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CHXI11:THE P-BLOCK ELEMENTS

316524 Aluminium is more reactive than iron because its standard reduction potential is higher still aluminium is less easily corroded than iron because

1 It has higher reducing power and forms protective layer of

{Al}_{2} O_{3}

.

2 It has higher reducing power and does not react with oxygen so easily.

3 Aluminium reacts with amphoteric carbon dioxide to form a self-protective layer of

{Al}_{2} O_{3} + {Al}_{4} C_{3}

.

4 Aluminium reacts with nitrogen in air to form a protective layer of AIN.

Explanation:

$4 Al + 3 O_{2} \to \underset{Alumina}{2 {Al}_{2} O_{3}}$ (Passivation of aluminium layer).The formed ${Al}_{2} O_{3}$ protects Al from corrosion.

CHXI11:THE P-BLOCK ELEMENTS

316525 Assertion :
${Pb}^{4 +}$ compounds are stronger oxidizing agents than ${Sn}^{4 +}$ compounds.
Reason :
The higher oxidation states for the group 14 elements are more stable for the heavier members of the group due to inert pair effect.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

The oxidizing action shows the following order ${Pb}^{4 +} > {Sn}^{4 +} > {Ge}^{4 +}$
The lower oxidation state for the group 14 elements is more stable for heavier elements in the group due to inert pair effect. So, option (3) is correct.

CHXI11:THE P-BLOCK ELEMENTS

316526 Ge(II) compounds are powerful reducing agents whereas $Pb (IV)$ compounds are strong oxidants. It can be due to

1

Pb

is more electronegative than

Ge

2 ionization potential of lead is less than that of Ge

3 ionic radii of

{Pb}^{2 +}

and

{Pb}^{4 +}

are larger than those of

{Ge}^{2 +}

and

{Ge}^{4 +}

4 more pronounced inert pair effect in lead than in Ge

CHXI11:THE P-BLOCK ELEMENTS

316557 In which among the following compounds, oxidation number of nitrogen is +5 ?

1

N_{2} O

2

N_{2} O_{3}

3

{NO}_{2}

4

H N O_{3}

Explanation:

Oxidation number of nitrogen is +5 in ${HNO}_{3}$ .
$1 + x + 3 (- 2) = 0$
$x - 5 = 0$
$x = + 5$

MHTCET - 2019

CHXI11:THE P-BLOCK ELEMENTS

316527 The number of ions from the following that are expected to behave as oxidising agents is :
$S n^{4 +}, S n^{2 +}, P b^{2 +}, T l^{3 +}, P b^{4 +}, T l^{+}$

1 4

2 2

3 1

4 3

Explanation:

${Pb}^{2 +}$ is more stable than ${Pb}^{4 -}$ and ${Tl}^{+}$ is more stable than ${Tl}^{3 +}$ due to inert pair effect. Thus, ${Pb}^{4 -}$ and ${Tl}^{3 +}$ act as oxidising agents and themselves get reduced to ${Pb}^{2 +}$ and ${Tl}^{3 +}$ respectively. So, the correct option is (2)

JEE Main - 2024

CHXI11:THE P-BLOCK ELEMENTS

316524 Aluminium is more reactive than iron because its standard reduction potential is higher still aluminium is less easily corroded than iron because

1 It has higher reducing power and forms protective layer of

{Al}_{2} O_{3}

.

2 It has higher reducing power and does not react with oxygen so easily.

3 Aluminium reacts with amphoteric carbon dioxide to form a self-protective layer of

{Al}_{2} O_{3} + {Al}_{4} C_{3}

.

4 Aluminium reacts with nitrogen in air to form a protective layer of AIN.

Explanation:

$4 Al + 3 O_{2} \to \underset{Alumina}{2 {Al}_{2} O_{3}}$ (Passivation of aluminium layer).The formed ${Al}_{2} O_{3}$ protects Al from corrosion.

CHXI11:THE P-BLOCK ELEMENTS

316525 Assertion :
${Pb}^{4 +}$ compounds are stronger oxidizing agents than ${Sn}^{4 +}$ compounds.
Reason :
The higher oxidation states for the group 14 elements are more stable for the heavier members of the group due to inert pair effect.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

The oxidizing action shows the following order ${Pb}^{4 +} > {Sn}^{4 +} > {Ge}^{4 +}$
The lower oxidation state for the group 14 elements is more stable for heavier elements in the group due to inert pair effect. So, option (3) is correct.

