The first four successive ionization enthalpies ( _ i H₁ , _ i H₂ , _ i H₃ , and _ i H₄ ) for an unknown main group element M are 801 , 2427 , 3660 , and 25025 ~kJ ~mol ⁻¹ respectively. The general formula of the stable oxide formed by element M is :

Step-by-step solution

The successive ionization enthalpies show a massive jump between the third ( _ i H₃ = 3660 ~kJ ~mol ⁻¹ ) and the fourth ( _ i H₄ = 25025 ~kJ ~mol ⁻¹ ) ionization enthalpies. This sudden large increase indicates that the fourth electron is being removed from a highly stable, inner noble gas core. Thus, element M has exactly three valence electrons. An element with three valence electrons belongs to Group 13 and exhibits a valency of 3 . Therefore, the formula of its stable oxide will be M ₂ O ₃ . Answer: M ₂ O ₃