Question

What is the key distinction between sublevel energies in one- electron species, such as the H atom, and those in manyelectron species, such as the C atom? What factors lead to this distinction? Would you expect the pattern of sublevel energies in Be³⁺ to be more like that in H or that in C? Explain.

Answer 1

• All sublevels of a species with one electron have the same energy.In contrast, the energy level divides into lower levels with varying energies in many-electron species.

• For instance: H atom, n = 1 main quantum number, one-electron species. L = 0 for the angular quantum number, and 1s for the orbital

• But the primary quantum number for the C atom is n = 4. Anglular quantum number $l$ = 0, 1, 2, and 3.

• The subshells come in varied energies as 1s, 2s, 2p, and 3s.

• The larger likelihood of core is what causes the staggering.

• When compared to p orbitals, s orbitals have significantly less penetration (less shielding by core electrons).

• Since there is no shielding for H or any one-electron species (such as Be³⁺), all the sublevels follow the same pattern.

What is sublevel energies ?

Quantum theory describes an energy level as a sublevel. Sublevels are the energies connected to electrons in chemistry. Sublevels in physics can also refer to energy related to the nucleus.

Learn more about sublevel energies here:

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