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CBSE Questions for Class 10 Chemistry Metals And Non Metals Quiz 8 - MCQExams.com
CBSE
Class 10 Chemistry
Metals And Non Metals
Quiz 8
The acid solution is taken in two test tubes. Zinc is introduced in the first test tube and magnesium in the second. Gas is evolved in the second test tube which burns with a pop sound while no gas is evolved from the first test tube. Identify the acid solution taken in the two test tubes.
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$$HCl$$
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$$HNO_{3}$$
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$$H_{2}SO_{4}$$
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$$H_{3}PO_{4}$$
Which of the following oxide(s) of iron would be obtained on prolonged reaction of iron with steam?
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$$FeO$$
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$$Fe_2O_3$$
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$$Fe_3O_4$$
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$$Fe_2O_3$$ and $$Fe_3O_4$$
Explanation
Hint: Less reactive metals like iron react with steam to form oxide and release hydrogen gas.
Step 1:
$$\bullet$$ Reactive metals like sodium, potassium, calcium, etc. react with cold or hot water to form hydroxides and release hydrogen gas.
$$\bullet$$ Moderately reactive metals like magnesium react with hot water to form less soluble hydroxide and release hydrogen gas.
$$\bullet$$ Less reactive metals do not react with cold or hot water but react with steam to form metallic oxides.
$$\bullet$$ Least reactive metals like gold, silver, etc. do not react at all.
Step 2:
Iron does not react with cold or hot water because it is a less reactive metal, but it reacts with steam to form mixed iron oxide and hydrogen gas. The reaction of iron with the steam is as follows:
$$3Fe(s)+4H_2O(g)\to Fe_3O_4(s)+4H_2(g)$$
Note: $$Fe_3O_4$$ is a mixed oxide of $$FeO$$ and $$Fe_2O_3.$$
Final step:
So, the correct option is
(C) $$Fe_3O_4$$.
Materials that can be drawn into wires are called ductile. Which of the following is not ductile material?
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Silver
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Sulphur
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Copper
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Aluminium
Explanation
Sulphur is not ductile because it is non-metal. Non-metals are not ductile.
Hence, option $$B$$ is the correct answer.
Which one of the following metal do not react with cold or hot water?
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Sodium (Na)
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Calcium (Ca)
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Magnesium (Mg)
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Iron (Fe)
Explanation
Reaction of metals with cold or hot water depends on the reactivity of the metals.
Reactive metals like sodium, potassium, calcium, etc. react with cold or hot water.
Moderately reactive metals like magnesium react with hot water.
Less reactive metals do not react with cold or hot water but react with steam.
Least reactive metals like gold, silver, etc. do not react at all.
Less reactive metals like iron react with steam to form an oxide and release hydrogen gas. The reaction is as follows:
$$3Fe(s)+4H_2O(g)\to Fe_3O_4(s)+4H_2(g)$$
Which one of the following figures correctly describes the process of electrolytic refining?
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Metals are good conductor of electricity but poor conductor of heat. True or False?
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True
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False
Explanation
Metals are good conductor of electricity as well as good conductor of heat.
Hence, the given statement is "False".
During electrolytic refining of zinc, it gets
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deposited on cathode
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deposited on anode
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deposited on cathode as well as anode
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remains in the solution
Explanation
Hint: Electrolytic refining is one method of refining impure metals like Cu, Zn, Ag, etc.
Step 1:
There are different methods available for refining metals. Some methods are - vapor phase refining, zone refining, distillation, electrolysis, etc. Electrolytic refining is one such method mainly used for metals like Cu, Zn, Ag, etc. In e
lectrolytic refining, electrical energy is used to convert non-spontaneous reactions to spontaneous reactions.
Step 2:
In the electrolytic refining of zinc, impure zinc is made as an anode, and a thin sheet of pure zinc is made as the cathode. A metal salt solution is taken as an electrolyte. At anode oxidation of zinc occurs and at the cathode reduction of zinc occurs.
