electron affinity vs ionization energy

[theonlytycrane]

Hoping to clarify my understanding:

For electron affinity we're talking about an atom gaining an electron (energy released). So more negative energies mean more affinity.

For ionization energy we're talking about an atom losing an electron (energy required). So more lower energies mean more ionizable.

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[betterfuture]

Yeah. That's how I know it, atleast.

Electron affinity: the energy released by an atom in a gaseous state when it gains an electron. (exothermic reaction)

More (-) value means it is really stable and so it releases alot of energy by gaining that electron. Electron is happy.

There are instances when it is actually really unfavorable to add an electron to an atom because you might have to open up another orbital or add an electron to the orbitals, if they are half full, leaving the atom quite unstable. So instead, you would add energy to add that electron to the atom rather that the atom releasing it. So it would be endothermic in this case.


Ionization energy: the energy needed to remove an electron from an atom in a gaseous state.(endothermic)

It takes energy to remove an electron because the electron is attracted to the really positive nucleus, and depending on which shell and orbital the electron is located that is being removed and the number of protons present in the nucleus, it will take different amounts of energy to complete that removal.

 

[BerkReviewTeach]

Once again, a helpful and well articulated thread.