What is the maximum number of electrons that can occupy an s orbital?

The maximum number of electrons that can occupy an s orbital is 2. This limitation is due to the unique properties of orbitals, which are defined by quantum mechanics.

Each s orbital can hold two electrons, and this is explained by the Pauli Exclusion Principle, which states that no two electrons can have the same set of quantum numbers. An s orbital has a spherical shape, and it can hold a maximum of two electrons, which must have opposite spins. Therefore, when one electron occupies the s orbital with a specific spin orientation, the second electron, if present, must have the opposite spin to comply with this principle.

Other types of orbitals, such as p, d, and f, can hold more electrons due to their increased complexity and different shapes. For example, a p orbital can hold up to 6 electrons, a d orbital can accommodate up to 10 electrons, and an f orbital can contain up to 14 electrons. However, when focusing specifically on the characteristics of the s orbital, 2 remains the maximum capacity.