XI_Chem_New Chap-7_Redox Reactions_[True or False Statement Questions]
Sl # Statements [Exercises] (HOTS Test) True/False
1 A Daniell cell is an electrochemical cell used to demonstrate redox reactions.
A galvanic cell, composed of two electrodes and an electrolyte, converts chemical energy into
2
electrical energy through redox reactions.
A redox reaction involves both oxidation and reduction processes occurring simultaneously.
3
4 A reducing agent tends to lose electrons and is oxidized in a redox reaction.
5 A salt bridge allows for the flow of ions between two half-cells in an electrochemical cell.
A salt bridge is a U-shaped tube containing an electrolyte that connects two half-cells in an
6
electrochemical cell.
7 A salt bridge is used to mix the contents of two half-cells in an electrochemical cell.
8 Acidic solutions are relevant when balancing redox reactions.
9 Acidic solutions contain excess H+ ions.
10 Acidic solutions have no relevance in balancing redox reactions.
11 An oxidizing agent tends to gain electrons and is reduced in a redox reaction.
12 Basic solutions are relevant when balancing redox reactions.
13 Basic solutions contain excess OH- ions.
14 Basic solutions have no relevance in balancing redox reactions.
15 Chlorine (Cl2) can displace bromide ions (Br-) in an aqueous solution.
139 Chlorine gets reduced in electron transfer reactions when it accepts electrons.
Combination reactions involve the formation of a new compound from two or more
16
substances.
Competitive Electron Transfer Reactions involve the exchange of electrons between
17
substances.
Competitive Electron Transfer Reactions involve the exchange of protons between
18
substances.
19 Copper ions in copper nitrate are reduced by gaining electrons from zinc.
20 Copper ions in copper nitrate are reduced by gaining protons from zinc.
Cupric sulphide (CuS) has high solubility, making it a poor test for the presence of Cu2+ ions.
21
Cupric sulphide (CuS) has low solubility, making it a sensitive test for the presence of Cu2+
22
ions.
Decomposition reactions involve the breakdown of a compound into simpler substances.
23
Displacement reactions do not always involve the exchange of ions between compounds.
24
Displacement reactions involve the replacement of one ion or atom in a compound with
25
another ion or atom.
Disproportionation reactions are a unique subtype of redox reactions, characterized by an
26
element simultaneously undergoing oxidation and reduction.
Disproportionation reactions involve an element simultaneously being oxidized and reduced.
27
Disproportionation reactions involve elements that never undergo oxidation or reduction
28
simultaneously.
29 Disproportionation reactions only involve the reduction of an element.
Disproportionation reactions, such as NO2 converting to NO2- and NO3-, exemplify redox
30
reactions where an element undergoes simultaneous oxidation and reduction.
Dry and wet batteries operate without any involvement of redox reactions, and corrosion of
31
metals is unrelated to oxidation and reduction.
32 Electrode potential is measured in volts.
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, XI_Chem_New Chap-7_Redox Reactions_[True or False Statement Questions]
Sl # Statements [Exercises] (HOTS Test) True/False
Electrode processes are central to the field of electrochemistry, offering insights into redox
33
reactions and cell behavior.
Electron shift and electron transfer are synonymous terms describing the same process in
34
redox reactions.
Electron shift, often seen in covalent compounds, describes the redistribution of electrons
35
without a complete loss or gain.
Electron transfer occurs during redox reactions, where one substance loses electrons
36
(oxidation) and another gains electrons (reduction).
39 Electronegativity has no influence on the direction of electron transfer in reactions.
Electronegativity plays a crucial role in determining the direction of electron transfer in
140
reactions.
Equilibrium in the copper-silver nitrate reaction greatly favors the formation of Cu2+ ions and
37
Ag metal.
Equilibrium in the copper-silver nitrate reaction greatly favors the formation of silver ions and
38
Cu metal.
Fractional oxidation numbers in compounds like C3O2 and Br3O8 accurately represent the
45
actual oxidation states of the elements within the compounds.
