Chemistry – The Periodic Table - Noble gases | e-Consult

The Group VIII noble gases (Helium, Neon, Argon, Krypton, Xenon, and Radon) are known for their exceptional unreactivity. This unreactivity stems directly from their electronic configuration. Each noble gas possesses a full outermost electron shell, meaning their valence shell (the outermost shell) contains eight electrons, fulfilling the octet rule. This full shell makes them exceptionally stable and prevents them from readily gaining, losing, or sharing electrons with other atoms.

Unlike other elements which tend to react to achieve a stable octet, noble gases have no need to do so. Their electron configuration is already in a very stable state. Therefore, they have very little tendency to form chemical bonds. The high ionization energy required to remove an electron from a noble gas further contributes to their inertness.

In summary, the full valence shell electronic configuration of the noble gases is the fundamental reason for their unreactivity. They are already in a stable, energetically favourable state.