JEE Main 202622 JanuaryEvening Shift
- Exam
- JEE Main
- Year
- 2026
- Date
- 22 January
- Shift
- Evening Shift
- Subject
- Chemistry
- Chapter
- Classification of Elements and Periodicity in Properties
JEE Main 2026 · 22 January · Evening Shift · Chemistry · Classification of Elements and Periodicity in Properties
Given below are two statements : Statement I : C Statement II :...
Given below are two statements :
Statement I: is the correct order in terms of first ionization enthalpy values.
Statement II: is the correct order in terms of the magnitude of electron gain enthalpy values.
In the light of the above statements, choose the correct answer from the options given below :
Statement I: is the correct order in terms of first ionization enthalpy values.
Statement II: is the correct order in terms of the magnitude of electron gain enthalpy values.
In the light of the above statements, choose the correct answer from the options given below :
Options
- AStatement I is true but Statement II is false
- BStatement I is false but Statement II is true
- CBoth Statement I and Statement II are false
- DBoth Statement I and Statement II are true
Correct answer
D. Both Statement I and Statement II are true
Step-by-step solution
Statement I:
Ionization enthalpy generally increases across a period from left to right.
However, Nitrogen () has a stable half-filled electronic configuration, making it harder to remove an electron compared to Oxygen ().
Thus, the order is .
Statement I is true.
Statement II:
For Group 16 elements, Oxygen has an exceptionally low magnitude of electron gain enthalpy due to its small size and high inter-electronic repulsions in the subshell.
The magnitude of electron gain enthalpy decreases down the group from Sulphur onwards.
The correct order of magnitude is .
Statement II is true.
Both statements are correct.
Ionization enthalpy generally increases across a period from left to right.
However, Nitrogen () has a stable half-filled electronic configuration, making it harder to remove an electron compared to Oxygen ().
Thus, the order is .
Statement I is true.
Statement II:
For Group 16 elements, Oxygen has an exceptionally low magnitude of electron gain enthalpy due to its small size and high inter-electronic repulsions in the subshell.
The magnitude of electron gain enthalpy decreases down the group from Sulphur onwards.
The correct order of magnitude is .
Statement II is true.
Both statements are correct.