Step 3:
During the course of refining, the size of the anode decreases and impurities settle down at the bottom of the anode as anodic mud. The size of the cathode increases due to the deposition of zinc on the surface thereby obtaining the pure metals of zinc at the cathode.
Cell reaction is as follows:
At anode: $$Zn(s)\to Zn^{2+}(aq)+2e^-$$
At cathode: $$Zn^{2+}(aq)+2e^-\to Zn(s)$$
Final step:
So, the correct option is
(A) deposited on cathode.
The reaction between X and Y forms the compound Z. X loses electron and Y gains electron. Which of the following properties is not shown by Z?
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Has high melting point
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Has low melting point
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Conducts electricity in molten state
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Occurs as solid
Explanation
Hint: Metals lose electrons and non-metals gain electrons to form ionic compounds.
Step 1:
Ionic compounds generally have high melting and boiling point, are hard and brittle and exist in solid state at room temperature because of the strong electrostatic force of attraction. It conducts electricity in the molten or solution phase due to the presence of mobile ions.
Step 2:
Among the given elements, X and Y to form the compound Z, X loses electron and Y gains electron. So, the compound formed will be an ionic compound since there is a transfer of electrons.
Step 3:
Compound Z will have a high melting and boiling point, hard and brittle and exist in the solid state at room temperature, and will conduct electricity in the molten or solution phase.
Final step:
So, the correct option is
(B) Has low melting point.
Which among the following statements are incorrect for magnesium metal?
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It burns in oxygen with a dazzling white flame
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It reacts with cold water to form magnesium oxide and evolves hydrogen gas
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It reacts with hot water to form magnesium hydroxide and evolves hydrogen gas
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It reacts with steam to form magnesium hydroxide and evolves hydrogen gas
Explanation
Hint: Magnesium reacts with hot water and steam, but not with cold water.
Step 1:
Magnesium is a reactive metal but less reactive compared to sodium, potassium, calcium, etc. It is because two electrons valence is strongly held to the nucleus compared to sodium, potassium, or calcium.
Step 2:
When magnesium ribbon burns in the presence of oxygen, it burns with a dazzling white flame. Before burning, the magnesium ribbon is rubbed with sandpaper to remove the oxide layer at the surface of the magnesium ribbon.
Step 3:
Magnesium metal does not show any significant reaction with cold water but reacts with hot water to give the slightly soluble magnesium hydroxide and reacts with steam to produce white magnesium oxide and hydrogen gas. The reactions are as follows:
$$a. Mg(s)+\underset{(cold)}{H_2O}\to Mg(OH)_2(s)+H_2(g) -----\text{Negligible Reaction}$$
$$b. Mg(s)+\underset{(hot)}{H_2O}\to Mg(OH)_2(s)+H_2(g)$$
$$c. Mg(s)+\underset{(steam)}{H_2O}\to MgO(s)+H_2(g)$$
Final step:
So, the correct options are -
B. It reacts with cold water to form magnesium oxide and evolves hydrogen gas.
D. It reacts with steam to form magnesium hydroxide and evolves hydrogen gas.
Which one of the following forms a brown flaky coat when exposed to air?
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Sodium
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Copper
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Iron
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Silver
Explanation
Iron when exposed to moist air for a long time acquires a coating of a brown flaky substance called rust (chemically hydrated ferric oxide).
Thus, option $$C$$ is correct.
Reacting with water, a metal produces
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oxygen
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nitric acid
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a base
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water
Explanation
Metals react with water and produce a metal oxide and hydrogen gas. Metal oxides that are soluble in water dissolve in it to further form metal hydroxide which are usually bases.
Elements and compounds that occur naturally in the earth's crust are called:
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materials
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metals
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gases
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minerals
Explanation
Minerals are elements and compounds found naturally in the earth's crust. They can be metals as well as non-metals.
The figure shows a car bumper coated with chromium.
Why are car bumpers often coated with chromium?
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(i) and (ii) only
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(ii) and (iii) only
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(iii) and (i) only
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(i),(ii) and (iii) only
Explanation
Car bumpers are coated with chromium because chromium forms an oxide layer and helps in the prevention of rust formation and corrosion.
