For n equals 3, the possible values of the azimuthal quantum number l are
Correct answer: C. 0, 1 and 2
- 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.
Report an error
The more specific you are, the faster it gets fixed. A source beats an opinion.
Prefer email? support@testustad.com
About Quantum Numbers
Quantum numbers describe an electron's energy level, subshell, orbital orientation and spin. You examine the principal, azimuthal, magnetic and spin quantum numbers, their allowed values, orbital capacity and how they determine electronic configurations and distinguish electrons within an atom.
Practise Atomic Structure
922 free Atomic Structure MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Discussion
Stuck on an option, or know a faster way to get there? Ask or explain it here.
No comments yet. Be the first to explain this one.
Exams that ask Chemistry questions like this
Chemistry is on 14 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
More Quantum Numbers questions
The principal quantum number n determines
The maximum number of electrons that can occupy the shell with n = 3 is
Which set of quantum numbers is not possible?
The maximum number of electrons that can occupy the third shell is
The magnetic quantum number m for an electron in a 2p subshell can take the values
Which set of quantum numbers is not permitted?