Metal and Non Metal : Practice Questions



CLICK HERE to watch second part

2 Mark questions

1. Name two solid metals and two solid non - metals along with their symbols.


2. Give reason for the following :           

(a) School bells are made up of metals.           

(b) Electrical wires are made up of copper.


3. Give reason for the following :           

(a) Sodium metal is kept immersed in kerosene.           

(b) Blue colour of copper sulphate solution disappear when some aluminium powder is a added in it.


4. Define the term 'amphoteric oxide'. Give its two examples.


5. Give reason as to why copper is used to make hot water tanks and not steel. (an alloy of iron)


6. A shiny brown coloured metal 'X' on heating in air becomes black in colour. name the black coloured compound formed  and identify 'X'.


7.  (a) Name two metals which evolve hydrogen gas with nitric acid.           

(b) Write product of any one of the metals.


8. Can we palce silver nitrate in an iron vessel ? Give reason for your answer with a balanced chemical equation.


9. Out of the two metals P and Q, P is less reactive than Q, Suggest an activity to arrange these metals in the order of their decreasing reactivity. Support your answer with a suitable chemical equation.


10. (i) Why metals like Cu, Al etc. become dull in appearance after some time ?             

(ii) Name the compound formed on the surface of copper which makes it dull.


11. Name two metals which are found in nature in the free state.


12. Justify the statement – 'All ores are minerals but all minerals are not ores'. Give one example which can be called both ore and mineral.


13. What is 'Thermite welding' ? Give balanced chemical equation of reaction involved in this process.


14. Can  we take anode made up of pure metals and cathode made up of impure metal during electro - refining ? Justify your answer.


15. Give composition of the alloy – 'brass' and 'branze'.


16. What is meant by corrosion ?             

(i) Why do aluminium sheets not corrode easily ?             

(ii) Why is copper vessel covered with a green coating in rainy season ?


17. What do you mean by 'galvanisation' ? Why it is done ?


18. Give reason why :             

(a) Electrical wires are coated with plastic.             

(b) It is necessary to paint iron grills frequently.             

(c) Aluminium is not found in native state.


19. Pure iron is soft and stretches easily when hot.             

(a) How do these property of iron change when :             

(i) small amount of carbon is mixed with it ? 

(ii) nickel and chromium are mixed with it ?             

(b) Define an alloy. How is an alloy prepared ?             

(c) An alloy has low melting point and is therefore used for electrical fuse. Name the alloy and write its constituents.

 

Solutions

1. Solid metals :  (i) Gold (Au), (ii) Silver (Ag).

Solid non - metals : (i) Carbon (C), (ii) Sulphur (S).


2. (a) Metals are sonorous, so school bells are made up of metals.           

(b) Copper is a very good conductor of electricity. So, it is used for making electrical wires.


3. (a) Sodium reacts so vigorously with air that it catches fire if kept in the open. Hence, to protect it and to prevent accidental fires, it is kept immersed in kerosene oil.

(b) Aluminium is more reactive than copper. It displaces copper from copper sulphate solution and forms aluminium sulphate, leaving copper behind. Hence, the colour changes.


4.  An oxide which reacts with acids as well as bases to produce salt and water is called amphoteric oxide.

- Examples : (i) Aluminium oxide (Al2O3), (ii) Zinc oxide (ZnO).


5. Copper and silver are the best conductors of heat. Hence, copper is used make hot water tanks and not steel.


6. Metal 'X' is copper and the black coloured substance is copper (II) oxide.


7. (a) (i) Magnesium (Mg), (ii) Manganese (Mn).           

(b) Magnesium nitrate [Mg(NO3)2]


8. No, we cannot place silver nitrate in an iron vessel because iron is more reactive than silver. It displaces silver from silver nitrate solution and forms ferrous nitrate.           

2AgN{O_3} + Fe \to Fe{\left( {N{O_3}} \right)_2} + 2Ag


9. Activity : In a test tube, a small amount of salt solution of P is taken and metal Q is added into it. Q being more reactive, displaces metal P from its salt solution.           

Chemical equation : Metal Q + Salt solution of P  \to Salt solution of Q + Metal P.


10. (i) Metals like Cu and Al become dull in appearance because of the formation of their oxides on them.             

(ii) Copper (I) oxide (Cu2O)


11. (i) Gold, (ii) Silver.


12. Examples : Minerals – Sodium chloride, magnesium chloride.             

Ore – Sulphide or oxide ores of Pb, Zn etc.


13. Thermite welding involves reaction between aluminium and iron (III) oxide to form aluminium oxide and iron, releasing large amount of heat.             