Hence, option A is correct.
The metal which does not displace hydrogen from dil. HCl is:
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Ag
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Mg
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Al
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Fe
Explanation
Metals such as copper, silver, gold and platinum are less reactive than hydrogen. Hence, they cannot displace hydrogen from dil. HCl.
In the electrolytic refining of metals, electrolysis of an aqueous solution of its complex salt is done with impure metal as anode and a strip of pure metal as cathode. This method cannot be used for the refining of:
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silver
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copper
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aluminium
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zinc
Explanation
Aluminium can be extracted by Hall's process.
The ore is first converted into pure aluminium oxide by the Bayer Process, and this is then electrolysed in solution in molten cryolite - another aluminium compound.
The aluminium oxide has too high a melting point to electrolyse on its own. The usual aluminium ore is bauxite.
Option C is correct.
The order of reactivity of four metals and hydrogen is given below.
Which of the following does not give hydrogen as a product?
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The adding of Rubidium to water.
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The adding of tin to dilute Hydrochloric acid.
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The electrolysis of aqueous gold chloride.
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The electrolysis of aqueous rubidium chloride.
Identify the non-metal which is a good conductor of electricity.
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Chlorine
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Sulphur
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Graphite
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Phosphorus
Explanation
Non-metals, in general, are bad conductors of electricity. But graphite, an allotrope of carbon, and a non-metal is an exception. It is a good conductor of electricity.
The gas given off when a metal reacts with an acid is
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hydrogen
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oxygen
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carbon dioxide
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water vapour
Explanation
When a metal reacts with an acid, the gas produced is hydrogen.
$$Metal + Acid \rightarrow Salt + Hydrogen$$
Carbon cannot reduce the oxides of sodium to sodium because
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$$Na$$ has less affinity for oxygen
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$$Na$$ has more affinity for carbon than oxygen
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$$Na$$ is non-reactive
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$$Na$$ has more affinity for oxygen than carbon
Explanation
T
he metals high up in the activity series are very reactive. They cannot obtain by reduction of their oxides by carbon. Since, sodium is high up in the acitivity series, carbon cannot reduce the oxides of sodium because it has more affinity for oxygen than carbon.
Observe the figure carefully and identify the substances marked as (p), (q) and (r).
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(p) - Zinc, (q) - Water, (r) - Carbon dioxide
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(p) - Magnesium, (q) - Hydrochloric acid, (r) - Oxygen
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(p) - Magnesium, (q) - Water, (r) - Carbon dioxide
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(p) - Zinc, (q) - Hydrochloric acid, (r) - Hydrogen
Fill in the blanks by selecting the option with the correct words.
The process of removing impurities from the impure metal to obtain pure metal is known as _____of metal. The most widely used method for refining is _________. In this method, the impure metal is taken as ________ and the pure metal is taken as _____.
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refining, electrolytic refining, anode, cathode
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calcination, electrolysis, cathode, anode
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refining, smelting, cathode, anode
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smelting, calcination, anode, cathode
Explanation
The process of removing impurities from impure metal is called refining.
Electrolytic refining is a widely used method of refining as it is a cost-effective and efficient method.
During the process, the impure metals are taken as anode and, pure metals are taken as the cathode. As electrolysis proceeds, the pure metal keeps depositing on the cathode and, the impurities settle at the bottom.
Hence the correct option is A.
A student added dilute HCl to a test tube containing zinc granules. Which of the following
observations are correct?
I. Zinc surface became dull and black.
II. A gas was evolved which burnt with a pop sound.
III. The solution remained colourless.
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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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I, II and III
Explanation
$$Zn + 2HCl \rightarrow ZnCl_2 + H_2$$
Due to the reaction of zinc with the acid, zinc loses its shiny appearance.
$$H_2$$ gas is evolved during the reaction. We can identify the gas with a burning match stick. A pop sound indicates its presence.
Zinc chloride formed in the reaction is colourless, so, the solution does not change its colour.
