Electron Affinity of Halogens
Electron affinity of halogens decreases as you move down the group, with fluorine having the highest electron affinity and astatine having the lowest. The trends in electron affinity for halogens can be summarized as follows:
- Electron affinity generally decreases as you move down the group, with atomic size increasing.
- Fluorine has a higher electron affinity than chlorine due to its smaller size, which results in a stronger attraction between the incoming electron and the nucleus.
- High electron affinities of halogens is due to their almost complete outer shell of electrons.
- Electron affinity of halogens is related to their electronegativity, which decreases as you move down the group. This is because the electrons are progressively farther from the nucleus, resulting in a weaker attraction between the nucleus and the electrons.
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