CBSE Class 10 Chemistry Metals And Non Metals Worksheet Set F

METALS AND NON-METALS

Question. Copper becomes green when exposed to moist air for a long period of time due to the
(a) formation of a layer of cupric oxide on the surface of copper.
(b) formation of a layer of basic carbonate on the surface of copper.
(c) formation of a layer of cupric hydroxide on the surface of copper.
(d) none of the above.
Answer : B

Question. Which of the following pair of metals exist in their native state in nature?
(a) Ag and Au
(b) Ag and Zn
(c) Au and Hg
(d) Au and Fe
Answer : A

Question. Reaction between X and Y forms compound Z. X loses electrons and Y gains electrons. Which of the following properties is not shown by Z?
(a) Has high melting point
(b) Has low melting point
(c) Conducts electricity in molten state
(d) Occurs as solid
Answer : B

Question. Read the statements carefully.
i Metals are generally ductile but metal W is the most ductile metal.
ii Metals generally possess high melting point but metals like X have very low melting point.
iii Metals generally exist in solid state but Y exists in liquid state.
iv. Among metals, Z is the poorest conductor of heat.
Choose the right option of sequencing W, X, Y and Z.
(a) Aluminium, Sodium, Lead and Silver.
(b) Gold, caesium, Mercury and Lea(d)
(c) Copper, Zinc, Silver and Mercury.
(d) Iron, Sodium, Gold and Lea(d)
Answer : B

Question. The best conductors of heat are
(a) Silver and Copper
(b) Lead and Mercury
(c) Iron and Tin
(d) Gold and Platinum
Answer : A

Question. The colour of aqueous solution of zinc sulphate as observed in the laboratory is:
(a) green
(b) Yellow
(c) Blue
(d) Colourless
Answer : D

Question. Which one of the following properties is not generally exhibited by ionic compounds?
(a) Solubility in water
(b) Electrical conductivity in solid state
(c) High melting and boiling points
(d) Electrical conductivity in molten state
Answer : B

Question. Sodium chloride is a_________ compound
(a) Covalent
(b) Ionic
(c) Non-ionic
(d) None of these
Answer : B

Question. Which of the given metals are obtained by electrolysis of their chlorides in molten state?
(a) Na (b) Ca (c) Fe (d) Cu
(a) (a) & (d)
(b) (c) & (d)
(c) (a) & (c)
(d) (a) & (b)
Answer : D

Question. The process in which a carbonate ore is heated strongly in the absence of air to convert it into metal oxide is called________
(a) Roasting
(b) Reduction
(c) Calcination
(d) Smelting
Answer : C

Case Study Based Questions

1) Metals react with non-metals by losing or gaining electrons. They have a give-andtake relation between them. Ionic compounds are usually solid and hard in nature. They are generally soluble in water and insoluble in solvent like petrol, kerosene, et(c) The melting and boiling points of electrovalent compounds are high. In order to change the physical state of the electrovalent compounds (from solid to liquid to gas) , a high temperature is needed to overcome the attractive forces.

i) Which of the following properties is not generally exhibited ionic compounds?
(a) Electrical conductivity in molten state
(b) Electrical conductivity in solid state
(c) High melting and boiling points
(d) Solubility in water
Answer : B

ii) Ionic compounds are usually solid and hard in nature. This is due to
(a) Strong forces of attraction between the oppositely charged ions.
(b) Weak forces of attraction between the oppositely charged ions.
(c) Strong forces of attraction between the same charged ions.
(d) Weak forces of attraction between the similarly charged ions.
Answer : A

iii) Transfer of one or more valence electrons from a metal to nonmetal takes place in case of
(a) Chemical bonding
(b) molecular bonding
(c) ionic bonding
(d) covalent bonding
Answer : C

iv) The atomic number of four elements A, B, C, D is 6, 8, 10 and 12 respectively. The two elements which can react to form ionic compounds are:
(a) A and B
(b) C and D
(c) B and D
(d) A and C
Answer : C