- Fe2O3 + 2Al  → 2 Fe + Al2O3 + Heat


14. No. Anode is made up of impure metal. On passing the current through the electrolyte, the pure metal from the anode dissolves into the electrolyte.


15. Brass – Cu and Zn             

Bronze – Cu and Tin


16. The surface of some metals, such as iron is corroded when they are exposed to moist air for a long period of time. This phenomenon is known as corrosion.             

(i) Aluminium does not corrode easily because on exposure to air, its surface is coated with a thin layer of aluminium oxide which is protective and non - reactive.             

(ii) It is because copper reacts with moist carbon dioxide in the air and slowly loses its shiny brown surface and gains a green coat.


17. - The process of coating a thin layer of zinc on iron articles is called galvanisation.             

- It is done to prevent corrosion.


18. (a) Electrical wires are made up of copper. Copper reacts with moist carbon dioxide in the air and slowly loses its shiny brown surface and gains a green coat. So, these are coated with plastic.     

(b) To prevent rusting, it is necessary to paint iron grills frequently.             

(c) It is because aluminium is a very reactive element.


19. (a) (i) When a small amount of carbon is mixed, the iron becomes hard and strong.             

(ii) When iron is mixed with nickel and chromium, we get stainless steel.             

(b) Homogeneous mixture of two or more metals or a metal and a non - metal is know as an alloy. It is prepared by first melting the  primary metal, and then, dissolving the other elements in it in define proportions.             

(c) Solde

 

3 Mark Questions

1.    List three properties of sodium in which it differs from the general physical properties of most metals.


2. (a) Define the term malleability and ductility.           

(b) Give and example of a metal which           

(i) is liquid at room temperature.           

(ii) can be cut with a knife.


3. Of the three metals 'A', 'B' and 'C', 'A' reacts with cold water vigorously. 'B' reacts with hot water and 'C' reacts with steam only.

Predict metals 'A', 'B' and 'C' and arrange these metals in order of increasing reactivity.


4. An element 'P' reacts vigorously with water. The product so formed, turns res litmus to blue. Write the equations of reactions of the elements 'P' with water and oxygen both. Write two uses of any one salt of element 'P'


5. Two metals P and Q do not react with water at all. They are found in earth's crust in free state. Comment on expected position of these metals with respect to hydrogen in reactivity series. Identify these metals also.


6. A, B and C are three elements which undergo chemical reactions according to the following equations :           

A2O3 + 2B →  B2O3 + 2A           

3CSO4 + 2B → B2 (SO4)3 + 3C           

3CO + 2A → A2O3 + 3C           

(a) Which element is the most reactive ?           

(b) Which element is the least reactive ?           

(c) What is the type of reactions listed above ?


7. (i) Arrange the following metals in the order of their decreasing activities :

Aluminium, Gold, Sodium, Copper.           

(ii) Give reaction of aluminium powder with manganese dioxide on heating.


8. (a) What are amphoteric oxides ?           

Choose the amphoteric oxides from amongst the following oxides :           

Na2O, ZnO, Al2O3, CO2, H2O           

(b) Why is it that the non - metals do not displace hydrogen from dilute acids ?


9. (a) Aluminium is a reactive metal but is still used for packing food articles.           

(b) Calcium starts floating when water is added to it.


10. Define the terms :           

(i) Mineral           

(ii) Ore           

(iii) Gangue.


11. Suggest the method of reduction for the following metals during their metallurgical processes. 

(i) Metal 'A' which is one of the last second or third position in reactivity series.             

(ii) Metal 'B' which  gives vigorous reaction even with water and air.             

(iii) Metal 'C' which is kept in middle of reactivity series.


12. Name two metals which are purified by electrolytic refining. Mention the anode cathode and the electrolyte used in the refining process. At which electrode would the pure metal be deposited ?


13. 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.


14. (i) Name the metal which does not stick to glass.             

(ii) Name the metal which is commonly used in thermite welding.             

(iii) What is the nature of zinc oxide.


15. (a) 'Sodium is a highly reactive metal and it cannot be obtained from its oxide by heating with carbon.' Give reason.             

(b) How can Sodium be obtained from sodium chloride ?


Q.16 (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.

 

Solutions
1. (i) Sodium is so soft that  it can be cut with a knife.           

(ii) It has low density.           

(iii) It has low melting point.


2. (a) (i) Malleability : The metal which can be hammered into thin sheet is known as malleable, e.g., gold and silver. This property of metals is known as malleability.                 

(ii) Ductility : The metal which can be drawn into thin wire is known as ductile e.g., gold and silver. This property of metals is known as ductility.           

