Answer:
The correct answer is option D: Te<Se<S<O.
Step-by-step explanation:
Ionization energy is the minimum amount of energy required to remove an electron from an atom or a positive ion. It is a measure of the strength of the atomic nucleus and the attraction between the nucleus and the outermost electrons. The higher the ionization energy, the harder it is to remove an electron from an atom.
Option D correctly orders the atoms from lowest to highest ionization energy. Te has the lowest ionization energy, followed by Se, S, and O. This is because Te has the largest atomic radius, which means its outermost electrons are farther from the nucleus and less strongly attracted to it. Se, S, and O have smaller atomic radii, so their outermost electrons are closer to the nucleus and more strongly attracted to it, resulting in higher ionization energies.