2) Alloying is a very good method of improving the properties of a metal. This gives the desired properties of the metal. For example, iron is the most widely used metal. But it is never used in its pure state. This is because pure iron is very soft and stretches easily when hot. But, if it is mixed with a small amount of carbon (about 0.05%) , it becomes hard and strong. When iron is mixed with nickel and chromium, we get stainless steel, which is hard and does not rust. Thus, if iron is mixed with some other substance, its properties change. In fact, the properties of any metal can be changed, if it is mixed with some other substance. The substance added may be a metal or a non-metal

i) Which among the following alloys contain non-metal as one of its constituents?
(a) Brass
(b) Bronze
(c) Amalgam
(d) Steel
Answer : D

ii) An alloy can be one of the following types:
(a) Homogenous
(b) Heterogeneous
(c) Intermetallic
(d) All of the above
Answer : A

iii) By adding silicon to stainless steel which of the following property is enhanced?
(a) Resistance to corrosion
(b) Electrical characteristics
(c) Ductility
(d) Magnetic property
Answer : B

iv) Which of the following alloy(s) contain mercury as one of its constituents?
(a) Zinc amalgam
(b) Alnico
(c) Solder
(d) Bronze
Answer : A

1. Write one example of each of the following:

(a) The most malleable metal and the 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.

2. A metal M does not liberate hydrogen from acids but reacts with oxygen to give a black colour product. Identify M and the black coloured product and also explain the reaction of M with oxygen.

3. A substance X which is an oxide of a metal is used intensively in the cement industry. This substance 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.

4. A solution of CuSO4 is kept in an iron pot. After few days the iron pot was found to have a number of holes in it. Explain the reason in terms of reactivity. Write the equation of the reaction involved.

5. Show the formation of Na2O and MgO by the transfer of electrons.

6. Generally, when metals are treated with mineral acids, hydrogen gas is liberated but when metals are treated with HNO3 , hydrogen gas is not liberated, why?

7. Compound X and Aluminium are used to join railway tracks.

a) Identify the compound X.

b) Name the reaction.

c) Write down the reaction.

8. Explain the following by giving examples

a) How metal oxides react with acids?

b) How non- metal oxides react with base?

9. Give reasons:

a) Carbon cannot reduce the oxides of Na or Mg.

b) NaCl is not a conductor of electricity in solid state.

c) Iron articles are galvanized.

d) Metals like Na, K, Ca and Mg are never found in their free state in nature.

10. a) Describe an activity to show the conditions needed for iron nails to rust.

b) Why do we apply paint on iron articles?

11. Give reasons:

a) The oxides of metal like Na, Mg and Ca cannot be reduced by carbon.

b) Aluminum containers used to transport nitric acid

c) Molten sodium chloride conducts electricity whereas solid NaCl will not.

d) The galvanized iron article is protected against rusting even if the zinc layer is broken.

e) An iron knife kept dipped in a blue copper sulphate solution colour of solution changes to light green.

f) Articles made of Aluminum do not corrode even though aluminum is an active metal.

12. (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.

13. A metal „X‟ displaces metal „Y‟ from Y2(SO4)3 (aq).Which metal is more reactive „X‟ or „Y‟?

14. 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.

15. 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.

16. Define a) Calcination and b) Roasting. Give an example for each.

17. Why should the metal sulphides and carbonates be converted to metal oxides in the process of extraction of metal from them?

18. How does the term “Ore” differ from “Mineral”? Give an example.

19. A metal that exists as liquid at room temperature is obtained by heating its sulphide in the presence of air. Identify the metal and its ore and give the reaction involved.

20. Given below are the steps for extraction of copper from its ore. Write the reactions involved.

a) Roasting of copper(I) sulphide.

b) Reduction of copper(I)oxide with copper(I) sulphide.

c) Electrolytic refining. Draw a neat labelled diagram for electrolytic refining

21. During extraction of metals, electrolytic refining is used to obtain pure metals.

a) Which material will be used as cathode and anode for the refining of pure silver metal by this process?

b) Suggest a suitable electrolyte.

c) In this electrolytic cell, where do we get pure silver after passing electric current?

22. What are the constituents of solder alloy? Which property of solder makes it suitable for welding electric wires?

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