What is the Difference Between Ionization Energy and Electron Affinity?
🆚 Go to Comparative Table 🆚Ionization energy and electron affinity are two distinct concepts in chemistry. Here are the main differences between them:
- Ionization Energy: This is the amount of energy required to remove an electron from an atom. It is a positive value because energy is needed to remove the electron. Ionization energy generally increases across a row on the periodic table and is minimum for the alkali metals, which have a single electron outside a closed shell.
- Electron Affinity: This is the amount of energy released when an atom gains an electron. It is a negative value because energy is released during the process. Electron affinities are more difficult to measure than ionization energies and are usually known to fewer significant figures.
In summary:
- Ionization energy is the energy required to remove an electron from an atom.
- Electron affinity is the energy released when an atom gains an electron.
While there is a relationship between ionization energy and electron affinity, they are not the same energy and have different sign conventions.
Comparative Table: Ionization Energy vs Electron Affinity
Ionization energy and electron affinity are both related to an atom's ability to attract or hold electrons, but they represent different concepts and processes. Here is a comparison between the two:
Ionization Energy | Electron Affinity |
---|---|
The energy required to remove an electron from an atom | The energy released when an electron is added to an atom |
Measures the attraction between the atom and its outermost valence electron | Measures the attraction between the atom and an incoming electron |
Always concerned with the formation of positive ions | Deals with the formation of negative ions |
First ionization energy is the energy needed to remove the first electron from a neutral atom | First electron affinity is the energy released when a neutral atom gains an electron |
Both ionization energy and electron affinity follow similar trends in the periodic table, as they are influenced by factors such as atomic size and electronegativity. However, they are not the same, and their values are typically different for a given element. For example, ionization energy is always measured in kilojoules per mole (kJ/mol), while electron affinity is typically given in kilojoules per mole (kJ/mol) but can be negative, indicating that energy is released during the process.
- Electronegativity vs Electron Affinity
- Electronegativity vs Ionization Energy
- Ionization Energy vs Binding Energy
- Electron Affinity vs Electron Gain Enthalpy
- Ionization vs Dissociation
- Excitation vs Ionization Potential
- Bond Energy vs Bond Dissociation Energy
- Isotope vs Ion
- Affinity vs Ion Exchange Chromatography
- Atom vs Ion
- Atom vs Ion
- Ions vs Electrons
- Ionization vs Electrolysis
- Bond Energy vs Bond Enthalpy
- First vs Second Ionization Energy (I1E vs I2E)
- Ionization vs Disassociation
- Protonation vs Ionization
- Enthalpy of Atomisation vs Bond Dissociation
- Energy vs Enthalpy