Final answer:
The electron configuration for neon ends with 2s²2p¶, indicating a full valence shell making neon a very stable and non-reactive noble gas. A neon atom has two electrons in its outermost energy level, making it a stable atom.
Step-by-step explanation:
The electron configuration for neon (Ne) should end with the configuration 2s22p6. A neon atom has ten electrons, with two in the first energy level (1s2) and the remaining eight in the second energy level. Since the second energy level (2s22p6) can hold a maximum of eight electrons and is full, neon is a very stable atom and is not reactive under normal conditions. Neon is a noble gas with a complete valence shell, which explains its chemical inertness.
A neon atom has two electrons in its outermost energy level, which is the second energy level. The electron configuration of neon is 1s²2s²2p⁶. The outermost energy level of neon is full, which makes it a very stable atom.