Final answer:
Based on the given successive ionization energies and the elimination of other options, the correct answer is Carbon (C), which matches this ionization pattern after accounting for its valence electrons.
Step-by-step explanation:
The student is asking which period 2 element has particular successive ionization energies. The sharp increase between the sixth (E_(i6)) and seventh (E_(i7)) ionization energies suggests that the first six electrons are from the valence shell, while the seventh electron is from a more tightly bound inner shell. This pattern is characteristic of elements that have six valence electrons in the second energy level, which corresponds to oxygen (O). However, oxygen is not one of the options given. If we look at the list, the only element that has fewer than six valence electrons and also fits the pattern of a sharp increase after losing a certain number of valence electrons is carbon (C) with its four valence electrons. After the loss of its valence electrons, a much higher energy is required to remove an electron from the next energy level. Therefore, based on the data provided and the process of elimination, the correct answer would be Carbon (C).