* Octet Rule: Atoms strive to achieve a stable electron configuration, resembling the noble gases. Noble gases have a full outer shell of electrons, making them very unreactive. The octet rule states that atoms tend to gain, lose, or share electrons to have eight electrons in their outermost shell.
* Sodium's Electron Configuration: Sodium (Na) has 11 electrons. Its electron configuration is 2, 8, 1. This means it has one electron in its outermost shell (valence shell).
* Losing an Electron: By losing its single valence electron, sodium becomes a positively charged ion (Na+). Its new electron configuration is 2, 8, which matches the stable electron configuration of neon (Ne), a noble gas.
* Stability Through Filled Shells: Having a full outer shell makes sodium more stable because:
* It eliminates the tendency to react with other atoms to gain or share electrons to achieve a full outer shell.
* The electrostatic attraction between the nucleus and the remaining electrons is stronger, making the ion more stable.
In summary: Sodium loses its valence electron to achieve a stable octet configuration like neon, making it more stable and less reactive.
