The first ionisation enthalpies of four consecutive elements present in the second period of the periodic table are 8.3,11.3,14.5 and 13.6eV respectively. Which one of the following is the first ionisation enthalpy of nitrogen ?

Question

The first ionisation enthalpies of four consecutive elements present in the second period of the periodic table are 8.3,11.3,14.5 and 13.6eV respectively. Which one of the following is the first ionisation enthalpy of nitrogen ? (A) 13.6 (B) 14.5 (C) 11.3 (D) 8.3

Tardigrade Admin · Accepted Answer

The electronic configuration of Nitrogen is 1s22s22p3 . It has a half-filled stable configuration. So nitrogen will have maximum ionisation enthalpy. So first ionisation enthalpy of nitrogen is 14.5 eV.

Q. The first ionisation enthalpies of four consecutive elements present in the second period of the periodic table are $8.3, 11.3, 14.5$ and $13.6 e V$ respectively. Which one of the following is the first ionisation enthalpy of nitrogen ?

$13.6$

$14.5$

$11.3$

$8.3$

The electronic configuration of Nitrogen is $1 s^{2} 2 s^{2} 2 p^{3}$ . It has a half-filled stable configuration. So nitrogen will have maximum ionisation enthalpy. So first ionisation enthalpy of nitrogen is $14.5$ eV.

Q. The first ionisation enthalpies of four consecutive elements present in the second period of the periodic table are 8.3,11.3,14.5 and 13.6eV respectively. Which one of the following is the first ionisation enthalpy of nitrogen ?

13.6

14.5

11.3

8.3