Electron Configuration:
* 1s² 2s² 2p⁶ 3s¹
Breakdown:
* 1s²: The first energy level (n=1) has one sublevel (s), which can hold up to 2 electrons. So, the 1s sublevel is filled with 2 electrons.
* 2s²: The second energy level (n=2) also has an s sublevel, which is filled with 2 electrons.
* 2p⁶: The second energy level also has a p sublevel, which can hold up to 6 electrons. This sublevel is completely filled.
* 3s¹: The third energy level (n=3) has an s sublevel, which contains only 1 electron.
Simplified Representation:
* [Ne] 3s¹ This is a shorthand notation using the electron configuration of the previous noble gas (Neon), [Ne], followed by the remaining electron in the 3s sublevel.
Key Points:
* Energy Levels: Electrons are organized into energy levels, with higher numbers representing higher energy levels.
* Sublevels: Within each energy level, there are sublevels (s, p, d, f) with different shapes and energies.
* Electron Filling: Electrons fill sublevels in order of increasing energy, following the Aufbau principle.
* Valence Electron: The outermost electron (3s¹) in sodium is called the valence electron and is responsible for sodium's chemical reactivity.
Let me know if you would like more detail on any of these points!
