Alloys are homogeneous mixture of metal with a metal or non-metal. Which among the following alloys contain non-metal as one of its constituents?
- (a) Brass
- (b) Bronze
- (c) Amalgam
- (d) Steel
Metals and Non-metals
7 topics · about 4 hours · 8% of the paper · asked in 4 of the last papers
Topics in this chapter
- Physical properties of metals and non-metals
- How metals react with air, water and acids
- The reactivity series
- Ionic bonding and the properties of ionic compounds
- Occurrence and extraction of metals
- Refining of metals
- Corrosion and how it is prevented
Board questions from this chapter
23 questions from the CBSE papers we hold.
Which one of the following metals does not react with cold water?
- (a) Sodium
- (b) Potassium
- (c) Calcium
- (d) Magnesium
(i) Which method will be used to convert each of them to their respective metal oxides? (a) Carbonate ore (b) Sulphide ore. (ii) Write a chemical reaction to illustrate the use of aluminium for joining cracked railway tracks. (iii) During extraction of metals, electrolytic refining is used to obtain pure metals. Which material will be used as anode and cathode for the refining of copper metal by this process?
(i) Write all the reactions involved in the extraction of Zn from ZnS. (ii) Hydrogen gas is not evolved when most of the metals react with nitric acid. Give reason.
The products formed when Aluminium and Magnesium are burnt in the presence of air respectively are :
- (a) Al_3O_4 and MgO_2
- (b) Al_2O_3 and MgO
- (c) Al_3O_4 and MgO
- (d) Al_2O_3 and MgO_2
(i) Name two metals which react violently with cold water. List any three observations which a student notes when these metal are dropped in a beaker containing water. (ii) Write a test to identify the gas evolved (if any) during the reaction of these metals with water.
Reaction between two elements A and B, forms a compound C. A loses electrons and B gains electrons. Which one of the following properties will not be shown by compound C ?
- (a) It has high melting point.
- (b) It is highly soluble in water.
- (c) It has weak electrostatic forces of attraction between its oppositely charged ions.
- (d) It conducts electricity in its molten state or aqueous solution.
The formation of magnesium oxide is correctly shown in option : (four options (A)-(D) each showing an electron-dot / Lewis structure representation of Mg reacting with O to form Mg^2+ and oxide ion - see figure).
(a) "Displacement reactions also play a key role in extracting metals in the middle of the reactivity series." Justify this statement with two examples. (b) Why can metals high up in the reactivity series not be obtained by reduction of their oxides by carbon ?
The metals obtained from their molten chlorides by the process of electrolytic reduction are :
- (a) Gold and silver
- (b) Calcium and magnesium
- (c) Aluminium and silver
- (d) Sodium and iron
With the help of an activity, explain the conditions under which iron articles get rusted.
A metal and a non-metal that exists in liquid state at the room temperature are respectively:
- (a) Bromine and Mercury
- (b) Mercury and Iodine
- (c) Mercury and Bromine
- (d) Iodine and Mercury
Oxides of aluminium and zinc are:
- (a) acidic
- (b) basic
- (c) amphoteric
- (d) neutral
electrolytic refining of impure copper.
You have two beakers 'A' and 'B' containing copper sulphate solution. What would you observe after about 2 hours if you dip a strip of zinc in beaker 'A' and a strip of silver in beaker 'B'? Give reason for your observations in each case.
The metals produced by various reduction processes are not very pure; the most widely used method for refining impure metals is electrolytic refining.
What is the cathode and anode made of in the refining of copper by this process?
electrolytic refining of impure copper.
Name the solution used in the above process and write its formula.
electrolytic refining of impure copper.
How copper gets refined when electric current is passed in the electrolytic cell?
Almost all metals combine with oxygen to form metal oxides; metal oxides are generally basic but some show both basic and acidic behaviour, and different metals show different reactivities towards oxygen.
What happens when copper is heated in air? (Give the equation of the reaction involved).
metal oxides are generally basic but some show both basic and acidic behaviour.
Why are some metal oxides categorized as amphoteric? Give one example.
reactions of metal oxides with water and with a base.
Complete the following equations: (i) Na_2O(s) + H_2O(l) -> (ii) Al_2O_3 + 2NaOH ->
non-metal reacting with oxygen - internal choice for sub-part (c).
On burning Sulphur in oxygen a colourless gas is produced. (i) Write chemical equation for the reaction. (ii) Name the gas formed. (iii) State the nature of the gas. (iv) What will be the action of this on a dry litmus paper?
Assertion (A): The colour of aqueous solution of copper sulphate turns colourless when a piece of lead is added to it. Reason (R): Lead is more reactive than copper, and hence displaces copper from its salt solution. Options:
- (a) Both
- (b) and (R) are true and (R) is the correct explanation of (A).
- (c) Both
- (d) and (R) are true, but (R) is not the correct explanation of (A).
- (e) is true, but (R) is false.
- (f) is false, but (R) is true.
A metal 'X' is used in thermite process. When X is burnt in air it gives an amphoteric oxide 'Y'. 'X' and 'Y' are respectively:
- (a) Fe and Fe_2O_3
- (b) Al and Al_2O_3
- (c) Fe and Fe_3O_4
- (d) Al and Al_3O_4