Question

Which of the following options correctly describe the trends in ionization energy (IE)? Select all that apply.

A) Ionization energy generally increases across a period.
B) Ionization energy generally decreases down a group.
C) Ionization energy is the energy required to add an electron to a neutral atom.
D) Noble gases have high ionization energy.

Answer 1

Ionization energy generally increases across a period and decreases down a group on the periodic table. Noble gases have high ionization energy.

Step-by-step explanation:

Ionization energy refers to the amount of energy needed to remove an electron from an atom. In terms of trends, ionization energy generally increases across a period from left to right on the periodic table. This is because as you move across a row, the atomic size decreases and the electrostatic interactions between the nucleus and valence electrons increases, which increases the energy required to remove electrons.

On the other hand, ionization energy generally decreases down a group from top to bottom. This is because the valence electrons are further away from the nucleus and experience less pull, making it easier to remove them.

Finally, noble gases, which are located in Group 18 of the periodic table, have high ionization energy. This is because noble gases have full valence electron shells, making it difficult to remove any electrons.