(b) (i) Mercury   (ii) Sodium.


3. - Metal A may be sodium or potassium. They react vigorously with water.

Metal B may be magnesium, which reacts with hot water to form magnesium hydroxide.

Metal C may be aluminium, iron or zinc which reacts only with steam.           

- Increasing order of reactivity : A > B > C.


4.     Element P is calcium (Ca).         

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

- Uses of CaOCl2 :           

- Bleaching power is used for :           

(a) Bleaching cotton and linen in textile industry.           

(b) Bleaching wood pulp in paper factories.           

(c) Bleaching washed clothes in laundry.           

(d) Disinfecting drinking water to make it germ free.


5. The metals at the bottom of the activity series are the least reactive. They are found in earth's crust in free state.           

- The metals may be copper, silver or god.


6. (a) Most reactive element is 'B' as it has replaced both 'A' and 'C' from their compounds.           

(b) Element 'C' is least reactive as it has been replaced by both 'A' and 'B'           

(c) Displacement reaction.


7. (i) Sodium > Aluminium > Copper > Gold           

(ii) 4Al(s) + 3MnO2  → 3Mn (l) + 2Al2O3(s)


8. (a) - Amphoteric oxides : An oxide which reacts with acids as well as bases to produce salt and water is called amphoteric oxide.           

- Examples : (i) Aluminium oxide (Al2O3), (ii) Zinc oxide (ZnO).           

- Na2O, ZnO, Al2O3           

(b) Non - metals are less reactive than hydrogen. So, they do not displace hydrogen from dilute acids.


9. (a) (i) Aluminium is highly malleable.                 

(ii) It has high melting point.           

(b) Calcium starts floating when water is added to it because the bubbles of hydrogen gas formed stick to the surface of the metal.


10. (i) Mineral : A natural material present in earth crust in which metal occurs is called mineral. 

(ii) Ore : A mineral from which metal can be extracted profitably is known as an ore.           

(iii) Gangue : Impurities of sand and rocky material present in ore are called gangue.


11. (i) By the process of heating.             

(ii) By heating with carbon.             

(iii) By the process of roasting and calcination.


12.  - Copper, zinc.             

- Impure metal is made the made the anode and thin strip of pure metal is made the cathode. A solution of the metal salt is used as an electrolyte.             

- Pure metal from the electrolyte is deposited on the cathode.


13. A process of removing unwanted impurities like, sand, soil etc present in an ore (called gangue) is called concentration of  ore. We need to concentrate the ore so that the earthly impurities do not interfere in the process of extraction.             

Ore of mercury : Cinnebar (HgS)             

Ore of copper : Copper sulphide (Cu2S)


14. (i) Mercury             

(ii) Aluminium             

(iii) Basic.


15. (a) Sodium cannot be obtained from its oxide by heating with carbon because carbon cannot reduce the oxides of sodium.             

(b) Sodium can be obtained from sodium chloride by the process of electrolytic eduction.


16.. (i) - The insoluble impurities which settle down at the bottom of the anode are known as anode mud.                   

- Cathode             

(ii) At anode : Cu(s) → Cu 2+ (aq) + 2e               

At Cathode :  Cu 2+ (aq) + 2e  → Cu(s)

 

5 Marks Questions

1. (a) Give two points of difference between metals and non - metals.           

(b) Give the names and formulae of two non - metallic chlorides.           

(c) Which type of ions are made by metals, cations or anions and why ?


2. It is well said, 'Exceptions are everywhere'.           

Here are some general statements. Give one exception for each statement.           

(i) Metals are lustrous.           

(ii) Metals are solids at room temperature.           

(iii) Metals have high melting points.           

(iv) Non - metals are non - lustrous.           

(v) Non - metals are insulators or non - conductors of electricity.


3. Give two properties of aluminium due to which it is used in making food wrappers.


4. (a) Give one point of difference between alkali and base.           

(b) Give equation of reaction of zinc oxide with acid as  well as with base and balance it.           

(c) Name the terms used for oxides which  can react with acids as well as with bases.


5. Write chemical equation when zinc granules react with :           

(i) Sulphuric acid           

(ii) Hydrochloric acid           

(iii) Aluminium chloride           

(iv) Sodium hydroxide           

(v) Nitric acid


6. Metal 'M' reacts vigorously with water to form a compound S and a gas G. The solution of S turns red litmus blue whereas gas G, which  is lighter than air, burns with a popping sound. Metal M has low melting point and kept in kerosene.           

(a) Identify the metal M and compound S. Write their chemical name and chemical formula.       

