Final answer:
The calculated orbitals for the zinc atom differ in the energy levels of the orbitals due to electron shielding and repulsion. These differences are described by the Pauli exclusion principle and Hund's rule, which explain the order of orbital filling based on relative energies.
Step-by-step explanation:
The calculated orbitals for the zinc atom differ from the electron configuration in the energy levels of the orbitals (option 3). This is because electrons fill the orbitals based on the observed experimental results and are confirmed by theoretical calculations. The energy of atomic orbitals increases with the principal quantum number, n, but this is not the only factor impacting energy levels. As l (azimuthal quantum number) increases within a shell, the energy of the orbitals increases in the order of s < p < d < f due to electron shielding and electron repulsion. This result is supported by the Pauli exclusion principle and Hund's rule, indicating that the order in which orbitals fill up correlates with their relative energies, not the spin of the electrons or the number of electrons in each orbital.