Electron Affinity Vs Ionization Energy
The difference between electron affinity and ionization energy is given below:
Electron Affinity |
Ionization Energy |
---|---|
Electron affinity is the energy released when an atom gains an electron. |
Ionization energy is the energy required to remove an electron from an atom. |
Electron affinity is typically expressed as a negative value for elements, indicating the release of energy. |
Ionization energy is a positive value, representing the energy input required. |
Electron affinity of an atom is related to its ability to attract an additional electron. |
Ionization energy is a measure of the ease with which an atom can lose an electron. |
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Electron Affinity
Electron Affinity is a measure of the attraction between an incoming electron and the nucleus of an atom or molecule. It is defined as the change in energy (in kJ/mole) of a neutral atom (in the gaseous phase) when an electron is added to the atom.
In this article, we will look into what electron affinity is, its periodic trends, the factors affecting electron affinity, and the values of electron affinity of different elements.
Table of Content
- What is Electron Affinity?
- Trends in Electron Affinity
- Types of Electron Affinity
- Factors Affecting Electron Affinity
- Electron Affinity Vs Ionization Energy