In a multielectron system, each electron is influenced by the attraction of the nucleus and the repulsion of the other electrons. This results in the energy of atomic orbitals being different from that of a single-electron system.
The energy of atomic orbitals in a multielectron system is affected by the shielding effect, which occurs when inner electrons block the attraction of the nucleus on outer electrons. This results in the outer electrons having a higher energy compared to those in a single-electron system.
The energy of atomic orbitals in a multielectron system determines the electron configuration and chemical properties of an atom. It also plays a crucial role in chemical bonding and the formation of molecules.
The energy of atomic orbitals in a multielectron system is calculated using the Schrödinger equation, which takes into account the electrostatic interactions between the electrons and the nucleus, as well as the repulsion between electrons.
The energy of atomic orbitals in a multielectron system is not directly observable or measurable. However, it can be indirectly determined through spectroscopic techniques, such as X-ray spectroscopy, which measure the energy differences between different atomic orbitals.