Angular Quantum Numbers Greater than 3

[Khoa Vu 3l]

When reviewing quantum numbers, I saw in the notes that the possible values of l are n-1, where l is the angular quantum number and n is the principal quantum number. I know that each value of l corresponds to a specific orbital (0=s, 1=p, 2=d, and 3=f). However, according to that notion, it should be possible to have an l value of 5 when the value of n is 6. Is n-1, then, simply a guideline to remind us that l cannot exceed the value of n or is it actually possible to have an l value greater than 3? If it is the latter, what orbital would an l value of 4 represent then?

[Halle Villalobos 3E]

Hi! According to the textbook, "although higher values of l (corresponding to g-, h-, . . . orbitals) are possible, the lower values of l (0, 1, 2, and 3) are the only ones that chemists need in practice." I hope this helps!

[Kat Stahl 2K]

Basically what she said^ It is possible but chemists don't use those and we won't need to know them. Here is a link that explains this: https://chem.libretexts.org/Courses/Ore ... um_Numbers