What is the number of orbitals when both the principal quantum number (n) and the azimuthal quantum number (l) values are provided?

The correct approach to determine the number of orbitals associated with specific quantum number values is by recognizing the relationship between the azimuthal quantum number (l) and the types of orbitals they represent. The azimuthal quantum number (l) defines the shape of the orbital and is directly correlated with the type of subshell: for l=0 (s), l=1 (p), l=2 (d), l=3 (f), and so forth.

For each type of orbital, the number of distinct orbitals is as follows:

• An s subshell (l=0) has 1 orbital.

• A p subshell (l=1) has 3 orbitals.
• A d subshell (l=2) has 5 orbitals.
• An f subshell (l=3) has 7 orbitals.

Therefore, by using the value of l to identify the type of subshell, we can directly state how many orbitals are present in that subshell. This makes option B the most appropriate choice as it provides a clear and straightforward method to determine the number of orbitals based solely on the value of l without any additional calculations or complexities. This understanding is crucial when analyzing electronic configurations