Which of the following exhibits the correct orders for both atomic radius and ionization energy, respectively?
A) S, O, F, and F, O, S
B) F, S, O, and O, S, F
C) S, F, O, and S, F, O
D) F, O, S, and S, O, F
E) none of these

Question

Quizplus · Accepted Answer

In general, atomic radius decreases across a period (from left to right) because as the atomic number increases, there are more protons in the nucleus attracting the electrons in the same energy level, thus reducing the size. Comparatively, atomic radius increases down a group (from top to bottom) because there are more energy levels and the outermost electrons are further from the nucleus.

In contrast, ionization energy increases across a period because the atomic radius decreases and the outermost electrons are held more tightly, requiring more energy to remove them. The group trend is the opposite, as ionization energy decreases down a group because the outermost electrons are further from the nucleus, making them easier to remove.

Based on these trends, the correct order for atomic radius from biggest to smallest is S, O, F, and the correct order for ionization energy from smallest to biggest is S, O, F. Therefore, choice D (F, O, S for atomic radius and S, O, F for ionization energy) is the best answer.

Which of the Following Exhibits the Correct Orders for Both