CHXI11:THE P-BLOCK ELEMENTS

316526 Ge(II) compounds are powerful reducing agents whereas $Pb (IV)$ compounds are strong oxidants. It can be due to

1

Pb

is more electronegative than

Ge

2 ionization potential of lead is less than that of Ge

3 ionic radii of

{Pb}^{2 +}

and

{Pb}^{4 +}

are larger than those of

{Ge}^{2 +}

and

{Ge}^{4 +}

4 more pronounced inert pair effect in lead than in Ge

CHXI11:THE P-BLOCK ELEMENTS

316557 In which among the following compounds, oxidation number of nitrogen is +5 ?

1

N_{2} O

2

N_{2} O_{3}

3

{NO}_{2}

4

H N O_{3}

Explanation:

Oxidation number of nitrogen is +5 in ${HNO}_{3}$ .
$1 + x + 3 (- 2) = 0$
$x - 5 = 0$
$x = + 5$

MHTCET - 2019

CHXI11:THE P-BLOCK ELEMENTS

316527 The number of ions from the following that are expected to behave as oxidising agents is :
$S n^{4 +}, S n^{2 +}, P b^{2 +}, T l^{3 +}, P b^{4 +}, T l^{+}$

1 4

2 2

3 1

4 3

Explanation:

${Pb}^{2 +}$ is more stable than ${Pb}^{4 -}$ and ${Tl}^{+}$ is more stable than ${Tl}^{3 +}$ due to inert pair effect. Thus, ${Pb}^{4 -}$ and ${Tl}^{3 +}$ act as oxidising agents and themselves get reduced to ${Pb}^{2 +}$ and ${Tl}^{3 +}$ respectively. So, the correct option is (2)

JEE Main - 2024

CHXI11:THE P-BLOCK ELEMENTS

316524 Aluminium is more reactive than iron because its standard reduction potential is higher still aluminium is less easily corroded than iron because

1 It has higher reducing power and forms protective layer of

{Al}_{2} O_{3}

.

2 It has higher reducing power and does not react with oxygen so easily.

3 Aluminium reacts with amphoteric carbon dioxide to form a self-protective layer of

{Al}_{2} O_{3} + {Al}_{4} C_{3}

.

4 Aluminium reacts with nitrogen in air to form a protective layer of AIN.

Explanation:

$4 Al + 3 O_{2} \to \underset{Alumina}{2 {Al}_{2} O_{3}}$ (Passivation of aluminium layer).The formed ${Al}_{2} O_{3}$ protects Al from corrosion.

CHXI11:THE P-BLOCK ELEMENTS

316525 Assertion :
${Pb}^{4 +}$ compounds are stronger oxidizing agents than ${Sn}^{4 +}$ compounds.
Reason :
The higher oxidation states for the group 14 elements are more stable for the heavier members of the group due to inert pair effect.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

The oxidizing action shows the following order ${Pb}^{4 +} > {Sn}^{4 +} > {Ge}^{4 +}$
The lower oxidation state for the group 14 elements is more stable for heavier elements in the group due to inert pair effect. So, option (3) is correct.

CHXI11:THE P-BLOCK ELEMENTS

316526 Ge(II) compounds are powerful reducing agents whereas $Pb (IV)$ compounds are strong oxidants. It can be due to

1

Pb

is more electronegative than

Ge

2 ionization potential of lead is less than that of Ge

3 ionic radii of

{Pb}^{2 +}

and

{Pb}^{4 +}

are larger than those of

{Ge}^{2 +}

and

{Ge}^{4 +}

4 more pronounced inert pair effect in lead than in Ge

CHXI11:THE P-BLOCK ELEMENTS

316557 In which among the following compounds, oxidation number of nitrogen is +5 ?

1

N_{2} O

2

N_{2} O_{3}

3

{NO}_{2}

4

H N O_{3}

Explanation:

Oxidation number of nitrogen is +5 in ${HNO}_{3}$ .
$1 + x + 3 (- 2) = 0$
$x - 5 = 0$
$x = + 5$

MHTCET - 2019

CHXI11:THE P-BLOCK ELEMENTS

316527 The number of ions from the following that are expected to behave as oxidising agents is :
$S n^{4 +}, S n^{2 +}, P b^{2 +}, T l^{3 +}, P b^{4 +}, T l^{+}$

1 4

2 2

3 1

4 3

Explanation:

${Pb}^{2 +}$ is more stable than ${Pb}^{4 -}$ and ${Tl}^{+}$ is more stable than ${Tl}^{3 +}$ due to inert pair effect. Thus, ${Pb}^{4 -}$ and ${Tl}^{3 +}$ act as oxidising agents and themselves get reduced to ${Pb}^{2 +}$ and ${Tl}^{3 +}$ respectively. So, the correct option is (2)

JEE Main - 2024

CHXI11:THE P-BLOCK ELEMENTS

316524 Aluminium is more reactive than iron because its standard reduction potential is higher still aluminium is less easily corroded than iron because

1 It has higher reducing power and forms protective layer of

{Al}_{2} O_{3}

.

2 It has higher reducing power and does not react with oxygen so easily.

3 Aluminium reacts with amphoteric carbon dioxide to form a self-protective layer of

{Al}_{2} O_{3} + {Al}_{4} C_{3}

.

4 Aluminium reacts with nitrogen in air to form a protective layer of AIN.

Explanation:

$4 Al + 3 O_{2} \to \underset{Alumina}{2 {Al}_{2} O_{3}}$ (Passivation of aluminium layer).The formed ${Al}_{2} O_{3}$ protects Al from corrosion.

