S1.3.4 Sublevels and orbitals Notes

Sublevels (s, p, d, f): Division of Main Energy Levels into Sublevels and Their Shapes

1. Let's assume that you are walking into a massive multi-story library.
2. Each floor represents a different energy level, and within each floor, there are sections labeled by genre: fiction, science, history, and more.
3. Within each section, shelves hold books, neatly arranged.

Similarly, electrons in an atom are organized into energy levels (floors), sublevels (sections), and orbitals (shelves).

The Division of Main Energy Levels into Sublevels

1. Electrons in an atom are not scattered randomly.
2. Instead, they occupy specific energy levels around the nucleus, denoted by the principal quantum number $n$ (e.g., n = 1, 2, 3, etc.).
3. Each energy level is further divided into sublevels, which represent regions where electrons are most likely to be found.
4. These sublevels are labeled as s, p, d, and f, and their energy increases in the order: $$ \text{s < p < d < f} $$

Key Features of Sublevels:

1. Sublevel Types:
   1. s (sharp): The lowest energy sublevel.
   2. p (principal): Higher energy than s.
   3. d (diffuse): Higher energy than p.
   4. f (fundamental): The highest energy of the four.
2. Number of Sublevels: The number of sublevels in a given energy level equals the value of n:
   1. For n = 1, only the s sublevel exists.
   2. For n = 2, there are two sublevels: s and p.
   3. For n = 3, there are three sublevels: s, p, and d.
   4. For n = 4, there are four sublevels: s, p, d, and f.
3. Maximum Electrons in a Sublevel: Each sublevel can hold a specific number of electrons:
   1. s: 2 electrons (1 orbital).
   2. p: 6 electrons (3 orbitals).
   3. d: 10 electrons (5 orbitals).
   4. f: 14 electrons (7 orbitals).

Shapes and Orientations of Sublevels