Why does ionization energy increase as atomic radius decreases?

Answer 1

Ionization energy is how much energy is needed to remove an electron from the valence shell (the outermost shell). When the atomic radius is smaller, you will need more energy to remove an electron because the pull from the nucleus on the electron is stronger. If the atomic radius is larger, then it will be much easier to remove an electron from the valence shell because there are more layers (shieldings) between the nucleus and valence shell.

Answer 2

The ionization energy is the energy it requires to remove an electron from an atom. As you go across the rows, the number of protons (atomic number) increases which increases the positive charge on the nucleus. That, in turn, holds its electrons closer to the atom making it more difficult to remove an electron.

Answer 3

The first ionization energy increases as you move from left to right across a period on the Periodic Table, but it decreases as you move down a group. This is because with each additional element down a group, you have a new energy level containing electrons. Each additional energy level is farther from the positively charged nucleus and is shielded from the nucleus by the inner electrons. Therefore, it becomes easier to remove the highest energy electron, and the first ionization energy decreases down the group.

Answer 4

it decreases because it'll be easier for the atom to lose its valence electrons the relation is inversely proportional