Final answer:
The number of sublevels within a principal energy level is equal to the principal quantum number (n), with the energy of these sublevels increasing in the order s < p < d < f. There are overlaps in energy levels in larger atoms, such as the 4s sublevel filling before the 3d. Sublevels are linked to orbitals where electrons are likely found, with each sublevel accommodating a specific number of electrons.
Step-by-step explanation:
When investigating the relationship between the number of principal energy levels and the number of sublevels in an atom, we observe that each principal energy level corresponds to a specific number of sublevels. The principal energy level, denoted by the quantum number n, has the same number of sublevels. For instance, the first energy level (n=1) has one sublevel (1s), the second energy level (n=2) has two sublevels (2s and 2p), and this pattern continues such that the nth energy level will have n sublevels.
Furthermore, the energy of sublevels within a principal energy level increases in the order of s < p < d < f, though there is an overlap in energy levels as atoms get larger. For instance, the 4s sublevel fills before the 3d sublevel, even though they are part of the third and fourth energy levels, respectively.
Understanding Electron Configurations
To determine the electron configuration of an element, we use the Aufbau principle, which states that electrons fill the lowest available energy sublevels first. As seen in various figures throughout the texts, such as Figure 9.6.6 and Figure 6.22, the energy levels for different orbitals are highlighted, showing the order in which electrons fill up the sublevels within the energy levels. This is crucial in predicting and understanding the chemical behavior of elements.
Each sublevel corresponds to one or more orbitals, regions in space where there is a high probability of finding an electron. For instance, the s sublevel has one orbital that can hold two electrons, the p sublevel has three orbitals that can hold a total of six electrons, the d sublevel has five orbitals holding up to ten electrons, and the f sublevel has seven orbitals holding up to fourteen electrons.