Question

In the electronic configuration of zinc (Z=30) find the total no. of occupied orbitals which do not possess any nodal plane?​ with explanation

Answer 1

Answer:

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Answer 2

We have to find the total number of occupied orbitals which do not possess any nodal plane.

what are node and nodal plane ?

node : It is a point where the probability of finding electrons must be zero.

• It is given by, node = n - 1, where n is principal quantum number.

nodal plane : It is the plane (or region) where the probability of finding electrons is zero.

• The number of nodal plane in an orbital is equal to azimuthal quantum number of that orbital.
• S - orbitals do not have any nodal plane.

electronic configuration of Zinc = 1s² , 2s² , 2p⁶ , 3s² , 3p⁶ , 4s², 3d¹⁰

no of S - orbitals = 4 [ 1s, 2s , 3s and 4s ]

from above explanation, we know only s-orbitals do not have nodal planes.

Therefore the total no of occupied orbitals which do not possess nodal plane is 4.