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CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313290 The first ionization potential of $Al$ , as compared to that of $Mg$ is :

1 Greater

2 Lower

3 The same

4 Twice as much

Explanation:

The first ionization potential of $Al$ is lower than that of Mg because valence shell configuration of Mg is $3 s^{2}$ and of Al is $3 s^{2}, 3 p^{1}$ . As
s-orbital is close to nucleus than p-orbital so removal of Ist $e^{-}$ from Mg is difficult and require more energy as compare to Al.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313291 Assertion :
Order of ionization potential across the period is $Na < Al < Mg < Si$
Reason :
Ionization potential decreases with decrease in atomic size.

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:

I.E. increases across a period. But $Mg$ has higher I.E. than $Al$ due to the fullfilled stability of $3 s^{2}$ configuration.Ionization potential decreases as atomic size increases .So option (3) is correct.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313292 Read the statement A and statement B to mark the correct option given below.
Statement A :
The correct order of first ionisation enthalpy values of $Li, Na, F$ and Cl is $Na < Li < Cl < F$ .
Statement B :
The correct order of negative electron gain enthalpy values of $Li, Na, F$ and
Cl is $Na < Li < F < Cl$ .

1 Statement A is correct but Statement B is incorrect.

2 Statement A is incorrect but Statement B is correct.

3 Both statements are correct.

4 Both statements are incorrect.

Explanation:

First ionisation enthalpy of $F > Cl$ as I.E. decreases down the group. Similarly, I.E. of $Li > Na$ . Alkali metals have lower I.E. than halogens. So, statement A is correct. Negative electron gain enthalpy of given elements follows the order $Na < Li < F < Cl$ . So, statement B is also correct. So, the correct option is (3).

JEE Main - 2024

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313293 Assertion :
Phosphorus' has higher I.E. than sulphur.
Reason :
I.E. increases from left to right in a period.

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:

Phosphorus $(P)$ exhibits a higher ionization energy (I.E.) due to its half-filled electron configuration. So option (2) is correct.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313290 The first ionization potential of $Al$ , as compared to that of $Mg$ is :

1 Greater

2 Lower

3 The same

4 Twice as much

Explanation:

The first ionization potential of $Al$ is lower than that of Mg because valence shell configuration of Mg is $3 s^{2}$ and of Al is $3 s^{2}, 3 p^{1}$ . As
s-orbital is close to nucleus than p-orbital so removal of Ist $e^{-}$ from Mg is difficult and require more energy as compare to Al.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313291 Assertion :
Order of ionization potential across the period is $Na < Al < Mg < Si$
Reason :
Ionization potential decreases with decrease in atomic size.

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:

I.E. increases across a period. But $Mg$ has higher I.E. than $Al$ due to the fullfilled stability of $3 s^{2}$ configuration.Ionization potential decreases as atomic size increases .So option (3) is correct.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313292 Read the statement A and statement B to mark the correct option given below.
Statement A :
The correct order of first ionisation enthalpy values of $Li, Na, F$ and Cl is $Na < Li < Cl < F$ .
Statement B :
The correct order of negative electron gain enthalpy values of $Li, Na, F$ and
Cl is $Na < Li < F < Cl$ .

1 Statement A is correct but Statement B is incorrect.

2 Statement A is incorrect but Statement B is correct.

3 Both statements are correct.

4 Both statements are incorrect.

Explanation:

First ionisation enthalpy of $F > Cl$ as I.E. decreases down the group. Similarly, I.E. of $Li > Na$ . Alkali metals have lower I.E. than halogens. So, statement A is correct. Negative electron gain enthalpy of given elements follows the order $Na < Li < F < Cl$ . So, statement B is also correct. So, the correct option is (3).

JEE Main - 2024

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313293 Assertion :
Phosphorus' has higher I.E. than sulphur.
Reason :
I.E. increases from left to right in a period.

