What is the electron configuration for an atom of Neon (Ne)?

The electron configuration for an atom of Neon (Ne) is 1s² 2s² 2p⁶, which indicates the distribution of electrons in atomic orbitals. Neon has an atomic number of 10, meaning it possesses a total of 10 electrons.

Starting from the lowest energy level, the 1s orbital can hold up to 2 electrons, which accounts for the first two electrons (1s²). Next, the 2s orbital also holds 2 electrons (2s²), bringing the total to 4. Finally, the 2p orbital can hold a maximum of 6 electrons. Since Neon has a total of 10 electrons, the 2p orbital is completely filled with 6 electrons (2p⁶).

This configuration results in a full outer electron shell, which is characteristic of noble gases. Neon is chemically inert due to this filled outer shell, making it stable and nonreactive under normal conditions.

The other configurations listed do not represent Neon accurately due to the number of electrons incorrectly inferred in their arrangements. For example, one suggests an incomplete filling of the 2p sublevel, while others indicate additional electrons that exceed the total of 10 electrons in Neon. This