For n equals 3, the possible values of the azimuthal quantum number l are
- A. 0 only
- B. 0 and 1
- C. 0, 1 and 2
- D. 1, 2 and 3
Explanation
The azimuthal quantum number runs from 0 up to n minus 1, so for the third shell it takes the values 0, 1 and 2, corresponding to the 3s, 3p and 3d subshells. It never equals n itself, which rules out the last option. This is why the first shell has only an s subshell.
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