Final answer:
An s subshell (ℓ=0) has 1 orbital, a p subshell (ℓ=1) has 3 orbitals, a d subshell (ℓ=2) has 5 orbitals, and an f subshell (ℓ=3) contains 7 orbitals. The number of orbitals and their shape complexity increase with higher values of the azimuthal quantum number.
Step-by-step explanation:
When the azimuthal quantum number (ℓ) is 0, the subshell is called an s subshell, which has a total of 1 orbital. The s orbitals are spherically symmetrical, with the spherical shape increasing in size as we go from 1s to 2s to 3s.
For ℓ = 1, the resulting subshell is a p subshell consisting of 3 orbitals: px, py, and pz, each having a shape. As the value of ℓ increases, the number of orbitals and their complexity also increase. The d subshell with ℓ = 2 contains 5 orbitals, the f subshell with ℓ = 3 consists of 7 orbitals, and so on for g and h subshells.
The subshell with l=1 is called the p subshell. The p subshell consists of three orbitals: px, py, and pz. Each p orbital is -shaped with two lobes. The px orbital is oriented along the x-axis, the py orbital is oriented along the y-axis, and the pz orbital is oriented along the z-axis.