CHXI11:THE P-BLOCK ELEMENTS

316525 Assertion :
${Pb}^{4 +}$ compounds are stronger oxidizing agents than ${Sn}^{4 +}$ compounds.
Reason :
The higher oxidation states for the group 14 elements are more stable for the heavier members of the group due to inert pair effect.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

The oxidizing action shows the following order ${Pb}^{4 +} > {Sn}^{4 +} > {Ge}^{4 +}$
The lower oxidation state for the group 14 elements is more stable for heavier elements in the group due to inert pair effect. So, option (3) is correct.

CHXI11:THE P-BLOCK ELEMENTS

316526 Ge(II) compounds are powerful reducing agents whereas $Pb (IV)$ compounds are strong oxidants. It can be due to

1

Pb

is more electronegative than

Ge

2 ionization potential of lead is less than that of Ge

3 ionic radii of

{Pb}^{2 +}

and

{Pb}^{4 +}

are larger than those of

{Ge}^{2 +}

and

{Ge}^{4 +}

4 more pronounced inert pair effect in lead than in Ge

CHXI11:THE P-BLOCK ELEMENTS

316557 In which among the following compounds, oxidation number of nitrogen is +5 ?

1

N_{2} O

2

N_{2} O_{3}

3

{NO}_{2}

4

H N O_{3}

Explanation:

Oxidation number of nitrogen is +5 in ${HNO}_{3}$ .
$1 + x + 3 (- 2) = 0$
$x - 5 = 0$
$x = + 5$

MHTCET - 2019

CHXI11:THE P-BLOCK ELEMENTS

316527 The number of ions from the following that are expected to behave as oxidising agents is :
$S n^{4 +}, S n^{2 +}, P b^{2 +}, T l^{3 +}, P b^{4 +}, T l^{+}$

1 4

2 2

3 1

4 3

Explanation:

${Pb}^{2 +}$ is more stable than ${Pb}^{4 -}$ and ${Tl}^{+}$ is more stable than ${Tl}^{3 +}$ due to inert pair effect. Thus, ${Pb}^{4 -}$ and ${Tl}^{3 +}$ act as oxidising agents and themselves get reduced to ${Pb}^{2 +}$ and ${Tl}^{3 +}$ respectively. So, the correct option is (2)

JEE Main - 2024

CHXI11:THE P-BLOCK ELEMENTS

316524 Aluminium is more reactive than iron because its standard reduction potential is higher still aluminium is less easily corroded than iron because

1 It has higher reducing power and forms protective layer of

{Al}_{2} O_{3}

.

2 It has higher reducing power and does not react with oxygen so easily.

3 Aluminium reacts with amphoteric carbon dioxide to form a self-protective layer of

{Al}_{2} O_{3} + {Al}_{4} C_{3}

.

4 Aluminium reacts with nitrogen in air to form a protective layer of AIN.

Explanation:

$4 Al + 3 O_{2} \to \underset{Alumina}{2 {Al}_{2} O_{3}}$ (Passivation of aluminium layer).The formed ${Al}_{2} O_{3}$ protects Al from corrosion.

CHXI11:THE P-BLOCK ELEMENTS

316525 Assertion :
${Pb}^{4 +}$ compounds are stronger oxidizing agents than ${Sn}^{4 +}$ compounds.
Reason :
The higher oxidation states for the group 14 elements are more stable for the heavier members of the group due to inert pair effect.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

The oxidizing action shows the following order ${Pb}^{4 +} > {Sn}^{4 +} > {Ge}^{4 +}$
The lower oxidation state for the group 14 elements is more stable for heavier elements in the group due to inert pair effect. So, option (3) is correct.

CHXI11:THE P-BLOCK ELEMENTS

316526 Ge(II) compounds are powerful reducing agents whereas $Pb (IV)$ compounds are strong oxidants. It can be due to

1

Pb

is more electronegative than

Ge

2 ionization potential of lead is less than that of Ge

3 ionic radii of

{Pb}^{2 +}

and

{Pb}^{4 +}

are larger than those of

{Ge}^{2 +}

and

{Ge}^{4 +}

4 more pronounced inert pair effect in lead than in Ge

CHXI11:THE P-BLOCK ELEMENTS

316557 In which among the following compounds, oxidation number of nitrogen is +5 ?

1

N_{2} O

2

N_{2} O_{3}

3

{NO}_{2}

4

H N O_{3}

Explanation:

Oxidation number of nitrogen is +5 in ${HNO}_{3}$ .
$1 + x + 3 (- 2) = 0$
$x - 5 = 0$
$x = + 5$

MHTCET - 2019

CHXI11:THE P-BLOCK ELEMENTS

316527 The number of ions from the following that are expected to behave as oxidising agents is :
$S n^{4 +}, S n^{2 +}, P b^{2 +}, T l^{3 +}, P b^{4 +}, T l^{+}$

1 4

2 2

3 1

4 3

Explanation:

${Pb}^{2 +}$ is more stable than ${Pb}^{4 -}$ and ${Tl}^{+}$ is more stable than ${Tl}^{3 +}$ due to inert pair effect. Thus, ${Pb}^{4 -}$ and ${Tl}^{3 +}$ act as oxidising agents and themselves get reduced to ${Pb}^{2 +}$ and ${Tl}^{3 +}$ respectively. So, the correct option is (2)

JEE Main - 2024