Hence, all the statements are correct.
Aluminium is not acted upon by pure water as
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Impurities inwater are essential for the reacionn to occure
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Itis light metal
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It is protected by a film of alumininum oxide
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It is not a reactive metal
Choose the correct statement
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Non-metals have higher ionisation enthalpies and higher electronegativity then the metals
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non metals and metalloids exist only in the p-block of the periodic table.
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change of non-metallic to metallic character can be illustrated by the nature of oxide they form
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all are correct,
A metal gives lilac colour in bunsen flame and the solution of its oxide turns red litmus paper blue. The metal is?
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$$Na$$
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$$K$$
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$$Ca$$
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$$Li$$
Explanation
Potassium metal ($$K$$) gives lilac (pink) colour in bunsen flame. Its oxide dissolves in water to form potassium hydroxide, which is an alkali. So, the solution of its oxide turns red litmus paper blue.
$$K_2O + H_2O \rightarrow 2KOH$$
Sodium metal ($$Na$$) gives yellow flame, calcium ($$Ca$$) gives orange red flame and lithium ($$Li$$) gives red flame.
Mark the correct statements:
(i) mercury can be refined by the process of distillation.
(ii) In poling, the molten impure metal is stirred with green poles of wood.
(iii) In electrolyte refining of metals, impure metal is made as cathode and a thin strip of pure metal is made as anode.
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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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(i), (ii) and (iii)
Explanation
Low boiling point metals like Mercury are purified with distillation.
Hence, statement (i) is correct.
The heat of copper makes the pole emit wood gas that reduces the cuprous oxide to copper.
In poling, the molten impure metal is stirred with green poles of wood.
Hence,option (ii) is correct.
In electrolyte refining of metals, impure metal is made as Anode
and a thin strip of pure metal is made as
cathode.
Hence, option (iii) is incorrect.
Sodium metal is extracted by the electrolysis of
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$$NaCl(l)$$
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$$NaCI(aq)$$
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$$ Na_2SO_4(aq) $$
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$$ NaNO_3(aq) $$
Which of the following metal evolves hydrogen on reacting with cold dilute $$HNO_{3}$$?
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Mg
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Al
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Fe
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Cu
Explanation
Only magnesium and manganese react with nitric acid to release hydrogen gas. So, option A is correct.
Hydrogen gas is not evolved when other metals react with nitric acid because it is a strong oxidising agent. It oxidises hydrogen produced to water and itself gets reduced to a nitrogen oxide.
A student was given few metals Mg, K, Fe and Cu. Which of them will react only with steam and not with cold or hot water to give $$H_{2}$$ gas?
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Mg
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K
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Fe
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Cu
Explanation
Iron (Fe) does not react with hot or cold water. It only reacts with steam to give hydrogen gas.
Magnesium (Mg) does not react with cold water but reacts with hot water to give hydrogen gas.
Potassium (K) reacts violently with cold water to give hydrogen gas.
Copper (Cu) does not react with hot/cold water or steam.
Silver articles become black on prolonged exposure to air. This is due to the formation of
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$$Ag_3N$$
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$$Ag_2O$$
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$$Ag_2S$$
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$$Ag_2S$$ and $$Ag_3N$$
Explanation
Hint: Silver articles become black on prolonged exposure to air due to the formation of sulphide.
Step 1: Corrosion.
Metals when exposed to air for a long period undergo corrosion. Corrosion is a common phenomenon for iron objects and corrosion of iron objects is called rusting.
Step 2: Corrosion in silver:
Unlike iron, silver
when
exposed to air for a long period undergo corrosion. Silver reacts with sulphur compounds present in the air to form silver sulphide. An example of such reaction is as follows:
$$Ag(s)+H_2S(g)\to Ag_2S(s)+H_2(g)$$
Step 3: Conclusion.
Corrosion or conversion of silver to silver sulphide
on prolonged exposure to air turns silver to black colour.
Final step:
So, the correct option is
(C) $$Ag_2S.$$
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