An element X on reacting with oxygen forms an oxide X2O. this oxide dissolves in water and turns blue litmus red.
Ans. X is a metal like Na or K. Sodium combines with oxygen, forms sodium oxide (Na2O). Sodium oxide dissolves in water and
forms an alkali, sodium hydroxide (NaOH). In sodium hydroxide, red litmus turns blue.
14. Q 3. What is the behavior of magnesium when I is heated and steam is passed over it? Represent the equation.
Ans: When steam is passed over heated magnesium a reaction takes place where a white powder magnesium oxide is formed along with
hydrogen. Magnesium will burn with a bright white flame in steam if previously ignited in air.
Q 4 A zinc rod was kept in a glass container having CuSO4 solution. On examining, it was found that the blue color of the solution had faded.
After few days when the zinc rod was taken out of the solution, a number of small holes were noticed in it. State the reason and give equation
of chemical reaction involved.
Ans. Zinc metal is more reactive than copper. Some of the zinc metal of zinc plate dissolves and displaces copper from copper sulphate
solution. ... Blue colour of copper sulphate solution gets lighter and lighter due to the formation of colourless zinc sulphate solution.
Q 5. What is gangue and what is concentration?
Ans. The unwanted impurities present in an ore such as sand etc is known as gangue. The removal of these impurities is known as
concentration of ore.
Q 6.Lemon or tamarind juice are effective in cleaning tarnished copper vessels.
Ans: In tarnished copper vessel there is layer formed due to corrosion which is basic in nature which is dissolved in the lemon or tamarind
juice which are acidic in nature ( Neutralisation reaction). Thus the vessel get thoroughly cleaned.
15. Four marks question
Question 1
(a) The following reactions are observed to occur:
(i) CuSO4 + Zn -> ZnSO4 + Cu
(ii) 3 ZnSO4 + 2Al -> Al2(SO4)3 + 3Zn
(iii) 2AgNO3 + Cu -> Cu(NO3)2 + 2Ag
Arrange Cu, Zn, Al and Ag in decreasing order of their reactivity.
(b) Write one example each of decomposition reaction carried out with the help of:
(i) Electricity (ii) Sunlight.
Answer: Al>Zn>Cu>Ag
Explanation:
Al is most reactive and Ag is least reactive element
(b) (i) Electricity H2O—-> H2+O2
(ii) Heat FeSO4—> Fe2O3+SO2+SO3
(iii)Light AgCl—-> Ag+Cl2
Question 2
Write the names and symbols of two most reactive metals. Explain by drawing electronic structure how any one of them reacts with
a halogen. Explain any two physical properties of the compound formed.
Answer : The most reactive metals are POTASSIUM (K) and SODIUM (Na) placed at the top of reactivity series.it will form an ionic bond
with halogens since they are metals, they lose their electron and will gain positive charge.
1) It is a white crystalline salt.
2) The compound is transparent over a wide range of wavelength.
3) Are inert to organic chemicals and many acids.
16. Question 3
In the formation of a compound XY2, atom X donates one electron to each Y atom. Show the electron dot structure of X, Y and the
formation of XY2. What is the nature of bond in XY2? Write any three properties of compound XY2. The electronic configurations of
the elements X and Y are as follows:
X - 2, 8, 2
Y - 2, 7
Ans. Nature of bond : Ionic bond
Properties:
1) It is a white crystalline salt.
2) The compound is transparent over a wide range of wavelength.
3) Are inert to organic chemicals and many acids.
Question 4
Explain why a salt which does not conduct electricity in the solid state but becomes a good conductor in molten state?
Ans. 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.
17. Question 5
Give reasons why:
(i) Ionic compounds have high melting and boiling points.
(ii) Ionic compounds are soluble in water.
(iii)Ionic compounds are solid and somewhat hard.
(iv)Ionic compounds conduct electricity in molten state.
Ans.
(i) Ionic compounds have high melting and boiling points because there is a strong electrostatic force of attraction between the oppositely
charged ions and hence a large amount of energy is required to break the strong bonding force between ions.
(ii)Most ionic compounds are soluble in water. Polar water molecules have a strong attraction for charged ions and the charged ions become
solvated as they dissociate into water and ionic compounds are soluble in water.
(iii). Ionic compounds are usually hard because they r held together by strong electrostatic forces of attraction. Therefore the oppositely
charged ions pack tightly with each other and form a crystalline structure which is very hard to break down.
(iv) Ionic compounds conduct electricity when molten (liquid) or in aqueous solution (dissolved in water), because their ions are free to move
from place to place. Ionic compounds cannot conduct electricity when solid, as their ions are held in fixed positions and cannot move.
