The successive 5 ionisation energies of an element are 800 , 2427, 3658, 25024 and , respectively. By using the above values predict the group in which the above element is present :
- (A)Group 2
- (B)Group 13✓ Correct
- (C)Group 4
- (D)Group 14
Answer: (B)
Solution
Successive ionization energies climb steadily as electrons are removed from the same shell, but jump sharply once an electron must be pulled from a completed, lower-lying shell. Here through (800, 2427, 3658 kJ/mol) rise only modestly, but leaps to 25024 kJ/mol — nearly a sevenfold jump.
This sharp discontinuity right after the third electron shows that the element has exactly three electrons in its valence shell; the fourth electron has to be extracted from a stable, noble-gas-like core, which demands far more energy. Three valence electrons place the element in Group 13.
This sharp discontinuity right after the third electron shows that the element has exactly three electrons in its valence shell; the fourth electron has to be extracted from a stable, noble-gas-like core, which demands far more energy. Three valence electrons place the element in Group 13.
JEE Main · 2025 · 24 Jan 2025 · Shift 2 · Single correct option