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:

Phosphorus $(P)$ exhibits a higher ionization energy (I.E.) due to its half-filled electron configuration. So option (2) is correct.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313290 The first ionization potential of $Al$ , as compared to that of $Mg$ is :

1 Greater

2 Lower

3 The same

4 Twice as much

Explanation:

The first ionization potential of $Al$ is lower than that of Mg because valence shell configuration of Mg is $3 s^{2}$ and of Al is $3 s^{2}, 3 p^{1}$ . As
s-orbital is close to nucleus than p-orbital so removal of Ist $e^{-}$ from Mg is difficult and require more energy as compare to Al.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313291 Assertion :
Order of ionization potential across the period is $Na < Al < Mg < Si$
Reason :
Ionization potential decreases with decrease in atomic size.

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:

I.E. increases across a period. But $Mg$ has higher I.E. than $Al$ due to the fullfilled stability of $3 s^{2}$ configuration.Ionization potential decreases as atomic size increases .So option (3) is correct.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313292 Read the statement A and statement B to mark the correct option given below.
Statement A :
The correct order of first ionisation enthalpy values of $Li, Na, F$ and Cl is $Na < Li < Cl < F$ .
Statement B :
The correct order of negative electron gain enthalpy values of $Li, Na, F$ and
Cl is $Na < Li < F < Cl$ .

1 Statement A is correct but Statement B is incorrect.

2 Statement A is incorrect but Statement B is correct.

3 Both statements are correct.

4 Both statements are incorrect.

Explanation:

First ionisation enthalpy of $F > Cl$ as I.E. decreases down the group. Similarly, I.E. of $Li > Na$ . Alkali metals have lower I.E. than halogens. So, statement A is correct. Negative electron gain enthalpy of given elements follows the order $Na < Li < F < Cl$ . So, statement B is also correct. So, the correct option is (3).

JEE Main - 2024

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313293 Assertion :
Phosphorus' has higher I.E. than sulphur.
Reason :
I.E. increases from left to right in a period.

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:

Phosphorus $(P)$ exhibits a higher ionization energy (I.E.) due to its half-filled electron configuration. So option (2) is correct.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313290 The first ionization potential of $Al$ , as compared to that of $Mg$ is :

1 Greater

2 Lower

3 The same

4 Twice as much

Explanation:

The first ionization potential of $Al$ is lower than that of Mg because valence shell configuration of Mg is $3 s^{2}$ and of Al is $3 s^{2}, 3 p^{1}$ . As
s-orbital is close to nucleus than p-orbital so removal of Ist $e^{-}$ from Mg is difficult and require more energy as compare to Al.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313291 Assertion :
Order of ionization potential across the period is $Na < Al < Mg < Si$
Reason :
Ionization potential decreases with decrease in atomic size.

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:

I.E. increases across a period. But $Mg$ has higher I.E. than $Al$ due to the fullfilled stability of $3 s^{2}$ configuration.Ionization potential decreases as atomic size increases .So option (3) is correct.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313292 Read the statement A and statement B to mark the correct option given below.
Statement A :
The correct order of first ionisation enthalpy values of $Li, Na, F$ and Cl is $Na < Li < Cl < F$ .
Statement B :
The correct order of negative electron gain enthalpy values of $Li, Na, F$ and
Cl is $Na < Li < F < Cl$ .

1 Statement A is correct but Statement B is incorrect.

2 Statement A is incorrect but Statement B is correct.

3 Both statements are correct.

4 Both statements are incorrect.

Explanation:

First ionisation enthalpy of $F > Cl$ as I.E. decreases down the group. Similarly, I.E. of $Li > Na$ . Alkali metals have lower I.E. than halogens. So, statement A is correct. Negative electron gain enthalpy of given elements follows the order $Na < Li < F < Cl$ . So, statement B is also correct. So, the correct option is (3).

JEE Main - 2024

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313293 Assertion :
Phosphorus' has higher I.E. than sulphur.
Reason :
I.E. increases from left to right in a period.

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:

Phosphorus $(P)$ exhibits a higher ionization energy (I.E.) due to its half-filled electron configuration. So option (2) is correct.

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