Consider the following quantum numbers sets; determine if they can occur together to specify an orbital. If not indicate which rule has been violated?

n=2, l=-1, ml=-1
n=3, l=1, ml=0
n=3, l=3, ml=-3

1 Answer
Truong-Son N.
Jan 26, 2018

Well, recall the ranges of each quantum number.

  • n > 0, and must be an integer.
  • 0 <= l <= n-1, and must be an integer.
  • |m_l| <= l

Thus, the first configuration is not possible since l must be nonnegative (the orbital shape doesn't exist), and the third configuration is not possible since l > n-1 (so, 3f orbitals don't exist).

The second configuration is a 3p_z orbital.

n = color(blue)(3) -> color(blue)(3)p_z

l = color(blue)(1) -> 3color(blue)(p)_z

m_l = color(blue)(0) -> 3p_color(blue)(z)

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