First check where neon is in the periodic table.

Neon atoms have atomic number ten, 10.

This means neon atoms have ten electrons moving around outside the nucleus.

Check the electron configuration for neon, 1s²2s²2p⁶ .

Neon atoms have a filled valence shell, 2s²2p⁶ .

You also know this because neon is in group 8A. All the elements in group 8A have filled s and p subshells,

with an outer set of electrons in the subshells, ns²np⁶.

There are no openings for electrons in the valence shell. Neon atoms will not form bonds.

This reasoning also applies to argon in group 8A

The rare gases like Xenon, Xe, which are lower in the group do not have to follow the octet rule because they can accept electrons in the "d" subshell. They form bonds under special conditions.