Electron Affinity

[905934067]

How does electron affinity relate to the reactivity and stability of atoms? Can you provide examples of elements or groups in the periodic table that exhibit particularly high or low electron affinity, and explain the implications for their chemical behavior? Additionally, how does electron affinity influence the formation of negative ions; are there any exceptions to the general trends in electron affinity within the periodic table?

[Isaac Wong 3F]

Electron affinity: energy released when adding e-
Energy is released when when adding an e- because the e- added allows the atom to become more stable. Therefore, higher e- affinity means greater reactivity (to gain an e-) and less stable before gaining that e-.
F would have a high e- affinity
K would have a low e- affinity
A greater e- affinity means a greater likelihood to form a negative ion, anion (see F, Cl, etc)

[305981900]

Electron affinity usually refers to energy that changes through adding an electron to a netural atom. If the atom his high electron affinity an element lill accept an additional electron to be able to fill the outer most shell. If the atom has low electron affinity then it is less likely to gain an electron . Low electron affinity are usually alkali metals and those with high electron affinity are halogens. Trend to talk about is to the left to the right it will Increase and from the top to the bottom it will decrease.