Which of the following statements best explains the trend in successive ionization energies for an element with the electron configuration of [Ne]3s²?

The first ionization removes one 3s electron, giving a Mg⁺ ion with a [Ne]3s¹ configuration; the second removes the last 3s electron, yielding a Mg²⁺ ion with a closed‑shell [Ne] configuration. Because both 3s electrons are in the same outer shell, their ionization energies are relatively low and close in value. After the second electron is removed, any further ionization must take an electron from the inner 2p shell, which is tightly bound to the nucleus. Consequently, the third ionization energy jumps sharply, reflecting the higher energy needed to remove an inner‑shell electron. Thus, the trend shows two similar, low ionization energies followed by a large increase.