Electronic Configuration of Zn (Z = 30)

The atomic number of zinc (Zn) is 30, which means it has 30 electrons. To determine the electronic configuration of Zn, we need to distribute these electrons among the available orbitals according to the Aufbau principle, Pauli exclusion principle, and Hund's rule.

Aufbau Principle:
The Aufbau principle states that electrons fill the lowest energy orbitals first before moving to higher energy orbitals. Therefore, we start by filling the 1s orbital, followed by the 2s, 2p, 3s, 3p, 4s, and so on.

Pauli Exclusion Principle:
The Pauli exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers. This means that each orbital can accommodate a maximum of two electrons with opposite spins.

Hund's Rule:
Hund's rule states that when filling degenerate orbitals (orbitals with the same energy level), electrons occupy each orbital singly with parallel spins before pairing up.

Electronic Configuration of Zinc (Zn):
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰

Breaking it down:
- 1s²: This represents the filling of the 1s orbital with two electrons.
- 2s²: This represents the filling of the 2s orbital with two electrons.
- 2p⁶: This represents the filling of the 2p orbitals (2px, 2py, 2pz) with six electrons.
- 3s²: This represents the filling of the 3s orbital with two electrons.
- 3p⁶: This represents the filling of the 3p orbitals (3px, 3py, 3pz) with six electrons.
- 4s²: This represents the filling of the 4s orbital with two electrons.
- 3d¹⁰: This represents the filling of the 3d orbitals (3dxy, 3dyz, 3dz², 3dxz, 3dx²-y²) with ten electrons.

Total Number of Occupied Orbitals:
To determine the total number of occupied orbitals that do not possess any nodal plane, we need to consider the orbitals up to the highest energy level filled.

In the electronic configuration of Zn, the highest energy level filled is the 3d orbitals (3d¹⁰). These orbitals do not possess any nodal plane.

Therefore, the total number of occupied orbitals that do not possess any nodal plane in the electronic configuration of Zn is 5 (2s, 2p, 3s, 3p, and 4s orbitals).

Conclusion:
The correct answer is '5'. The electronic configuration of Zn (Z = 30) has a total of 5 occupied orbitals that do not possess any nodal plane.