The full electron configuration for Neon (Ne) is 1s²2s²2p⁶.
Neon (Ne) is a noble gas, element number 10 on the periodic table, meaning it possesses 10 electrons. Its electron configuration describes how these electrons are arranged in orbitals around the nucleus. This specific arrangement contributes to Neon's stability and its unreactive nature.
Understanding Neon's Electron Configuration
The process of filling electron orbitals follows a specific order, beginning with the lowest energy levels. For Neon, with its 10 electrons, the orbitals are filled as follows:
- 1s Orbital: The first two electrons occupy the 1s orbital, which is the closest to the nucleus and has the lowest energy level. Since a single s-orbital can hold a maximum of two electrons, this orbital becomes full.
- 2s Orbital: With the 1s orbital filled, the next two electrons proceed to fill the 2s orbital. Like the 1s orbital, the 2s orbital can also hold a maximum of two electrons, making it full as well.
- 2p Orbital: After the 1s and 2s orbitals are filled (accounting for 4 electrons), the remaining six electrons occupy the 2p orbital. A p-subshell consists of three individual p-orbitals (2px, 2py, 2pz), each capable of holding two electrons. Therefore, the 2p subshell can accommodate a total of six electrons, which perfectly matches the remaining number of electrons for Neon.
This sequential filling results in the final configuration 1s²2s²2p⁶.
Breakdown of Electron Distribution for Neon (Ne)
| Orbital | Number of Electrons | Total Electrons (Cumulative) |
|---|---|---|
| 1s | 2 | 2 |
| 2s | 2 | 4 |
| 2p | 6 | 10 |
This configuration shows that Neon has a completely filled outer electron shell (the second shell, containing 2s²2p⁶), which is characteristic of noble gases and explains their chemical inertness.
