The structure of an atom is organized into shells, which can be further divided into subshells or sublevels. Each shell is associated with a principal quantum number, denoted as \( n \), which indicates the energy level of the electron. The possible subshells corresponding to each shell number are defined as follows:
- For \( n = 1 \), the only subshell is s.
- For \( n = 2 \), the available subshells are s and p.
- For \( n = 3 \), the subshells include s, p, and d.
- For \( n = 4 \), the subshells expand to s, p, d, and f.
As the principal quantum number \( n \) increases, the variety of subshells also increases. It is important to note that even at \( n = 5 \), the subshells remain limited to s, p, d, and f. Understanding these subshells is crucial for grasping the arrangement of electrons in an atom, which ultimately influences its chemical properties and behavior.
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