The noble gas elements have outermost energy levels with full s and p orbitals.
Depending on what the level is, it may start filling d orbitals, or start on a new shell with s orbitals available.
the noble gases, in row 18
Elements with full s and p orbitals in their highest electron shell are the noble, or inert, gases of the last column on the periodic table: He, Ne, Ar, Kr, Xe, and Rn.
Electrons fill orbitals following the Aufbau principle, which states that electrons occupy the lowest energy orbital available first before moving to higher energy levels. This means filling orbitals in order of increasing energy levels: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, etc.
Noble gases are unreactive with the outermost energy level full.
Outermost energy level is full if there are 8 electrons in the valence shell.
When they fill their outermost energy levels. Metals will WANT more electrons and Non-Metals will have EXTRA electrons to give. So in a way, Metals will actually fill their outermost energy levels while Non-Metals will empty them; all with the goal of having a FULL valency shell which is stable. This is the basis for ionic bonding.
All of the Nobel gases do (He Ne Ar Kr Xe and Rn)
The 2 outermost orbitals that must be filled to satisfy the octet rule are the s and p orbitals. These orbitals can hold a maximum of 8 electrons in total, which is needed to achieve a stable, full octet configuration for many elements.
Helium has a full outermost energy level containing only two electrons.
Atoms form chemical bonds to achieve a full outermost energy level by sharing, gaining, or losing electrons. Valence electrons are the electrons in the outermost energy level of an atom, and having a full outermost energy level makes the atom more stable. This stability is achieved when there are eight electrons in the outermost energy level, known as the octet rule.
Atoms filled with outermost energy levels tend to be stable and are less likely to participate in chemical reactions. These atoms have a full valence shell, so they are less reactive and more likely to form stable compounds.