Atomic StructureEasy
Question
When the value of azimuthal quantum number is 3, the maximum and minimum values of spin multiplicity are
Options
A.1, 8
B.8, 1
C.6, 1
D.7, 0
Solution
Spin multiplicity = 2s + 1, where s = magnitude of total spin quantum number.
$l$ = 3 ⇒ Number of orbitals = 2 × 3 + 1 = 7
∴ Maximum spin multiplicity = $2 \times \frac{7}{2} + 1 = 8$
(When each orbital has single electron in same spin)
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