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Ionization energy is the energy required to eject an electron from an element, which increases across a period because the distance and force between proton and electron become greater. Electron affinity is the energy given off when a neutral atom in the gas phase gains an extra electron to form a negatively charged ion, therefore as you move across a period, atoms with more protons with smaller radius wants to attract electrons.
electron affinity is the energy it takes for an atom to gain an electron. ionization energy is the energy needed for an atom to lose an electron. the trend for both is the same, it increases across a group and decreases down a period.
Electron affinity is the energy given off when electrons are added to the atom. So basically, the electron affinity of an atom can determine if the atom wants electrons or not. On the other hand, ionization energy is the energy needed to remove an electron from an atom. They both increase across the periodic table and decrease down a group.
For the most part, electron affinity and ionization energy show the same trend across the periodic table. Fluorine has one of the greatest electron affinities and ionization energies, and these values decrease as you get closer to group 1/period 7. That being said, it's important to remember that electron affinity isn't as periodic as ionization energy - there are many, many exceptions for electron affinity. Some examples are group 2 having a lower electron affinity than group 3, and Manganese having a surprisingly low electron affinity as well.
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