For an atomic orbital described by the principal quantum number n and azimuthal (angular momentum) quantum number l: - The number of angular nodes is equal to l. - The total number of nodes is equal to n - 1. - The number of radial nodes is the total number of nodes minus the number of angular nodes, i.e., (n - 1) - l. For a 4d orbital: - Principal quantum number n = 4. - For a d orbital, the azimuthal quantum number l = 2 (s=0, p=1, d=2, f=3). - Number of angular nodes = l = 2. - Number of radial nodes = (n - 1) - l = (4 - 1) - 2 = 3 - 2 = 1. The question asks for the number of angular and radial nodes respectively.
The number of angular and radial nodes for 4d orbital is respectively
Asked in UPSC CAPF 2018 · Topic: Atomic Structure (Atomic Orbitals (Shapes and energies of s, p, d, f orbitals, nodal surfaces))
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