Hydrogen atom has only one electron, so mutual repulsion between electrons is absent. However, in multielectron atoms mutual repulsion between the electrons is significant. How does this affect the energy of an electron in the orbitals of the same principal quantum number in multielectron atoms?
Answers
"We know that", the "energy" of electron is determined by the value of n in hydrogen atom and by n + l in multi electron atom.
So for a given "principal quantum number" electrons of s, p, d, and f orbitals have different energy.
In hydrogen atom, energy of different orbitals depends on the principal quantum numbers only.
1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f
In multi-electron species, the energy of orbitals depends on both n and f
1s < 2s < 2p < 3s < 3p < 4s < 3d
Lower is the values of (n+1), lower is the energy of orbitals. If (n+1) values are same then the orbital with "lower value" of n will have lesser energy. "
Answer:
Solution : In case of hydrogen atom, the energies of the electron in different orbitals depends only on the value of n. Hence, different orbitals of the same shell have same energy. ... However, in multielectron atoms mutual repulsion between the electrons is significant.