Potassium (K)
* Electron Configuration: Potassium has 19 electrons. Its electron configuration is [Ar] 4s¹. This means it has one electron in its outermost shell (the 4s shell).
* Tendency to Lose an Electron: Potassium has a low ionization energy, meaning it doesn't require much energy to remove its outermost electron. By losing this electron, potassium achieves a stable electron configuration like the noble gas argon (Ar).
* Formation of a Cation: When potassium loses an electron, it becomes a positively charged ion (K⁺). The positive charge comes from the imbalance between protons (positive charge) and electrons (negative charge).
Fluorine (F)
* Electron Configuration: Fluorine has 9 electrons. Its electron configuration is [He] 2s² 2p⁵. It has 7 electrons in its outermost shell (the 2p shell).
* Tendency to Gain an Electron: Fluorine has a high electronegativity, meaning it strongly attracts electrons. By gaining one electron, it completes its outermost shell (2p) and achieves a stable electron configuration like the noble gas neon (Ne).
* Formation of an Anion: When fluorine gains an electron, it becomes a negatively charged ion (F⁻). The negative charge comes from the excess of electrons compared to protons.
Summary
Potassium loses an electron to achieve a stable electron configuration, becoming a positively charged cation (K⁺). Fluorine gains an electron to achieve a stable electron configuration, becoming a negatively charged anion (F⁻). This exchange of electrons is what drives the formation of ionic bonds, where the oppositely charged ions attract each other.