Fractional oxidation numbers in compounds like C3O2, Br3O8, and Na2S4O6 represent
46
average oxidation states rather than the actual states.
47 Half reactions encompass both oxidation and reduction processes.
48 Half reactions represent either oxidation or reduction processes.
Half-reaction method involves splitting redox reactions into oxidation and reduction
49
reactions.
50 Half-reactions represent either the oxidation or reduction process in a redox reaction.
51 Half-reactions represent the oxidation and reduction processes in a redox reaction.
Hydrogen combines with oxygen to form water through a redox reaction, involving electron
52
transfer from hydrogen to oxygen.
53 In a combination reaction, at least one of the substances must be in its elemental form.
54 In a decomposition reaction, at least one product must be in its elemental form.
In a redox reaction, one substance is oxidized (loses electrons), and another is reduced (gains
55
electrons).
40 In electron transfer reactions, oxygen always loses electrons.
In electron transfer reactions, species either lose or gain electrons, resulting in new
141
compounds.
56 In redox reactions, oxidation only involves the removal of hydrogen.
57 In redox reactions, the oxidation state of elements remains constant.
In the context of redox reactions, oxidation is not limited to the addition of oxygen but can
58
involve other electronegative elements.
In the reaction between copper metal and silver nitrate solution, copper is oxidized to Cu2+
59
ions, and silver ions are reduced to form Ag metal.
In the reaction between copper metal and silver nitrate solution, copper is reduced to Cu2+
60
ions, and silver ions are oxidized to form Ag metal.
In the reaction between metallic zinc and copper nitrate, copper loses electrons and is
61
oxidized to Cu2+ ions.
In the reaction between metallic zinc and copper nitrate, zinc loses electrons and is oxidized
62
to Zn2+ ions.
63 In the redox reaction equation 7.15, manganese dioxide (MnO2) is formed.
41 Ionic compounds are exclusively covalently bonded.
64 Ionic equations include all species participating in a chemical reaction.
65 Ionic equations show only the ions involved in a chemical reaction.
2 OF 5 RI_Best Wishes
Sl # Statements [Exercises] (HOTS Test) True/False
1 A Daniell cell is an electrochemical cell used to demonstrate redox reactions.
A galvanic cell, composed of two electrodes and an electrolyte, converts chemical energy into
2
electrical energy through redox reactions.
A redox reaction involves both oxidation and reduction processes occurring simultaneously.
3
4 A reducing agent tends to lose electrons and is oxidized in a redox reaction.
5 A salt bridge allows for the flow of ions between two half-cells in an electrochemical cell.
A salt bridge is a U-shaped tube containing an electrolyte that connects two half-cells in an
6
electrochemical cell.
7 A salt bridge is used to mix the contents of two half-cells in an electrochemical cell.
8 Acidic solutions are relevant when balancing redox reactions.
9 Acidic solutions contain excess H+ ions.
10 Acidic solutions have no relevance in balancing redox reactions.
11 An oxidizing agent tends to gain electrons and is reduced in a redox reaction.
12 Basic solutions are relevant when balancing redox reactions.
13 Basic solutions contain excess OH- ions.
14 Basic solutions have no relevance in balancing redox reactions.
15 Chlorine (Cl2) can displace bromide ions (Br-) in an aqueous solution.
139 Chlorine gets reduced in electron transfer reactions when it accepts electrons.
Combination reactions involve the formation of a new compound from two or more
16
substances.
Competitive Electron Transfer Reactions involve the exchange of electrons between
17
substances.
Competitive Electron Transfer Reactions involve the exchange of protons between
18
substances.
19 Copper ions in copper nitrate are reduced by gaining electrons from zinc.
20 Copper ions in copper nitrate are reduced by gaining protons from zinc.
Cupric sulphide (CuS) has high solubility, making it a poor test for the presence of Cu2+ ions.
21
Cupric sulphide (CuS) has low solubility, making it a sensitive test for the presence of Cu2+
22
ions.
Decomposition reactions involve the breakdown of a compound into simpler substances.
