Ionization Energy and Electron Affinity

[Hannah Faris 1C]

Can someone explain the difference between ionization energy and electron affinity?

[Kyle Golden Dis 2G]

Ionization energy is the amount of energy needed to remove an electron from an atom. Atoms that form cations have lower IE because they want to give away their electrons, which requires less energy. Electron affinity is the energy released when an electron is added to an atom. In simple terms, atoms that form anions have the highest electron affinity because they really want more electrons. Both properties increases up a group and across a period.

[Josephine Lu 4L]

Ionization energy is the energy needed to remove an electron from an atom in the gas phase. The further an electron is from the nucleus, the easier it is to remove. Ionization energies tend to decrease down a group (because of shielding from shells) and increase across a period (because greater attraction between electrons and nucleus). On the other hand, electron affinity is the energy released when an electron is added to a gas-phase atom.

[Yukta Italia 3I]

Why are electrons that are further away from the nucleus easier to remove?

[Nicolette_Canlian_2L]

Why are electrons that are further away from the nucleus easier to remove?

The inner electrons shield the other electrons, causing a decrease in the effective nuclear charge. This allows for an easier removal of a valence electron.

[Krista Mercado 1B]

Why are electrons that are further away from the nucleus easier to remove?

The nucleus has a positive charge, which attracts negatively charged electrons. If electrons are farther away from the nucleus, this positive nuclear charge is weaker, so the electrons aren't pulled as tightly towards the nucleus.

[SophiaKohlhoff4B]

Is there a trend for electron affinities?

[LorenzoDuvergne3I]

Ionization energy is the amount of energy needed to remove an electron from an atom. Atoms that form cations have lower IE because they want to give away their electrons, which requires less energy. Electron affinity is the energy released when an electron is added to an atom. In simple terms, atoms that form anions have the highest electron affinity because they really want more electrons. Both properties increases up a group and across a period.

I understand why anions would have an "affinity" for electrons but with regards to the actual definition how do they release more energy upon gaining an electron?

[Estelle Jung]

Ionization energy increases from left to right on the periodic table because of nuclear charge. The more protons there are in the nucleus, the stronger the attraction of the nucleus to the electrons.

[Selina Bellin 2B]

Is there a trend for electron affinities?

the trend for electron affinity is
-down a column it decreases due to the weaker force of attraction as energy levels increase
-across a row it increases because adding protons increase the force of attraction