Final answer:
This question involves determining the order of orbital filling or the electron configuration for an atom, following the rules of electron arrangement in quantum chemistry.
Step-by-step explanation:
The subject of this question is electron configurations, specifically the order of orbital filling according to the rules outlined in quantum mechanics and illustrated in various figures provided as reference. Electron configurations describe the arrangement of electrons in atomic orbitals and abide by principles such as the Aufbau principle, which dictates the order in which orbitals are filled, and Hund's rule regarding the filling of sublevels within orbitals.
When filling orbitals with electrons, the 1s orbital is filled first, followed by the 2s, and then the 2p orbitals. For example, the electron configuration for oxygen, which has 8 electrons, would be written as 1s² 2s² 2p⁴ following the described principles.
Students may also use noble gas shorthand notation to simplify writing electron configurations for elements with many electrons by representing core electrons as the noble gas from the preceding period. For instance, fluorine's electron configuration can be abbreviated as [He] 2s² 2p⁵ instead of writing out all the individual lower level electron states.
The complete question is: Express your answer in complete form in the order of orbital filling as a string without blank space between orbitals. For example, 1s²²s² should be entered as 1s²²s². is: