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CBSE Questions for Class 10 Chemistry Metals And Non Metals Quiz 2 - MCQExams.com
CBSE
Class 10 Chemistry
Metals And Non Metals
Quiz 2
The conduction of electricity through a solution involves the movement of_________ particles.
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neutral
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charged
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fixed
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none of these
Explanation
The aqueous solution of ionic compounds contains charged particles and these particles or ions help in the conduction of electricity. Thus, the correct option is $$B$$
During the formation of ionic bond ________transfer takes place from one atom to the others.
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electron
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proton
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neutron
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None of these
Explanation
The compounds formed by the transfer of electrons from a metal to a non-metal are known as ionic compounds or electrovalent compounds.
Thus, option $$A$$ is correct.
Which of the following metals are refined by electrolytic refining?
(i)$$Au$$
(ii)$$Cu$$
(iii)$$Na$$
(iv)$$K$$
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(i) and (ii)
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(i) and (iii)
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(ii) and (iii)
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(iii) and (iv)
Explanation
The metals produced by various reduction processes are not very pure. They contain impurities, which must be removed to obtain pure metals. The most widely used method for refining impure metals is electrolytic refining. Many metals, such as copper and silver are refined electrolytically.
Hence the correct option is A.
The state in which $$NaCl$$ is a bad conductor of electricity is _________ and the state in which $$NaCl$$ is a good conductor of electricity is __________.
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solid, vapour
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vapour, molten
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molten, solid
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solid, molten
Explanation
$$NaCl$$ is a bad conductor of electricity in the solid-state as there are no free ions.
In the molten state, the ions are free to move around and therefore, can conduct electricity.
Hence, option $$D$$ is correct.
Generally, pure metals react with acids to give salt and hydrogen gas. Which of the following acids does not give hydrogen gas on reacting with metals (except $$Mn$$ and $$Mg$$)?
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$$H_{2}SO_{4}$$
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$$HCl$$
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$$HNO_{3}$$
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All of the above
Explanation
Some of the metals react with dilute acid, forming metal salt and hydrogen, while a few do not react with dilute acids.
Hydrogen gas is not evolved when a metal reacts with nitric acid. It is because $$HNO_3$$ is a strong oxidizing agent. It oxidises the $$H_2$$ produced to water and itself gets reduced to any of the nitrogen oxides ($$N_2O$$, $$NO$$, $$NO_2$$).
What happens when calcium is treated with water?
(i) It does not react with water
(ii) It reacts violently with water
(iii) It reacts less violently with water
(iv) Bubbles of hydrogen gas formed stick to the surface of calcium
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(i) and (iv)
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(ii) and (iii)
0%
(i) and (ii)
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(iii) and (iv)
Explanation
In general, metals form a metal oxide and hydrogen gas and this metal oxide when soluble in water dissolve further forming a metal hydroxide. But some metals form metal hydroxide directly.
In the case of calcium, the reaction with water is less violent and hydrogen starts floating on water and bubbles of hydrogen gas will stick to the metal surface.
$$ Ca + 2H_2O \rightarrow Ca(OH)_2+ H_2$$
In an ionic compound, cations and anions are held together by:
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gravitational forces
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electrostatic forces
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magnetic forces
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frictional forces
Explanation
Ionic compounds are solids held by the strong forces of attraction called electrostatic forces between the positive and negative ions (i.e, cations and anions). Thus, option $$B$$ is correct.
Which of the following is not a property of ionic
compounds?
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They are solids.
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They have low melting points.
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They are good conductors in molten state.
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They are soluble in water
Explanation
Ionic compounds have high melting and boiling points. This is because a considerable amount of energy is required to break the strong inter-ionic attraction.
Hence, the correct option is $$B$$.
Which one of the following four metals would be displaced from the solution of its salts by other three metals?
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$$Mg$$
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$$Ag$$
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$$Zn$$
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$$Cu$$
Explanation
In a displacement reaction, a more reactive metal of the activity series can displace a less reactive one in its salt solution.
Reactivity order is:
$$Mg> Zn> Cu> Ag.$$
Thus, we see that Ag is least reactive and of the given
four metals, Ag would be displaced from the solution of its salts by the other three metals.
Which of the following conducts electricity?
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Crystalline NaCl
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Molten NaCl
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Molten sulphur
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Diamond
Explanation
Ionic compounds in the solid state do not conduct electricity because movement of ions in the solid is not possible due to their rigid structure. But ionic compounds conduct electricity in the molten state. This is possible in the molten state since the elecrostatic forces of attraction between the oppositely charged ions are overcome due to the heat. Thus, the ions move freely and conduct electricity.
Molten sulphur and diamond don't conduct electricity as they are non-metals.
Hence, correct option is $$B$$
A metal $$M$$ does not liberate hydrogen from dilute hydrochloric acid but reacts with oxygen to give a black coloured product. Identify the black coloured product:
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$$MgO$$
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$$CuO$$
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$$FeO$$
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$$ZnO$$
Explanation
The metal $$M$$ is copper $$(Cu)$$ which reacts with oxygen when heated in the air to form black coloured copper(ll) oxide. The reaction can be written as:
$$2Cu + O_{2} \rightarrow 2CuO$$
Copper is present below hydrogen in the reactivity series of metals. So, it does not react with dilute acids like hydrochloric acid or sulfuric acid.
