Final answer:
The ground-state electron configuration of a neutral atom of neon is 1s², 2s², 2p⁶, representing a completely filled first and second energy levels and making neon a noble gas.
Step-by-step explanation:
The ground-state electron configuration of a neutral atom of neon. Neon, with an atomic number of 10, has its first two energy levels completely filled, with two electrons in the 1s orbital, two in the 2s orbital, and six in the 2p orbitals. This configuration reflects a filled valence shell, making neon a noble gas with stable electron configuration that corresponds to the electron configuration of the noble gas neon itself. Noble gases have their orbitals in the n = 1 and n = 2 shells filled, which is true for neon as well, indicating a stable and nonreactive atomic structure.