* Energy Levels: S orbitals are at a lower energy level than p orbitals within the same electron shell. This means that an electron in an s orbital is closer to the nucleus on average and experiences a stronger attraction.
* Shape: S orbitals are spherical, while p orbitals are dumbbell-shaped. This difference in shape affects the spatial distribution of electrons and influences their energy levels.
* Electron-Electron Repulsion: The s orbital is smaller and more compact than the p orbital. This means that the electrons in an s orbital experience less repulsion from each other, making the s orbital a more energetically favorable location for electrons.
Summary:
The combination of lower energy levels, smaller size, and less electron-electron repulsion in s orbitals compared to p orbitals leads to the filling of s orbitals before p orbitals. This principle is fundamental to understanding the electronic configuration of atoms and the behavior of chemical elements.