Which of the following can undergo a chemical reaction?
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$$MgSO_{4} + Fe$$
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$$ZnSO_{4} + Fe$$
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$$MgSO_{4} + Pb$$
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$$CuSO_{4} + Fe$$
Explanation
The Reactivity series is an arrangement of metals in the order of decreasing reactivities. We can infer that a more reactive metal displaces a less reactive metal from a solution of its salt.
$$K>Na>Ca>Mg> Al>Zn> Fe>Pb>H>Cu>Hg>Ag>Au$$
From the reactivity series, it is clear that $$Fe$$ is more reactive than $$Cu$$ and can replace $$Cu$$. But in the case of $$Mg$$ and $$Zn$$, we find that they are more reactive than $$Fe$$ and same in the case of $$Mg$$ and $$Pb$$ where $$Mg$$ is more reactive than $$Pb$$.
Hence, the reaction of $$CuSO_4$$ and $$Fe$$ is possible.
A metal that exists as a liquid at room temperature is obtained by heating its sulphide in the presence of air. Identify the metal.
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$$Hg$$
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$$I$$
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$$Cl$$
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$$Br$$
Explanation
Metals low in activity series can be obtained by reducing their sulphides or oxides by heating. Mercury is the only metal that exists as a liquid at room temperature. It can be obtained by heating cinnabar ($$HgS$$), the sulphide ore of mercury.
The reactions are as follows :
$$2HgS+3{ O }_{ 2 }\xrightarrow { heat } 2HgO+2S{ O }_{ 2 }\\ 2HgO\xrightarrow { heat } 2Hg+{ O }_{ 2 }$$
Option A is correct.
$$Fe_{x}O_{3}(s) + 2Al(s) \rightarrow 2Fe(l) + Al_{2}O_{y}(s) + Heat$$
What are the values of $$x$$ and $$y$$?
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$$ x = 2 , y = 3 $$
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$$ x = 3 , y =2 $$
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$$ x = 2 , y = 2 $$
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$$ x = 3 , y = 3 $$
Explanation
When aluminium replaces iron in a reaction, a lot of heat is evolved which is used to join railway tracks or cracked machine parts.
The reaction is called thermite reaction and can be balanced as:
$$Fe_{2}O_{3} + 2Al \rightarrow 2Fe + Al_{2}O_{3} + heat$$
During electrolytic refining of zinc, pure zinc gets:
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deposited at cathode
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deposited at anode
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deposited at cathode as well at anode
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remains in the solution
Explanation
In the electrolytic refining process, the impure metal is made the anode and a thin strip of pure metal is made the cathode.
A solution of the metal salt is used as an electrolyte.
On passing the current through the electrolyte, the pure metal from the anode dissolves into the electrolyte.
An equivalent amount of pure metal is deposited on the cathode.
What happens when a piece of aluminium metal is added to dilute hydrochloric acid?
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Aluminium displaces hydrogen
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Aluminium chloride is formed along with dilute hydrochloric acid
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Hydrogen gas is evolved
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No reaction
Explanation
The reactivity series follows the order :
A
l
>
Z
n
>
F
e
>
P
b
>
H
>
C
u
Thus, a
luminium being more reactive than hydrogen, displaces the latter in hydrochloric acid $$(HCl)$$ to form aluminium chloride ($$AlCl_{3}$$) and releases $$H_2$$ gas
$$2Al(s) + 6HCl(aq) \rightarrow 2AlCl_{3}(aq) + 3H_{2}(g)$$
Zinc granules give $$H_2$$ gas when treated with dilute solution of:
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$$H_{2}SO_{4}$$
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$$HCl$$
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$$NaOH$$
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all of these
Explanation
i) Zinc reacts with dilute sulphuric acid($$H_{2}SO_{4}$$) to form zinc sulphate ($$ZnSO_{4}$$) and hydrogen($$H_{2}$$) gas.
$$ Zn(s) + H_{2}SO_{4}(aq) \rightarrow ZnSO_{4}(aq) + H_{2}(g)$$
ii) Zinc reacts with hydrochloric acid to form zinc chloride($$ ZnCl_{2}$$) and hydrogen($$ H_{2}$$) gas.
$$ Zn(s) + 2HCl(aq) \rightarrow ZnCl_{2}(aq) + H_{2}(g)$$
iii) Zinc reacts with sodium hydroxide to form sodium zincate($$Na_{2}ZnO_{2}$$) and hydrogen($$H_{2}$$).
$$Zn(s) + 2NaOH(aq) \rightarrow Na_{2}ZnO_{2}(aq) + H_{2}(g)$$
What happens when a piece of silver metal is added to the copper sulfate solution?
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Silver sulfate is formed
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Silver displaces copper sulfate
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Oxygen gas is evolved
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No reaction
Explanation
The reactivity series follows the order:
$$Cu>Hg>Au>Ag$$
Thus,
When silver $$(Ag)$$ metal is added to copper sulfate ($$CuSO_{4}$$) solution, no reaction takes place as silver is less reactive than copper so it can not displace copper from its solution.
$$Ag + CuSO_{4} \rightarrow $$ no reaction
A list of common metals arranged in order of their decreasing reactivity is known as:
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activity series
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reactivity series
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conductivity series
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both $$A$$ and $$B$$
Explanation
An activity or reactivity series is a list of substances ranked in order of relative reactivity formed after displacement experiments. The most active metals are at the top of the table and least reactive at the bottom of the table.
Metals generally react with dilute acids to produce hydrogen gas. Which one of the following metals does not react with dilute hydrochloric acid?
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Magnesium
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Aluminium
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Iron
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Copper
Explanation
In the case of copper, no bubbles are seen and the temperature also remains unchanged. This shows that copper does not react with dilute HCl.
Magnesium ribbon on burning in air produces:
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magnesium oxide, water and light
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magnesium oxide and heat
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magnesium oxide, heat and light
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magnesium oxide, water and heat
Explanation
When a piece of magnesium ribbon is ignited, light and heat are produced.
Magnesium reacts with oxygen to form a compound called magnesium oxide.
The reaction is as follows:
$$2Mg + O_2 \rightarrow 2MgO + \text{heat} + \text{light}$$
Hence, the correct option is $$\text{C}$$
The metal which produces hydrogen gas on reaction with dilute hydrochloric acid as well as sodium hydroxide solution is:
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copper
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iron
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aluminium
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sodium
Explanation
$$\bullet$$ Metals that react with both acid and base are called amphoteric metals. These reactions produce Hydrogen.
Examples - zinc, tin, lead, aluminum, and beryllium.
$$\bullet$$ Since aluminum is an amphoteric metal it can react with both dilute hydrochloric acid as well as sodium hydroxides solution
Respective reactions are :
(i)Reaction of Aluminium with NaOH (base)
$$2 \mathrm{Al}+2 \mathrm{NaOH}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{NaAlO}_{2}+3 \mathrm{H}_{2} $$
(ii)Reaction of Aluminium with HCl (Acid)
$$2 \mathrm{Al}+6 \mathrm{HCl} \rightarrow 2 \mathrm{AlCl}_{3}+3 \mathrm{H}_{2}$$
In electrolytic refining, impure metal is used as anode.
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True
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False
Explanation
In the electrolytic refining process, the impure metal is made the anode and a thin strip of pure metal is made the cathode. Hence, the given statement is true.
Zinc sulphate forms a colourless solution in water. The colour on adding copper is:
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blue
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black
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brown
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no change in colour
Explanation
There will be no change in colour as copper(Cu) is less reactive metal than zinc(Zn) and thus can not displace the latter from $$ZnSO_{4}$$ solution.
Which of the following reacts with cold water vigorously?
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Carbon
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Sodium
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Magnesium
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Sulphur
Explanation
Sodium is a light and soft metal that reacts vigorously with cold water. The reaction is so violent and exothermic that the evolved hydrogen gas immediately catches fire.
$$2Na+2H_2O \rightarrow 2NaOH +H_2$$
Of the three metals X, Y and Z, X reacts with cold water, Y with hot water and Z with steam only. Increasing order of reactivity with their identity is:
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$$Na > Mg> Fe$$
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$$Mg > Na > Fe$$
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$$Na > Fe > Mg$$
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$$Na = Fe =Mg$$
Explanation
Alkali metals are the most reactive metals, therefore X is an alkali metal. (e.g: $$Na$$ or $$K$$)
Alkaline Earth metals are most reactive than other metals except alkali metals, therefore Y is an alkaline earth metal. (e.g: $$Mg$$ or $$Ca$$)
Z is any other metal less reactive than alkali and alkaline earth metals but more active than hydrogen. (e.g: $$Fe$$)
The increasing reactivity series can be written as: X > Y > Z.
Which of the following metals can displace the other three metals from their salt solutions?
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Iron
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Copper
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Zinc
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Aluminium
Explanation
The reactivity series follows the order:
$$Al>Zn>Fe>Pb>H>Cu$$
Thus, aluminum is above the other metals given and is more reactive to them and thus, can displace them from their salt solution.
Identify the metal which reacts with concentrated $$H_2SO_4$$ or $$HNO_3$$, but not with concentrated HCl.
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Fe
0%
Zn
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Cu
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Al
Explanation
Cu metal reacts with concentrated $$H_2SO_4$$ or$$HNO_3$$ but it doesn't react with dilute HCl
A solid compound "A" consists of simple ions. The nature of the bond present in "A" will be:
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ionic
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covalent
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molecular
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hydrogen bond
Explanation
Compound "A" is solid and contains ions. So, there are electrostatic forces between the ions, which results in an ionic bond.
Option A is correct.
What are the properties of a metal?
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Malleable
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Ductile
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Non-Lustrous
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Conductor
Explanation
Metals are hard and can be cast into thin sheets and wired example Al, iron, etc. Therefore they are malleable and ductile respectively. They are good conductors of heat and electricity and possess luster.
options A,B,D are correct
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