1s22s22p6

1s22s22p6 refers to an electron configuration. This notation describes the arrangement of electrons within the atomic orbitals of an atom. The numbers indicate the principal energy level, and the letters (s, p) denote the type of atomic orbital. The superscripts show the number of electrons occupying each orbital.

In this configuration, there are two electrons in the 1s orbital. The principal energy level 2 contains two electrons in the 2s orbital and six electrons in the 2p orbitals. The 2p subshell consists of three individual orbitals, each capable of holding a maximum of two electrons, hence a total of six electrons can be accommodated.

The 1s22s22p6 electron configuration represents a filled valence shell. This specific arrangement of electrons is characteristic of the noble gas Neon (Ne), which has an atomic number of 10. Atoms with fully filled electron shells are generally very stable and unreactive due to the low energy state achieved by having all available electron energy levels occupied. This stability is a fundamental concept in understanding chemical bonding and the periodic trends of elements.