The noble gases have a particularly stable outer shell electronic configuration represented as

The noble gases, found in Group 18 of the periodic table, have a complete outer shell of electrons, which makes them particularly stable and unreactive. Their electronic configurations reflect this stability.

1. Helium (He): $1s^2$ - Helium has two electrons, filling its first and only shell.
2. Neon (Ne): $1s^2 2s^2 2p^6$ - Neon has a total of ten electrons, fully occupying both the first (2 electrons) and second shells (8 electrons).
3. Argon (Ar): $1s^2 2s^2 2p^6 3s^2 3p^6$ - Argon has eighteen electrons, completely filling its first three shells.
4. Krypton (Kr): $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6$ - Krypton has thirty-six electrons with full outer shells.
5. Xenon (Xe): $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6$ - Xenon has fifty-four electrons.
6. Radon (Rn): $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^{10} 6p^6$ - Radon has eighty-six electrons.

This complete outer electron shell is the reason why noble gases are chemically inert and do not readily form compounds under standard conditions.