Practice Quiz

IB Chemistry Test Prep

Category - IB Chemistry

Start a Study Session Sign up for Question of the Day
Which of the following sets of quantum numbers is impossible for an electron?
  1. n = 4, l = 3, ml = 2, s = ½
  2. n = 2, l = 1, ml = 2, s = -½
  3. n = 3, l = 2, ml = -1, s = ½
  4. n = 4, l = 1, ml = 1, s = -½
  5. n = 2, l = 1, ml = 1, s = ½
Explanation
Answer: n = 2, l = 1, ml = 2, s = -½

The principle quantum number can take any positive integer value. The angular quantum number can take any positive integer value up to (n-1). The magnetic quantum number can take any value -l through +l. Thus, the set of quantum numbers n = 2, l = 1, ml = 2, s = -½ is impossible because the magnetic quantum number is larger than the angular quantum number.
Previous Next
Was this helpful? Upvote!
Login to contribute your own answer or details
Start a Study Session Sign up for Question of the Day

Top questions

Related questions

Most popular on PracticeQuiz