(b) What is the nature of compound ?           

(c) Identify the gas G and mention its one use.           

(d) Write a balanced equation for the reaction which takes place when metal M reacts with water.

(e) Why this metal M cannot be kept in water ?


7. (a) Define reactivity  series of metals. Arrange the metals gold, copper, iron, zinc and magnesium in their increasing order in reactivity.           

(b) What will you observe when :           

(i) Some zinc pieces are put into copper sulphate solution ?           

(ii) Some silver pieces are put into green coloured ferrous sulphate solution


8. Describe ionic compounds on the basis of the following properties :           

(i) Strong force of attraction between positive and negative ions.           

(ii) Solubility of compounds in water.           

(iii) Electrical conductivity.


9. Identify the compounds which can conduct electricity in molten state from the following : 

MgCl2, KCl, CHCl3, Cs2, CaCl2, BCl2         

Predict the type of bonding in those compounds.


10. (a) Name the particles which are responsible for conduction of electricity in a solution. Which type of compounds give rise to these particles in solution ?             

(b) Rain water conducts electricity while distilled water not. Give reason.


11. Name the metal which             

(a) become blackish after certain time.             

(b) develops green coating on exposure to air.             

(c) does not corrode at all.             

(d) is used in making steel.             

(e) is non - lustrous.


12. A metal 'E' is stored under kerosene oil. When small piece of it is left open in the air, it catches fire. When the product formed is dissolved in water it turns red litmus blue.             

(i) Name the metal E.             

(ii) Write the chemical equation for the reaction when it is exposed to air and when the product is dissolved in water.             

(iii) Explain the process by which the metal is obtained from its molten chloride.

 

Solution

1. (a) (i) Metals are malleable whereas non - metals are non - malleable.               

(ii) Metals form basic oxides. Non - metals form acidic oxides.           

(b) (i) Hydrogen chloride (HCl)               

(ii) Phosphorus trichloride (PCl3)           

(c) Metals form cations because they have tendency to lose electrons.


2. (i) Sodium           

(ii) Mercury           

(iii) Gallium           

(iv) Iodine           

(v) Carbon.


3. (i) Aluminium is highly malleable.           

(ii) It has high melting point.


4. (a) Alkali is water soluble while base is not.           

(b) ZnO + 2HCl → ZnCl2 + H2O               

ZnO  + 2NaOH  H2O  → Na2[Zn(OH)4]           

(c) Amphoteric oxides


5. (i) Zn + H2SO4 → ZnSO4 + H2           

(ii) Zn + 2HCl → ZnCl2 + H2           

(iii) Zn + AlCl3 → No reaction           

(iv) Zn + 2NaOH → Na2ZnO2 + H2           

(v) Zn + 4HNO3 → Zn(NO3)2 + 2NO2 + 2H2O


6. (a) Metal M is sodium (Na) and compound S is sodium hydroxide (NaOH).           

(b) The nature of the compound is basic.           

(c) The gas G is hydrogen (H2). It is used as a fuel.           

(d) 2Na(s) + 2H2O(l) →2NaOH(aq) + H2(g) + Heat energy           

(e) Because it reacts violently with water and catches fire.


7. (a) - The reactivity series is a list of metals arranged in the order of the decreasing activities. 

- Gold < Copper < Iron < Zinc < Magnesium           

(b) (i) Zinc displaces copper from copper sulphate solution. The blue colour of the solution becomes colourless.               

(ii) No reaction will occur.


8. (i) Due to strong force of attraction between the positive and negative ions, ionic compounds are solids. These compound are generally brittle and break into pieces when pressure is applied.       

(ii) Ionic compounds are generally soluble in water.           

(iii) Ionic compounds in the solid state do not conduct electricity but in molten state, they do conduct electricity.


9.  - MgCl2, Kcl, CaCl2, BaCl2           

- Electrovalent bond.


10. (a) - Positive ions, negative ions                   

- Ionic compounds             

(b) Rain water contains dissolved ions, which help in conducting electricity, whereas distilled water does not contain any ion. So, it does not conduct electricity.


11. (a) Silver             

(b) Copper             

(c) Platinum             

(d) Nickel, Chromium             

(e) Sodium. 


12. (i) Sodium             

(ii) 4Na + O2 → 2Na2O                   

Na2O + H2O → 2NaOH             

(iii) Sodium is obtained from sodium chloride by the process of electrolytic reduction.       

Reactions : At cathode : Na+ + e  → Na             

At anode : 2Cl → Cl2 + 2e



6 Comments

Leave a Reply

Get FREE guidance for study-at-home!! Register
NOW