JEE Main 2026 — Apr 4, Shift 2 — Chemistry solution

JEE Main2026Apr 4, Shift 2Chemistry

The 1 $^{s t}$ ionization enthalpy for Mg is +737 kJ/mol. The most probable estimated value of the 2 $^{n d}$ ionization enthalpy of Mg is _____.

A
– 906 kJ/mol
B
–856 kJ/mol
C
+1450 kJ/mol
D
+590 kJ/mol

Solution

Successive ionization enthalpies always increase: removing a second electron from a now-positively-charged ion requires more energy. So $I E_{2} > I E_{1} = 737$ kJ/mol.

Furthermore, since IE values are always positive (energy is absorbed), negative options are ruled out. Only +1450 kJ/mol satisfies both conditions.

$∴ I E_{2} (Mg) \approx + 1450$ kJ/mol.

← Back to full paper

Practice more Chemistry

Concept-wise practice with instant solutions on Fundamenthol.

Start practicing →