Question

Four elements from the second period Boron to Oxygen can have the following IE$_1$ values (in kJ mol$^{-1}$): 1086.5, 800.6, 1313.9, 1402.3. The value of IE$_1$ for Nitrogen is:

• A. 1086.5
• B. 800.6
• C. 1402.3
• D. 1313.9

Hint:

In ionization energy trends, the half-filled p-orbitals of Nitrogen make it more stable, requiring more energy to remove an electron.

Answer 1

The Correct Option is C

Step 1: Identifying the elements.
The elements from Boron to Oxygen have the following trend in IE$_1$:
Boron (B) → 1086.5, Carbon (C) → 800.6, Nitrogen (N) → 1402.3, Oxygen (O) → 1313.9

Step 2: Analyzing the trends.
The ionization energies for Nitrogen (N) are higher than those for Carbon (C) and Oxygen (O) due to the stability of its half-filled p-orbital configuration.

Step 3: Conclusion.
The value of IE$_1$ for Nitrogen is 1402.3 kJ/mol, corresponding to option (3).