23
Displacement reactions do not always involve the exchange of ions between compounds.
24
Displacement reactions involve the replacement of one ion or atom in a compound with
25
another ion or atom.
Disproportionation reactions are a unique subtype of redox reactions, characterized by an
26
element simultaneously undergoing oxidation and reduction.
Disproportionation reactions involve an element simultaneously being oxidized and reduced.
27
Disproportionation reactions involve elements that never undergo oxidation or reduction
28
simultaneously.
29 Disproportionation reactions only involve the reduction of an element.
Disproportionation reactions, such as NO2 converting to NO2- and NO3-, exemplify redox
30
reactions where an element undergoes simultaneous oxidation and reduction.
Dry and wet batteries operate without any involvement of redox reactions, and corrosion of
31
metals is unrelated to oxidation and reduction.
32 Electrode potential is measured in volts.
1 OF 5 RI_Best Wishes
, XI_Chem_New Chap-7_Redox Reactions_[True or False Statement Questions]
Sl # Statements [Exercises] (HOTS Test) True/False
Electrode processes are central to the field of electrochemistry, offering insights into redox
33
reactions and cell behavior.
Electron shift and electron transfer are synonymous terms describing the same process in
34
redox reactions.
Electron shift, often seen in covalent compounds, describes the redistribution of electrons
35
without a complete loss or gain.
Electron transfer occurs during redox reactions, where one substance loses electrons
36
(oxidation) and another gains electrons (reduction).
39 Electronegativity has no influence on the direction of electron transfer in reactions.
Electronegativity plays a crucial role in determining the direction of electron transfer in
140
reactions.
Equilibrium in the copper-silver nitrate reaction greatly favors the formation of Cu2+ ions and
37
Ag metal.
Equilibrium in the copper-silver nitrate reaction greatly favors the formation of silver ions and
38
Cu metal.
Fractional oxidation numbers in compounds like C3O2 and Br3O8 accurately represent the
45
actual oxidation states of the elements within the compounds.
Fractional oxidation numbers in compounds like C3O2, Br3O8, and Na2S4O6 represent
46
average oxidation states rather than the actual states.
47 Half reactions encompass both oxidation and reduction processes.
48 Half reactions represent either oxidation or reduction processes.
Half-reaction method involves splitting redox reactions into oxidation and reduction
49
reactions.
50 Half-reactions represent either the oxidation or reduction process in a redox reaction.
51 Half-reactions represent the oxidation and reduction processes in a redox reaction.
Hydrogen combines with oxygen to form water through a redox reaction, involving electron
52
transfer from hydrogen to oxygen.
53 In a combination reaction, at least one of the substances must be in its elemental form.
54 In a decomposition reaction, at least one product must be in its elemental form.
In a redox reaction, one substance is oxidized (loses electrons), and another is reduced (gains
55
electrons).
40 In electron transfer reactions, oxygen always loses electrons.
In electron transfer reactions, species either lose or gain electrons, resulting in new
141
compounds.
56 In redox reactions, oxidation only involves the removal of hydrogen.
57 In redox reactions, the oxidation state of elements remains constant.
In the context of redox reactions, oxidation is not limited to the addition of oxygen but can
58
involve other electronegative elements.
In the reaction between copper metal and silver nitrate solution, copper is oxidized to Cu2+
59
ions, and silver ions are reduced to form Ag metal.
In the reaction between copper metal and silver nitrate solution, copper is reduced to Cu2+
60
ions, and silver ions are oxidized to form Ag metal.
In the reaction between metallic zinc and copper nitrate, copper loses electrons and is
61
oxidized to Cu2+ ions.
In the reaction between metallic zinc and copper nitrate, zinc loses electrons and is oxidized
62
to Zn2+ ions.
63 In the redox reaction equation 7.15, manganese dioxide (MnO2) is formed.
41 Ionic compounds are exclusively covalently bonded.
64 Ionic equations include all species participating in a chemical reaction.
65 Ionic equations show only the ions involved in a chemical reaction.
2 OF 5 RI_Best Wishes
