Atomic Properties

[Sofia Cerpa 2E]

what is the relation between ionization energy and electron affinity?

[Anton Truskovsky 2K]

Ionization energy is the amount of energy required to strip an electron off of an atom.
Electron affinity is the tendency of an atom to hold on to its electrons.
So Ionization energy and Electron affinity (better thought of as electronegativity in this comparison) follow the same trend on the periodic table, increase down a period, decrease down a group.

[Lily Dabrowski 2G]

Ionization energy and electronegativity both increase up and across the periodic table. Electronegativity is the measure of how likely an atom is to attract electrons, while ionization energy is the measure of energy required to remove an electron from an atom in its neutral gas state. Both increase up and across because later group elements approach a fuller valence shell; they are more inclined to gain electrons to fill that valence shell, and as a result it is more difficult to remove an electron from them.

[Ellie Fox 2K]

Ionization energy is the amount of energy required to remove an electron from an isolated atom or molecule. On the other hand, electron affinity is the degree to which an atom or molecule attracts additional electrons or the minimum energy required to remove an electron.